{"id":1419,"date":"2018-04-11T22:51:46","date_gmt":"2018-04-12T02:51:46","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/4-2-classifying-chemical-reactions\/"},"modified":"2019-05-14T13:49:52","modified_gmt":"2019-05-14T17:49:52","slug":"4-2-classifying-chemical-reactions","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/4-2-classifying-chemical-reactions\/","title":{"raw":"6.2 Precipitation Reactions","rendered":"6.2 Precipitation Reactions"},"content":{"raw":"<div class=\"bcc-box bcc-highlight\">\r\n<h3>Learning Objectives<\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Define precipitation reactions<\/li>\r\n \t<li>Recognize and identify examples of precipitation reactions<\/li>\r\n \t<li>Predict the solubility of common inorganic compounds by using solubility rules<\/li>\r\n<\/ul>\r\n<\/div>\r\n<p id=\"fs-idp140132627979408\">Humans interact with one another in various and complex ways, and we classify these interactions according to common patterns of behavior. When two humans exchange information, we say they are communicating. When they exchange blows with their fists or feet, we say they are fighting. Faced with a wide range of varied interactions between chemical substances, scientists have likewise found it convenient (or even necessary) to classify chemical interactions by identifying common patterns of reactivity. The following sections of this chapter (section 6.2-6.4) will provide an introduction to three of the most prevalent types of chemical reactions: precipitation, acid-base, and oxidation-reduction.<\/p>\r\n\r\n<section id=\"fs-idp140132627979792\">\r\n<h2>Precipitation Reactions and Solubility Rules<\/h2>\r\n<p id=\"fs-idp140132618169728\">A <strong>precipitation reaction<\/strong> is one in which dissolved substances react to form one (or more) solid products. Many reactions of this type involve the exchange of ions between ionic compounds in aqueous solution and are sometimes referred to as <em>double displacement<\/em>, <em>double replacement<\/em>, or <em>metathesis<\/em> reactions. These reactions are common in nature and are responsible for the formation of coral reefs in ocean waters and kidney stones in animals. They are used widely in industry for production of a number of commodity and specialty chemicals. Precipitation reactions also play a central role in many chemical analysis techniques, including spot tests used to identify metal ions and <em>gravimetric methods<\/em> for determining the composition of matter (see the last module of this chapter).<\/p>\r\n<p id=\"fs-idp140132617792992\">The extent to which a substance may be dissolved in water, or any solvent, is quantitatively expressed as its <strong>solubility<\/strong>, defined as the maximum concentration of a substance that can be achieved under specified conditions. Substances with relatively large solubilities are said to be <strong>soluble<\/strong>. A substance will <strong>precipitate<\/strong> when solution conditions are such that its concentration exceeds its solubility. Substances with relatively low solubilities are said to be <strong>insoluble<\/strong>, and these are the substances that readily precipitate from solution. More information on these important concepts is provided in the text chapter on solutions. For purposes of predicting the identities of solids formed by precipitation reactions, one may simply refer to patterns of solubility that have been observed for many ionic compounds (<a href=\"#fs-idp140132617697568\" class=\"autogenerated-content\">Table 1<\/a>).<\/p>\r\n\r\n\r\n[caption id=\"attachment_4191\" align=\"aligncenter\" width=\"1008\"]<img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM.png\" alt=\"\" width=\"1008\" height=\"353\" class=\"wp-image-4191 size-full\" \/> <strong>Table 1.<\/strong> Solubilities of Common Ionic Compounds in Water[\/caption]\r\n<p id=\"fs-idm63476864\">A vivid example of precipitation is observed when solutions of potassium iodide and lead nitrate are mixed, resulting in the formation of solid lead iodide:<\/p>\r\n\r\n<div class=\"equation\" id=\"fs-idp98445312\" style=\"text-align: center\">$latex 2\\text{KI}(aq) + \\text{Pb(NO}_3)_2(aq) \\longrightarrow \\text{PbI}_2(s) + 2\\text{KNO}_3(aq)$<\/div>\r\n<p id=\"fs-idp24544224\">This observation is consistent with the solubility guidelines: The only insoluble compound among all those involved is lead iodide, one of the exceptions to the general solubility of iodide salts.<\/p>\r\n<p id=\"fs-idp30939280\">The net ionic equation representing this reaction is:<\/p>\r\n\r\n<div class=\"equation\" id=\"fs-idp31365696\" style=\"text-align: center\">$latex \\text{Pb}^{2+}(aq) + 2\\text{I}^{-}(aq) \\longrightarrow \\text{PbI}_2(s)$<\/div>\r\n<div>\r\n<p id=\"fs-idp157312304\">Lead iodide is a bright yellow solid that was formerly used as an artist\u2019s pigment known as iodine yellow (<a href=\"#CNX_Chem_04_02_LeadIodide\" class=\"autogenerated-content\">Figure 1<\/a>). The properties of pure PbI<sub>2<\/sub> crystals make them useful for fabrication of X-ray and gamma ray detectors.<\/p>\r\n\r\n\r\n[caption id=\"attachment_1413\" align=\"aligncenter\" width=\"250\"]<a href=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2.jpg\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2-274x300.jpg\" alt=\"\" width=\"250\" height=\"274\" class=\"wp-image-1413\" \/><\/a> <strong>Figure 1.<\/strong> A precipitate of PbI2 forms when solutions containing Pb2+ and I\u2212 are mixed. (credit: Der Kreole\/Wikimedia Commons)[\/caption]\r\n\r\n<\/div>\r\nThe solubility table in <a href=\"#fs-idp55395904\" class=\"autogenerated-content\">Table 1<\/a> may be used to predict whether a precipitation reaction will occur when solutions of soluble ionic compounds are mixed together. One merely needs to identify all the ions present in the solution and then consider if possible cation\/anion pairing could result in an insoluble compound.\r\n\r\nFor example, mixing solutions of silver nitrate and sodium fluoride will yield a solution containing Ag<sup>+<\/sup>, NO<sub>3<\/sub><sup>\u2212<\/sup>, Na<sup>+<\/sup>, and F<sup>\u2212<\/sup> ions. Aside from the two ionic compounds originally present in the solutions, AgNO<sub>3<\/sub> and NaF, two additional ionic compounds may be derived from this collection of ions: NaNO<sub>3<\/sub> and AgF.\r\n\r\nThe solubility table indicate all nitrate salts are soluble but that AgF is one of the exceptions to the general solubility of fluoride salts. A precipitation reaction, therefore, is predicted to occur, as described by the following equations:\r\n<div class=\"equation\" id=\"fs-idm4746128\">\r\n<p style=\"text-align: center\">$latex \\text{NaF}(aq) + \\text{AgNO}_3(aq) \\longrightarrow \\text{AgF}(s) + \\text{NaNO}_3(aq) \\;\\text{(molecular)}$$latex \\text{Ag}^{+}(aq) + \\text{F}^{-}(aq) \\longrightarrow \\text{AgF}(s) \\;\\text{(net ionic)}$<\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox shaded\" id=\"fs-idp3608096\">\r\n<h3>Example 1<\/h3>\r\n<p id=\"fs-idm5664816\">Predict the result of mixing reasonably concentrated solutions of the following ionic compounds. If precipitation is expected, write a balanced net ionic equation for the reaction.<\/p>\r\n<p id=\"fs-idp8541200\">a) potassium sulfate and barium nitrate<\/p>\r\n<p id=\"fs-idm5793440\">b) lithium chloride and silver acetate<\/p>\r\n<p id=\"fs-idm605024\">c) lead nitrate and ammonium carbonate<\/p>\r\n&nbsp;\r\n<p id=\"fs-idp65557120\"><strong>Solution\r\n<\/strong>a) The two possible products for this combination are KNO<sub>3<\/sub> and BaSO<sub>4<\/sub>. The solubility guidelines indicate BaSO<sub>4<\/sub> is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is<\/p>\r\n\r\n<div class=\"equation\" id=\"eip-799\" style=\"text-align: center\">$latex \\text{Ba}^{2+}(aq) + {\\text{SO}_4}^{2-}(aq) \\longrightarrow \\text{BaSO}_4(s)$<\/div>\r\n<p id=\"fs-idm27273344\">b) The two possible products for this combination are LiC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub> and AgCl. The solubility guidelines indicate AgCl is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is<\/p>\r\n\r\n<div class=\"equation\" id=\"fs-idm70392576\" style=\"text-align: center\">$latex \\text{Ag}^{+}(aq) + \\text{Cl}^{-}(aq) \\longrightarrow \\text{AgCl}(s)$<\/div>\r\n<p id=\"fs-idm5437216\">c) The two possible products for this combination are PbCO<sub>3<\/sub> and NH<sub>4<\/sub>NO<sub>3<\/sub>. The solubility guidelines indicate PbCO<sub>3<\/sub> is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is<\/p>\r\n\r\n<div class=\"equation\" id=\"eip-767\" style=\"text-align: center\">$latex \\text{Pb}^{2+}(aq) + {\\text{CO}_3}^{2-}(aq) \\longrightarrow \\text{PbCO}_3(s) $<\/div>\r\n&nbsp;\r\n<p id=\"fs-idm72085968\"><em><strong>Test Yourself<\/strong><\/em>\r\nWhich solution could be used to precipitate the barium ion, Ba<sup>2+<\/sup>, in a water sample: sodium chloride, sodium hydroxide, or sodium sulfate? What is the formula for the expected precipitate?<\/p>\r\n&nbsp;\r\n\r\n<em><strong>Answers<\/strong><\/em>\r\n\r\nsodium sulfate, BaSO<sub>4<\/sub>\r\n\r\n<\/div>\r\n<\/section><section id=\"fs-idp128853312\"><\/section><section id=\"fs-idm51820592\" class=\"summary\">\r\n<h2>Key Concepts and Summary<\/h2>\r\nChemical reactions are classified according to similar patterns of behavior. \u00a0Precipitation is one type of chemical reaction which involves the formation of one or more insoluble products. \u00a0Precipitation reactions, also called double displacement reactions can be summarized with the following reaction equation:\r\n<p style=\"text-align: center\">$latex \\text{AB}(aq) + \\text{CD}(aq) \\longrightarrow \\text{AD}(s) + \\text{CB}(aq) or (s)$<\/p>\r\nThe formation of the solid is the <em>DRIVING FORCE\u00a0<\/em>of the reaction (the factor that makes the reaction go).\r\n<p id=\"fs-idp62302320\">A precipitation reaction can be predicted to occur with the help of a solubility table (Table 1). There are three ways of representing a precipitation reaction, using a molecular equation, complete ionic equation or net ionic equation, as described in section 6.1.<\/p>\r\n\r\n<\/section><section id=\"fs-idp59588640\" class=\"exercises\">\r\n<div class=\"bcc-box bcc-info\">\r\n<h3>Exercises<\/h3>\r\n<div class=\"qandaset block\" id=\"ball-ch04_s02_qs01\"><\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch04_s02_qs01_p3\" class=\"para\">1. What are the general characteristics that help you recognize double replacement reactions?<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\"><span style=\"font-size: 1em\">2. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span><\/div>\r\n<div class=\"question\">\r\n\r\na) \u00a0Zn(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0NaOH $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) \u00a0HCl +\u00a0Na<sub class=\"subscript\">2<\/sub>S $latex \\longrightarrow$ ?\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">3. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0Ca(C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0HNO<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) \u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> +\u00a0Sr(NO<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> $latex \\longrightarrow$ ?\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">4. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0KBr $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0K<sub class=\"subscript\">2<\/sub>O +\u00a0MgCO<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ ?\r\n\r\n<\/div>\r\n5<span style=\"font-size: 1em\">. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0Sn(OH)<sub class=\"subscript\">2<\/sub> +\u00a0FeBr<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) \u00a0CsNO<sub class=\"subscript\">3<\/sub> +\u00a0KCl $latex \\longrightarrow$ ?\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">6. \u00a0Use the solubility table (Table 1) to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0KBr $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0K<sub class=\"subscript\">2<\/sub>O +\u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ ?\r\n\r\n<\/div>\r\n7<span style=\"font-size: 1em\">. \u00a0Use the solubility table (Table 1) to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> +\u00a0Sr(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0(NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub> +\u00a0Ba(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> $latex \\longrightarrow$ ?\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">8. \u00a0Use the solubility rules to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0K<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub> +\u00a0SrCl<sub class=\"subscript\">2<\/sub> $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0NaOH +\u00a0MgCl<sub class=\"subscript\">2<\/sub> $latex \\longrightarrow$ ?\r\n\r\n<\/div>\r\n9<span style=\"font-size: 1em\">. \u00a0Use the solubility rules to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0KC<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub> +\u00a0Li<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0KOH +\u00a0AgNO<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ ?\r\n\r\n&nbsp;\r\n\r\n<strong>Answers<\/strong>\r\n\r\n<section class=\"exercises\">\r\n<div class=\"qandaset block\" id=\"ball-ch04_s02_qs01_ans\">\r\n\r\n1.\u00a0<span style=\"font-size: 1em\">A double replacement reaction\u00a0<\/span><span style=\"font-size: 1em\">occurs when parts of two ionic compounds are exchanged, making two new compounds. A characteristic of a double-replacement equation is that there are two compounds as reactants and two different compounds as products.<\/span>\r\n\r\n2. a)\u00a0<span style=\"font-size: 1rem\">Zn(NO<\/span><sub class=\"subscript\">3<\/sub><span style=\"font-size: 1rem\">)<\/span><sub class=\"subscript\">2<\/sub><span style=\"font-size: 1rem\"> +\u00a02 NaOH $latex \\longrightarrow$ Zn(OH)<\/span><sub class=\"subscript\">2<\/sub><span style=\"font-size: 1rem\"> +\u00a02 NaNO<\/span><sub class=\"subscript\">3<\/sub>\r\n\r\nb)\u00a02 HCl +\u00a0Na<sub class=\"subscript\">2<\/sub>S $latex \\longrightarrow$ 2 NaCl +\u00a0H<sub class=\"subscript\">2<\/sub>S\r\n\r\n3.\u00a0a) \u00a0Ca(C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> + 2 HNO<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ Ca(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> + 2 HC<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub>\r\n\r\nb) \u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> + Sr(NO<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> $latex \\longrightarrow$ 2 NaNO<sub class=\"subscript\">2<\/sub>\u00a0+\u00a0SrCO<sub class=\"subscript\">3<\/sub>\r\n\r\n4.a) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a02 KBr $latex \\longrightarrow$ PbBr<sub class=\"subscript\">2<\/sub> +\u00a02 KNO<sub class=\"subscript\">3<\/sub>\r\n\r\nb) \u00a0K<sub class=\"subscript\">2<\/sub>O +\u00a0MgCO<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ K<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> +\u00a0MgO\r\n\r\n5.\u00a0a) \u00a03 Sn(OH)<sub class=\"subscript\">2<\/sub> + 2 FeBr<sub class=\"subscript\">3<\/sub> $latex \\longrightarrow$ 3\u00a0Sn(Br)<sub class=\"subscript\">2<\/sub>\u00a0 + \u00a02\u00a0Fe(OH)<sub class=\"subscript\">3<\/sub>\r\n\r\nb) \u00a0CsNO<sub class=\"subscript\">3<\/sub> +\u00a0KCl $latex \\longrightarrow$ KNO<sub class=\"subscript\">3<\/sub> +\u00a0CsCl\r\n\r\n6.a) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub>(aq) +\u00a02 KBr(aq) $latex \\longrightarrow$ PbBr<sub class=\"subscript\">2<\/sub>(s) +\u00a02 KNO<sub class=\"subscript\">3<\/sub>(aq)\r\n\r\nb) \u00a0No reaction occurs.\r\n\r\n7. a)\u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub>(aq) + Sr(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub>(aq) $latex \\longrightarrow$ 2 NaNO<sub class=\"subscript\">3<\/sub>(aq)\u00a0+\u00a0SrCO<sub class=\"subscript\">3<\/sub>(s)\r\n\r\nb)\u00a0\u00a0(NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub>(aq) +\u00a0Ba(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub>(aq) $latex \\longrightarrow$ BaSO<sub class=\"subscript\">4<\/sub>(s) + 2\u00a0NH<sub class=\"subscript\">4<\/sub>NO<sub class=\"subscript\">3<\/sub>(aq)\r\n\r\n8.a) \u00a02 K<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub>(aq) +\u00a03 SrCl<sub class=\"subscript\">2<\/sub>(aq) $latex \\longrightarrow$ Sr<sub class=\"subscript\">3<\/sub>(PO<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>(s) +\u00a06 KCl(aq)\r\n\r\nb) \u00a02 NaOH(aq) +\u00a0MgCl<sub class=\"subscript\">2<\/sub>(aq) $latex \\longrightarrow$ 2 NaCl(aq) +\u00a0Mg(OH)<sub class=\"subscript\">2<\/sub>(s)\r\n\r\n<\/div>\r\n<\/section>\r\n<div>\r\n\r\n9.\u00a0a) No reaction occurs.\r\n\r\nb) \u00a0KOH(aq) +\u00a0AgNO<sub class=\"subscript\">3<\/sub>(aq) $latex \\longrightarrow$ AgOH(s) +\u00a0KNO<sub class=\"subscript\">3<\/sub>(aq)\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/section>\r\n<div>\r\n<h2>Glossary<\/h2>\r\n<strong>insoluble:<\/strong>\u00a0of relatively low solubility; dissolving only to a slight extent\r\n\r\n<strong>precipitate:<\/strong>\u00a0insoluble product that forms from reaction of soluble reactants\r\n\r\n<strong>precipitation reaction:\u00a0<\/strong>reaction that produces one or more insoluble products; when reactants are ionic compounds, sometimes called double displacement or metathesis\r\n\r\n<strong>salt:\u00a0<\/strong>ionic compound that can be formed by the reaction of an acid with a base that contains a cation and an anion other than hydroxide or oxide\r\n\r\n<strong>soluble:\u00a0<\/strong>of relatively high solubility; dissolving to a relatively large extent\r\n\r\n<strong>solubility:\u00a0<\/strong>the extent to which a substance may be dissolved in water, or any solvent\r\n\r\n<\/div>","rendered":"<div class=\"bcc-box bcc-highlight\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Define precipitation reactions<\/li>\n<li>Recognize and identify examples of precipitation reactions<\/li>\n<li>Predict the solubility of common inorganic compounds by using solubility rules<\/li>\n<\/ul>\n<\/div>\n<p id=\"fs-idp140132627979408\">Humans interact with one another in various and complex ways, and we classify these interactions according to common patterns of behavior. When two humans exchange information, we say they are communicating. When they exchange blows with their fists or feet, we say they are fighting. Faced with a wide range of varied interactions between chemical substances, scientists have likewise found it convenient (or even necessary) to classify chemical interactions by identifying common patterns of reactivity. The following sections of this chapter (section 6.2-6.4) will provide an introduction to three of the most prevalent types of chemical reactions: precipitation, acid-base, and oxidation-reduction.<\/p>\n<section id=\"fs-idp140132627979792\">\n<h2>Precipitation Reactions and Solubility Rules<\/h2>\n<p id=\"fs-idp140132618169728\">A <strong>precipitation reaction<\/strong> is one in which dissolved substances react to form one (or more) solid products. Many reactions of this type involve the exchange of ions between ionic compounds in aqueous solution and are sometimes referred to as <em>double displacement<\/em>, <em>double replacement<\/em>, or <em>metathesis<\/em> reactions. These reactions are common in nature and are responsible for the formation of coral reefs in ocean waters and kidney stones in animals. They are used widely in industry for production of a number of commodity and specialty chemicals. Precipitation reactions also play a central role in many chemical analysis techniques, including spot tests used to identify metal ions and <em>gravimetric methods<\/em> for determining the composition of matter (see the last module of this chapter).<\/p>\n<p id=\"fs-idp140132617792992\">The extent to which a substance may be dissolved in water, or any solvent, is quantitatively expressed as its <strong>solubility<\/strong>, defined as the maximum concentration of a substance that can be achieved under specified conditions. Substances with relatively large solubilities are said to be <strong>soluble<\/strong>. A substance will <strong>precipitate<\/strong> when solution conditions are such that its concentration exceeds its solubility. Substances with relatively low solubilities are said to be <strong>insoluble<\/strong>, and these are the substances that readily precipitate from solution. More information on these important concepts is provided in the text chapter on solutions. For purposes of predicting the identities of solids formed by precipitation reactions, one may simply refer to patterns of solubility that have been observed for many ionic compounds (<a href=\"#fs-idp140132617697568\" class=\"autogenerated-content\">Table 1<\/a>).<\/p>\n<figure id=\"attachment_4191\" aria-describedby=\"caption-attachment-4191\" style=\"width: 1008px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM.png\" alt=\"\" width=\"1008\" height=\"353\" class=\"wp-image-4191 size-full\" srcset=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM.png 1008w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM-300x105.png 300w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM-768x269.png 768w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM-65x23.png 65w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM-225x79.png 225w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Screen-Shot-2018-06-05-at-12.40.15-PM-350x123.png 350w\" sizes=\"auto, (max-width: 1008px) 100vw, 1008px\" \/><figcaption id=\"caption-attachment-4191\" class=\"wp-caption-text\"><strong>Table 1.<\/strong> Solubilities of Common Ionic Compounds in Water<\/figcaption><\/figure>\n<p id=\"fs-idm63476864\">A vivid example of precipitation is observed when solutions of potassium iodide and lead nitrate are mixed, resulting in the formation of solid lead iodide:<\/p>\n<div class=\"equation\" id=\"fs-idp98445312\" style=\"text-align: center\">[latex]2\\text{KI}(aq) + \\text{Pb(NO}_3)_2(aq) \\longrightarrow \\text{PbI}_2(s) + 2\\text{KNO}_3(aq)[\/latex]<\/div>\n<p id=\"fs-idp24544224\">This observation is consistent with the solubility guidelines: The only insoluble compound among all those involved is lead iodide, one of the exceptions to the general solubility of iodide salts.<\/p>\n<p id=\"fs-idp30939280\">The net ionic equation representing this reaction is:<\/p>\n<div class=\"equation\" id=\"fs-idp31365696\" style=\"text-align: center\">[latex]\\text{Pb}^{2+}(aq) + 2\\text{I}^{-}(aq) \\longrightarrow \\text{PbI}_2(s)[\/latex]<\/div>\n<div>\n<p id=\"fs-idp157312304\">Lead iodide is a bright yellow solid that was formerly used as an artist\u2019s pigment known as iodine yellow (<a href=\"#CNX_Chem_04_02_LeadIodide\" class=\"autogenerated-content\">Figure 1<\/a>). The properties of pure PbI<sub>2<\/sub> crystals make them useful for fabrication of X-ray and gamma ray detectors.<\/p>\n<figure id=\"attachment_1413\" aria-describedby=\"caption-attachment-1413\" style=\"width: 250px\" class=\"wp-caption aligncenter\"><a href=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2.jpg\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2-274x300.jpg\" alt=\"\" width=\"250\" height=\"274\" class=\"wp-image-1413\" srcset=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2-274x300.jpg 274w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2-65x71.jpg 65w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2-225x246.jpg 225w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2-350x383.jpg 350w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_04_02_LeadIodide-2.jpg 650w\" sizes=\"auto, (max-width: 250px) 100vw, 250px\" \/><\/a><figcaption id=\"caption-attachment-1413\" class=\"wp-caption-text\"><strong>Figure 1.<\/strong> A precipitate of PbI2 forms when solutions containing Pb2+ and I\u2212 are mixed. (credit: Der Kreole\/Wikimedia Commons)<\/figcaption><\/figure>\n<\/div>\n<p>The solubility table in <a href=\"#fs-idp55395904\" class=\"autogenerated-content\">Table 1<\/a> may be used to predict whether a precipitation reaction will occur when solutions of soluble ionic compounds are mixed together. One merely needs to identify all the ions present in the solution and then consider if possible cation\/anion pairing could result in an insoluble compound.<\/p>\n<p>For example, mixing solutions of silver nitrate and sodium fluoride will yield a solution containing Ag<sup>+<\/sup>, NO<sub>3<\/sub><sup>\u2212<\/sup>, Na<sup>+<\/sup>, and F<sup>\u2212<\/sup> ions. Aside from the two ionic compounds originally present in the solutions, AgNO<sub>3<\/sub> and NaF, two additional ionic compounds may be derived from this collection of ions: NaNO<sub>3<\/sub> and AgF.<\/p>\n<p>The solubility table indicate all nitrate salts are soluble but that AgF is one of the exceptions to the general solubility of fluoride salts. A precipitation reaction, therefore, is predicted to occur, as described by the following equations:<\/p>\n<div class=\"equation\" id=\"fs-idm4746128\">\n<p style=\"text-align: center\">[latex]\\text{NaF}(aq) + \\text{AgNO}_3(aq) \\longrightarrow \\text{AgF}(s) + \\text{NaNO}_3(aq) \\;\\text{(molecular)}[\/latex][latex]\\text{Ag}^{+}(aq) + \\text{F}^{-}(aq) \\longrightarrow \\text{AgF}(s) \\;\\text{(net ionic)}[\/latex]<\/p>\n<\/div>\n<div class=\"textbox shaded\" id=\"fs-idp3608096\">\n<h3>Example 1<\/h3>\n<p id=\"fs-idm5664816\">Predict the result of mixing reasonably concentrated solutions of the following ionic compounds. If precipitation is expected, write a balanced net ionic equation for the reaction.<\/p>\n<p id=\"fs-idp8541200\">a) potassium sulfate and barium nitrate<\/p>\n<p id=\"fs-idm5793440\">b) lithium chloride and silver acetate<\/p>\n<p id=\"fs-idm605024\">c) lead nitrate and ammonium carbonate<\/p>\n<p>&nbsp;<\/p>\n<p id=\"fs-idp65557120\"><strong>Solution<br \/>\n<\/strong>a) The two possible products for this combination are KNO<sub>3<\/sub> and BaSO<sub>4<\/sub>. The solubility guidelines indicate BaSO<sub>4<\/sub> is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is<\/p>\n<div class=\"equation\" id=\"eip-799\" style=\"text-align: center\">[latex]\\text{Ba}^{2+}(aq) + {\\text{SO}_4}^{2-}(aq) \\longrightarrow \\text{BaSO}_4(s)[\/latex]<\/div>\n<p id=\"fs-idm27273344\">b) The two possible products for this combination are LiC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub> and AgCl. The solubility guidelines indicate AgCl is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is<\/p>\n<div class=\"equation\" id=\"fs-idm70392576\" style=\"text-align: center\">[latex]\\text{Ag}^{+}(aq) + \\text{Cl}^{-}(aq) \\longrightarrow \\text{AgCl}(s)[\/latex]<\/div>\n<p id=\"fs-idm5437216\">c) The two possible products for this combination are PbCO<sub>3<\/sub> and NH<sub>4<\/sub>NO<sub>3<\/sub>. The solubility guidelines indicate PbCO<sub>3<\/sub> is insoluble, and so a precipitation reaction is expected. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is<\/p>\n<div class=\"equation\" id=\"eip-767\" style=\"text-align: center\">[latex]\\text{Pb}^{2+}(aq) + {\\text{CO}_3}^{2-}(aq) \\longrightarrow \\text{PbCO}_3(s)[\/latex]<\/div>\n<p>&nbsp;<\/p>\n<p id=\"fs-idm72085968\"><em><strong>Test Yourself<\/strong><\/em><br \/>\nWhich solution could be used to precipitate the barium ion, Ba<sup>2+<\/sup>, in a water sample: sodium chloride, sodium hydroxide, or sodium sulfate? What is the formula for the expected precipitate?<\/p>\n<p>&nbsp;<\/p>\n<p><em><strong>Answers<\/strong><\/em><\/p>\n<p>sodium sulfate, BaSO<sub>4<\/sub><\/p>\n<\/div>\n<\/section>\n<section id=\"fs-idp128853312\"><\/section>\n<section id=\"fs-idm51820592\" class=\"summary\">\n<h2>Key Concepts and Summary<\/h2>\n<p>Chemical reactions are classified according to similar patterns of behavior. \u00a0Precipitation is one type of chemical reaction which involves the formation of one or more insoluble products. \u00a0Precipitation reactions, also called double displacement reactions can be summarized with the following reaction equation:<\/p>\n<p style=\"text-align: center\">[latex]\\text{AB}(aq) + \\text{CD}(aq) \\longrightarrow \\text{AD}(s) + \\text{CB}(aq) or (s)[\/latex]<\/p>\n<p>The formation of the solid is the <em>DRIVING FORCE\u00a0<\/em>of the reaction (the factor that makes the reaction go).<\/p>\n<p id=\"fs-idp62302320\">A precipitation reaction can be predicted to occur with the help of a solubility table (Table 1). There are three ways of representing a precipitation reaction, using a molecular equation, complete ionic equation or net ionic equation, as described in section 6.1.<\/p>\n<\/section>\n<section id=\"fs-idp59588640\" class=\"exercises\">\n<div class=\"bcc-box bcc-info\">\n<h3>Exercises<\/h3>\n<div class=\"qandaset block\" id=\"ball-ch04_s02_qs01\"><\/div>\n<div class=\"question\">\n<p id=\"ball-ch04_s02_qs01_p3\" class=\"para\">1. What are the general characteristics that help you recognize double replacement reactions?<\/p>\n<\/div>\n<div class=\"question\"><span style=\"font-size: 1em\">2. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span><\/div>\n<div class=\"question\">\n<p>a) \u00a0Zn(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0NaOH [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) \u00a0HCl +\u00a0Na<sub class=\"subscript\">2<\/sub>S [latex]\\longrightarrow[\/latex] ?<\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">3. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0Ca(C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0HNO<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) \u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> +\u00a0Sr(NO<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> [latex]\\longrightarrow[\/latex] ?<\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">4. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0KBr [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0K<sub class=\"subscript\">2<\/sub>O +\u00a0MgCO<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] ?<\/p>\n<\/div>\n<p>5<span style=\"font-size: 1em\">. \u00a0Assuming that each double replacement reaction occurs, predict the products and write each balanced chemical equation.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0Sn(OH)<sub class=\"subscript\">2<\/sub> +\u00a0FeBr<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) \u00a0CsNO<sub class=\"subscript\">3<\/sub> +\u00a0KCl [latex]\\longrightarrow[\/latex] ?<\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">6. \u00a0Use the solubility table (Table 1) to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a0KBr [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0K<sub class=\"subscript\">2<\/sub>O +\u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] ?<\/p>\n<\/div>\n<p>7<span style=\"font-size: 1em\">. \u00a0Use the solubility table (Table 1) to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> +\u00a0Sr(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0(NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub> +\u00a0Ba(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> [latex]\\longrightarrow[\/latex] ?<\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">8. \u00a0Use the solubility rules to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0K<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub> +\u00a0SrCl<sub class=\"subscript\">2<\/sub> [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0NaOH +\u00a0MgCl<sub class=\"subscript\">2<\/sub> [latex]\\longrightarrow[\/latex] ?<\/p>\n<\/div>\n<p>9<span style=\"font-size: 1em\">. \u00a0Use the solubility rules to predict if each double replacement reaction will occur and, if so, write a balanced chemical equation.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0KC<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub> +\u00a0Li<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] ? \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0KOH +\u00a0AgNO<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] ?<\/p>\n<p>&nbsp;<\/p>\n<p><strong>Answers<\/strong><\/p>\n<section class=\"exercises\">\n<div class=\"qandaset block\" id=\"ball-ch04_s02_qs01_ans\">\n<p>1.\u00a0<span style=\"font-size: 1em\">A double replacement reaction\u00a0<\/span><span style=\"font-size: 1em\">occurs when parts of two ionic compounds are exchanged, making two new compounds. A characteristic of a double-replacement equation is that there are two compounds as reactants and two different compounds as products.<\/span><\/p>\n<p>2. a)\u00a0<span style=\"font-size: 1rem\">Zn(NO<\/span><sub class=\"subscript\">3<\/sub><span style=\"font-size: 1rem\">)<\/span><sub class=\"subscript\">2<\/sub><span style=\"font-size: 1rem\"> +\u00a02 NaOH [latex]\\longrightarrow[\/latex] Zn(OH)<\/span><sub class=\"subscript\">2<\/sub><span style=\"font-size: 1rem\"> +\u00a02 NaNO<\/span><sub class=\"subscript\">3<\/sub><\/p>\n<p>b)\u00a02 HCl +\u00a0Na<sub class=\"subscript\">2<\/sub>S [latex]\\longrightarrow[\/latex] 2 NaCl +\u00a0H<sub class=\"subscript\">2<\/sub>S<\/p>\n<p>3.\u00a0a) \u00a0Ca(C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> + 2 HNO<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] Ca(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> + 2 HC<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub><\/p>\n<p>b) \u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> + Sr(NO<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">2<\/sub> [latex]\\longrightarrow[\/latex] 2 NaNO<sub class=\"subscript\">2<\/sub>\u00a0+\u00a0SrCO<sub class=\"subscript\">3<\/sub><\/p>\n<p>4.a) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub> +\u00a02 KBr [latex]\\longrightarrow[\/latex] PbBr<sub class=\"subscript\">2<\/sub> +\u00a02 KNO<sub class=\"subscript\">3<\/sub><\/p>\n<p>b) \u00a0K<sub class=\"subscript\">2<\/sub>O +\u00a0MgCO<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] K<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub> +\u00a0MgO<\/p>\n<p>5.\u00a0a) \u00a03 Sn(OH)<sub class=\"subscript\">2<\/sub> + 2 FeBr<sub class=\"subscript\">3<\/sub> [latex]\\longrightarrow[\/latex] 3\u00a0Sn(Br)<sub class=\"subscript\">2<\/sub>\u00a0 + \u00a02\u00a0Fe(OH)<sub class=\"subscript\">3<\/sub><\/p>\n<p>b) \u00a0CsNO<sub class=\"subscript\">3<\/sub> +\u00a0KCl [latex]\\longrightarrow[\/latex] KNO<sub class=\"subscript\">3<\/sub> +\u00a0CsCl<\/p>\n<p>6.a) \u00a0Pb(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub>(aq) +\u00a02 KBr(aq) [latex]\\longrightarrow[\/latex] PbBr<sub class=\"subscript\">2<\/sub>(s) +\u00a02 KNO<sub class=\"subscript\">3<\/sub>(aq)<\/p>\n<p>b) \u00a0No reaction occurs.<\/p>\n<p>7. a)\u00a0Na<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub>(aq) + Sr(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub>(aq) [latex]\\longrightarrow[\/latex] 2 NaNO<sub class=\"subscript\">3<\/sub>(aq)\u00a0+\u00a0SrCO<sub class=\"subscript\">3<\/sub>(s)<\/p>\n<p>b)\u00a0\u00a0(NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub>(aq) +\u00a0Ba(NO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">2<\/sub>(aq) [latex]\\longrightarrow[\/latex] BaSO<sub class=\"subscript\">4<\/sub>(s) + 2\u00a0NH<sub class=\"subscript\">4<\/sub>NO<sub class=\"subscript\">3<\/sub>(aq)<\/p>\n<p>8.a) \u00a02 K<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub>(aq) +\u00a03 SrCl<sub class=\"subscript\">2<\/sub>(aq) [latex]\\longrightarrow[\/latex] Sr<sub class=\"subscript\">3<\/sub>(PO<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>(s) +\u00a06 KCl(aq)<\/p>\n<p>b) \u00a02 NaOH(aq) +\u00a0MgCl<sub class=\"subscript\">2<\/sub>(aq) [latex]\\longrightarrow[\/latex] 2 NaCl(aq) +\u00a0Mg(OH)<sub class=\"subscript\">2<\/sub>(s)<\/p>\n<\/div>\n<\/section>\n<div>\n<p>9.\u00a0a) No reaction occurs.<\/p>\n<p>b) \u00a0KOH(aq) +\u00a0AgNO<sub class=\"subscript\">3<\/sub>(aq) [latex]\\longrightarrow[\/latex] AgOH(s) +\u00a0KNO<sub class=\"subscript\">3<\/sub>(aq)<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/section>\n<div>\n<h2>Glossary<\/h2>\n<p><strong>insoluble:<\/strong>\u00a0of relatively low solubility; dissolving only to a slight extent<\/p>\n<p><strong>precipitate:<\/strong>\u00a0insoluble product that forms from reaction of soluble reactants<\/p>\n<p><strong>precipitation reaction:\u00a0<\/strong>reaction that produces one or more insoluble products; when reactants are ionic compounds, sometimes called double displacement or metathesis<\/p>\n<p><strong>salt:\u00a0<\/strong>ionic compound that can be formed by the reaction of an acid with a base that contains a cation and an anion other than hydroxide or oxide<\/p>\n<p><strong>soluble:\u00a0<\/strong>of relatively high solubility; dissolving to a relatively large extent<\/p>\n<p><strong>solubility:\u00a0<\/strong>the extent to which a substance may be dissolved in water, or any solvent<\/p>\n<\/div>\n","protected":false},"author":330,"menu_order":3,"template":"","meta":{"pb_show_title":"on","pb_short_title":"6.2 Precipitation Reactions","pb_subtitle":"","pb_authors":[],"pb_section_license":"cc-by-nc-sa"},"chapter-type":[],"contributor":[],"license":[54],"class_list":["post-1419","chapter","type-chapter","status-publish","hentry","license-cc-by-nc-sa"],"part":2162,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/1419","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/users\/330"}],"version-history":[{"count":25,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/1419\/revisions"}],"predecessor-version":[{"id":4184,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/1419\/revisions\/4184"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/parts\/2162"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/1419\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/media?parent=1419"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapter-type?post=1419"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/contributor?post=1419"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/license?post=1419"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}