{"id":1897,"date":"2020-04-30T17:55:18","date_gmt":"2020-04-30T21:55:18","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/chapter\/ph-and-poh\/"},"modified":"2021-11-08T17:13:40","modified_gmt":"2021-11-08T22:13:40","slug":"ph-and-poh","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/chapter\/ph-and-poh\/","title":{"raw":"8.3 pH and pOH","rendered":"8.3 pH and pOH"},"content":{"raw":"[latexpage]\r\n<div>\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>Explain the characterization of aqueous solutions as acidic, basic, or neutral<\/li>\r\n \t<li>Express hydronium and hydroxide ion concentrations on the pH and pOH scales<\/li>\r\n \t<li>Perform calculations relating pH and pOH<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<p id=\"fs-idp11137424\">As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (<em data-effect=\"italics\">K<\/em><sub>w<\/sub>). The concentrations of these ions in a solution are often critical determinants of the solution\u2019s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is <span data-type=\"term\">neutral<\/span> if it contains equal concentrations of hydronium and hydroxide ions; <span data-type=\"term\">acidic<\/span> if it contains a greater concentration of hydronium ions than hydroxide ions; and <span data-type=\"term\">basic<\/span> if it contains a lesser concentration of hydronium ions than hydroxide ions.<\/p>\r\n<p id=\"fs-idm21650320\">A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where \u201cX\u201d is the quantity of interest and \u201clog\u201d is the base-10 logarithm:<\/p>\r\n&nbsp;\r\n<div id=\"fs-idp27819744\" data-type=\"equation\">\\(\\text{pX}={-}\\text{log X}\\)<\/div>\r\n<div data-type=\"equation\"><\/div>\r\n<p id=\"fs-idm40569744\">The <span data-type=\"term\">pH<\/span> of a solution is therefore defined as shown here, where [H<sub>3<\/sub>O<sup>+<\/sup>] is the molar concentration of hydronium ion in the solution:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm104306928\" data-type=\"equation\">\\(\\text{pH}={-}\\text{log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm112635600\">Rearranging this equation to isolate the hydronium ion molarity yields the equivalent expression:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm34387328\" data-type=\"equation\">\\(\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]={10}^{{-}\\text{pH}}\\)<\/div>\r\n<div data-type=\"equation\"><\/div>\r\n<p id=\"fs-idp55544688\">Likewise, the hydroxide ion molarity may be expressed as a p-function, or <span data-type=\"term\">pOH<\/span>:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp66748048\" data-type=\"equation\">\\(\\text{pOH}={-}\\text{log}\\left[{\\text{OH}^-}^{\\text{}}\\right]\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idp67153952\">or<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp102994080\" data-type=\"equation\">\\(\\left[{\\text{OH}^-}^{\\text{}}\\right]={10}^{{-}\\text{pOH}}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm97029664\">Finally, the relation between these two ion concentration expressed as p-functions is easily derived from the <em data-effect=\"italics\">K<\/em><sub>w<\/sub> expression:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp158230176\" data-type=\"equation\">\\({K}_{\\text{w}}=\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]\\left[{\\text{OH}^-}^{\\text{}}\\right]\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idp50288944\" data-type=\"equation\">\\({-}\\text{log}\\phantom{\\rule{0.2em}{0ex}}{K}_{\\text{w}}={-}\\text{log}\\left(\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]\\left[{\\text{OH}^-}^{\\text{}}\\right]\\right)={-}\\text{log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]+{-}\\text{log}\\left[{\\text{OH}^-}^{\\text{}}\\right]\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm65790448\" data-type=\"equation\">\\(\\text{p}{K}_{\\text{w}}=\\text{pH}+\\text{pOH}\\)<\/div>\r\n<div data-type=\"equation\"><\/div>\r\n<p id=\"fs-idp11266224\">At 25 \u00b0C, the value of <em data-effect=\"italics\">K<\/em><sub>w<\/sub> is 1.0 \\(\\times\\) 10<sup>\u221214<\/sup>, and so:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm26101984\" data-type=\"equation\">\\(14.00=\\text{pH}+\\text{pOH}\\)<\/div>\r\n<div data-type=\"equation\"><\/div>\r\n<p id=\"fs-idm103103632\">The hydronium ion molarity in pure water (or any neutral solution) is 1.0 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em> at 25 \u00b0C. The pH and pOH of a neutral solution at this temperature are therefore:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp111835440\" data-type=\"equation\">\\(\\text{pH}={-}\\text{\u2212log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]={-}\\text{log}\\left(1.0\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}1{0}^{-7}\\right)=7.00\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm65159184\" data-type=\"equation\">\\(\\text{pOH}={-}\\text{\u2212log}\\left[{\\text{OH}^-}^{\\text{}}\\right]={-}\\text{\u2212log}\\left(1.0\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}1{0}^{-7}\\right)=7.00\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idp108462720\">And so, <em data-effect=\"italics\">at this temperature<\/em>, acidic solutions are those with hydronium ion molarities greater than 1.0 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em> and hydroxide ion molarities less than 1.0 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em> (corresponding to pH values less than 7.00 and pOH values greater than 7.00). Basic solutions are those with hydronium ion molarities less than 1.0 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em> and hydroxide ion molarities greater than 1.0 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em> (corresponding to pH values greater than 7.00 and pOH values less than 7.00).<\/p>\r\n<p id=\"fs-idm84564368\">Since the autoionization constant <em data-effect=\"italics\">K<\/em><sub>w<\/sub> is temperature dependent, these correlations between pH values and the acidic\/neutral\/basic adjectives will be different at temperatures other than 25 \u00b0C. For example, the hydronium molarity of pure water at 80 \u00b0C is 4.9 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em>, which corresponds to pH and pOH values of:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm62771680\" data-type=\"equation\">\\(\\text{pH}={-}\\text{log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]={-}\\text{log}\\left(4.9\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-7}\\right)=6.31\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm102114704\" data-type=\"equation\">\\(\\text{pOH}={-}\\text{log}\\left[{\\text{OH}^-}^{\\text{}}\\right]={-}\\text{log}\\left(4.9\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-7}\\right)=6.31\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm67617872\">At this temperature, then, neutral solutions exhibit pH = pOH = 6.31, acidic solutions exhibit pH less than 6.31 and pOH greater than 6.31, whereas basic solutions exhibit pH greater than 6.31 and pOH less than 6.31. This distinction can be important when studying certain processes that occur at other temperatures, such as enzyme reactions in warm-blooded organisms at a temperature around 36\u201340 \u00b0C. Unless otherwise noted, references to pH values are presumed to be those at 25 \u00b0C <a class=\"autogenerated-content\" href=\"#fs-idp56820128\">(Table 8.3.1)<\/a>.<\/p>\r\n\r\n<table id=\"fs-idp56820128\" class=\"aligncenter\" summary=\"This table has three columns and four rows. The first row is a header row, and it labels each column: \u201cClassification,\u201d \u201cRelative ion concentrations,\u201d and \u201cp H at 25 degrees C.\u201d Under the \u201cClassification\u201d column are the following: \u201cacidic,\u201d \u201cneutral,\u201d and \u201cbasic.\u201d Under the \u201cRelative ion concentrations\u201d column are the following, \u201c[ H subscript 2 O superscript plus sign ] is greater than [ O H superscript negative sign],\u201d \u201c[ H subscript 2 O superscript plus sign ] equals [ O H superscript negative sign ],\u201d and, \u201c[ H subscript 2 O superscript plus sign ] is less than [ O H superscript negative sing ].\u201d Under the \u201cp H at 25 degrees C\u201d column are the following: \u201cp H is less than 7,\u201d \u201cp H equals 7,\u201d and \u201cp H is greater than 7.\u201d\"><caption>Table 8.3.1 - Summary of Relations for Acidic, Basic and Neutral Solutions<\/caption>\r\n<thead>\r\n<tr valign=\"top\">\r\n<th data-align=\"center\">Classification<\/th>\r\n<th data-align=\"center\">Relative Ion Concentrations<\/th>\r\n<th data-align=\"center\">pH at 25 \u00b0C<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr valign=\"top\">\r\n<td data-align=\"center\">acidic<\/td>\r\n<td data-align=\"center\">[H<sub>3<\/sub>O<sup>+<\/sup>] &gt; [OH<sup>\u2212<\/sup>]<\/td>\r\n<td data-align=\"center\">pH &lt; 7<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"center\">neutral<\/td>\r\n<td data-align=\"center\">[H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]<\/td>\r\n<td data-align=\"center\">pH = 7<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td data-align=\"center\">basic<\/td>\r\n<td data-align=\"center\">[H<sub>3<\/sub>O<sup>+<\/sup>] &lt; [OH<sup>\u2212<\/sup>]<\/td>\r\n<td data-align=\"center\">pH &gt; 7<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"fs-idp96882128\"><a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_phscale\">(Figure 8.3.1)<\/a> shows the relationships between [H<sub>3<\/sub>O<sup>+<\/sup>], [OH<sup>\u2212<\/sup>], pH, and pOH for solutions classified as acidic, basic, and neutral.<\/p>\r\n\r\n<div id=\"CNX_Chem_14_02_phscale\" class=\"bc-figure figure\">\r\n<div class=\"bc-figcaption figcaption\">The pH and pOH scales represent concentrations of H<sub>3<\/sub>O<sup>+<\/sup> and OH<sup>\u2212<\/sup>, respectively. The pH and pOH values of some common substances at 25 \u00b0C are shown in this chart.<\/div>\r\n<div><\/div>\r\n\r\n[caption id=\"\" align=\"alignnone\" width=\"1300\"]<img src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_02_phscale-1.jpg\" alt=\"A table is provided with 5 columns. The first column is labeled \u201cleft bracket H subscript 3 O superscript plus right bracket (M).\u201d Powers of ten are listed in the column beginning at 10 superscript 1, including 10 superscript 0 or 1, 10 superscript negative 1, decreasing by single powers of 10 to 10 superscript negative 15. The second column is labeled \u201cleft bracket O H superscript negative right bracket (M).\u201d Powers of ten are listed in the column beginning at 10 superscript negative 15, increasing by single powers of 10 to including 10 superscript 0 or 1, and 10 superscript 1. The third column is labeled \u201cp H.\u201d Values listed in this column are integers beginning at negative 1, increasing by ones up to 14. The fourth column is labeled \u201cp O H.\u201d Values in this column are integers beginning at 15, decreasing by ones up to negative 1. The fifth column is labeled \u201cSample Solution.\u201d A vertical line at the left of the column has tick marks corresponding to each p H level in the table. Substances are listed next to this line segment with line segments connecting them to the line to show approximate p H and p O H values. 1 M H C l is listed at a p H of 0. Gastric juices are listed at a p H of about 1.5. Lime juice is listed at a p H of about 2, followed by 1 M C H subscript 3 C O subscript 2 H, followed by stomach acid at a p H value of nearly 3. Wine is listed around 3.5. Coffee is listed just past 5. Pure water is listed at a p H of 7. Pure blood is just beyond 7. Milk of Magnesia is listed just past a p H of 10.5. Household ammonia is listed just before a pH of 12. 1 M N a O H is listed at a p H of 0. To the right of this labeled arrow is an arrow that points up and down through the height of the column. A beige strip passes through the table and to this double headed arrow at p H 7. To the left of the double headed arrow in this beige strip is the label \u201cneutral.\u201d A narrow beige strip runs through the arrow. Just above and below this region, the arrow is purple. It gradually turns to a bright red as it extends upward. At the top of the arrow, near the head of the arrow is the label \u201cacidic.\u201d Similarly, the lower region changes color from purple to blue moving to the bottom of the column. The head at this end of the arrow is labeled \u201cbasic.\u201d\" width=\"1300\" height=\"1139\" data-media-type=\"image\/jpeg\" \/> <strong>Figure 8.3.1 - The hydronium and hydroxide concentrations, and pH and pOH values for common solutions.<\/strong>[\/caption]\r\n\r\n<div class=\"textbox textbox--examples\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\"><strong>Activity 8.3.1 - Calculation of pH from [H<sub>3<\/sub>O<sup>+<\/sup>]\u00a0<\/strong><\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<p id=\"fs-idp97421056\">What is the pH of stomach acid, a solution of HCl with a hydronium ion concentration of 1.2 \\(\\times\\) 10<sup>\u22123<\/sup><em data-effect=\"italics\">M<\/em>?<\/p>\r\n\r\n<h2 id=\"fs-idm103954896\">Solution<\/h2>\r\n<div id=\"fs-idm98702480\" data-type=\"equation\">\\(\\text{pH}={-}\\text{log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm79624528\" data-type=\"equation\">\\(={-}\\text{log(}1.2\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-3}\\right)\\)<\/div>\r\n<div id=\"fs-idm7356256\" data-type=\"equation\">\\(=\\text{\u2212}\\left(-2.92\\right)=2.92\\)<\/div>\r\n<span data-type=\"newline\">\r\n<\/span> (The use of logarithms is explained in <a class=\"target-chapter\" href=\"\/contents\/dff91a60-20dc-4c42-9824-1c616ee6a1c6\">Appendix B<\/a>. When taking the log of a value, keep as many decimal places in the result as there are significant figures in the value.)\r\n\r\n<hr \/>\r\n\r\n<h2 id=\"fs-idp57469360\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\r\nWater exposed to air contains carbonic acid, H<sub>2<\/sub>CO<sub>3<\/sub>, due to the reaction between carbon dioxide and water:\r\n\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm45568144\" data-type=\"equation\">\\({\\text{CO}}_{2}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\phantom{\\rule{0.2em}{0ex}}\\rightleftharpoons\\phantom{\\rule{0.2em}{0ex}}{\\text{H}}_{2}{\\text{CO}}_{3}\\left(aq\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm106049328\">Air-saturated water has a hydronium ion concentration caused by the dissolved CO<sub>2<\/sub> of 2.0 \\(\\times\\) 10<sup>\u22126<\/sup><em data-effect=\"italics\">M<\/em>, about 20-times larger than that of pure water. Calculate the pH of the solution at 25 \u00b0C.<\/p>\r\n\r\n<div id=\"fs-idm61631152\" data-type=\"note\">\r\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\r\n<p id=\"fs-idm99369680\" style=\"text-align: right\">5.70<\/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\"><strong>Activity 8.3.2 - Calculation of Hydronium Ion Concentration from pH<\/strong><\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<p id=\"fs-idm102910496\">Calculate the hydronium ion concentration of blood, the pH of which is 7.3.<\/p>\r\n\r\n<h2 id=\"fs-idp11945040\">Solution<\/h2>\r\n<div id=\"fs-idm108531776\" data-type=\"equation\">\\(\\text{pH}={-}\\text{log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]=7.3\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm49363536\" data-type=\"equation\">\\(\\text{log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]=-7.3\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idp46442128\" data-type=\"equation\">\\(\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]={10}^{-7.3}\\phantom{\\rule{0.2em}{0ex}}\\text{or}\\phantom{\\rule{0.4em}{0ex}}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]=\\text{antilog of \u22127.3}\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm58086272\" data-type=\"equation\">\\(\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]=5\\phantom{\\rule{0.2em}{0ex}}\\times\\phantom{\\rule{0.2em}{0ex}}{10}^{-8}\\phantom{\\rule{0.2em}{0ex}}M\\)<\/div>\r\n<span data-type=\"newline\"><em>\u00a0<\/em>\r\n<\/span> (On a calculator take the antilog, or the \u201cinverse\u201d log, of \u22127.3, or calculate 10<sup>\u22127.3<\/sup>.)\r\n\r\n<hr \/>\r\n\r\n<h2 id=\"fs-idp487584\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\r\nCalculate the hydronium ion concentration of a solution with a pH of \u22121.07.\r\n<div id=\"fs-idp89672320\" data-type=\"note\">\r\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\r\n<p id=\"fs-idm9452560\" style=\"text-align: right\">12 <em data-effect=\"italics\">M<\/em><\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp48828576\" class=\"chemistry sciences-interconnect\" data-type=\"note\">\r\n<h2 data-type=\"title\">Environmental Science<\/h2>\r\n<p id=\"fs-idm116727232\">Normal rainwater has a pH between 5 and 6 due to the presence of dissolved CO<sub>2<\/sub> which forms carbonic acid:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp66992000\" data-type=\"equation\">\\({\\text{H}}_{2}\\text{O}\\left(l\\right)+{\\text{CO}}_{2}\\left(g\\right)\u00a0 \\phantom{\\rule{0.2em}{0ex}}$\\rightarrow$\\phantom{\\rule{0.2em}{0ex}}{\\text{H}}_{2}{\\text{CO}}_{3}\\left(aq\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm103550896\" data-type=\"equation\">\\({\\text{H}}_{2}{\\text{CO}}_{3}\\left(aq\\right)\\phantom{\\rule{0.2em}{0ex}}\\rightleftharpoons\\phantom{\\rule{0.2em}{0ex}}{\\text{H}}^{\\text{+}}\\left(aq\\right)+{\\text{HCO}}_{3}{^-}^{\\text{}}\\left(aq\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idp13883280\">Acid rain is rainwater that has a pH of less than 5, due to a variety of nonmetal oxides, including CO<sub>2<\/sub>, SO<sub>2<\/sub>, SO<sub>3<\/sub>, NO, and NO<sub>2<\/sub> being dissolved in the water and reacting with it to form not only carbonic acid, but sulfuric acid and nitric acid. The formation and subsequent ionization of sulfuric acid are shown here:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp39536896\" data-type=\"equation\">\\({\\text{H}}_{2}\\text{O}\\left(l\\right)+{\\text{SO}}_{3}\\left(g\\right)\\phantom{\\rule{0.2em}{0ex}}$\\rightarrow$\\phantom{\\rule{0.2em}{0ex}}{\\text{H}}_{2}{\\text{SO}}_{4}\\left(aq\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idp62631392\" data-type=\"equation\">\\({\\text{H}}_{2}{\\text{SO}}_{4}\\left(aq\\right)\\phantom{\\rule{0.2em}{0ex}}$\\rightarrow$\\phantom{\\rule{0.2em}{0ex}}{\\text{H}}^{\\text{+}}\\left(aq\\right)+{\\text{HSO}}_{4}{^-}^{\\text{}}\\left(aq\\right)\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idp93018416\">Carbon dioxide is naturally present in the atmosphere because most organisms produce it as a waste product of metabolism. Carbon dioxide is also formed when fires release carbon stored in vegetation or fossil fuels. Sulfur trioxide in the atmosphere is naturally produced by volcanic activity, but it also originates from burning fossil fuels, which have traces of sulfur, and from the process of \u201croasting\u201d ores of metal sulfides in metal-refining processes. Oxides of nitrogen are formed in internal combustion engines where the high temperatures make it possible for the nitrogen and oxygen in air to chemically combine.<\/p>\r\n<p id=\"fs-idm22038432\">Acid rain is a particular problem in industrial areas where the products of combustion and smelting are released into the air without being stripped of sulfur and nitrogen oxides. In North America and Europe until the 1980s, it was responsible for the destruction of forests and freshwater lakes, when the acidity of the rain actually killed trees, damaged soil, and made lakes uninhabitable for all but the most acid-tolerant species. Acid rain also corrodes statuary and building facades that are made of marble and limestone <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_AcidRain\">(Figure 8.3.2)<\/a>. Regulations limiting the amount of sulfur and nitrogen oxides that can be released into the atmosphere by industry and automobiles have reduced the severity of acid damage to both natural and manmade environments in North America and Europe. It is now a growing problem in industrial areas of China and India.<\/p>\r\n<p id=\"fs-idm22123696\">For further information on acid rain, visit this <a href=\"http:\/\/openstaxcollege.org\/l\/16EPA\">website<\/a> hosted by the US Environmental Protection Agency.<\/p>\r\n\r\n<div id=\"CNX_Chem_14_02_AcidRain\" class=\"scaled-down\">\r\n<div class=\"bc-figcaption figcaption\"><\/div>\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"975\"]<img src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_02_AcidRain-1-1.jpg\" alt=\"Two photos are shown. Photograph a on the left shows the upper portion of trees against a bright blue sky. The tops of several trees at the center of the photograph have bare branches and appear to be dead. Image b shows a statue of a man that appears to from the revolutionary war era in either marble or limestone.\" width=\"975\" height=\"396\" data-media-type=\"image\/jpeg\" \/> <strong>Figure 8.3.2 - (a) Acid rain makes trees more susceptible to drought and insect infestation, and depletes nutrients in the soil. (b) It also is corrodes statues that are carved from marble or limestone. (credit a: modification of work by Chris M Morris; credit b: modification of work by \u201cEden, Janine and Jim\u201d\/Flickr)<\/strong>[\/caption]\r\n\r\n<div class=\"textbox textbox--examples\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\"><strong>Activity 8.3.3 - Calculation of pOH\u00a0<\/strong><\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n<p id=\"fs-idp57499040\">What are the pOH and the pH of a 0.0125-<em data-effect=\"italics\">M<\/em> solution of potassium hydroxide, KOH?<\/p>\r\n\r\n<h2 id=\"fs-idm55606544\">Solution<\/h2>\r\nPotassium hydroxide is a highly soluble ionic compound and completely dissociates when dissolved in dilute solution, yielding [OH<sup>\u2212<\/sup>] = 0.0125 <em data-effect=\"italics\">M<\/em>:\r\n\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idp97197664\" data-type=\"equation\">\\(\\text{pOH}={-}\\text{log}\\left[{\\text{OH}^-}^{\\text{}}\\right]={-}\\text{log}\\phantom{\\rule{0.2em}{0ex}}0.0125\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idp138082848\" data-type=\"equation\">\\(={-}\\text{}\\left(-1.903\\right)=1.903\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<p id=\"fs-idm11584304\">The pH can be found from the pOH:<\/p>\r\n<em>\u00a0<\/em>\r\n<div id=\"fs-idm77730624\" data-type=\"equation\">\\(\\text{pH}+\\text{pOH}=14.00\\)<\/div>\r\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\r\n<div id=\"fs-idm71245120\" data-type=\"equation\">\\(\\text{pH}=14.00-\\text{pOH}=14.00-1.903=12.10\\)<\/div>\r\n<div data-type=\"equation\">\r\n\r\n<hr \/>\r\n\r\n<\/div>\r\n<h2 data-type=\"equation\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\r\nThe hydronium ion concentration of vinegar is approximately 4 \\(\\times\\) 10<sup>\u22123<\/sup><em data-effect=\"italics\">M<\/em>. What are the corresponding values of pOH and pH?\r\n<div id=\"fs-idm58824960\" data-type=\"note\">\r\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\r\n<p id=\"fs-idm165995920\" style=\"text-align: right\">pOH = 11.6, pH = 2.4<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<p id=\"fs-idm165634608\">The acidity of a solution is typically assessed experimentally by measurement of its pH. The pOH of a solution is not usually measured, as it is easily calculated from an experimentally determined pH value. The pH of a solution can be directly measured using a pH meter <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_pHMeter\">(Figure 8.3.3)<\/a>.<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"CNX_Chem_14_02_pHMeter\" class=\"bc-figure figure\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"1300\"]<img style=\"color: #373d3f;font-weight: bold;font-size: 1em\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_02_pHMeter-1-1.jpg\" alt=\"This figure contains two images. The first, image a, is of an analytical digital p H meter on a laboratory counter. The second, image b, is of a portable hand held digital p H meter.\" width=\"1300\" height=\"745\" data-media-type=\"image\/jpeg\" \/> <strong>Figure 8.3.3 - (a) A research-grade pH meter used in a laboratory can have a resolution of 0.001 pH units, an accuracy of \u00b1 0.002 pH units, and may cost in excess of ?1000. (b) A portable pH meter has lower resolution (0.01 pH units), lower accuracy (\u00b1 0.2 pH units), and a far lower price tag. (credit b: modification of work by Jacopo Werther)<\/strong>[\/caption]\r\n\r\n<span style=\"text-align: initial;font-size: 1em\">The pH of a solution may also be visually estimated using colored indicators <\/span><a class=\"autogenerated-content\" style=\"text-align: initial;font-size: 1em\" href=\"#CNX_Chem_14_02_indicator\">(Figure 8.3.4)<\/a><span style=\"text-align: initial;font-size: 1em\">. The acid-base equilibria that enable use of these indicator dyes for pH measurements are described in a later section of this chapter.<\/span>\r\n\r\n<\/div>\r\n<div id=\"CNX_Chem_14_02_indicator\" 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_02_indicator-1-1.jpg\" alt=\"This figure contains two images. The first shows a variety of colors of solutions in labeled beakers. A red solution in a beaker is labeled \u201c0.10 M H C l.\u201d An orange solution is labeled \u201c0.10 M C H subscript 3 C O O H.\u201d A yellow-orange solution is labeled \u201c0.1 M N H subscript 4 C l.\u201d A yellow solution is labeled \u201cdeionized water.\u201d A second solution beaker is labeled \u201c0.10 M K C l.\u201d A green solution is labeled \u201c0.10 M aniline.\u201d A blue solution is labeled \u201c0.10 M N H subscript 4 C l (a q).\u201d A final beaker containing a dark blue solution is labeled \u201c0.10 M N a O H.\u201d Image b shows pHydrion paper that is used for measuring pH in the range of p H from 1 to 12. The color scale for identifying p H based on color is shown along with several of the test strips used to evaluate p H.\" width=\"1300\" height=\"427\" data-media-type=\"image\/jpeg\" \/> <strong>Figure 8.4.4 - (a) A solution containing a dye mixture, called universal indicator, takes on different colors depending upon its pH. (b) Convenient test strips, called pH paper, contain embedded indicator dyes that yield pH-dependent color changes on contact with aqueous solutions.(credit: modification of work by Sahar Atwa)<\/strong>[\/caption]\r\n\r\n<\/div>\r\n<h1 data-type=\"title\">Key Concepts and Summary<\/h1>\r\n<p id=\"fs-idp58752272\">Concentrations of hydronium and hydroxide ions in aqueous media are often represented as logarithmic pH and pOH values, respectively. At 25 \u00b0C, the autoprotolysis equilibrium for water requires the sum of pH and pOH to equal 14 for any aqueous solution. The relative concentrations of hydronium and hydroxide ion in a solution define its status as acidic ([H<sub>3<\/sub>O<sup>+<\/sup>] &gt; [OH<sup>\u2212<\/sup>]), basic ([H<sub>3<\/sub>O<sup>+<\/sup>] &lt; [OH<sup>\u2212<\/sup>]), or neutral ([H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]). At 25 \u00b0C, a pH &lt; 7 indicates an acidic solution, a pH &gt; 7 a basic solution, and a pH = 7 a neutral solution.<\/p>\r\n\r\n<h2 data-type=\"title\">Key Equations<\/h2>\r\n<ul id=\"fs-idp46607520\" data-bullet-style=\"bullet\">\r\n \t<li>\\(\\text{pH}={-}\\text{log}\\left[{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\right]\\)<\/li>\r\n \t<li>pOH = \u2212log[OH<sup>\u2212<\/sup>]<\/li>\r\n \t<li>[H<sub>3<\/sub>O<sup>+<\/sup>] = 10<sup>\u2212pH<\/sup><\/li>\r\n \t<li>[OH<sup>\u2212<\/sup>] = 10<sup>\u2212pOH<\/sup><\/li>\r\n \t<li>pH + pOH = p<em data-effect=\"italics\">K<\/em><sub>w<\/sub> = 14.00 at 25 \u00b0C<\/li>\r\n<\/ul>\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-idp63054032\" data-type=\"exercise\">\r\n<div id=\"fs-idp57993664\" data-type=\"problem\">\r\n<p id=\"fs-idm105009936\">(1) Explain why a sample of pure water at 40 \u00b0C is neutral even though [H<sub>3<\/sub>O<sup>+<\/sup>] = 1.7 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em>. <em data-effect=\"italics\">K<\/em><sub>w<\/sub> is 2.9 \\(\\times\\) 10<sup>\u221214<\/sup> at 40 \u00b0C.<\/p>\r\n<em>\u00a0<\/em>\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idp57620032\" style=\"padding-left: 40px\" data-type=\"solution\">\r\n<p id=\"fs-idm57658080\">In a neutral solution [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]. At 40 \u00b0C, [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>] = (2.910<sup>\u221214<\/sup>)<sup>1\/2<\/sup> = 1.7 \\(\\times\\) 10<sup>\u22127<\/sup>.<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm59232064\" data-type=\"exercise\">\r\n<div id=\"fs-idm111412048\" data-type=\"problem\">\r\n<p id=\"fs-idm103446336\">(2) The ionization constant for water (<em data-effect=\"italics\">K<\/em><sub>w<\/sub>) is 2.9 \\(\\times\\) 10<sup>\u221214<\/sup> at 40 \u00b0C. Calculate [H<sub>3<\/sub>O<sup>+<\/sup>], [OH<sup>\u2212<\/sup>], pH, and pOH for pure water at 40 \u00b0C.<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp62460480\" data-type=\"exercise\">\r\n<div id=\"fs-idm118037232\" data-type=\"problem\">\r\n<p id=\"fs-idm58452160\">(3) The ionization constant for water (<em data-effect=\"italics\">K<\/em><sub>w<\/sub>) is 9.311 \\(\\times\\) 10<sup>\u221214<\/sup> at 60 \u00b0C. Calculate [H<sub>3<\/sub>O<sup>+<\/sup>], [OH<sup>\u2212<\/sup>], pH, and pOH for pure water at 60 \u00b0C.<\/p>\r\n<em>\u00a0<\/em>\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idm86228288\" style=\"padding-left: 40px\" data-type=\"solution\">\r\n<p id=\"fs-idm6526512\"><em data-effect=\"italics\">x<\/em> = 3.051 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em> = [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]; pH = \u2212log3.051 \\(\\times\\) 10<sup>\u22127<\/sup> = \u2212(\u22126.5156) = 6.5156; pOH = pH = 6.5156<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp100037936\" data-type=\"exercise\">\r\n<div id=\"fs-idm133230528\" data-type=\"problem\">\r\n<p id=\"fs-idm193547792\">(4) Calculate the pH and the pOH of each of the following solutions at 25 \u00b0C for which the substances ionize completely:<\/p>\r\n<p id=\"fs-idm62343936\">(4a) 0.200 <em data-effect=\"italics\">M<\/em> HCl<\/p>\r\n<p id=\"fs-idm110199712\">(4b) 0.0143 <em data-effect=\"italics\">M<\/em> NaOH<\/p>\r\n<p id=\"fs-idm139511424\">(4c) 3.0 <em data-effect=\"italics\">M<\/em> HNO<sub>3<\/sub><\/p>\r\n<p id=\"fs-idm85222640\">(4d) 0.0031 <em data-effect=\"italics\">M<\/em> Ca(OH)<sub>2<\/sub><\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm78388032\" data-type=\"exercise\">\r\n<div id=\"fs-idp5531424\" data-type=\"problem\">\r\n<p id=\"fs-idm103266944\">(5) Calculate the pH and the pOH of each of the following solutions at 25 \u00b0C for which the substances ionize completely:<\/p>\r\n<p id=\"fs-idm85929872\">(5a) 0.000259 <em data-effect=\"italics\">M<\/em> HClO<sub>4<\/sub><\/p>\r\n<p id=\"fs-idm105046336\">(5b) 0.21 <em data-effect=\"italics\">M<\/em> NaOH<\/p>\r\n<p id=\"fs-idm71623520\">(5c) 0.000071 <em data-effect=\"italics\">M<\/em> Ba(OH)<sub>2<\/sub><\/p>\r\n<p id=\"fs-idm90266032\">(5d) 2.5 <em data-effect=\"italics\">M<\/em> KOH<\/p>\r\n<em>\u00a0<\/em>\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idp82965184\" style=\"padding-left: 40px\" data-type=\"solution\">\r\n<p id=\"fs-idp96688048\">(a) pH = 3.587; pOH = 10.413; (b) pH = 0.68; pOH = 13.32; (c) pOH = 3.85; pH = 10.15; (d) pH = \u22120.40; pOH = 14.4<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm113520992\" data-type=\"exercise\">\r\n<div id=\"fs-idm96702128\" data-type=\"problem\">\r\n<p id=\"fs-idp57446720\">(6) What are the pH and pOH of a solution of 2.0 M HCl, which ionizes completely?<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp61935360\" data-type=\"exercise\">\r\n<div id=\"fs-idp46399056\" data-type=\"problem\">\r\n<p id=\"fs-idm68044912\">(7) What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52?<\/p>\r\n<em>\u00a0<\/em>\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idm117888064\" style=\"padding-left: 40px\" data-type=\"solution\">\r\n<p id=\"fs-idm86400944\">[H<sub>3<\/sub>O<sup>+<\/sup>] = 3.0 \\(\\times\\) 10<sup>\u22127<\/sup><em data-effect=\"italics\">M<\/em>; [OH<sup>\u2212<\/sup>] = 3.3 \\(\\times\\) 10<sup>\u22128<\/sup><em data-effect=\"italics\">M<\/em><\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm93267520\" data-type=\"exercise\">\r\n<div id=\"fs-idp62546496\" data-type=\"problem\">\r\n<p id=\"fs-idp137408320\">(8) Calculate the hydrogen ion concentration and the hydroxide ion concentration in wine from its pH. See <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_phscale\">(Figure 8.3.1)<\/a> for useful information.<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp268784\" data-type=\"exercise\">\r\n<div id=\"fs-idm38151312\" data-type=\"problem\">\r\n<p id=\"fs-idm117014192\">(9) Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice from its pH. See <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_phscale\">(Figure 8.3.1)<\/a> for useful information.<\/p>\r\n<em>\u00a0<\/em>\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idp129019440\" style=\"padding-left: 40px\" data-type=\"solution\">\r\n<p id=\"fs-idp135394192\">[H<sub>3<\/sub>O<sup>+<\/sup>] = 1 \\(\\times\\) 10<sup>\u22122<\/sup><em data-effect=\"italics\">M<\/em>; [OH<sup>\u2212<\/sup>] = 1 \\(\\times\\) 10<sup>\u221212<\/sup><em data-effect=\"italics\">M<\/em><\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm60999568\" data-type=\"exercise\">\r\n<div id=\"fs-idm95843200\" data-type=\"problem\">\r\n<p id=\"fs-idp10174528\">(10) The hydronium ion concentration in a sample of rainwater is found to be 1.7 \\(\\times\\) 10<sup>\u22126<\/sup><em data-effect=\"italics\">M<\/em> at 25 \u00b0C. What is the concentration of hydroxide ions in the rainwater?<\/p>\r\n<em>\u00a0<\/em>\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm209904880\" data-type=\"exercise\">\r\n<div id=\"fs-idp143540592\" data-type=\"problem\">\r\n<p id=\"fs-idm121774336\">(11) The hydroxide ion concentration in household ammonia is 3.2 \\(\\times\\) 10<sup>\u22123<\/sup><em data-effect=\"italics\">M<\/em> at 25 \u00b0C. What is the concentration of hydronium ions in the solution?<\/p>\r\n<em>\u00a0<\/em>\r\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\r\n\r\n<\/div>\r\n<div id=\"fs-idm15687280\" style=\"padding-left: 40px\" data-type=\"solution\">\r\n<p id=\"fs-idm81860944\">[OH<sup>\u2212<\/sup>] = 3.1 \\(\\times\\) 10<sup>\u221212<\/sup><em data-effect=\"italics\">M<\/em><\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n&nbsp;\r\n\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-idm64563696\">\r\n \t<dt>[pb_glossary id=\"3238\"]acidic[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idm110209904\">a solution in which [H<sub>3<\/sub>O<sup>+<\/sup>] &gt; [OH<sup>\u2212<\/sup>]<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idm111671584\">\r\n \t<dt>[pb_glossary id=\"3239\"]basic[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idp49209968\">a solution in which [H<sub>3<\/sub>O<sup>+<\/sup>] &lt; [OH<sup>\u2212<\/sup>]<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idp143891408\">\r\n \t<dt>[pb_glossary id=\"3240\"]neutral[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idm153784960\">describes a solution in which [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idm103907536\">\r\n \t<dt>[pb_glossary id=\"3241\"]pH[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idm14698528\">logarithmic measure of the concentration of hydronium ions in a solution<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idp46966768\">\r\n \t<dt>[pb_glossary id=\"3242\"]pOH[\/pb_glossary]<\/dt>\r\n \t<dd id=\"fs-idm67584528\">logarithmic measure of the concentration of hydroxide ions in a solution<\/dd>\r\n<\/dl>\r\n<\/div>","rendered":"<div>\n<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>Explain the characterization of aqueous solutions as acidic, basic, or neutral<\/li>\n<li>Express hydronium and hydroxide ion concentrations on the pH and pOH scales<\/li>\n<li>Perform calculations relating pH and pOH<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<p id=\"fs-idp11137424\">As discussed earlier, hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (<em data-effect=\"italics\">K<\/em><sub>w<\/sub>). The concentrations of these ions in a solution are often critical determinants of the solution\u2019s properties and the chemical behaviors of its other solutes, and specific vocabulary has been developed to describe these concentrations in relative terms. A solution is <span data-type=\"term\">neutral<\/span> if it contains equal concentrations of hydronium and hydroxide ions; <span data-type=\"term\">acidic<\/span> if it contains a greater concentration of hydronium ions than hydroxide ions; and <span data-type=\"term\">basic<\/span> if it contains a lesser concentration of hydronium ions than hydroxide ions.<\/p>\n<p id=\"fs-idm21650320\">A common means of expressing quantities that may span many orders of magnitude is to use a logarithmic scale. One such scale that is very popular for chemical concentrations and equilibrium constants is based on the p-function, defined as shown where \u201cX\u201d is the quantity of interest and \u201clog\u201d is the base-10 logarithm:<\/p>\n<p>&nbsp;<\/p>\n<div id=\"fs-idp27819744\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-154f915375f8968bf30b7bf72bad18e7_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#88;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#32;&#88;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"102\" style=\"vertical-align: -4px;\" \/><\/div>\n<div data-type=\"equation\"><\/div>\n<p id=\"fs-idm40569744\">The <span data-type=\"term\">pH<\/span> of a solution is therefore defined as shown here, where [H<sub>3<\/sub>O<sup>+<\/sup>] is the molar concentration of hydronium ion in the solution:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm104306928\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-fa8841d54ed308d1c741e31f293e112e_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;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"144\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm112635600\">Rearranging this equation to isolate the hydronium ion molarity yields the equivalent expression:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm34387328\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-201c4c1aebc7395081b9325029bac646_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;&#123;&#49;&#48;&#125;&#94;&#123;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"128\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><\/div>\n<p id=\"fs-idp55544688\">Likewise, the hydroxide ion molarity may be expressed as a p-function, or <span data-type=\"term\">pOH<\/span>:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp66748048\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-23d1da1c19f3789964699e77d06e9f72_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;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"151\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idp67153952\">or<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp102994080\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-032a3dbc404ffca77344a30c32824a79_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;&#123;&#49;&#48;&#125;&#94;&#123;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#79;&#72;&#125;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"132\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm97029664\">Finally, the relation between these two ion concentration expressed as p-functions is easily derived from the <em data-effect=\"italics\">K<\/em><sub>w<\/sub> expression:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp158230176\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-d18974ff17ffee1f99e31f5db2ebde2b_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#119;&#125;&#125;&#61;&#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;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"164\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idp50288944\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-f2a22028d4c9af8e6ec4fba09554f53f_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#45;&#125;&#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;&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#119;&#125;&#125;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#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;&#79;&#72;&#125;&#94;&#45;&#125;&#94;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#093;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#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;&#43;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"498\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm65790448\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-40d2ae99c00c66c1dcb9f5fb77e777e1_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#125;&#123;&#75;&#125;&#95;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#119;&#125;&#125;&#61;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#79;&#72;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"141\" style=\"vertical-align: -3px;\" \/><\/div>\n<div data-type=\"equation\"><\/div>\n<p id=\"fs-idp11266224\">At 25 \u00b0C, the value of <em data-effect=\"italics\">K<\/em><sub>w<\/sub> is 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>\u221214<\/sup>, and so:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm26101984\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-2f693dffa7482686dd388631060acc93_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#49;&#52;&#46;&#48;&#48;&#61;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#79;&#72;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"145\" style=\"vertical-align: -3px;\" \/><\/div>\n<div data-type=\"equation\"><\/div>\n<p id=\"fs-idm103103632\">The hydronium ion molarity in pure water (or any neutral solution) is 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>\u22127<\/sup><em data-effect=\"italics\">M<\/em> at 25 \u00b0C. The pH and pOH of a neutral solution at this temperature are therefore:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp111835440\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-be1874a37e596fdcb50010e04dc5156f_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;&#8722;&#108;&#111;&#103;&#125;&#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;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#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;&#49;&#123;&#48;&#125;&#94;&#123;&#45;&#55;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#55;&#46;&#48;&#48;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"370\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm65159184\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-35ba8a7b15af4a235791aacb586c6c17_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;&#8722;&#108;&#111;&#103;&#125;&#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;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#8722;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#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;&#49;&#123;&#48;&#125;&#94;&#123;&#45;&#55;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#55;&#46;&#48;&#48;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"377\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idp108462720\">And so, <em data-effect=\"italics\">at this temperature<\/em>, acidic solutions are those with hydronium ion molarities greater than 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>\u22127<\/sup><em data-effect=\"italics\">M<\/em> and hydroxide ion molarities less than 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>\u22127<\/sup><em data-effect=\"italics\">M<\/em> (corresponding to pH values less than 7.00 and pOH values greater than 7.00). Basic solutions are those with hydronium ion molarities less than 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>\u22127<\/sup><em data-effect=\"italics\">M<\/em> and hydroxide ion molarities greater than 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>\u22127<\/sup><em data-effect=\"italics\">M<\/em> (corresponding to pH values greater than 7.00 and pOH values less than 7.00).<\/p>\n<p id=\"fs-idm84564368\">Since the autoionization constant <em data-effect=\"italics\">K<\/em><sub>w<\/sub> is temperature dependent, these correlations between pH values and the acidic\/neutral\/basic adjectives will be different at temperatures other than 25 \u00b0C. For example, the hydronium molarity of pure water at 80 \u00b0C is 4.9 <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>\u22127<\/sup><em data-effect=\"italics\">M<\/em>, which corresponds to pH and pOH values of:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm62771680\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-0c3ffb579d434fa5edcb8b93aa53507e_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;&#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;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#52;&#46;&#57;&#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;&#55;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#54;&#46;&#51;&#49;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"369\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm102114704\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-f6f760bc2be68667187a6ba2f88d8759_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;&#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;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#52;&#46;&#57;&#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;&#55;&#125;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#54;&#46;&#51;&#49;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"376\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm67617872\">At this temperature, then, neutral solutions exhibit pH = pOH = 6.31, acidic solutions exhibit pH less than 6.31 and pOH greater than 6.31, whereas basic solutions exhibit pH greater than 6.31 and pOH less than 6.31. This distinction can be important when studying certain processes that occur at other temperatures, such as enzyme reactions in warm-blooded organisms at a temperature around 36\u201340 \u00b0C. Unless otherwise noted, references to pH values are presumed to be those at 25 \u00b0C <a class=\"autogenerated-content\" href=\"#fs-idp56820128\">(Table 8.3.1)<\/a>.<\/p>\n<table id=\"fs-idp56820128\" class=\"aligncenter\" summary=\"This table has three columns and four rows. The first row is a header row, and it labels each column: \u201cClassification,\u201d \u201cRelative ion concentrations,\u201d and \u201cp H at 25 degrees C.\u201d Under the \u201cClassification\u201d column are the following: \u201cacidic,\u201d \u201cneutral,\u201d and \u201cbasic.\u201d Under the \u201cRelative ion concentrations\u201d column are the following, \u201c[ H subscript 2 O superscript plus sign ] is greater than [ O H superscript negative sign],\u201d \u201c[ H subscript 2 O superscript plus sign ] equals [ O H superscript negative sign ],\u201d and, \u201c[ H subscript 2 O superscript plus sign ] is less than [ O H superscript negative sing ].\u201d Under the \u201cp H at 25 degrees C\u201d column are the following: \u201cp H is less than 7,\u201d \u201cp H equals 7,\u201d and \u201cp H is greater than 7.\u201d\">\n<caption>Table 8.3.1 &#8211; Summary of Relations for Acidic, Basic and Neutral Solutions<\/caption>\n<thead>\n<tr valign=\"top\">\n<th data-align=\"center\">Classification<\/th>\n<th data-align=\"center\">Relative Ion Concentrations<\/th>\n<th data-align=\"center\">pH at 25 \u00b0C<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr valign=\"top\">\n<td data-align=\"center\">acidic<\/td>\n<td data-align=\"center\">[H<sub>3<\/sub>O<sup>+<\/sup>] &gt; [OH<sup>\u2212<\/sup>]<\/td>\n<td data-align=\"center\">pH &lt; 7<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"center\">neutral<\/td>\n<td data-align=\"center\">[H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]<\/td>\n<td data-align=\"center\">pH = 7<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td data-align=\"center\">basic<\/td>\n<td data-align=\"center\">[H<sub>3<\/sub>O<sup>+<\/sup>] &lt; [OH<sup>\u2212<\/sup>]<\/td>\n<td data-align=\"center\">pH &gt; 7<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"fs-idp96882128\"><a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_phscale\">(Figure 8.3.1)<\/a> shows the relationships between [H<sub>3<\/sub>O<sup>+<\/sup>], [OH<sup>\u2212<\/sup>], pH, and pOH for solutions classified as acidic, basic, and neutral.<\/p>\n<div id=\"CNX_Chem_14_02_phscale\" class=\"bc-figure figure\">\n<div class=\"bc-figcaption figcaption\">The pH and pOH scales represent concentrations of H<sub>3<\/sub>O<sup>+<\/sup> and OH<sup>\u2212<\/sup>, respectively. The pH and pOH values of some common substances at 25 \u00b0C are shown in this chart.<\/div>\n<div><\/div>\n<figure style=\"width: 1300px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_02_phscale-1.jpg\" alt=\"A table is provided with 5 columns. The first column is labeled \u201cleft bracket H subscript 3 O superscript plus right bracket (M).\u201d Powers of ten are listed in the column beginning at 10 superscript 1, including 10 superscript 0 or 1, 10 superscript negative 1, decreasing by single powers of 10 to 10 superscript negative 15. The second column is labeled \u201cleft bracket O H superscript negative right bracket (M).\u201d Powers of ten are listed in the column beginning at 10 superscript negative 15, increasing by single powers of 10 to including 10 superscript 0 or 1, and 10 superscript 1. The third column is labeled \u201cp H.\u201d Values listed in this column are integers beginning at negative 1, increasing by ones up to 14. The fourth column is labeled \u201cp O H.\u201d Values in this column are integers beginning at 15, decreasing by ones up to negative 1. The fifth column is labeled \u201cSample Solution.\u201d A vertical line at the left of the column has tick marks corresponding to each p H level in the table. Substances are listed next to this line segment with line segments connecting them to the line to show approximate p H and p O H values. 1 M H C l is listed at a p H of 0. Gastric juices are listed at a p H of about 1.5. Lime juice is listed at a p H of about 2, followed by 1 M C H subscript 3 C O subscript 2 H, followed by stomach acid at a p H value of nearly 3. Wine is listed around 3.5. Coffee is listed just past 5. Pure water is listed at a p H of 7. Pure blood is just beyond 7. Milk of Magnesia is listed just past a p H of 10.5. Household ammonia is listed just before a pH of 12. 1 M N a O H is listed at a p H of 0. To the right of this labeled arrow is an arrow that points up and down through the height of the column. A beige strip passes through the table and to this double headed arrow at p H 7. To the left of the double headed arrow in this beige strip is the label \u201cneutral.\u201d A narrow beige strip runs through the arrow. Just above and below this region, the arrow is purple. It gradually turns to a bright red as it extends upward. At the top of the arrow, near the head of the arrow is the label \u201cacidic.\u201d Similarly, the lower region changes color from purple to blue moving to the bottom of the column. The head at this end of the arrow is labeled \u201cbasic.\u201d\" width=\"1300\" height=\"1139\" data-media-type=\"image\/jpeg\" \/><figcaption class=\"wp-caption-text\"><strong>Figure 8.3.1 &#8211; The hydronium and hydroxide concentrations, and pH and pOH values for common solutions.<\/strong><\/figcaption><\/figure>\n<div class=\"textbox textbox--examples\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\"><strong>Activity 8.3.1 &#8211; Calculation of pH from [H<sub>3<\/sub>O<sup>+<\/sup>]\u00a0<\/strong><\/p>\n<\/header>\n<div class=\"textbox__content\">\n<p id=\"fs-idp97421056\">What is the pH of stomach acid, a solution of HCl with a hydronium ion concentration of 1.2 <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>\u22123<\/sup><em data-effect=\"italics\">M<\/em>?<\/p>\n<h2 id=\"fs-idm103954896\">Solution<\/h2>\n<div id=\"fs-idm98702480\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-fa8841d54ed308d1c741e31f293e112e_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;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"144\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm79624528\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-7972df881abfd85069f25da7e461a817_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#40;&#125;&#49;&#46;&#50;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"20\" width=\"149\" style=\"vertical-align: -5px;\" \/><\/div>\n<div id=\"fs-idm7356256\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-42d7fbca7d1336a73dbde41367cbbfbe_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#61;&#92;&#116;&#101;&#120;&#116;&#123;&#8722;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#45;&#50;&#46;&#57;&#50;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#50;&#46;&#57;&#50;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"135\" style=\"vertical-align: -4px;\" \/><\/div>\n<p><span data-type=\"newline\"><br \/>\n<\/span> (The use of logarithms is explained in <a class=\"target-chapter\" href=\"\/contents\/dff91a60-20dc-4c42-9824-1c616ee6a1c6\">Appendix B<\/a>. When taking the log of a value, keep as many decimal places in the result as there are significant figures in the value.)<\/p>\n<hr \/>\n<h2 id=\"fs-idp57469360\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\n<p>Water exposed to air contains carbonic acid, H<sub>2<\/sub>CO<sub>3<\/sub>, due to the reaction between carbon dioxide and water:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm45568144\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-7163d9d2f3c2891f30c105c25f2fea0d_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#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;&#92;&#114;&#105;&#103;&#104;&#116;&#108;&#101;&#102;&#116;&#104;&#97;&#114;&#112;&#111;&#111;&#110;&#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;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#51;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"19\" width=\"274\" style=\"vertical-align: -5px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm106049328\">Air-saturated water has a hydronium ion concentration caused by the dissolved CO<sub>2<\/sub> of 2.0 <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>\u22126<\/sup><em data-effect=\"italics\">M<\/em>, about 20-times larger than that of pure water. Calculate the pH of the solution at 25 \u00b0C.<\/p>\n<div id=\"fs-idm61631152\" data-type=\"note\">\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\n<p id=\"fs-idm99369680\" style=\"text-align: right\">5.70<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox textbox--examples\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\"><strong>Activity 8.3.2 &#8211; Calculation of Hydronium Ion Concentration from pH<\/strong><\/p>\n<\/header>\n<div class=\"textbox__content\">\n<p id=\"fs-idm102910496\">Calculate the hydronium ion concentration of blood, the pH of which is 7.3.<\/p>\n<h2 id=\"fs-idp11945040\">Solution<\/h2>\n<div id=\"fs-idm108531776\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-35a30ff328a52ba63aec9ecdadf17fb2_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;&#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;&#55;&#46;&#51;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"194\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm49363536\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-ceee32b2dc326f2e91d94a21e220cc02_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#108;&#111;&#103;&#125;&#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;&#45;&#55;&#46;&#51;\" title=\"Rendered by QuickLaTeX.com\" height=\"23\" width=\"147\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idp46442128\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-5054aee7c667e17a3c7f6e4ee8f8465c_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;&#123;&#49;&#48;&#125;&#94;&#123;&#45;&#55;&#46;&#51;&#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;&#101;&#120;&#116;&#123;&#111;&#114;&#125;&#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;&#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;&#116;&#101;&#120;&#116;&#123;&#97;&#110;&#116;&#105;&#108;&#111;&#103;&#32;&#111;&#102;&#32;&#8722;&#55;&#46;&#51;&#125;\" title=\"Rendered by QuickLaTeX.com\" height=\"23\" width=\"344\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm58086272\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-a9074a16de56d234413e1a63ea819943_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;&#53;&#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;&#56;&#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=\"22\" width=\"178\" style=\"vertical-align: -7px;\" \/><\/div>\n<p><span data-type=\"newline\"><em>\u00a0<\/em><br \/>\n<\/span> (On a calculator take the antilog, or the \u201cinverse\u201d log, of \u22127.3, or calculate 10<sup>\u22127.3<\/sup>.)<\/p>\n<hr \/>\n<h2 id=\"fs-idp487584\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\n<p>Calculate the hydronium ion concentration of a solution with a pH of \u22121.07.<\/p>\n<div id=\"fs-idp89672320\" data-type=\"note\">\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\n<p id=\"fs-idm9452560\" style=\"text-align: right\">12 <em data-effect=\"italics\">M<\/em><\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"fs-idp48828576\" class=\"chemistry sciences-interconnect\" data-type=\"note\">\n<h2 data-type=\"title\">Environmental Science<\/h2>\n<p id=\"fs-idm116727232\">Normal rainwater has a pH between 5 and 6 due to the presence of dissolved CO<sub>2<\/sub> which forms carbonic acid:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp66992000\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-69828fc0141d281bf07d87815fb02107_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#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;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#50;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#32;&#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;&#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;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#51;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"256\" style=\"vertical-align: -4px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm103550896\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-f9b2d6b2d77d462eea3eb37ba876761c_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#67;&#79;&#125;&#125;&#95;&#123;&#51;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#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;&#92;&#114;&#105;&#103;&#104;&#116;&#108;&#101;&#102;&#116;&#104;&#97;&#114;&#112;&#111;&#111;&#110;&#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;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#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;&#72;&#67;&#79;&#125;&#125;&#95;&#123;&#51;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"20\" width=\"302\" style=\"vertical-align: -5px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idp13883280\">Acid rain is rainwater that has a pH of less than 5, due to a variety of nonmetal oxides, including CO<sub>2<\/sub>, SO<sub>2<\/sub>, SO<sub>3<\/sub>, NO, and NO<sub>2<\/sub> being dissolved in the water and reacting with it to form not only carbonic acid, but sulfuric acid and nitric acid. The formation and subsequent ionization of sulfuric acid are shown here:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp39536896\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-f036f62928bd6a5a361acdf4eb4626b7_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#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;&#43;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#83;&#79;&#125;&#125;&#95;&#123;&#51;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#103;&#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;&#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;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#83;&#79;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#92;&#114;&#105;&#103;&#104;&#116;&#41;\" title=\"Rendered by QuickLaTeX.com\" height=\"18\" width=\"250\" style=\"vertical-align: -4px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idp62631392\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-d80cb9437ebc5615f043e6a60997d38b_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#72;&#125;&#125;&#95;&#123;&#50;&#125;&#123;&#92;&#116;&#101;&#120;&#116;&#123;&#83;&#79;&#125;&#125;&#95;&#123;&#52;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#97;&#113;&#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;&#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;&#72;&#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;&#72;&#83;&#79;&#125;&#125;&#95;&#123;&#52;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"19\" width=\"287\" style=\"vertical-align: -5px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idp93018416\">Carbon dioxide is naturally present in the atmosphere because most organisms produce it as a waste product of metabolism. Carbon dioxide is also formed when fires release carbon stored in vegetation or fossil fuels. Sulfur trioxide in the atmosphere is naturally produced by volcanic activity, but it also originates from burning fossil fuels, which have traces of sulfur, and from the process of \u201croasting\u201d ores of metal sulfides in metal-refining processes. Oxides of nitrogen are formed in internal combustion engines where the high temperatures make it possible for the nitrogen and oxygen in air to chemically combine.<\/p>\n<p id=\"fs-idm22038432\">Acid rain is a particular problem in industrial areas where the products of combustion and smelting are released into the air without being stripped of sulfur and nitrogen oxides. In North America and Europe until the 1980s, it was responsible for the destruction of forests and freshwater lakes, when the acidity of the rain actually killed trees, damaged soil, and made lakes uninhabitable for all but the most acid-tolerant species. Acid rain also corrodes statuary and building facades that are made of marble and limestone <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_AcidRain\">(Figure 8.3.2)<\/a>. Regulations limiting the amount of sulfur and nitrogen oxides that can be released into the atmosphere by industry and automobiles have reduced the severity of acid damage to both natural and manmade environments in North America and Europe. It is now a growing problem in industrial areas of China and India.<\/p>\n<p id=\"fs-idm22123696\">For further information on acid rain, visit this <a href=\"http:\/\/openstaxcollege.org\/l\/16EPA\">website<\/a> hosted by the US Environmental Protection Agency.<\/p>\n<div id=\"CNX_Chem_14_02_AcidRain\" class=\"scaled-down\">\n<div class=\"bc-figcaption figcaption\"><\/div>\n<figure style=\"width: 975px\" 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_02_AcidRain-1-1.jpg\" alt=\"Two photos are shown. Photograph a on the left shows the upper portion of trees against a bright blue sky. The tops of several trees at the center of the photograph have bare branches and appear to be dead. Image b shows a statue of a man that appears to from the revolutionary war era in either marble or limestone.\" width=\"975\" height=\"396\" data-media-type=\"image\/jpeg\" \/><figcaption class=\"wp-caption-text\"><strong>Figure 8.3.2 &#8211; (a) Acid rain makes trees more susceptible to drought and insect infestation, and depletes nutrients in the soil. (b) It also is corrodes statues that are carved from marble or limestone. (credit a: modification of work by Chris M Morris; credit b: modification of work by \u201cEden, Janine and Jim\u201d\/Flickr)<\/strong><\/figcaption><\/figure>\n<div class=\"textbox textbox--examples\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\"><strong>Activity 8.3.3 &#8211; Calculation of pOH\u00a0<\/strong><\/p>\n<\/header>\n<div class=\"textbox__content\">\n<p id=\"fs-idp57499040\">What are the pOH and the pH of a 0.0125-<em data-effect=\"italics\">M<\/em> solution of potassium hydroxide, KOH?<\/p>\n<h2 id=\"fs-idm55606544\">Solution<\/h2>\n<p>Potassium hydroxide is a highly soluble ionic compound and completely dissociates when dissolved in dilute solution, yielding [OH<sup>\u2212<\/sup>] = 0.0125 <em data-effect=\"italics\">M<\/em>:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idp97197664\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-e030e33a744fbee677b3a6b4e94579f2_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;&#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;&#123;&#45;&#125;&#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;&#48;&#46;&#48;&#49;&#50;&#53;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"267\" style=\"vertical-align: -7px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idp138082848\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c0383c30faef23a94c1eee6b396e5ae7_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#61;&#123;&#45;&#125;&#92;&#116;&#101;&#120;&#116;&#123;&#125;&#92;&#108;&#101;&#102;&#116;&#40;&#45;&#49;&#46;&#57;&#48;&#51;&#92;&#114;&#105;&#103;&#104;&#116;&#41;&#61;&#49;&#46;&#57;&#48;&#51;\" title=\"Rendered by QuickLaTeX.com\" height=\"19\" width=\"168\" style=\"vertical-align: -5px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<p id=\"fs-idm11584304\">The pH can be found from the pOH:<\/p>\n<p><em>\u00a0<\/em><\/p>\n<div id=\"fs-idm77730624\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-c3376bb27daeb0b1eafe145c6f409eef_l3.png\" class=\"ql-img-inline-formula quicklatex-auto-format\" alt=\"&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#72;&#125;&#43;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#79;&#72;&#125;&#61;&#49;&#52;&#46;&#48;&#48;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"146\" style=\"vertical-align: -3px;\" \/><\/div>\n<div data-type=\"equation\"><em>\u00a0<\/em><\/div>\n<div id=\"fs-idm71245120\" data-type=\"equation\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-5df663d3b76efc1ba3e0614c102aeaf3_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;&#92;&#116;&#101;&#120;&#116;&#123;&#112;&#79;&#72;&#125;&#61;&#49;&#52;&#46;&#48;&#48;&#45;&#49;&#46;&#57;&#48;&#51;&#61;&#49;&#50;&#46;&#49;&#48;\" title=\"Rendered by QuickLaTeX.com\" height=\"16\" width=\"336\" style=\"vertical-align: -3px;\" \/><\/div>\n<div data-type=\"equation\">\n<hr \/>\n<\/div>\n<h2 data-type=\"equation\"><span data-type=\"title\">Check Your Learning<\/span><\/h2>\n<p>The hydronium ion concentration of vinegar is approximately 4 <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>\u22123<\/sup><em data-effect=\"italics\">M<\/em>. What are the corresponding values of pOH and pH?<\/p>\n<div id=\"fs-idm58824960\" data-type=\"note\">\n<h3 style=\"text-align: right\" data-type=\"title\">Answer<\/h3>\n<p id=\"fs-idm165995920\" style=\"text-align: right\">pOH = 11.6, pH = 2.4<\/p>\n<\/div>\n<\/div>\n<\/div>\n<p id=\"fs-idm165634608\">The acidity of a solution is typically assessed experimentally by measurement of its pH. The pOH of a solution is not usually measured, as it is easily calculated from an experimentally determined pH value. The pH of a solution can be directly measured using a pH meter <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_pHMeter\">(Figure 8.3.3)<\/a>.<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"CNX_Chem_14_02_pHMeter\" class=\"bc-figure figure\">\n<figure style=\"width: 1300px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" style=\"color: #373d3f;font-weight: bold;font-size: 1em\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/uploads\/sites\/989\/2020\/04\/CNX_Chem_14_02_pHMeter-1-1.jpg\" alt=\"This figure contains two images. The first, image a, is of an analytical digital p H meter on a laboratory counter. The second, image b, is of a portable hand held digital p H meter.\" width=\"1300\" height=\"745\" data-media-type=\"image\/jpeg\" \/><figcaption class=\"wp-caption-text\"><strong>Figure 8.3.3 &#8211; (a) A research-grade pH meter used in a laboratory can have a resolution of 0.001 pH units, an accuracy of \u00b1 0.002 pH units, and may cost in excess of ?1000. (b) A portable pH meter has lower resolution (0.01 pH units), lower accuracy (\u00b1 0.2 pH units), and a far lower price tag. (credit b: modification of work by Jacopo Werther)<\/strong><\/figcaption><\/figure>\n<p><span style=\"text-align: initial;font-size: 1em\">The pH of a solution may also be visually estimated using colored indicators <\/span><a class=\"autogenerated-content\" style=\"text-align: initial;font-size: 1em\" href=\"#CNX_Chem_14_02_indicator\">(Figure 8.3.4)<\/a><span style=\"text-align: initial;font-size: 1em\">. The acid-base equilibria that enable use of these indicator dyes for pH measurements are described in a later section of this chapter.<\/span><\/p>\n<\/div>\n<div id=\"CNX_Chem_14_02_indicator\" 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_02_indicator-1-1.jpg\" alt=\"This figure contains two images. The first shows a variety of colors of solutions in labeled beakers. A red solution in a beaker is labeled \u201c0.10 M H C l.\u201d An orange solution is labeled \u201c0.10 M C H subscript 3 C O O H.\u201d A yellow-orange solution is labeled \u201c0.1 M N H subscript 4 C l.\u201d A yellow solution is labeled \u201cdeionized water.\u201d A second solution beaker is labeled \u201c0.10 M K C l.\u201d A green solution is labeled \u201c0.10 M aniline.\u201d A blue solution is labeled \u201c0.10 M N H subscript 4 C l (a q).\u201d A final beaker containing a dark blue solution is labeled \u201c0.10 M N a O H.\u201d Image b shows pHydrion paper that is used for measuring pH in the range of p H from 1 to 12. The color scale for identifying p H based on color is shown along with several of the test strips used to evaluate p H.\" width=\"1300\" height=\"427\" data-media-type=\"image\/jpeg\" \/><figcaption class=\"wp-caption-text\"><strong>Figure 8.4.4 &#8211; (a) A solution containing a dye mixture, called universal indicator, takes on different colors depending upon its pH. (b) Convenient test strips, called pH paper, contain embedded indicator dyes that yield pH-dependent color changes on contact with aqueous solutions.(credit: modification of work by Sahar Atwa)<\/strong><\/figcaption><\/figure>\n<\/div>\n<h1 data-type=\"title\">Key Concepts and Summary<\/h1>\n<p id=\"fs-idp58752272\">Concentrations of hydronium and hydroxide ions in aqueous media are often represented as logarithmic pH and pOH values, respectively. At 25 \u00b0C, the autoprotolysis equilibrium for water requires the sum of pH and pOH to equal 14 for any aqueous solution. The relative concentrations of hydronium and hydroxide ion in a solution define its status as acidic ([H<sub>3<\/sub>O<sup>+<\/sup>] &gt; [OH<sup>\u2212<\/sup>]), basic ([H<sub>3<\/sub>O<sup>+<\/sup>] &lt; [OH<sup>\u2212<\/sup>]), or neutral ([H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]). At 25 \u00b0C, a pH &lt; 7 indicates an acidic solution, a pH &gt; 7 a basic solution, and a pH = 7 a neutral solution.<\/p>\n<h2 data-type=\"title\">Key Equations<\/h2>\n<ul id=\"fs-idp46607520\" data-bullet-style=\"bullet\">\n<li><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-content\/ql-cache\/quicklatex.com-fa8841d54ed308d1c741e31f293e112e_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;&#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;\" title=\"Rendered by QuickLaTeX.com\" height=\"22\" width=\"144\" style=\"vertical-align: -7px;\" \/><\/li>\n<li>pOH = \u2212log[OH<sup>\u2212<\/sup>]<\/li>\n<li>[H<sub>3<\/sub>O<sup>+<\/sup>] = 10<sup>\u2212pH<\/sup><\/li>\n<li>[OH<sup>\u2212<\/sup>] = 10<sup>\u2212pOH<\/sup><\/li>\n<li>pH + pOH = p<em data-effect=\"italics\">K<\/em><sub>w<\/sub> = 14.00 at 25 \u00b0C<\/li>\n<\/ul>\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-idp63054032\" data-type=\"exercise\">\n<div id=\"fs-idp57993664\" data-type=\"problem\">\n<p id=\"fs-idm105009936\">(1) Explain why a sample of pure water at 40 \u00b0C is neutral even though [H<sub>3<\/sub>O<sup>+<\/sup>] = 1.7 <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>\u22127<\/sup><em data-effect=\"italics\">M<\/em>. <em data-effect=\"italics\">K<\/em><sub>w<\/sub> is 2.9 <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>\u221214<\/sup> at 40 \u00b0C.<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<\/div>\n<div id=\"fs-idp57620032\" style=\"padding-left: 40px\" data-type=\"solution\">\n<p id=\"fs-idm57658080\">In a neutral solution [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]. At 40 \u00b0C, [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>] = (2.910<sup>\u221214<\/sup>)<sup>1\/2<\/sup> = 1.7 <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>\u22127<\/sup>.<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm59232064\" data-type=\"exercise\">\n<div id=\"fs-idm111412048\" data-type=\"problem\">\n<p id=\"fs-idm103446336\">(2) The ionization constant for water (<em data-effect=\"italics\">K<\/em><sub>w<\/sub>) is 2.9 <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>\u221214<\/sup> at 40 \u00b0C. Calculate [H<sub>3<\/sub>O<sup>+<\/sup>], [OH<sup>\u2212<\/sup>], pH, and pOH for pure water at 40 \u00b0C.<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idp62460480\" data-type=\"exercise\">\n<div id=\"fs-idm118037232\" data-type=\"problem\">\n<p id=\"fs-idm58452160\">(3) The ionization constant for water (<em data-effect=\"italics\">K<\/em><sub>w<\/sub>) is 9.311 <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>\u221214<\/sup> at 60 \u00b0C. Calculate [H<sub>3<\/sub>O<sup>+<\/sup>], [OH<sup>\u2212<\/sup>], pH, and pOH for pure water at 60 \u00b0C.<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<\/div>\n<div id=\"fs-idm86228288\" style=\"padding-left: 40px\" data-type=\"solution\">\n<p id=\"fs-idm6526512\"><em data-effect=\"italics\">x<\/em> = 3.051 <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>\u22127<\/sup><em data-effect=\"italics\">M<\/em> = [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]; pH = \u2212log3.051 <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>\u22127<\/sup> = \u2212(\u22126.5156) = 6.5156; pOH = pH = 6.5156<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idp100037936\" data-type=\"exercise\">\n<div id=\"fs-idm133230528\" data-type=\"problem\">\n<p id=\"fs-idm193547792\">(4) Calculate the pH and the pOH of each of the following solutions at 25 \u00b0C for which the substances ionize completely:<\/p>\n<p id=\"fs-idm62343936\">(4a) 0.200 <em data-effect=\"italics\">M<\/em> HCl<\/p>\n<p id=\"fs-idm110199712\">(4b) 0.0143 <em data-effect=\"italics\">M<\/em> NaOH<\/p>\n<p id=\"fs-idm139511424\">(4c) 3.0 <em data-effect=\"italics\">M<\/em> HNO<sub>3<\/sub><\/p>\n<p id=\"fs-idm85222640\">(4d) 0.0031 <em data-effect=\"italics\">M<\/em> Ca(OH)<sub>2<\/sub><\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm78388032\" data-type=\"exercise\">\n<div id=\"fs-idp5531424\" data-type=\"problem\">\n<p id=\"fs-idm103266944\">(5) Calculate the pH and the pOH of each of the following solutions at 25 \u00b0C for which the substances ionize completely:<\/p>\n<p id=\"fs-idm85929872\">(5a) 0.000259 <em data-effect=\"italics\">M<\/em> HClO<sub>4<\/sub><\/p>\n<p id=\"fs-idm105046336\">(5b) 0.21 <em data-effect=\"italics\">M<\/em> NaOH<\/p>\n<p id=\"fs-idm71623520\">(5c) 0.000071 <em data-effect=\"italics\">M<\/em> Ba(OH)<sub>2<\/sub><\/p>\n<p id=\"fs-idm90266032\">(5d) 2.5 <em data-effect=\"italics\">M<\/em> KOH<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<\/div>\n<div id=\"fs-idp82965184\" style=\"padding-left: 40px\" data-type=\"solution\">\n<p id=\"fs-idp96688048\">(a) pH = 3.587; pOH = 10.413; (b) pH = 0.68; pOH = 13.32; (c) pOH = 3.85; pH = 10.15; (d) pH = \u22120.40; pOH = 14.4<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm113520992\" data-type=\"exercise\">\n<div id=\"fs-idm96702128\" data-type=\"problem\">\n<p id=\"fs-idp57446720\">(6) What are the pH and pOH of a solution of 2.0 M HCl, which ionizes completely?<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idp61935360\" data-type=\"exercise\">\n<div id=\"fs-idp46399056\" data-type=\"problem\">\n<p id=\"fs-idm68044912\">(7) What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52?<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<\/div>\n<div id=\"fs-idm117888064\" style=\"padding-left: 40px\" data-type=\"solution\">\n<p id=\"fs-idm86400944\">[H<sub>3<\/sub>O<sup>+<\/sup>] = 3.0 <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>\u22127<\/sup><em data-effect=\"italics\">M<\/em>; [OH<sup>\u2212<\/sup>] = 3.3 <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>\u22128<\/sup><em data-effect=\"italics\">M<\/em><\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm93267520\" data-type=\"exercise\">\n<div id=\"fs-idp62546496\" data-type=\"problem\">\n<p id=\"fs-idp137408320\">(8) Calculate the hydrogen ion concentration and the hydroxide ion concentration in wine from its pH. See <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_phscale\">(Figure 8.3.1)<\/a> for useful information.<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idp268784\" data-type=\"exercise\">\n<div id=\"fs-idm38151312\" data-type=\"problem\">\n<p id=\"fs-idm117014192\">(9) Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice from its pH. See <a class=\"autogenerated-content\" href=\"#CNX_Chem_14_02_phscale\">(Figure 8.3.1)<\/a> for useful information.<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<\/div>\n<div id=\"fs-idp129019440\" style=\"padding-left: 40px\" data-type=\"solution\">\n<p id=\"fs-idp135394192\">[H<sub>3<\/sub>O<sup>+<\/sup>] = 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>\u22122<\/sup><em data-effect=\"italics\">M<\/em>; [OH<sup>\u2212<\/sup>] = 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>\u221212<\/sup><em data-effect=\"italics\">M<\/em><\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm60999568\" data-type=\"exercise\">\n<div id=\"fs-idm95843200\" data-type=\"problem\">\n<p id=\"fs-idp10174528\">(10) The hydronium ion concentration in a sample of rainwater is found to be 1.7 <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>\u22126<\/sup><em data-effect=\"italics\">M<\/em> at 25 \u00b0C. What is the concentration of hydroxide ions in the rainwater?<\/p>\n<p><em>\u00a0<\/em><\/p>\n<\/div>\n<\/div>\n<div id=\"fs-idm209904880\" data-type=\"exercise\">\n<div id=\"fs-idp143540592\" data-type=\"problem\">\n<p id=\"fs-idm121774336\">(11) The hydroxide ion concentration in household ammonia is 3.2 <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>\u22123<\/sup><em data-effect=\"italics\">M<\/em> at 25 \u00b0C. What is the concentration of hydronium ions in the solution?<\/p>\n<p><em>\u00a0<\/em><\/p>\n<p style=\"padding-left: 40px\"><em>Solution<\/em><\/p>\n<\/div>\n<div id=\"fs-idm15687280\" style=\"padding-left: 40px\" data-type=\"solution\">\n<p id=\"fs-idm81860944\">[OH<sup>\u2212<\/sup>] = 3.1 <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>\u221212<\/sup><em data-effect=\"italics\">M<\/em><\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<p>&nbsp;<\/p>\n<\/div>\n<div class=\"textbox shaded\" data-type=\"glossary\">\n<h2 data-type=\"glossary-title\">Glossary<\/h2>\n<dl id=\"fs-idm64563696\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1897_3238\">acidic<\/a><\/dt>\n<dd id=\"fs-idm110209904\">a solution in which [H<sub>3<\/sub>O<sup>+<\/sup>] &gt; [OH<sup>\u2212<\/sup>]<\/dd>\n<\/dl>\n<dl id=\"fs-idm111671584\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1897_3239\">basic<\/a><\/dt>\n<dd id=\"fs-idp49209968\">a solution in which [H<sub>3<\/sub>O<sup>+<\/sup>] &lt; [OH<sup>\u2212<\/sup>]<\/dd>\n<\/dl>\n<dl id=\"fs-idp143891408\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1897_3240\">neutral<\/a><\/dt>\n<dd id=\"fs-idm153784960\">describes a solution in which [H<sub>3<\/sub>O<sup>+<\/sup>] = [OH<sup>\u2212<\/sup>]<\/dd>\n<\/dl>\n<dl id=\"fs-idm103907536\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1897_3241\">pH<\/a><\/dt>\n<dd id=\"fs-idm14698528\">logarithmic measure of the concentration of hydronium ions in a solution<\/dd>\n<\/dl>\n<dl id=\"fs-idp46966768\">\n<dt><a class=\"glossary-term\" aria-haspopup=\"dialog\" aria-describedby=\"definition\" href=\"#term_1897_3242\">pOH<\/a><\/dt>\n<dd id=\"fs-idm67584528\">logarithmic measure of the concentration of hydroxide ions in a solution<\/dd>\n<\/dl>\n<\/div>\n<div class=\"glossary\"><span class=\"screen-reader-text\" id=\"definition\">definition<\/span><template id=\"term_1897_3238\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1897_3238\"><div tabindex=\"-1\"><p>a solution in which [H3O+] &gt; [OH\u2212]<\/p>\n<\/div><button><span aria-hidden=\"true\">&times;<\/span><span class=\"screen-reader-text\">Close definition<\/span><\/button><\/div><\/template><template id=\"term_1897_3239\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1897_3239\"><div tabindex=\"-1\"><p>a solution in which [H3O+] &lt; [OH\u2212]<\/p>\n<\/div><button><span aria-hidden=\"true\">&times;<\/span><span class=\"screen-reader-text\">Close definition<\/span><\/button><\/div><\/template><template id=\"term_1897_3240\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1897_3240\"><div tabindex=\"-1\"><p>describes a solution in which [H3O+] = [OH\u2212]<\/p>\n<\/div><button><span aria-hidden=\"true\">&times;<\/span><span class=\"screen-reader-text\">Close definition<\/span><\/button><\/div><\/template><template id=\"term_1897_3241\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1897_3241\"><div tabindex=\"-1\"><p>logarithmic measure of the concentration of hydronium ions in a solution<\/p>\n<\/div><button><span aria-hidden=\"true\">&times;<\/span><span class=\"screen-reader-text\">Close definition<\/span><\/button><\/div><\/template><template id=\"term_1897_3242\"><div class=\"glossary__definition\" role=\"dialog\" data-id=\"term_1897_3242\"><div tabindex=\"-1\"><p>logarithmic measure of the concentration of hydroxide ions in a solution<\/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":3,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-1897","chapter","type-chapter","status-publish","hentry"],"part":1885,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1897","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":11,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1897\/revisions"}],"predecessor-version":[{"id":3663,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapters\/1897\/revisions\/3663"}],"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\/1897\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/media?parent=1897"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/pressbooks\/v2\/chapter-type?post=1897"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/contributor?post=1897"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/inorganicchemistrychem250\/wp-json\/wp\/v2\/license?post=1897"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}