{"id":1929,"date":"2020-04-30T17:55:29","date_gmt":"2020-04-30T21:55:29","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/chapter\/acid-base-titrations\/"},"modified":"2022-01-13T16:49:51","modified_gmt":"2022-01-13T21:49:51","slug":"acid-base-titrations","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/chapter\/acid-base-titrations\/","title":{"raw":"8.7 Acid-Base Titrations","rendered":"8.7 Acid-Base Titrations"},"content":{"raw":"[latexpage]\r\n<div class=\"textbox textbox--learning-objectives\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\">Learning Objectives<\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Interpret titration curves for strong and weak acid-base systems<\/li>\r\n \t<li>Compute sample pH at important stages of a titration<\/li>\r\n \t<li>Explain the function of acid-base indicators<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<p id=\"fs-idm43847120\">As seen in the chapter on the stoichiometry of chemical reactions, titrations can be used to quantitatively analyze solutions for their acid or base concentrations. In this section, we will explore the underlying chemical equilibria that make acid-base titrimetry a useful analytical technique.<\/p>\r\n\r\n<div id=\"fs-idm84795552\" class=\"bc-section section\" data-depth=\"1\">\r\n<h2 data-type=\"title\">Titration Curves<\/h2>\r\n<p id=\"fs-idp135875056\">A <span data-type=\"term\">titration curve<\/span> is a plot of some solution property versus the amount of added titrant. For acid-base titrations, solution pH is a useful property to monitor because it varies predictably with the solution composition and, therefore, may be used to monitor the titration\u2019s progress and detect its endpoint. The following example exercise demonstrates the computation of pH for a titration solution after the additions of several specified titrant volumes. The first example involves a strong acid titration that requires only stoichiometric calculations to derive the solution pH. The second example addresses a weak acid titration requiring equilibrium calculations.<\/p>\r\n\r\n<div class=\"textbox textbox--examples\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\">Activity 8.7.1 - <span data-type=\"title\">Calculating pH for Titration Solutions: Strong Acid\/Strong Base<\/span><\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<p id=\"fs-idp245005248\">A titration is carried out for 25.00 mL of 0.100 <em data-effect=\"italics\">M<\/em> HCl (strong acid) with 0.100 <em data-effect=\"italics\">M<\/em> of a strong base NaOH (the titration curve is shown in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration\">(Figure 8.7.1)<\/a>). Calculate the pH at these volumes of added base solution:<\/p>\r\n<p id=\"fs-idp67154976\">(a) 0.00 mL<\/p>\r\n<p id=\"fs-idm80154320\">(b) 12.50 mL<\/p>\r\n<p id=\"fs-idm39390080\">(c) 25.00 mL<\/p>\r\n<p id=\"fs-idp81988928\">(d) 37.50 mL<\/p>\r\n\r\n<h2 id=\"fs-idp22584832\"><span data-type=\"title\">Solution<\/span><\/h2>\r\n(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 <em data-effect=\"italics\">M<\/em>. The pH of the solution is then:\r\n\r\n&nbsp;\r\n<div id=\"fs-idm213177360\" data-type=\"equation\">\\(\\text{pH}=-\\text{log}\\phantom{\\rule{0.2em}{0ex}}\\left(0.100\\right)=1.000\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0\u00a0<\/em><\/div>\r\n<p id=\"fs-idm214456576\">(b) Titrant volume = 12.50 mL. Since the acid sample and the base titrant are both monoprotic and equally concentrated, this titrant addition involves less than a stoichiometric amount of base, and so it is completely consumed by reaction with the excess acid in the sample. The concentration of acid remaining is computed by subtracting the consumed amount from the intial amount and then dividing by the solution volume:<\/p>\r\n&nbsp;\r\n<div id=\"fs-idp80308976\" data-type=\"equation\">\\(\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]=\\phantom{\\rule{0.2em}{0ex}}\\frac{\\text{n}\\left({\\text{H}}^{\\text{+}}\\right)}{V}\\phantom{\\rule{0.2em}{0ex}}=\\phantom{\\rule{0.2em}{0ex}}\\frac{\\text{0.002500 mol}\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}\\left(\\phantom{\\rule{0.2em}{0ex}}\\frac{\\text{1000 mL}}{\\text{1 L}}\\right)\\phantom{\\rule{0.2em}{0ex}}-0.100\\phantom{\\rule{0.4em}{0ex}}M\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}\\text{12.50 mL}}{\\text{25.00 mL}+\\text{12.50 mL}}\\phantom{\\rule{0.2em}{0ex}}=0.0333\\phantom{\\rule{0.4em}{0ex}}M\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0 <\/em><\/div>\r\n(c) Titrant volume = 25.00 mL. This titrant addition involves a stoichiometric amount of base (the <em data-effect=\"italics\">equivalence point<\/em>), and so only products of the neutralization reaction are in solution (water and NaCl). Neither the cation nor the anion of this salt undergoes acid-base ionization; the only process generating hydronium ions is the autoprotolysis of water. The solution is neutral, having a pH = 7.00.\r\n<p id=\"fs-idm173154048\">(d) Titrant volume = 37.50 mL. This involves the addition of titrant in excess of the equivalence point. The solution pH is then calculated using the concentration of hydroxide ion:<\/p>\r\n<em>\u00a0\u00a0<\/em>\r\n<div id=\"fs-idp66422816\" data-type=\"equation\">\\(\\text{n}{\\left({\\text{OH}^-}^{\\text{}}\\right)}_{0}&gt;\\text{n}{\\left({\\text{H}}^{\\text{+}}\\right)}_{0}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0\u00a0<\/em><\/div>\r\n<div id=\"fs-idm15386080\" data-type=\"equation\">\\(\\left[{\\text{OH}^-}^{\\text{}}\\right]=\\phantom{\\rule{0.2em}{0ex}}\\frac{\\text{n}\\left({\\text{OH}^-}^{\\text{}}\\right)}{V}\\phantom{\\rule{0.2em}{0ex}}=\\phantom{\\rule{0.2em}{0ex}}\\frac{0.100\\phantom{\\rule{0.4em}{0ex}}M\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}\\text{35.70 mL}-\\text{0.002500 mol}\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}\\left(\\phantom{\\rule{0.2em}{0ex}}\\frac{\\text{1000 mL}}{\\text{1 L}}\\right)\\phantom{\\rule{0.2em}{0ex}}}{\\text{25.00 mL}+\\text{37.50 mL}}\\phantom{\\rule{0.2em}{0ex}}=0.0200\\phantom{\\rule{0.4em}{0ex}}M\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0\u00a0<\/em><\/div>\r\n<p id=\"fs-idm41259968\">pH = 14 \u2212 pOH = 14 + log([OH<sup>\u2212<\/sup>]) = 14 + log(0.0200) = 12.30<\/p>\r\n\r\n\r\n<hr \/>\r\n\r\n<h2 id=\"fs-idm15929056\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\r\nCalculate the pH for the strong acid\/strong base titration between 50.0 mL of 0.100 <em data-effect=\"italics\">M<\/em> HNO<sub>3<\/sub>(<em data-effect=\"italics\">aq<\/em>) and 0.200 <em data-effect=\"italics\">M<\/em> NaOH (titrant) at the listed volumes of added base: 0.00 mL, 15.0 mL, 25.0 mL, and 40.0 mL.\r\n<div id=\"fs-idm44981872\" data-type=\"note\">\r\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\r\n<p id=\"fs-idm89702512\" style=\"text-align: right\">0.00 mL, pH =\u00a0 1.000<\/p>\r\n<p style=\"text-align: right\">15.0 mL, pH = 1.5111<\/p>\r\n<p style=\"text-align: right\">25.0 mL, pH =\u00a0 7<\/p>\r\n<p style=\"text-align: right\">40.0 mL, pH = 12.523<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox textbox--examples\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\">Activity 8.7.2 - <span data-type=\"title\">Titration of a Weak Acid with a Strong Base<\/span><\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<p id=\"fs-idp114806608\">Consider the titration of 25.00 mL of 0.100 <em data-effect=\"italics\">M<\/em> CH<sub>3<\/sub>CO<sub>2<\/sub>H with 0.100 <em data-effect=\"italics\">M<\/em> NaOH. The reaction can be represented as:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp77362464\" data-type=\"equation\">\\({\\text{CH}}_{3}{\\text{CO}}_{2}\\text{H}+{\\text{OH}^-}^{\\text{}}\\phantom{\\rule{0.2em}{0ex}}$\\rightarrow$\\phantom{\\rule{0.2em}{0ex}}{\\text{CH}}_{3}{\\text{CO}}_{2}{^-}^{\\text{}}+{\\text{H}}_{2}\\text{O}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm41606112\">Calculate the pH of the titration solution after the addition of the following volumes of NaOH titrant:<\/p>\r\n<p id=\"fs-idm192768656\">(a) 0.00 mL<\/p>\r\n<p id=\"fs-idm178030592\">(b) 25.00 mL<\/p>\r\n<p id=\"fs-idm214305872\">(c) 12.50 mL<\/p>\r\n<p id=\"fs-idm223741312\">(d) 37.50 mL<\/p>\r\n\r\n<h2 id=\"fs-idp3678224\"><span data-type=\"title\">Solution<\/span><\/h2>\r\n(a) The initial pH is computed for the acetic acid solution in the usual ICE approach:\r\n\r\n<em>\u00a0<\/em>\r\n<p id=\"fs-idp30610784\">\\({K}_{\\text{a}}=\\phantom{\\rule{0.2em}{0ex}}\\frac{\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]\\left[{\\text{CH}}_{3}{\\text{CO}}_{2}{^-}^{\\text{}}\\right]}{\\left[{\\text{CH}}_{3}{\\text{CO}}_{2}\\text{H}\\right]}\\phantom{\\rule{0.2em}{0ex}}\\approx \\phantom{\\rule{0.2em}{0ex}}\\frac{{\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]}^{\\text{2}}}{{\\left[{\\text{CH}}_{3}{\\text{CO}}_{2}\\text{H}\\right]}_{0}}\\phantom{\\rule{0.2em}{0ex}},\\) and \\(\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]=\\sqrt{{K}_{a}\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}\\left[{\\text{CH}}_{3}{\\text{CO}}_{2}\\text{H}\\right]}=\\sqrt{1.8\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-5}\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}0.100}=1.3\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-3}\\)<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm76922320\" data-type=\"equation\">\\(\\text{pH}={-}\\text{log}\\left(1.3\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-3}\\right)=2.87\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm935760\">(b) The acid and titrant are both monoprotic and the sample and titrant solutions are equally concentrated; thus, this volume of titrant represents the equivalence point. Unlike the strong-acid example above, however, the reaction mixture, in this case, contains a weak conjugate base (acetate ion). The solution pH is computed considering the base ionization of acetate, which is present at a concentration of:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm33154592\" data-type=\"equation\">\\(\\frac{\\text{0.00250 mol}}{\\text{0.0500 L}}\\phantom{\\rule{0.2em}{0ex}}=\\text{0.0500 M} {\\text{CH}}_{3}{\\text{CO}}_{2}{^-}^{\\text{\u2212}}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm2004176\">Base ionization of acetate is represented by the equation:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp77139280\" data-type=\"equation\">\\({\\text{CH}}_{3}{\\text{CO}}_{2}{^-}^{\\text{}}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\phantom{\\rule{0.2em}{0ex}}$\\rightleftharpoons$\\phantom{\\rule{0.2em}{0ex}}{\\text{CH}}_{3}{\\text{CO}}_{2}\\text{H}\\left(aq\\right)+{\\text{OH}^-}^{\\text{}}\\left(aq\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idp75313664\" data-type=\"equation\">\\({K}_{\\text{b}}=\\phantom{\\rule{0.2em}{0ex}}\\frac{\\left[{\\text{H}}^{\\text{+}}\\right]\\left[{\\text{OH}^-}^{\\text{}}\\right]}{{K}_{\\text{a}}}\\phantom{\\rule{0.2em}{0ex}}=\\phantom{\\rule{0.2em}{0ex}}\\frac{{K}_{\\text{w}}}{{K}_{\\text{a}}}\\phantom{\\rule{0.2em}{0ex}}=\\phantom{\\rule{0.2em}{0ex}}\\frac{1.0\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-14}}{1.8\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-5}}\\phantom{\\rule{0.2em}{0ex}}=\\phantom{\\rule{0.2em}{0ex}}5.6\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-10}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idp58734736\">Assuming <em data-effect=\"italics\">x<\/em> &lt;&lt; 0.0500, the pH may be calculated via the usual ICE approach:<\/p>\r\n<em>\u00a0\u00a0<\/em>\r\n\r\n\\({K}_{\\text{b}}=\\phantom{\\rule{0.2em}{0ex}}\\frac{{x}^{\\text{2}}}{0.0500\\phantom{\\rule{0.2em}{0ex}}M}\\)\r\n\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm58971824\" data-type=\"equation\">\\(x=\\left[{\\text{OH}^-}^{\\text{}}\\right]=5.3\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-6}\\)<\/div>\r\n<div id=\"fs-idp1478112\" data-type=\"equation\">\\(\\text{pOH}={-}\\text{log}\\left(5.3\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-6}\\right)=5.28\\)<\/div>\r\n<div id=\"fs-idm54099632\" data-type=\"equation\">\\(\\text{pH}=14.00-5.28=8.72\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm40620912\">Note that the pH at the equivalence point of this titration is significantly greater than 7, as expected when titrating a weak acid with a strong base.<\/p>\r\n<p id=\"fs-idm15954576\">(c) Titrant volume = 12.50 mL. This volume represents one-half of the stoichiometric amount of titrant, and so one-half of the acetic acid has been neutralized to yield an equivalent amount of acetate ion. The concentrations of these conjugate acid-base partners, therefore, are equal. A convenient approach to computing the pH is use of the Henderson-Hasselbalch equation:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp121571008\" data-type=\"equation\">\\(\\text{pH}=p{K}_{\\text{a}}+\\text{log}\\phantom{\\rule{0.2em}{0ex}}\\frac{\\left[\\text{Base}\\right]}{\\left[\\text{Acid}\\right]}\\phantom{\\rule{0.2em}{0ex}}={-}\\text{log}\\left({K}_{\\text{a}}\\right)+\\text{log}\\phantom{\\rule{0.2em}{0ex}}\\frac{\\left[{\\text{CH}}_{3}{\\text{CO}}_{2}{^-}^{\\text{}}\\right]}{\\left[{\\text{CH}}_{3}{\\text{CO}}_{2}\\text{H}\\right]}\\phantom{\\rule{0.2em}{0ex}}={-}\\text{log}\\left(1.8\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-5}\\right)+\\text{log}\\left(1\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idp163867552\" data-type=\"equation\">\\(\\text{pH}={-}\\text{log}\\left(1.8\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-5}\\right)=4.74\\)<\/div>\r\n<em>\u00a0\u00a0<\/em>\r\n<p id=\"fs-idm42058672\">(pH = p<em data-effect=\"italics\">K<\/em><sub>a<\/sub> at the half-equivalence point in a titration of a weak acid)<\/p>\r\n<em>\u00a0<\/em>\r\n<p id=\"fs-idp85997072\">(d) Titrant volume = 37.50 mL. This volume represents a stoichiometric excess of titrant, and a reaction solution containing both the titration product, acetate ion, and the excess strong titrant. In such solutions, the solution pH is determined primarily by the amount of excess strong base:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm52967552\" data-type=\"equation\">\\(\\left[{\\text{OH}^-}^{\\text{}}\\right]=\\phantom{\\rule{0.2em}{0ex}}\\frac{\\left(\\text{0.003750 mol}-\\text{0.00250 mol}\\right)}{\\text{0.06250 L}}\\phantom{\\rule{0.2em}{0ex}}=2.00\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-2}\\phantom{\\rule{0.2em}{0ex}}M\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0 <\/em><\/div>\r\n<div id=\"fs-idm21431696\" data-type=\"equation\">\\(\\text{pOH}={-}\\text{log}\\left(2.00\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-2}\\right)=\\text{1.70, and pH}=14.00-1.70=12.30\\)<\/div>\r\n<div data-type=\"equation\">\r\n\r\n<hr \/>\r\n\r\n<\/div>\r\n<h2 id=\"fs-idm41682336\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\r\nCalculate the pH for the weak acid\/strong base titration between 50.0 mL of 0.100 <em data-effect=\"italics\">M<\/em> HCOOH(<em data-effect=\"italics\">aq<\/em>) (formic acid) and 0.200 <em data-effect=\"italics\">M<\/em> NaOH (titrant) at the listed volumes of added base: 0.00 mL, 15.0 mL, 25.0 mL, and 30.0 mL.\r\n<div id=\"fs-idp68668928\" data-type=\"note\">\r\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\r\n<p id=\"fs-idm37877472\" style=\"text-align: right\">0.00 mL, pH = 2.37<\/p>\r\n<p style=\"text-align: right\">15.0 mL, pH = 3.92<\/p>\r\n<p style=\"text-align: right\">25.00 mL, pH = 8.29<\/p>\r\n<p style=\"text-align: right\">30.0 mL, pH = 12.097<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<p id=\"fs-idm198420960\">Performing additional calculations similar to those in the preceding example permits a more full assessment of titration curves. A summary of pH\/volume data pairs for the strong and weak acid titrations is provided in <a class=\"autogenerated-content\" href=\"#fs-idm87178400\">(Table 8.7.1)<\/a> and plotted as titration curves in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration\">(Figure 8.7.1)<\/a>. A comparison of these two curves illustrates several important concepts that are best addressed by identifying the four stages of a titration:<\/p>\r\n<p id=\"fs-idm201863856\"><strong>Initial state (added titrant volume = 0 mL)<\/strong>: pH is determined by the acid being titrated; because the two acid samples are equally concentrated, the weak acid will exhibit a greater initial pH<\/p>\r\n<p id=\"fs-idm444217232\"><strong>Pre-equivalence point (0 mL &lt; <em data-effect=\"italics\">V<\/em> &lt; 25 mL)<\/strong>: solution pH increases gradually and the acid is consumed by reaction with added titrant; composition includes unreacted acid and the reaction product, its conjugate base<\/p>\r\n<p id=\"fs-idm183388016\"><strong>Equivalence point (<em data-effect=\"italics\">V<\/em> = 25 mL)<\/strong>: a drastic rise in pH is observed as the solution composition transitions from acidic to either neutral (for the strong acid sample) or basic (for the weak acid sample), with pH determined by ionization of the conjugate base of the acid<\/p>\r\n<p id=\"fs-idm183509856\"><strong>Postequivalence point (<em data-effect=\"italics\">V<\/em> &gt; 25 mL)<\/strong>: pH is determined by the amount of excess strong base titrant added; since both samples are titrated with the same titrant, both titration curves appear similar at this stage.<\/p>\r\n\r\n<table id=\"fs-idm87178400\" class=\"aligncenter\" summary=\"This table has four columns and twenty rows. The first row is a header row, and it labels each column, \u201cVolume of 0.100 M N a O H Added ( m L ),\u201d \u201cMoles of N a O H Added,\u201d \u201cp H Values 0.100 M H C l footnote one,\u201d \u201cp H Values 0.100 M C H subscript 3 C O subscript 2 H footnote 2.\u201d Under the \u201cVolume of 0.100 M N a O H Added ( m L )\u201d column are the following values: 0.0, 5.0, 10.0, 15.0, 20.0, 22.0, 24.0, 24.5, 24.9, 25.0, 25.1, 25.5, 26.0, 28.0, 30.0, 35.0, 40.0, 45.0, and 50.0. Under the \u201cMoles of N a O H Added\u201d column are the following values: 0.0, 0.00050, 0.00100, 0.00150, 0.00200, 0.00220, 0.00240, 0.00245, 0.00249, 0.00250, 0.00251, 0.00255, 0.00260, 0.00280, 0.00300, 0.00350, 0.00400, 0.00450, and 0.00500. Under the \u201cp H Values 0.100 M H C l footnote one\u201d column are the following values: 1.00, 1.18, 1.37, 1.60, 1.95, 2.20, 2.69, 3.00, 3.70, 7.00, 10.30, 11.00, 11.29, 11.75, 11.96, 12.22, 12.36, 12.46, and 12.52. Foot note one reads, \u201cTitration of 25.00 m L of 0.100 M H C l ( 0.00250 mol of H C I ) with 0.100 M N a O H.\u201d Under the \u201cp H Values 0.100 M C H subscript 3 C O subscript 2 H footnote 2\u201d column are the following values: 2.87, 4.14, 4.57, 4.92, 5.35, 5.61, 6.13, 6.44, 7.17, 8.72, 10.30, 11.00, 11.29, 11.75, 11.96, 12.22, 12.36, 12.46, and 12.52. Footnote two reads, \u201cTitration of 25.00 m L of 0.100 M C H subscript 3 C O subscript 2 H ( 0.00250 mol of C H subscript 3C O subscript 2 H) with 0.100 M N a O H.\u201d\"><caption>Table 8.7.1 -\u00a0 pH Values in the Titrations of a Strong Acid and of a Weak Acid<\/caption>\r\n<thead>\r\n<tr valign=\"top\">\r\n<th data-align=\"left\">Volume of 0.100 <em data-effect=\"italics\">M<\/em> NaOH Added (mL)<\/th>\r\n<th data-align=\"left\">Moles of NaOH Added<\/th>\r\n<th data-align=\"left\">pH Values 0.100 <em data-effect=\"italics\">M<\/em> HCl[footnote]Titration of 25.00 mL of 0.100 M HCl (0.00250 mol of HCI) with 0.100 M NaOH.[\/footnote]<\/th>\r\n<th data-align=\"left\">pH Values 0.100 <em data-effect=\"italics\">M<\/em> CH<sub>3<\/sub>CO<sub>2<\/sub>H[footnote]Titration of 25.00 mL of 0.100 <em data-effect=\"italics\">M<\/em> CH<sub>3<\/sub>CO<sub>2<\/sub>H (0.00250 mol of CH<sub>3<\/sub>CO<sub>2<\/sub>H) with 0.100 <em data-effect=\"italics\">M<\/em> NaOH.[\/footnote]<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">0.0<\/td>\r\n<td data-align=\"left\">0.0<\/td>\r\n<td data-align=\"left\">1.00<\/td>\r\n<td data-align=\"left\">2.87<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">5.0<\/td>\r\n<td data-align=\"left\">0.00050<\/td>\r\n<td data-align=\"left\">1.18<\/td>\r\n<td data-align=\"left\">4.14<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">10.0<\/td>\r\n<td data-align=\"left\">0.00100<\/td>\r\n<td data-align=\"left\">1.37<\/td>\r\n<td data-align=\"left\">4.57<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">15.0<\/td>\r\n<td data-align=\"left\">0.00150<\/td>\r\n<td data-align=\"left\">1.60<\/td>\r\n<td data-align=\"left\">4.92<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">20.0<\/td>\r\n<td data-align=\"left\">0.00200<\/td>\r\n<td data-align=\"left\">1.95<\/td>\r\n<td data-align=\"left\">5.35<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">22.0<\/td>\r\n<td data-align=\"left\">0.00220<\/td>\r\n<td data-align=\"left\">2.20<\/td>\r\n<td data-align=\"left\">5.61<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">24.0<\/td>\r\n<td data-align=\"left\">0.00240<\/td>\r\n<td data-align=\"left\">2.69<\/td>\r\n<td data-align=\"left\">6.13<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">24.5<\/td>\r\n<td data-align=\"left\">0.00245<\/td>\r\n<td data-align=\"left\">3.00<\/td>\r\n<td data-align=\"left\">6.44<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">24.9<\/td>\r\n<td data-align=\"left\">0.00249<\/td>\r\n<td data-align=\"left\">3.70<\/td>\r\n<td data-align=\"left\">7.14<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">25.0<\/td>\r\n<td data-align=\"left\">0.00250<\/td>\r\n<td data-align=\"left\">7.00<\/td>\r\n<td data-align=\"left\">8.72<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">25.1<\/td>\r\n<td data-align=\"left\">0.00251<\/td>\r\n<td data-align=\"left\">10.30<\/td>\r\n<td data-align=\"left\">10.30<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">25.5<\/td>\r\n<td data-align=\"left\">0.00255<\/td>\r\n<td data-align=\"left\">11.00<\/td>\r\n<td data-align=\"left\">11.00<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">26.0<\/td>\r\n<td data-align=\"left\">0.00260<\/td>\r\n<td data-align=\"left\">11.29<\/td>\r\n<td data-align=\"left\">11.29<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">28.0<\/td>\r\n<td data-align=\"left\">0.00280<\/td>\r\n<td data-align=\"left\">11.75<\/td>\r\n<td data-align=\"left\">11.75<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">30.0<\/td>\r\n<td data-align=\"left\">0.00300<\/td>\r\n<td data-align=\"left\">11.96<\/td>\r\n<td data-align=\"left\">11.96<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">35.0<\/td>\r\n<td data-align=\"left\">0.00350<\/td>\r\n<td data-align=\"left\">12.22<\/td>\r\n<td data-align=\"left\">12.22<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">40.0<\/td>\r\n<td data-align=\"left\">0.00400<\/td>\r\n<td data-align=\"left\">12.36<\/td>\r\n<td data-align=\"left\">12.36<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">45.0<\/td>\r\n<td data-align=\"left\">0.00450<\/td>\r\n<td data-align=\"left\">12.46<\/td>\r\n<td data-align=\"left\">12.46<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"left\">50.0<\/td>\r\n<td data-align=\"left\">0.00500<\/td>\r\n<td data-align=\"left\">12.52<\/td>\r\n<td data-align=\"left\">12.52<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<div id=\"CNX_Chem_14_07_titration\" class=\"bc-figure figure\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"1300\"]<img src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_07_titration-1.jpg\" alt=\"Two graphs are shown. The first graph on the left is titled \u201cTitration of Weak Acid.\u201d The horizontal axis is labeled \u201cVolume of 0.100 M N a O H added (m L).\u201d Markings and vertical gridlines are provided every 5 units from 0 to 50. The vertical axis is labeled \u201cp H\u201d and is marked every 1 unis beginning at 0 extending to 14. A red curve is drawn on the graph which increases steadily from the point (0, 3) up to about (20, 5.5) after which the graph has a vertical section from (25, 7) up to (25, 11). The graph then levels off to a value of about 12.5 from about 40 m L up to 50 m L. The midpoint of the vertical segment of the curve is labeled \u201cEquivalence point p H, 8.72.\u201d The second graph on the right is titled \u201cTitration of Strong Acid.\u201d The horizontal axis is labeled \u201cVolume of 0.100 M N a O H added (m L).\u201d Markings and vertical gridlines are provided every 5 units from 0 to 50. The vertical axis is labeled \u201cp H\u201d and is marked every 1 units beginning at 0 extending to 14. A red curve is drawn on the graph which increases gradually from the point (0, 1) up to about (22.5, 2.2) after which the graph has a vertical section from (25, 4) up to nearly (25, 11). The graph then levels off to a value of about 12.4 from about 40 m L up to 50 m L. The midpoint of the vertical segment of the curve is labeled \u201cEquivalence point p H, 7.00.\u201d\" width=\"1300\" height=\"731\" data-media-type=\"image\/jpeg\" \/> <strong>Figure 8.7.1 - (a) The titration curve for the titration of 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M NaOH (strong base) has an equivalence point of 7.00 pH. (b) The titration curve for the titration of 25.00 mL of 0.100 M acetic acid (weak acid) with 0.100 M NaOH (strong base) has an equivalence point of 8.72 pH.<\/strong>[\/caption]\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp22610576\" class=\"bc-section section\" data-depth=\"1\">\r\n<h2 data-type=\"title\">Acid-Base Indicators<\/h2>\r\n<p id=\"fs-idm39085312\">Certain organic substances change color in dilute solution when the hydronium ion concentration reaches a particular value. For example, phenolphthalein is a colorless substance in an aqueous solution with a hydronium ion concentration greater than 5.0 \\(\u00d7\\) 10<sup>\u22129<\/sup><em data-effect=\"italics\">M<\/em> (pH &lt; 8.3). In more basic solutions where the hydronium ion concentration is less than 5.0 \\(\u00d7\\) 10<sup>\u22129<\/sup><em data-effect=\"italics\">M<\/em> (pH &gt; 8.3), it is red or pink. Substances such as phenolphthalein, which can be used to determine the pH of a solution, are called <span data-type=\"term\">acid-base indicators<\/span>. Acid-base indicators are either weak organic acids or weak organic bases.<\/p>\r\n<p id=\"fs-idm28417392\">The equilibrium in a solution of the acid-base indicator methyl orange, a weak acid, can be represented by an equation in which we use HIn as a simple representation for the complex methyl orange molecule:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp80468176\" data-type=\"equation\">\\(\\begin{array}{ccc}\\text{HIn}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)&amp; \\phantom{\\rule{0.2em}{0ex}}$\\rightleftharpoons$\\phantom{\\rule{0.2em}{0ex}}&amp; {\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\left(aq\\right)+{\\text{In}^-}^{\\text{}}\\left(aq\\right)\\\\ \\phantom{\\rule{0.5em}{0ex}}\\text{red}\\hfill &amp; &amp; \\phantom{\\rule{5.5em}{0ex}}\\text{yellow}\\hfill &amp; \\end{array}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm87967824\" data-type=\"equation\">\\({K}_{a}=\\phantom{\\rule{0.2em}{0ex}}\\frac{\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]\\left[{\\text{In}^-}^{\\text{}}\\right]}{\\left[\\text{HIn}\\right]}\\phantom{\\rule{0.2em}{0ex}}=4.0\\phantom{\\rule{0.2em}{0ex}}\u00d7\\phantom{\\rule{0.2em}{0ex}}{10}^{-4}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm68547888\">The anion of methyl orange, In<sup>\u2212<\/sup>, is yellow, and the nonionized form, HIn, is red. When we add acid to a solution of methyl orange, the increased hydronium ion concentration shifts the equilibrium toward the nonionized red form, in accordance with Le Ch\u00e2telier\u2019s principle. If we add base, we shift the equilibrium towards the yellow form. This behavior is completely analogous to the action of buffers.<\/p>\r\n<p id=\"fs-idp64938256\">The perceived color of an indicator solution is determined by the ratio of the concentrations of the two species In<sup>\u2212<\/sup> and HIn. If most of the indicator (typically about 60\u221290% or more) is present as In<sup>\u2212<\/sup>, the perceived color of the solution is yellow. If most is present as HIn, then the solution color appears red. The Henderson-Hasselbalch equation is useful for understanding the relationship between the pH of an indicator solution and its composition (thus, perceived color):<\/p>\r\n&nbsp;\r\n<div id=\"fs-idp80076272\" data-type=\"equation\">\\(\\text{pH}=\\text{p}K\\text{a}+\\text{log}\\left(\\phantom{\\rule{0.2em}{0ex}}\\frac{\\left[{\\text{In}^-}^{\\text{}}\\right]}{\\left[\\text{HIn}\\right]}\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm188576256\">In solutions where pH &gt; p<em data-effect=\"italics\">K<\/em><sub>a<\/sub>, the logarithmic term must be positive, indicating an excess of the conjugate base form of the indicator (yellow solution). When pH &gt; p<em data-effect=\"italics\">K<\/em><sub>a<\/sub>, the log term must be negative, indicating an excess of the conjugate acid (red solution). When the solution pH is close to the indicator pKa, appreciable amounts of both conjugate partners are present, and the solution color is that of an additive combination of each (yellow and red, yielding orange). The <span data-type=\"term\">color change interval<\/span> (or <em data-effect=\"italics\">pH interval<\/em>) for an acid-base indicator is defined as the range of pH values over which a change in color is observed, and for most indicators this range is approximately p<em data-effect=\"italics\">K<\/em><sub>a<\/sub> \u00b1 1.<\/p>\r\n<p id=\"fs-idm92451888\">There are many different acid-base indicators that cover a wide range of pH values and can be used to determine the approximate pH of an unknown solution by a process of elimination. Universal indicators and pH paper contain a mixture of indicators and exhibit different colors at different pHs. <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_indicators\">(Figure 8.7.2)<\/a> presents several indicators, their colors, and their color-change intervals.<\/p>\r\n\r\n<div id=\"CNX_Chem_14_07_indicators\" class=\"bc-figure figure\">\r\n<div class=\"bc-figcaption figcaption\"><\/div>\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"1300\"]<img src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_07_indicators-1-1.jpg\" alt=\"This figure provides a graphical representation of indicators and color ranges. A horizontal axis is labeled \u201cp H.\u201d This axis begins at zero and increases by ones up to 13. The left side of the graphic provides a column with the names of indicators. To the right of each indicator name is either one or two colored bars that are shaded according to the indicator color at various p H ranges. From the top, the first row is labeled \u201cCrystal violet.\u201d The associated colored bar is yellow at its left end at a p H of 0 and changes to green and blue moving right to its endpoint at a p H of 1.8. The second row is labeled \u201cCresol red.\u201d The associated colored bar is red at its left end at a p H of 1 and changes to orange and yellow moving right to its endpoint at a p H of just over 2. A second bar to its right is yellow at a p H of around 7 and proceeds through orange to red at a p H of about 9. The third row is labeled \u201cThymol blue.\u201d The associated colored bar is red at its left end at a p H of nearly 1.2 and changes to orange and red moving right to its endpoint at a p H of 2.8. A second bar begins in yellow at a p H of 8 and proceeds through green and blue to its end at a p H of around 9.1. The fourth row is labeled \u201cErythrosin B.\u201d The associated colored bar is red from a p H of 2.2 to its endpoint at a p H of 3.6. The fifth row is labeled \u201c2 comma 4 dash Dinitrophenol.\u201d The associated colored bar is white at its left end at a p H of 2.6 and changes to yellow at its endpoint at a p H of 4. The sixth row is labeled \u201cBromophenol blue.\u201d The associated colored bar is yellow at its left end at a p H of 3 and changes to green and blue moving right to its endpoint at a p H of 4.5. The seventh row is labeled \u201cMethyl orange.\u201d The associated colored bar is red-orange at its left end at a p H of 4.2 and changes to yellow moving right to its endpoint at a p H of 6.3. The eighth row is labeled \u201cBromocresol green.\u201d The associated colored bar is yellow at its left end at a p H of 3.8 and changes to green and blue moving right to its endpoint at a p H of 5.4. The ninth row is labeled \u201cMethyl red.\u201d The associated colored bar is orange at its left end at a p H of 4.2 and changes to yellow moving right to its endpoint at a p H of 6.3. The tenth row is labeled \u201cEriochrome * Black T.\u201d The associated colored bar is red at its left end at a p H of 5 and changes to purple and blue moving right to its endpoint at a p H of 6.5. The eleventh row is labeled \u201cBromocresol purple.\u201d The associated colored bar is yellow at its left end at a p H of 5.2 and changes to purple moving right to its endpoint at a p H of 6.8. The twelfth row is labeled \u201cAlizarin.\u201d The first associated colored bar is yellow-orange at its left end at a p H of 5.7 and changes to red moving right to its endpoint at a p H of 7.2. A second bar begins in red at a p H of 11 and changes to purple, then dark blue at its right end at a p H of 12.4. The thirteenth row is labeled \u201cBromothymol blue.\u201d The associated colored bar is yellow at its left end at a p H of 6 and changes to green and blue moving right to its endpoint at a p H of 7.6. The fourteenth row is labeled \u201cPhenol red.\u201d The associated colored bar is yellow-orange at its left end at a p H of 6.8 and changes to orange and red moving right to its endpoint at a p H of 8.2. The fifteenth row is labeled \u201cm dash Nitrophenol.\u201d The associated colored bar is white at its left end at a p H of 6.8 and changes to yellow moving right to its endpoint at a p H of 8.6. The sixteenth row is labeled \u201co dash Cresolphthalein.\u201d The associated colored bar is white at its left end at a p H of 8.3 and changes to red moving right to its endpoint at a p H of 9.8. The seventeenth row is labeled \u201cPhenolphthalein.\u201d The associated colored bar is white at its left end at a p H of 8 and changes to pink moving right to its endpoint at a p H of 10. The eighteenth row is labeled \u201cThymolphthalein.\u201d The associated colored bar is light blue at its left end at a p H of 9.3 and changes to a deep, dark blue moving right to its endpoint at a p H of 10.5. The nineteenth row is labeled \u201cAlizarin yellow R.\u201d The associated colored bar is yellow-orange at its left end at a p H of 10 and changes to red moving right to its endpoint at a p H of 12.\" width=\"1300\" height=\"1137\" data-media-type=\"image\/jpeg\" \/> <strong>Figure 8.7.2 - This chart illustrates the color change intervals for several acid-base indicators.<\/strong>[\/caption]\r\n\r\n<\/div>\r\n<div id=\"CNX_Chem_14_07_titration2\" class=\"bc-figure figure\">\r\n<div class=\"bc-figcaption figcaption\"><\/div>\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"1300\"]<img src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_07_titration2-1-1.jpg\" alt=\"A graph is shown which is titled \u201cTitration of Weak Acid.\u201d The horizontal axis is labeled \u201cVolume of 0.100 M N a O H added (m L)\u201d and begins at 0 with markings every 5 units up to 50. The vertical axis is labeled \u201cp H\u201d and begins at 0 and increases by single units up to 14. A red curve is drawn on the graph. The curve begins at (0, 3) and passes through the points (5, 4.1), (10, 4.7), (15, 5), (20, 5.5), and (22.5, 6), after which it rapidly increases, forming a vertical section centered at the point (25, 8.7). The rapid increase of the curve then levels off and the curve passes through the points (30, 12), (35, 12.4), (40, 12.5), (45, 12.6), and (50, 12.6). A brown rectangle extends horizontally across the graph covering the p H of 3 to 4.2 range. To the right, this rectangle is labeled \u201cMethyl orange p H range.\u201d A blue rectangle extends horizontally across the graph covering the p H of 4.6 to 8 range. To the right, this rectangle is labeled \u201cLitmus p H range.\u201d A purple rectangle extends horizontally across the graph covering the p H of 8.4 to 10 range. To the right, this rectangle is labeled \u201cPhenolphthalein p H range.\u201d The midpoint of the vertical segment of the curve is labeled \u201cEquivalence point p H, 8.72.\u201d\" width=\"1300\" height=\"872\" data-media-type=\"image\/jpeg\" \/> <strong>Figure 8.7.3 - Titration curves for strong and weak acids illustrating the proper choice of acid-base indicator. Any of the three indicators will exhibit a reasonably sharp color change at the equivalence point of the strong acid titration, but only phenolphthalein is suitable for use in the weak acid titration.<\/strong>[\/caption]\r\n\r\n<\/div>\r\n<p id=\"fs-idm188916592\">The titration curves shown in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration2\">(Figure 8.7.3)<\/a> illustrate the choice of a suitable indicator for specific titrations. In the strong acid titration, use of any of the three indicators should yield reasonably sharp color changes and accurate end point determinations. For this titration, the solution pH reaches the lower limit of the methyl orange color change interval after addition of ~24 mL of titrant, at which point the initially red solution would begin to appear orange. When 25 mL of titrant has been added (the equivalence point), the pH is well above the upper limit and the solution will appear yellow. The titration's end point may then be estimated as the volume of titrant that yields a distinct orange-to-yellow color change. This color change would be challenging for most human eyes to precisely discern. More-accurate estimates of the titration end point are possible using either litmus or phenolphthalein, both of which exhibit color change intervals that are encompassed by the steep rise in pH that occurs around the 25.00 mL equivalence point.<\/p>\r\n<p id=\"fs-idm224614176\">The weak acid titration curve in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration2\">(Figure 8.7.3)<\/a> shows that only one of the three indicators is suitable for end point detection. If methyl orange is used in this titration, the solution will undergo a gradual red-to-orange-to-yellow color change over a relatively large volume interval (0\u20136 mL), completing the color change well before the equivalence point (25 mL) has been reached. Use of litmus would show a color change that begins after adding 7\u20138 mL of titrant and ends just before the equivalence point. Phenolphthalein, on the other hand, exhibits a color change interval that nicely brackets the abrupt change in pH occurring at the titration's equivalence point. A sharp color change from colorless to pink will be observed within a very small volume interval around the equivalence point.<\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idp81138704\" class=\"summary\" data-depth=\"1\">\r\n<h1 data-type=\"title\">Key Concepts and Summary<\/h1>\r\n<div class=\"textbox textbox--exercises\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\">End of Chapter Exercises<\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<div id=\"fs-idp81138704\" class=\"summary\" data-depth=\"1\">\r\n<p id=\"fs-idp77329840\">(1) The titration curve for an acid-base titration is typically a plot of pH versus volume of added titrant. These curves are useful in selecting appropriate acid-base indicators that will permit accurate determinations of titration end points.<\/p>\r\n&nbsp;\r\n\r\n<\/div>\r\n<div id=\"fs-idp63641264\" class=\"exercises\" data-depth=\"1\">\r\n<div id=\"fs-idm5595328\" data-type=\"exercise\">\r\n<div id=\"fs-idp5936080\" data-type=\"problem\">\r\n<p id=\"fs-idp67232528\">(2) Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.<\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idp131233712\" data-type=\"solution\">\r\n\r\n&nbsp;\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n<p id=\"fs-idm66845488\" style=\"padding-left: 40px\">At the equivalence point in the titration of a weak base with a strong acid, the resulting solution is slightly acidic due to the presence of the conjugate acid. Thus, pick an indicator that changes color in the acidic range and brackets the pH at the equivalence point. Methyl orange is a good example.<\/p>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm81056688\" data-type=\"exercise\">\r\n<div id=\"fs-idm86623888\" data-type=\"problem\">\r\n<p id=\"fs-idp73771216\">(3) Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.<\/p>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp255636208\" data-type=\"exercise\">\r\n<div id=\"fs-idp255636464\" data-type=\"problem\">\r\n<p id=\"fs-idp255636720\">(4) Calculate the pH at the following points in a titration of 40 mL (0.040 L) of 0.100 <em data-effect=\"italics\">M<\/em> barbituric acid (<em data-effect=\"italics\">K<\/em><sub>a<\/sub> = 9.8 \\(\\times\\) 10<sup>\u22125<\/sup>) with 0.100 <em data-effect=\"italics\">M<\/em> KOH.<\/p>\r\n<p id=\"fs-idp164478416\">(4a) no KOH added<\/p>\r\n<p id=\"fs-idp164478800\">(4b) 20 mL of KOH solution added<\/p>\r\n<p id=\"fs-idp164479184\">(4c) 39 mL of KOH solution added<\/p>\r\n<p id=\"fs-idp164479568\">(4d) 40 mL of KOH solution added<\/p>\r\n<p id=\"fs-idp177607408\">(4e) 41 mL of KOH solution added<\/p>\r\n&nbsp;\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idp177607920\" style=\"padding-left: 40px\" data-type=\"solution\">\r\n<p id=\"fs-idp177608176\">(a) pH = 2.50; (b) pH = 4.01; (c) pH = 5.60; (d) pH = 8.35; (e) pH = 11.08<\/p>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp105330480\" data-type=\"exercise\">\r\n<div id=\"fs-idp105330736\" data-type=\"problem\">\r\n<p id=\"fs-idp105330992\">(5) The indicator dinitrophenol is an acid with a <em data-effect=\"italics\">K<\/em><sub>a<\/sub> of 1.1 \\(\\times\\) 10<sup>\u22124<\/sup>. In a 1.0 \\(\\times\\) 10<sup>\u22124<\/sup>-<em data-effect=\"italics\">M<\/em> solution, it is colorless in acid and yellow in base. Calculate the pH range over which it goes from 10% ionized (colorless) to 90% ionized (yellow).<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox shaded\" data-type=\"glossary\">\r\n<h2 data-type=\"glossary-title\">Glossary<\/h2>\r\n<dl id=\"fs-idp67176144\">\r\n \t<dt>[pb_glossary id=\"3262\"]acid-base indicator[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idp67176784\">weak acid or base whose conjugate partner imparts a different solution color; used in visual assessments of solution pH<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idp67177296\">\r\n \t<dt>[pb_glossary id=\"3263\"]color-change interval[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idp67177936\">range in pH over which the color change of an indicator is observed<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idp67179744\">\r\n \t<dt>[pb_glossary id=\"3264\"]titration curve[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idp67180384\">plot of some sample property (such as pH) versus volume of added titrant<\/dd>\r\n<\/dl>\r\n<\/div>","rendered":"<div class=\"textbox textbox--learning-objectives\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\">Learning Objectives<\/p>\n<\/header>\n<div class=\"textbox__content\">\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Interpret titration curves for strong and weak acid-base systems<\/li>\n<li>Compute sample pH at important stages of a titration<\/li>\n<li>Explain the function of acid-base indicators<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<p id=\"fs-idm43847120\">As seen in the chapter on the stoichiometry of chemical reactions, titrations can be used to quantitatively analyze solutions for their acid or base concentrations. In this section, we will explore the underlying chemical equilibria that make acid-base titrimetry a useful analytical technique.<\/p>\n<div id=\"fs-idm84795552\" class=\"bc-section section\" data-depth=\"1\">\n<h2 data-type=\"title\">Titration Curves<\/h2>\n<p id=\"fs-idp135875056\">A <span data-type=\"term\">titration curve<\/span> is a plot of some solution property versus the amount of added titrant. For acid-base titrations, solution pH is a useful property to monitor because it varies predictably with the solution composition and, therefore, may be used to monitor the titration\u2019s progress and detect its endpoint. The following example exercise demonstrates the computation of pH for a titration solution after the additions of several specified titrant volumes. The first example involves a strong acid titration that requires only stoichiometric calculations to derive the solution pH. The second example addresses a weak acid titration requiring equilibrium calculations.<\/p>\n<div class=\"textbox textbox--examples\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\">Activity 8.7.1 &#8211; <span data-type=\"title\">Calculating pH for Titration Solutions: Strong Acid\/Strong Base<\/span><\/p>\n<\/header>\n<div class=\"textbox__content\">\n<p id=\"fs-idp245005248\">A titration is carried out for 25.00 mL of 0.100 <em data-effect=\"italics\">M<\/em> HCl (strong acid) with 0.100 <em data-effect=\"italics\">M<\/em> of a strong base NaOH (the titration curve is shown in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration\">(Figure 8.7.1)<\/a>). Calculate the pH at these volumes of added base solution:<\/p>\n<p id=\"fs-idp67154976\">(a) 0.00 mL<\/p>\n<p id=\"fs-idm80154320\">(b) 12.50 mL<\/p>\n<p id=\"fs-idm39390080\">(c) 25.00 mL<\/p>\n<p id=\"fs-idp81988928\">(d) 37.50 mL<\/p>\n<h2 id=\"fs-idp22584832\"><span data-type=\"title\">Solution<\/span><\/h2>\n<p>(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 <em data-effect=\"italics\">M<\/em>. The pH of the solution is then:<\/p>\n<p>&nbsp;<\/p>\n<div id=\"fs-idm213177360\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-d24b2d7c92135c8105828050283b68fb_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#61;&#45;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#48;&#46;&#49;&#48;&#48;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#49;&#46;&#48;&#48;&#48;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"209\" style=\"vertical-align: -4px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0\u00a0<\/em><\/div>\n<p id=\"fs-idm214456576\">(b) Titrant volume = 12.50 mL. Since the acid sample and the base titrant are both monoprotic and equally concentrated, this titrant addition involves less than a stoichiometric amount of base, and so it is completely consumed by reaction with the excess acid in the sample. The concentration of acid remaining is computed by subtracting the consumed amount from the intial amount and then dividing by the solution volume:<\/p>\n<p>&nbsp;<\/p>\n<div id=\"fs-idp80308976\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-51855fe8d3aa27998062b13412d6be87_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#110;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#125;&#123;&#86;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#48;&#50;&#53;&#48;&#48;&#32;&#109;&#111;&#108;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#48;&#48;&#48;&#32;&#109;&#76;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#32;&#76;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#45;&#48;&#46;&#49;&#48;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#52;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#77;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#50;&#46;&#53;&#48;&#32;&#109;&#76;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#50;&#53;&#46;&#48;&#48;&#32;&#109;&#76;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#50;&#46;&#53;&#48;&#32;&#109;&#76;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#48;&#46;&#48;&#51;&#51;&#51;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#52;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#77;\" title=\"Rendered by QuickLaTeX.com\" height=\"32\" width=\"572\" style=\"vertical-align: -8px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0 <\/em><\/div>\n<p>(c) Titrant volume = 25.00 mL. This titrant addition involves a stoichiometric amount of base (the <em data-effect=\"italics\">equivalence point<\/em>), and so only products of the neutralization reaction are in solution (water and NaCl). Neither the cation nor the anion of this salt undergoes acid-base ionization; the only process generating hydronium ions is the autoprotolysis of water. The solution is neutral, having a pH = 7.00.<\/p>\n<p id=\"fs-idm173154048\">(d) Titrant volume = 37.50 mL. This involves the addition of titrant in excess of the equivalence point. The solution pH is then calculated using the concentration of hydroxide ion:<\/p>\n<p><em>\u00a0\u00a0<\/em><\/p>\n<div id=\"fs-idp66422816\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-f498e3d5e73ec4e0b7cc52bcef58dac6_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#110;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#40;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#125;&#95;&#123;&#48;&#125;&#62;&#92;&#116;&#101;&#120;&#116;&#123;&#110;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#40;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#125;&#95;&#123;&#48;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"155\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0\u00a0<\/em><\/div>\n<div id=\"fs-idm15386080\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-e5d9e3ff2c9e28a2c944a9df3bd67bd3_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#110;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#125;&#123;&#86;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#48;&#46;&#49;&#48;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#52;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#77;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#51;&#53;&#46;&#55;&#48;&#32;&#109;&#76;&#125;&#45;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#48;&#50;&#53;&#48;&#48;&#32;&#109;&#111;&#108;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#48;&#48;&#48;&#32;&#109;&#76;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#32;&#76;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#50;&#53;&#46;&#48;&#48;&#32;&#109;&#76;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#51;&#55;&#46;&#53;&#48;&#32;&#109;&#76;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#48;&#46;&#48;&#50;&#48;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#52;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#77;\" title=\"Rendered by QuickLaTeX.com\" height=\"32\" width=\"576\" style=\"vertical-align: -8px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0\u00a0<\/em><\/div>\n<p id=\"fs-idm41259968\">pH = 14 \u2212 pOH = 14 + log([OH<sup>\u2212<\/sup>]) = 14 + log(0.0200) = 12.30<\/p>\n<hr \/>\n<h2 id=\"fs-idm15929056\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\n<p>Calculate the pH for the strong acid\/strong base titration between 50.0 mL of 0.100 <em data-effect=\"italics\">M<\/em> HNO<sub>3<\/sub>(<em data-effect=\"italics\">aq<\/em>) and 0.200 <em data-effect=\"italics\">M<\/em> NaOH (titrant) at the listed volumes of added base: 0.00 mL, 15.0 mL, 25.0 mL, and 40.0 mL.<\/p>\n<div id=\"fs-idm44981872\" data-type=\"note\">\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\n<p id=\"fs-idm89702512\" style=\"text-align: right\">0.00 mL, pH =\u00a0 1.000<\/p>\n<p style=\"text-align: right\">15.0 mL, pH = 1.5111<\/p>\n<p style=\"text-align: right\">25.0 mL, pH =\u00a0 7<\/p>\n<p style=\"text-align: right\">40.0 mL, pH = 12.523<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox textbox--examples\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\">Activity 8.7.2 &#8211; <span data-type=\"title\">Titration of a Weak Acid with a Strong Base<\/span><\/p>\n<\/header>\n<div class=\"textbox__content\">\n<p id=\"fs-idp114806608\">Consider the titration of 25.00 mL of 0.100 <em data-effect=\"italics\">M<\/em> CH<sub>3<\/sub>CO<sub>2<\/sub>H with 0.100 <em data-effect=\"italics\">M<\/em> NaOH. The reaction can be represented as:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp77362464\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-96d86069c2f8a2cdaf2b9ef706629b0a_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#36;&#92;&#114;&#105;&#103;&#104;&#116;&#97;&#114;&#114;&#111;&#119;&#36;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"15\" width=\"303\" style=\"vertical-align: -3px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm41606112\">Calculate the pH of the titration solution after the addition of the following volumes of NaOH titrant:<\/p>\n<p id=\"fs-idm192768656\">(a) 0.00 mL<\/p>\n<p id=\"fs-idm178030592\">(b) 25.00 mL<\/p>\n<p id=\"fs-idm214305872\">(c) 12.50 mL<\/p>\n<p id=\"fs-idm223741312\">(d) 37.50 mL<\/p>\n<h2 id=\"fs-idp3678224\"><span data-type=\"title\">Solution<\/span><\/h2>\n<p>(a) The initial pH is computed for the acetic acid solution in the usual ICE approach:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p id=\"fs-idp30610784\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-13d69d2a579f7dfdf1e57a6530b80cc5_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#97;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#97;&#112;&#112;&#114;&#111;&#120;&#32;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#50;&#125;&#125;&#125;&#123;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#95;&#123;&#48;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#44;\" title=\"Rendered by QuickLaTeX.com\" height=\"36\" width=\"298\" style=\"vertical-align: -10px;\" \/> and <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-1a425009f8137ec0d0999c6a148d4240_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#61;&#92;&#115;&#113;&#114;&#116;&#123;&#123;&#75;&#125;&#95;&#123;&#97;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#61;&#92;&#115;&#113;&#114;&#116;&#123;&#49;&#46;&#56;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#53;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#48;&#46;&#49;&#48;&#48;&#125;&#61;&#49;&#46;&#51;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#51;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"24\" width=\"551\" style=\"vertical-align: -7px;\" \/><\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm76922320\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-65c2e696a47f3776c867fab62c04959e_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#49;&#46;&#51;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#51;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#50;&#46;&#56;&#55;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"246\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm935760\">(b) The acid and titrant are both monoprotic and the sample and titrant solutions are equally concentrated; thus, this volume of titrant represents the equivalence point. Unlike the strong-acid example above, however, the reaction mixture, in this case, contains a weak conjugate base (acetate ion). The solution pH is computed considering the base ionization of acetate, which is present at a concentration of:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm33154592\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-3cc9aff73d434a378372fde6df44c411_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#48;&#50;&#53;&#48;&#32;&#109;&#111;&#108;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#53;&#48;&#48;&#32;&#76;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#53;&#48;&#48;&#32;&#77;&#125;&#32;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#8722;&#125;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"250\" style=\"vertical-align: -6px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm2004176\">Base ionization of acetate is represented by the equation:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp77139280\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-e513222f370530337a2d6b02be66fd77_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#108;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#36;&#92;&#114;&#105;&#103;&#104;&#116;&#108;&#101;&#102;&#116;&#104;&#97;&#114;&#112;&#111;&#111;&#110;&#115;&#36;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"19\" width=\"433\" style=\"vertical-align: -5px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idp75313664\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-cbe5554f577f7607ab167bfb653f7a2d_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#98;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#123;&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#97;&#125;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#119;&#125;&#125;&#125;&#123;&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#97;&#125;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#49;&#46;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#49;&#52;&#125;&#125;&#123;&#49;&#46;&#56;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#53;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#53;&#46;&#54;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#49;&#48;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"31\" width=\"413\" style=\"vertical-align: -8px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idp58734736\">Assuming <em data-effect=\"italics\">x<\/em> &lt;&lt; 0.0500, the pH may be calculated via the usual ICE approach:<\/p>\n<p><em>\u00a0\u00a0<\/em><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-670e4a683ae6472c3bbbc63ec433bb65_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#98;&#125;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#123;&#120;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#50;&#125;&#125;&#125;&#123;&#48;&#46;&#48;&#53;&#48;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#77;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"24\" width=\"110\" style=\"vertical-align: -6px;\" \/><\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm58971824\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-d1bd1928ff57c1f28839368c21504f54_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#120;&#61;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#61;&#53;&#46;&#51;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#54;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"199\" style=\"vertical-align: -7px;\" \/><\/div>\n<div id=\"fs-idp1478112\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-dcb57a49a41cbd5f0c027af8cb044533_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#79;&#72;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#53;&#46;&#51;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#54;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#53;&#46;&#50;&#56;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"259\" style=\"vertical-align: -7px;\" \/><\/div>\n<div id=\"fs-idm54099632\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-3f83bcc9d493b9119caccb169c889d4c_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#61;&#49;&#52;&#46;&#48;&#48;&#45;&#53;&#46;&#50;&#56;&#61;&#56;&#46;&#55;&#50;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"195\" style=\"vertical-align: -3px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm40620912\">Note that the pH at the equivalence point of this titration is significantly greater than 7, as expected when titrating a weak acid with a strong base.<\/p>\n<p id=\"fs-idm15954576\">(c) Titrant volume = 12.50 mL. This volume represents one-half of the stoichiometric amount of titrant, and so one-half of the acetic acid has been neutralized to yield an equivalent amount of acetate ion. The concentrations of these conjugate acid-base partners, therefore, are equal. A convenient approach to computing the pH is use of the Henderson-Hasselbalch equation:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp121571008\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-47cc535dec34e4f909011783f18fa6c2_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#61;&#112;&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#97;&#125;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#92;&#116;&#101;&#120;&#116;&#123;&#66;&#97;&#115;&#101;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#92;&#116;&#101;&#120;&#116;&#123;&#65;&#99;&#105;&#100;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#97;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#49;&#46;&#56;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#53;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#49;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"52\" width=\"582\" style=\"vertical-align: -5px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idp163867552\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-30fdbac80113732d014cd4d1f57a8e55_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#49;&#46;&#56;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#53;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#52;&#46;&#55;&#52;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"246\" style=\"vertical-align: -7px;\" \/><\/div>\n<p><em>\u00a0\u00a0<\/em><\/p>\n<p id=\"fs-idm42058672\">(pH = p<em data-effect=\"italics\">K<\/em><sub>a<\/sub> at the half-equivalence point in a titration of a weak acid)<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p id=\"fs-idp85997072\">(d) Titrant volume = 37.50 mL. This volume represents a stoichiometric excess of titrant, and a reaction solution containing both the titration product, acetate ion, and the excess strong titrant. In such solutions, the solution pH is determined primarily by the amount of excess strong base:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm52967552\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-2084f6b6942aa27a26c76992e7b5e8b7_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#108;&#101;&#102;&#116;&#40;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#48;&#51;&#55;&#53;&#48;&#32;&#109;&#111;&#108;&#125;&#45;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#48;&#50;&#53;&#48;&#32;&#109;&#111;&#108;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#48;&#46;&#48;&#54;&#50;&#53;&#48;&#32;&#76;&#125;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#50;&#46;&#48;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#50;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#77;\" title=\"Rendered by QuickLaTeX.com\" height=\"26\" width=\"400\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0 <\/em><\/div>\n<div id=\"fs-idm21431696\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-361b6dd6ec5dd434c15fc9a6355b52f0_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#79;&#72;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#50;&#46;&#48;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#105;&#109;&#101;&#115;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#50;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#92;&#116;&#101;&#120;&#116;&#123;&#49;&#46;&#55;&#48;&#44;&#32;&#97;&#110;&#100;&#32;&#112;&#72;&#125;&#61;&#49;&#52;&#46;&#48;&#48;&#45;&#49;&#46;&#55;&#48;&#61;&#49;&#50;&#46;&#51;&#48;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"518\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\">\n<hr \/>\n<\/div>\n<h2 id=\"fs-idm41682336\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\n<p>Calculate the pH for the weak acid\/strong base titration between 50.0 mL of 0.100 <em data-effect=\"italics\">M<\/em> HCOOH(<em data-effect=\"italics\">aq<\/em>) (formic acid) and 0.200 <em data-effect=\"italics\">M<\/em> NaOH (titrant) at the listed volumes of added base: 0.00 mL, 15.0 mL, 25.0 mL, and 30.0 mL.<\/p>\n<div id=\"fs-idp68668928\" data-type=\"note\">\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\n<p id=\"fs-idm37877472\" style=\"text-align: right\">0.00 mL, pH = 2.37<\/p>\n<p style=\"text-align: right\">15.0 mL, pH = 3.92<\/p>\n<p style=\"text-align: right\">25.00 mL, pH = 8.29<\/p>\n<p style=\"text-align: right\">30.0 mL, pH = 12.097<\/p>\n<\/div>\n<\/div>\n<\/div>\n<p id=\"fs-idm198420960\">Performing additional calculations similar to those in the preceding example permits a more full assessment of titration curves. A summary of pH\/volume data pairs for the strong and weak acid titrations is provided in <a class=\"autogenerated-content\" href=\"#fs-idm87178400\">(Table 8.7.1)<\/a> and plotted as titration curves in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration\">(Figure 8.7.1)<\/a>. A comparison of these two curves illustrates several important concepts that are best addressed by identifying the four stages of a titration:<\/p>\n<p id=\"fs-idm201863856\"><strong>Initial state (added titrant volume = 0 mL)<\/strong>: pH is determined by the acid being titrated; because the two acid samples are equally concentrated, the weak acid will exhibit a greater initial pH<\/p>\n<p id=\"fs-idm444217232\"><strong>Pre-equivalence point (0 mL &lt; <em data-effect=\"italics\">V<\/em> &lt; 25 mL)<\/strong>: solution pH increases gradually and the acid is consumed by reaction with added titrant; composition includes unreacted acid and the reaction product, its conjugate base<\/p>\n<p id=\"fs-idm183388016\"><strong>Equivalence point (<em data-effect=\"italics\">V<\/em> = 25 mL)<\/strong>: a drastic rise in pH is observed as the solution composition transitions from acidic to either neutral (for the strong acid sample) or basic (for the weak acid sample), with pH determined by ionization of the conjugate base of the acid<\/p>\n<p id=\"fs-idm183509856\"><strong>Postequivalence point (<em data-effect=\"italics\">V<\/em> &gt; 25 mL)<\/strong>: pH is determined by the amount of excess strong base titrant added; since both samples are titrated with the same titrant, both titration curves appear similar at this stage.<\/p>\n<table id=\"fs-idm87178400\" class=\"aligncenter\" summary=\"This table has four columns and twenty rows. The first row is a header row, and it labels each column, \u201cVolume of 0.100 M N a O H Added ( m L ),\u201d \u201cMoles of N a O H Added,\u201d \u201cp H Values 0.100 M H C l footnote one,\u201d \u201cp H Values 0.100 M C H subscript 3 C O subscript 2 H footnote 2.\u201d Under the \u201cVolume of 0.100 M N a O H Added ( m L )\u201d column are the following values: 0.0, 5.0, 10.0, 15.0, 20.0, 22.0, 24.0, 24.5, 24.9, 25.0, 25.1, 25.5, 26.0, 28.0, 30.0, 35.0, 40.0, 45.0, and 50.0. Under the \u201cMoles of N a O H Added\u201d column are the following values: 0.0, 0.00050, 0.00100, 0.00150, 0.00200, 0.00220, 0.00240, 0.00245, 0.00249, 0.00250, 0.00251, 0.00255, 0.00260, 0.00280, 0.00300, 0.00350, 0.00400, 0.00450, and 0.00500. Under the \u201cp H Values 0.100 M H C l footnote one\u201d column are the following values: 1.00, 1.18, 1.37, 1.60, 1.95, 2.20, 2.69, 3.00, 3.70, 7.00, 10.30, 11.00, 11.29, 11.75, 11.96, 12.22, 12.36, 12.46, and 12.52. Foot note one reads, \u201cTitration of 25.00 m L of 0.100 M H C l ( 0.00250 mol of H C I ) with 0.100 M N a O H.\u201d Under the \u201cp H Values 0.100 M C H subscript 3 C O subscript 2 H footnote 2\u201d column are the following values: 2.87, 4.14, 4.57, 4.92, 5.35, 5.61, 6.13, 6.44, 7.17, 8.72, 10.30, 11.00, 11.29, 11.75, 11.96, 12.22, 12.36, 12.46, and 12.52. Footnote two reads, \u201cTitration of 25.00 m L of 0.100 M C H subscript 3 C O subscript 2 H ( 0.00250 mol of C H subscript 3C O subscript 2 H) with 0.100 M N a O H.\u201d\">\n<caption>Table 8.7.1 &#8211;\u00a0 pH Values in the Titrations of a Strong Acid and of a Weak Acid<\/caption>\n<thead>\n<tr valign=\"top\">\n<th data-align=\"left\">Volume of 0.100 <em data-effect=\"italics\">M<\/em> NaOH Added (mL)<\/th>\n<th data-align=\"left\">Moles of NaOH Added<\/th>\n<th data-align=\"left\">pH Values 0.100 <em data-effect=\"italics\">M<\/em> HCl<a class=\"footnote\" title=\"Titration of 25.00 mL of 0.100 M HCl (0.00250 mol of HCI) with 0.100 M NaOH.\" id=\"return-footnote-1929-1\" href=\"#footnote-1929-1\" aria-label=\"Footnote 1\"><sup class=\"footnote\">[1]<\/sup><\/a><\/th>\n<th data-align=\"left\">pH Values 0.100 <em data-effect=\"italics\">M<\/em> CH<sub>3<\/sub>CO<sub>2<\/sub>H<a class=\"footnote\" title=\"Titration of 25.00 mL of 0.100 M CH3CO2H (0.00250 mol of CH3CO2H) with 0.100 M NaOH.\" id=\"return-footnote-1929-2\" href=\"#footnote-1929-2\" aria-label=\"Footnote 2\"><sup class=\"footnote\">[2]<\/sup><\/a><\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr valign=\"top\">\n<td data-align=\"left\">0.0<\/td>\n<td data-align=\"left\">0.0<\/td>\n<td data-align=\"left\">1.00<\/td>\n<td data-align=\"left\">2.87<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">5.0<\/td>\n<td data-align=\"left\">0.00050<\/td>\n<td data-align=\"left\">1.18<\/td>\n<td data-align=\"left\">4.14<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">10.0<\/td>\n<td data-align=\"left\">0.00100<\/td>\n<td data-align=\"left\">1.37<\/td>\n<td data-align=\"left\">4.57<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">15.0<\/td>\n<td data-align=\"left\">0.00150<\/td>\n<td data-align=\"left\">1.60<\/td>\n<td data-align=\"left\">4.92<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">20.0<\/td>\n<td data-align=\"left\">0.00200<\/td>\n<td data-align=\"left\">1.95<\/td>\n<td data-align=\"left\">5.35<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">22.0<\/td>\n<td data-align=\"left\">0.00220<\/td>\n<td data-align=\"left\">2.20<\/td>\n<td data-align=\"left\">5.61<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">24.0<\/td>\n<td data-align=\"left\">0.00240<\/td>\n<td data-align=\"left\">2.69<\/td>\n<td data-align=\"left\">6.13<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">24.5<\/td>\n<td data-align=\"left\">0.00245<\/td>\n<td data-align=\"left\">3.00<\/td>\n<td data-align=\"left\">6.44<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">24.9<\/td>\n<td data-align=\"left\">0.00249<\/td>\n<td data-align=\"left\">3.70<\/td>\n<td data-align=\"left\">7.14<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">25.0<\/td>\n<td data-align=\"left\">0.00250<\/td>\n<td data-align=\"left\">7.00<\/td>\n<td data-align=\"left\">8.72<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">25.1<\/td>\n<td data-align=\"left\">0.00251<\/td>\n<td data-align=\"left\">10.30<\/td>\n<td data-align=\"left\">10.30<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">25.5<\/td>\n<td data-align=\"left\">0.00255<\/td>\n<td data-align=\"left\">11.00<\/td>\n<td data-align=\"left\">11.00<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">26.0<\/td>\n<td data-align=\"left\">0.00260<\/td>\n<td data-align=\"left\">11.29<\/td>\n<td data-align=\"left\">11.29<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">28.0<\/td>\n<td data-align=\"left\">0.00280<\/td>\n<td data-align=\"left\">11.75<\/td>\n<td data-align=\"left\">11.75<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">30.0<\/td>\n<td data-align=\"left\">0.00300<\/td>\n<td data-align=\"left\">11.96<\/td>\n<td data-align=\"left\">11.96<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">35.0<\/td>\n<td data-align=\"left\">0.00350<\/td>\n<td data-align=\"left\">12.22<\/td>\n<td data-align=\"left\">12.22<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">40.0<\/td>\n<td data-align=\"left\">0.00400<\/td>\n<td data-align=\"left\">12.36<\/td>\n<td data-align=\"left\">12.36<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">45.0<\/td>\n<td data-align=\"left\">0.00450<\/td>\n<td data-align=\"left\">12.46<\/td>\n<td data-align=\"left\">12.46<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"left\">50.0<\/td>\n<td data-align=\"left\">0.00500<\/td>\n<td data-align=\"left\">12.52<\/td>\n<td data-align=\"left\">12.52<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<div id=\"CNX_Chem_14_07_titration\" class=\"bc-figure figure\">\n<figure style=\"width: 1300px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_07_titration-1.jpg\" alt=\"Two graphs are shown. The first graph on the left is titled \u201cTitration of Weak Acid.\u201d The horizontal axis is labeled \u201cVolume of 0.100 M N a O H added (m L).\u201d Markings and vertical gridlines are provided every 5 units from 0 to 50. The vertical axis is labeled \u201cp H\u201d and is marked every 1 unis beginning at 0 extending to 14. A red curve is drawn on the graph which increases steadily from the point (0, 3) up to about (20, 5.5) after which the graph has a vertical section from (25, 7) up to (25, 11). The graph then levels off to a value of about 12.5 from about 40 m L up to 50 m L. The midpoint of the vertical segment of the curve is labeled \u201cEquivalence point p H, 8.72.\u201d The second graph on the right is titled \u201cTitration of Strong Acid.\u201d The horizontal axis is labeled \u201cVolume of 0.100 M N a O H added (m L).\u201d Markings and vertical gridlines are provided every 5 units from 0 to 50. The vertical axis is labeled \u201cp H\u201d and is marked every 1 units beginning at 0 extending to 14. A red curve is drawn on the graph which increases gradually from the point (0, 1) up to about (22.5, 2.2) after which the graph has a vertical section from (25, 4) up to nearly (25, 11). The graph then levels off to a value of about 12.4 from about 40 m L up to 50 m L. The midpoint of the vertical segment of the curve is labeled \u201cEquivalence point p H, 7.00.\u201d\" width=\"1300\" height=\"731\" data-media-type=\"image\/jpeg\" \/><figcaption class=\"wp-caption-text\"><strong>Figure 8.7.1 &#8211; (a) The titration curve for the titration of 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M NaOH (strong base) has an equivalence point of 7.00 pH. (b) The titration curve for the titration of 25.00 mL of 0.100 M acetic acid (weak acid) with 0.100 M NaOH (strong base) has an equivalence point of 8.72 pH.<\/strong><\/figcaption><\/figure>\n<\/div>\n<\/div>\n<div id=\"fs-idp22610576\" class=\"bc-section section\" data-depth=\"1\">\n<h2 data-type=\"title\">Acid-Base Indicators<\/h2>\n<p id=\"fs-idm39085312\">Certain organic substances change color in dilute solution when the hydronium ion concentration reaches a particular value. For example, phenolphthalein is a colorless substance in an aqueous solution with a hydronium ion concentration greater than 5.0 <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c9448d0c3ab42155fc705b58fe04b3b0_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&times;\" title=\"Rendered by QuickLaTeX.com\" height=\"1\" width=\"1\" style=\"vertical-align: 0px;\" \/> 10<sup>\u22129<\/sup><em data-effect=\"italics\">M<\/em> (pH &lt; 8.3). In more basic solutions where the hydronium ion concentration is less than 5.0 <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c9448d0c3ab42155fc705b58fe04b3b0_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&times;\" title=\"Rendered by QuickLaTeX.com\" height=\"1\" width=\"1\" style=\"vertical-align: 0px;\" \/> 10<sup>\u22129<\/sup><em data-effect=\"italics\">M<\/em> (pH &gt; 8.3), it is red or pink. Substances such as phenolphthalein, which can be used to determine the pH of a solution, are called <span data-type=\"term\">acid-base indicators<\/span>. Acid-base indicators are either weak organic acids or weak organic bases.<\/p>\n<p id=\"fs-idm28417392\">The equilibrium in a solution of the acid-base indicator methyl orange, a weak acid, can be represented by an equation in which we use HIn as a simple representation for the complex methyl orange molecule:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp80468176\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-599490d3dc870935c496951787059efd_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#98;&#101;&#103;&#105;&#110;&#123;&#97;&#114;&#114;&#97;&#121;&#125;&#123;&#99;&#99;&#99;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#73;&#110;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#108;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#38;&#32;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#36;&#92;&#114;&#105;&#103;&#104;&#116;&#108;&#101;&#102;&#116;&#104;&#97;&#114;&#112;&#111;&#111;&#110;&#115;&#36;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#38;&#32;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#73;&#110;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#92;&#92;&#32;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#53;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#114;&#101;&#100;&#125;&#92;&#104;&#102;&#105;&#108;&#108;&#32;&#38;&#32;&#38;&#32;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#53;&#46;&#53;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#121;&#101;&#108;&#108;&#111;&#119;&#125;&#92;&#104;&#102;&#105;&#108;&#108;&#32;&#38;&#32;&#92;&#101;&#110;&#100;&#123;&#97;&#114;&#114;&#97;&#121;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"41\" width=\"365\" style=\"vertical-align: -15px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm87967824\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-9879f62f1459fd327f9e795bd4125e9f_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#75;&#125;&#95;&#123;&#97;&#125;&#61;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#51;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#79;&#125;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#43;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#73;&#110;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#73;&#110;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#61;&#52;&#46;&#48;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&times;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#52;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"32\" width=\"228\" style=\"vertical-align: -9px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm68547888\">The anion of methyl orange, In<sup>\u2212<\/sup>, is yellow, and the nonionized form, HIn, is red. When we add acid to a solution of methyl orange, the increased hydronium ion concentration shifts the equilibrium toward the nonionized red form, in accordance with Le Ch\u00e2telier\u2019s principle. If we add base, we shift the equilibrium towards the yellow form. This behavior is completely analogous to the action of buffers.<\/p>\n<p id=\"fs-idp64938256\">The perceived color of an indicator solution is determined by the ratio of the concentrations of the two species In<sup>\u2212<\/sup> and HIn. If most of the indicator (typically about 60\u221290% or more) is present as In<sup>\u2212<\/sup>, the perceived color of the solution is yellow. If most is present as HIn, then the solution color appears red. The Henderson-Hasselbalch equation is useful for understanding the relationship between the pH of an indicator solution and its composition (thus, perceived color):<\/p>\n<p>&nbsp;<\/p>\n<div id=\"fs-idp80076272\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-0d602c17577a2cc802733b87eb003542_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#61;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#125;&#75;&#92;&#116;&#101;&#120;&#116;&#123;&#97;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#92;&#112;&#104;&#97;&#110;&#116;&#111;&#109;&#123;&#92;&#114;&#117;&#108;&#101;&#123;&#48;&#46;&#50;&#101;&#109;&#125;&#123;&#48;&#101;&#120;&#125;&#125;&#92;&#102;&#114;&#97;&#99;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#73;&#110;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#123;&#92;&#108;&#101;&#102;&#116;&#091;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#73;&#110;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"43\" width=\"193\" style=\"vertical-align: -17px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm188576256\">In solutions where pH &gt; p<em data-effect=\"italics\">K<\/em><sub>a<\/sub>, the logarithmic term must be positive, indicating an excess of the conjugate base form of the indicator (yellow solution). When pH &gt; p<em data-effect=\"italics\">K<\/em><sub>a<\/sub>, the log term must be negative, indicating an excess of the conjugate acid (red solution). When the solution pH is close to the indicator pKa, appreciable amounts of both conjugate partners are present, and the solution color is that of an additive combination of each (yellow and red, yielding orange). The <span data-type=\"term\">color change interval<\/span> (or <em data-effect=\"italics\">pH interval<\/em>) for an acid-base indicator is defined as the range of pH values over which a change in color is observed, and for most indicators this range is approximately p<em data-effect=\"italics\">K<\/em><sub>a<\/sub> \u00b1 1.<\/p>\n<p id=\"fs-idm92451888\">There are many different acid-base indicators that cover a wide range of pH values and can be used to determine the approximate pH of an unknown solution by a process of elimination. Universal indicators and pH paper contain a mixture of indicators and exhibit different colors at different pHs. <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_indicators\">(Figure 8.7.2)<\/a> presents several indicators, their colors, and their color-change intervals.<\/p>\n<div id=\"CNX_Chem_14_07_indicators\" class=\"bc-figure figure\">\n<div class=\"bc-figcaption figcaption\"><\/div>\n<figure style=\"width: 1300px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_07_indicators-1-1.jpg\" alt=\"This figure provides a graphical representation of indicators and color ranges. A horizontal axis is labeled \u201cp H.\u201d This axis begins at zero and increases by ones up to 13. The left side of the graphic provides a column with the names of indicators. To the right of each indicator name is either one or two colored bars that are shaded according to the indicator color at various p H ranges. From the top, the first row is labeled \u201cCrystal violet.\u201d The associated colored bar is yellow at its left end at a p H of 0 and changes to green and blue moving right to its endpoint at a p H of 1.8. The second row is labeled \u201cCresol red.\u201d The associated colored bar is red at its left end at a p H of 1 and changes to orange and yellow moving right to its endpoint at a p H of just over 2. A second bar to its right is yellow at a p H of around 7 and proceeds through orange to red at a p H of about 9. The third row is labeled \u201cThymol blue.\u201d The associated colored bar is red at its left end at a p H of nearly 1.2 and changes to orange and red moving right to its endpoint at a p H of 2.8. A second bar begins in yellow at a p H of 8 and proceeds through green and blue to its end at a p H of around 9.1. The fourth row is labeled \u201cErythrosin B.\u201d The associated colored bar is red from a p H of 2.2 to its endpoint at a p H of 3.6. The fifth row is labeled \u201c2 comma 4 dash Dinitrophenol.\u201d The associated colored bar is white at its left end at a p H of 2.6 and changes to yellow at its endpoint at a p H of 4. The sixth row is labeled \u201cBromophenol blue.\u201d The associated colored bar is yellow at its left end at a p H of 3 and changes to green and blue moving right to its endpoint at a p H of 4.5. The seventh row is labeled \u201cMethyl orange.\u201d The associated colored bar is red-orange at its left end at a p H of 4.2 and changes to yellow moving right to its endpoint at a p H of 6.3. The eighth row is labeled \u201cBromocresol green.\u201d The associated colored bar is yellow at its left end at a p H of 3.8 and changes to green and blue moving right to its endpoint at a p H of 5.4. The ninth row is labeled \u201cMethyl red.\u201d The associated colored bar is orange at its left end at a p H of 4.2 and changes to yellow moving right to its endpoint at a p H of 6.3. The tenth row is labeled \u201cEriochrome * Black T.\u201d The associated colored bar is red at its left end at a p H of 5 and changes to purple and blue moving right to its endpoint at a p H of 6.5. The eleventh row is labeled \u201cBromocresol purple.\u201d The associated colored bar is yellow at its left end at a p H of 5.2 and changes to purple moving right to its endpoint at a p H of 6.8. The twelfth row is labeled \u201cAlizarin.\u201d The first associated colored bar is yellow-orange at its left end at a p H of 5.7 and changes to red moving right to its endpoint at a p H of 7.2. A second bar begins in red at a p H of 11 and changes to purple, then dark blue at its right end at a p H of 12.4. The thirteenth row is labeled \u201cBromothymol blue.\u201d The associated colored bar is yellow at its left end at a p H of 6 and changes to green and blue moving right to its endpoint at a p H of 7.6. The fourteenth row is labeled \u201cPhenol red.\u201d The associated colored bar is yellow-orange at its left end at a p H of 6.8 and changes to orange and red moving right to its endpoint at a p H of 8.2. The fifteenth row is labeled \u201cm dash Nitrophenol.\u201d The associated colored bar is white at its left end at a p H of 6.8 and changes to yellow moving right to its endpoint at a p H of 8.6. The sixteenth row is labeled \u201co dash Cresolphthalein.\u201d The associated colored bar is white at its left end at a p H of 8.3 and changes to red moving right to its endpoint at a p H of 9.8. The seventeenth row is labeled \u201cPhenolphthalein.\u201d The associated colored bar is white at its left end at a p H of 8 and changes to pink moving right to its endpoint at a p H of 10. The eighteenth row is labeled \u201cThymolphthalein.\u201d The associated colored bar is light blue at its left end at a p H of 9.3 and changes to a deep, dark blue moving right to its endpoint at a p H of 10.5. The nineteenth row is labeled \u201cAlizarin yellow R.\u201d The associated colored bar is yellow-orange at its left end at a p H of 10 and changes to red moving right to its endpoint at a p H of 12.\" width=\"1300\" height=\"1137\" data-media-type=\"image\/jpeg\" \/><figcaption class=\"wp-caption-text\"><strong>Figure 8.7.2 &#8211; This chart illustrates the color change intervals for several acid-base indicators.<\/strong><\/figcaption><\/figure>\n<\/div>\n<div id=\"CNX_Chem_14_07_titration2\" class=\"bc-figure figure\">\n<div class=\"bc-figcaption figcaption\"><\/div>\n<figure style=\"width: 1300px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_07_titration2-1-1.jpg\" alt=\"A graph is shown which is titled \u201cTitration of Weak Acid.\u201d The horizontal axis is labeled \u201cVolume of 0.100 M N a O H added (m L)\u201d and begins at 0 with markings every 5 units up to 50. The vertical axis is labeled \u201cp H\u201d and begins at 0 and increases by single units up to 14. A red curve is drawn on the graph. The curve begins at (0, 3) and passes through the points (5, 4.1), (10, 4.7), (15, 5), (20, 5.5), and (22.5, 6), after which it rapidly increases, forming a vertical section centered at the point (25, 8.7). The rapid increase of the curve then levels off and the curve passes through the points (30, 12), (35, 12.4), (40, 12.5), (45, 12.6), and (50, 12.6). A brown rectangle extends horizontally across the graph covering the p H of 3 to 4.2 range. To the right, this rectangle is labeled \u201cMethyl orange p H range.\u201d A blue rectangle extends horizontally across the graph covering the p H of 4.6 to 8 range. To the right, this rectangle is labeled \u201cLitmus p H range.\u201d A purple rectangle extends horizontally across the graph covering the p H of 8.4 to 10 range. To the right, this rectangle is labeled \u201cPhenolphthalein p H range.\u201d The midpoint of the vertical segment of the curve is labeled \u201cEquivalence point p H, 8.72.\u201d\" width=\"1300\" height=\"872\" data-media-type=\"image\/jpeg\" \/><figcaption class=\"wp-caption-text\"><strong>Figure 8.7.3 &#8211; Titration curves for strong and weak acids illustrating the proper choice of acid-base indicator. Any of the three indicators will exhibit a reasonably sharp color change at the equivalence point of the strong acid titration, but only phenolphthalein is suitable for use in the weak acid titration.<\/strong><\/figcaption><\/figure>\n<\/div>\n<p id=\"fs-idm188916592\">The titration curves shown in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration2\">(Figure 8.7.3)<\/a> illustrate the choice of a suitable indicator for specific titrations. In the strong acid titration, use of any of the three indicators should yield reasonably sharp color changes and accurate end point determinations. For this titration, the solution pH reaches the lower limit of the methyl orange color change interval after addition of ~24 mL of titrant, at which point the initially red solution would begin to appear orange. When 25 mL of titrant has been added (the equivalence point), the pH is well above the upper limit and the solution will appear yellow. The titration&#8217;s end point may then be estimated as the volume of titrant that yields a distinct orange-to-yellow color change. This color change would be challenging for most human eyes to precisely discern. More-accurate estimates of the titration end point are possible using either litmus or phenolphthalein, both of which exhibit color change intervals that are encompassed by the steep rise in pH that occurs around the 25.00 mL equivalence point.<\/p>\n<p id=\"fs-idm224614176\">The weak acid titration curve in <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_07_titration2\">(Figure 8.7.3)<\/a> shows that only one of the three indicators is suitable for end point detection. If methyl orange is used in this titration, the solution will undergo a gradual red-to-orange-to-yellow color change over a relatively large volume interval (0\u20136 mL), completing the color change well before the equivalence point (25 mL) has been reached. Use of litmus would show a color change that begins after adding 7\u20138 mL of titrant and ends just before the equivalence point. Phenolphthalein, on the other hand, exhibits a color change interval that nicely brackets the abrupt change in pH occurring at the titration&#8217;s equivalence point. A sharp color change from colorless to pink will be observed within a very small volume interval around the equivalence point.<\/p>\n<\/div>\n<div id=\"fs-idp81138704\" class=\"summary\" data-depth=\"1\">\n<h1 data-type=\"title\">Key Concepts and Summary<\/h1>\n<div class=\"textbox textbox--exercises\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\">End of Chapter Exercises<\/p>\n<\/header>\n<div class=\"textbox__content\">\n<div id=\"fs-idp81138704\" class=\"summary\" data-depth=\"1\">\n<p id=\"fs-idp77329840\">(1) The titration curve for an acid-base titration is typically a plot of pH versus volume of added titrant. These curves are useful in selecting appropriate acid-base indicators that will permit accurate determinations of titration end points.<\/p>\n<p>&nbsp;<\/p>\n<\/div>\n<div id=\"fs-idp63641264\" class=\"exercises\" data-depth=\"1\">\n<div id=\"fs-idm5595328\" data-type=\"exercise\">\n<div id=\"fs-idp5936080\" data-type=\"problem\">\n<p id=\"fs-idp67232528\">(2) Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.<\/p>\n<\/div>\n<div id=\"fs-idp131233712\" data-type=\"solution\">\n<p>&nbsp;<\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<p id=\"fs-idm66845488\" style=\"padding-left: 40px\">At the equivalence point in the titration of a weak base with a strong acid, the resulting solution is slightly acidic due to the presence of the conjugate acid. Thus, pick an indicator that changes color in the acidic range and brackets the pH at the equivalence point. Methyl orange is a good example.<\/p>\n<p>&nbsp;<\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm81056688\" data-type=\"exercise\">\n<div id=\"fs-idm86623888\" data-type=\"problem\">\n<p id=\"fs-idp73771216\">(3) Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.<\/p>\n<p>&nbsp;<\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idp255636208\" data-type=\"exercise\">\n<div id=\"fs-idp255636464\" data-type=\"problem\">\n<p id=\"fs-idp255636720\">(4) Calculate the pH at the following points in a titration of 40 mL (0.040 L) of 0.100 <em data-effect=\"italics\">M<\/em> barbituric acid (<em data-effect=\"italics\">K<\/em><sub>a<\/sub> = 9.8 <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-3e2a3b7b9d8913e71519bf7df9eb51b3_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#105;&#109;&#101;&#115;\" title=\"Rendered by QuickLaTeX.com\" height=\"9\" width=\"10\" style=\"vertical-align: 0px;\" \/> 10<sup>\u22125<\/sup>) with 0.100 <em data-effect=\"italics\">M<\/em> KOH.<\/p>\n<p id=\"fs-idp164478416\">(4a) no KOH added<\/p>\n<p id=\"fs-idp164478800\">(4b) 20 mL of KOH solution added<\/p>\n<p id=\"fs-idp164479184\">(4c) 39 mL of KOH solution added<\/p>\n<p id=\"fs-idp164479568\">(4d) 40 mL of KOH solution added<\/p>\n<p id=\"fs-idp177607408\">(4e) 41 mL of KOH solution added<\/p>\n<p>&nbsp;<\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<\/div>\n<div id=\"fs-idp177607920\" style=\"padding-left: 40px\" data-type=\"solution\">\n<p id=\"fs-idp177608176\">(a) pH = 2.50; (b) pH = 4.01; (c) pH = 5.60; (d) pH = 8.35; (e) pH = 11.08<\/p>\n<p>&nbsp;<\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idp105330480\" data-type=\"exercise\">\n<div id=\"fs-idp105330736\" data-type=\"problem\">\n<p id=\"fs-idp105330992\">(5) The indicator dinitrophenol is an acid with a <em data-effect=\"italics\">K<\/em><sub>a<\/sub> of 1.1 <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-3e2a3b7b9d8913e71519bf7df9eb51b3_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#105;&#109;&#101;&#115;\" title=\"Rendered by QuickLaTeX.com\" height=\"9\" width=\"10\" style=\"vertical-align: 0px;\" \/> 10<sup>\u22124<\/sup>. In a 1.0 <img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-3e2a3b7b9d8913e71519bf7df9eb51b3_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#105;&#109;&#101;&#115;\" title=\"Rendered by QuickLaTeX.com\" height=\"9\" width=\"10\" style=\"vertical-align: 0px;\" \/> 10<sup>\u22124<\/sup>&#8211;<em data-effect=\"italics\">M<\/em> solution, it is colorless in acid and yellow in base. Calculate the pH range over which it goes from 10% ionized (colorless) to 90% ionized (yellow).<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox shaded\" data-type=\"glossary\">\n<h2 data-type=\"glossary-title\">Glossary<\/h2>\n<dl id=\"fs-idp67176144\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1929_3262\">acid-base indicator<\/a><\/dt>\n<dd id=\"fs-idp67176784\">weak acid or base whose conjugate partner imparts a different solution color; used in visual assessments of solution pH<\/dd>\n<\/dl>\n<dl id=\"fs-idp67177296\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1929_3263\">color-change interval<\/a><\/dt>\n<dd id=\"fs-idp67177936\">range in pH over which the color change of an indicator is observed<\/dd>\n<\/dl>\n<dl id=\"fs-idp67179744\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1929_3264\">titration curve<\/a><\/dt>\n<dd id=\"fs-idp67180384\">plot of some sample property (such as pH) versus volume of added titrant<\/dd>\n<\/dl>\n<\/div>\n<hr class=\"before-footnotes clear\" \/><div class=\"footnotes\"><ol><li id=\"footnote-1929-1\">Titration of 25.00 mL of 0.100 M HCl (0.00250 mol of HCI) with 0.100 M NaOH. <a href=\"#return-footnote-1929-1\" class=\"return-footnote\" aria-label=\"Return to footnote 1\">&crarr;<\/a><\/li><li id=\"footnote-1929-2\">Titration of 25.00 mL of 0.100 <em data-effect=\"italics\">M<\/em> CH<sub>3<\/sub>CO<sub>2<\/sub>H (0.00250 mol of CH<sub>3<\/sub>CO<sub>2<\/sub>H) with 0.100 <em data-effect=\"italics\">M<\/em> NaOH. <a href=\"#return-footnote-1929-2\" class=\"return-footnote\" aria-label=\"Return to footnote 2\">&crarr;<\/a><\/li><\/ol><\/div><div class=\"glossary\"><span class=\"screen-reader-text\" id=\"definition\">definition<\/span><template id=\"term_1929_3262\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1929_3262\"><div tabindex=\"-1\"><p>weak acid or base whose conjugate partner imparts a different solution color; used in visual assessments of solution pH<\/p>\n<\/div><button><span aria-hidden=\"true\">&times;<\/span><span class=\"screen-reader-text\">Close definition<\/span><\/button><\/div><\/template><template id=\"term_1929_3263\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1929_3263\"><div tabindex=\"-1\"><p>range in pH over which the color change of an indicator is observed<\/p>\n<\/div><button><span aria-hidden=\"true\">&times;<\/span><span class=\"screen-reader-text\">Close definition<\/span><\/button><\/div><\/template><template id=\"term_1929_3264\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1929_3264\"><div tabindex=\"-1\"><p>plot of some sample property (such as pH) versus volume of added titrant<\/p>\n<\/div><button><span aria-hidden=\"true\">&times;<\/span><span class=\"screen-reader-text\">Close definition<\/span><\/button><\/div><\/template><\/div>","protected":false},"author":801,"menu_order":7,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-1929","chapter","type-chapter","status-publish","hentry"],"part":1885,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1929","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/users\/801"}],"version-history":[{"count":13,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1929\/revisions"}],"predecessor-version":[{"id":3684,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1929\/revisions\/3684"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/parts\/1885"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1929\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/media?parent=1929"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapter-type?post=1929"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/contributor?post=1929"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/license?post=1929"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}