{"id":2748,"date":"2016-08-24T18:16:39","date_gmt":"2016-08-24T18:16:39","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=2748"},"modified":"2017-09-06T19:00:39","modified_gmt":"2017-09-06T19:00:39","slug":"solubility-product-constant-ksp","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/solubility-product-constant-ksp\/","title":{"raw":"Solubility Product Constant (Ksp)","rendered":"Solubility Product Constant (Ksp)"},"content":{"raw":"<div class=\"x-ck12-data-objectives\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\n<ul>\r\n \t<li>Define solubility product constant.<\/li>\r\n \t<li>Perform calculations involving solubility product constants.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3><strong style=\"line-height: 1.5;\">No more weighing<\/strong><\/h3>\r\n<p id=\"x-ck12-NmQxNDk4NGUwMWI0MzI2NjJlYTIyN2M1ZjM0M2Y1MzI.-edu\"><img class=\"alignright\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213024\/20140811155758396743.jpeg\" alt=\"Gravimetric analysis used to be used to determine the amount of ion present in a solution\" width=\"200\" \/>At one time, a major analytical technique was gravimetric analysis. An ion would be precipitated out of solution, purified, and weighed to determine the amount of that ion in the original material. As an example, measurement of Ca <sup> 2+ <\/sup> involved dissolving the sample in water, precipitating the calcium as calcium oxalate, purifying the precipitate, drying it, and weighing the final product. Although this approach can be very accurate (atomic weights for many elements were determined this way), the process is slow, tedious, and prone to a number of errors in technique. Newer methods are now available that measure minute amounts of calcium ions in solution without the long, involved gravimetric approach.<\/p>\r\n\r\n<\/div>\r\n<h2>Solubility Product Constant<\/h2>\r\n<p id=\"x-ck12-NGMyNjU5MDRkZDg2MmM3YzNiNWNkOGUxMjE2YmRiOGU.-zdm\">Ionic compounds have widely differing solubilities. Sodium chloride has a solubility of about 360 g per liter of water at 25\u00b0C. Salts of alkali metals tend to be quite soluble. On the other end of the spectrum, the solubility of zinc hydroxide is only 4.2\u00a0\u00d7\u00a010 <sup> -4 <\/sup> \u00a0g\/L of water at the same temperature. Many ionic compounds containing hydroxide are relatively insoluble.<\/p>\r\n<p id=\"x-ck12-M2UzNjZiMGE5MWYzY2I3N2I1Yjc2MmQ3NmNkZjEyMjU.-mop\">Most ionic compounds that are considered to be insoluble will still dissolve to a small extent in water. These \u201cmostly insoluble\u201d compounds are considered to be strong electrolytes because whatever portion of the compound that dissolved also dissociates. As an example, silver chloride dissociates to a small extent into silver ions and chloride ions upon being added to water.<\/p>\r\n<p id=\"x-ck12-knz\"><img id=\"x-ck12-MTM2Nzk0OTA2MzU4Ng..\" class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213025\/b27955a80662145f0f100ed79b3cf1d6.png\" alt=\"text{AgCl}(s) rightleftarrows text{Ag}^+(aq)+text{Cl}^-(aq)\" width=\"238\" height=\"21\" \/><\/p>\r\n<p id=\"x-ck12-MGQzNzAxM2NjZjUxMGNmMjQ5ZmYzMjZkMWQyMzc5NmQ.-dkt\">The process is written as an equilibrium because the dissociation occurs only to a small extent. Therefore, an equilibrium expression can be written for the process. Keep in mind that the solid silver chloride does not have a variable concentration and so is not included in the expression.<\/p>\r\n<p id=\"x-ck12-3tz\"><img class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213026\/07159934c562b92cb9d4db2e0612b31e.png\" alt=\"K_{sp}=[text{Ag}^+][text{Cl}^-]\" width=\"132\" height=\"23\" \/><\/p>\r\n<p id=\"x-ck12-YWZlZjA4NmMxNzQyMDlkNGI2MWUyYjkyNmFlMDRkMzA.-uob\">This equilibrium constant is called the <strong> solubility product constant [latex]\\left(K_{sp}\\right)[\/latex]<\/strong>\u00a0and is equal to the mathematical product of the ions each raised to the power of the coefficient of the ion in the dissociation equation.<\/p>\r\n<p id=\"x-ck12-NjQwNzhkZWViNTRjNmY3YWQ3MGIzMjYyZTkxMzdmMDM.-gwh\">The stoichiometry of the formula of the ionic compound dictates the form of the \u00a0[latex]K_{sp}[\/latex]\u00a0expression. For example the formula of calcium phosphate is Ca <sub> 3 <\/sub> (PO <sub> 4 <\/sub> ) <sub> 2 <\/sub> . The dissociation equation and\u00a0 [latex]K_{sp}[\/latex]\u00a0expression are shown below:<\/p>\r\n<p id=\"x-ck12-3gx\"><img class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213027\/66dee2776086f9a3aa068c44d536608c.png\" alt=\"text{Ca}_3(text{PO}_4)_2(s) rightleftarrows 3text{Ca}^{2+}(aq)+2text{PO}^{3-}_4(aq) quad K_{sp}=[text{Ca}^{2+}]^3[text{PO}^{3-}_4]^2\" width=\"507\" height=\"23\" \/><\/p>\r\n<p id=\"x-ck12-NDY1NDUyMDAxYzI0Yjc5NDFkZDJmOTAyYjM3MDc2ZmE.-jt2\">The <strong> Table <\/strong> below lists solubility product constants for some common nearly insoluble ionic compounds.<\/p>\r\n\r\n<table id=\"x-ck12-ZWFhYzllOGJkMWMzYWRhY2YwODU0NWEwNjY3NmFiOWU.-aqx\" class=\"x-ck12-nofloat\" border=\"1\"><caption>Solubility Product Constants (25\u00b0C)<\/caption>\r\n<tbody>\r\n<tr>\r\n<td><strong> Compound <\/strong><\/td>\r\n<td>[latex]K_{sp}[\/latex]<\/td>\r\n<td>\u00a0 <strong> Compound <\/strong><\/td>\r\n<td>[latex]K_{sp}[\/latex]<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>AgBr<\/td>\r\n<td>5.0 \u00d7 10 <sup> -13 <\/sup><\/td>\r\n<td>CuS<\/td>\r\n<td>8.0 \u00d7 10 <sup> -37 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>AgCl<\/td>\r\n<td>1.8 \u00d7 10 <sup> -10 <\/sup><\/td>\r\n<td>Fe(OH) <sub> 2 <\/sub><\/td>\r\n<td>7.9 \u00d7 10 <sup> -16 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Al(OH) <sub> 3 <\/sub><\/td>\r\n<td>3.0 \u00d7 10 <sup> -34 <\/sup><\/td>\r\n<td>Mg(OH) <sub> 2 <\/sub><\/td>\r\n<td>7.1 \u00d7 10 <sup> -12 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>BaCO <sub> 3 <\/sub><\/td>\r\n<td>5.0 \u00d7 10 <sup> -9 <\/sup><\/td>\r\n<td>PbCl <sub> 2 <\/sub><\/td>\r\n<td>1.7 \u00d7 10 <sup> -5 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>BaSO <sub> 4 <\/sub><\/td>\r\n<td>1.1 \u00d7 10 <sup> -10 <\/sup><\/td>\r\n<td>PbCO <sub> 3 <\/sub><\/td>\r\n<td>7.4 \u00d7 10 <sup> -14 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CaCO <sub> 3 <\/sub><\/td>\r\n<td>4.5 \u00d7 10 <sup> -9 <\/sup><\/td>\r\n<td>PbI <sub> 2 <\/sub><\/td>\r\n<td>7.1 \u00d7 10 <sup> -9 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Ca(OH) <sub> 2 <\/sub><\/td>\r\n<td>6.5 \u00d7 10 <sup> -6 <\/sup><\/td>\r\n<td>PbSO <sub> 4 <\/sub><\/td>\r\n<td>6.3 \u00d7 10 <sup> -7 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Ca <sub> 3 <\/sub> (PO <sub> 4 <\/sub> ) <sub> 2 <\/sub><\/td>\r\n<td>1.2 \u00d7 10 <sup> -26 <\/sup><\/td>\r\n<td>Zn(OH) <sub> 2 <\/sub><\/td>\r\n<td>3.0 \u00d7 10 <sup> -16 <\/sup><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CaSO <sub> 4 <\/sub><\/td>\r\n<td>2.4 \u00d7 10 <sup> -5 <\/sup><\/td>\r\n<td>ZnS<\/td>\r\n<td>3.0 \u00d7 10 <sup> -23 <\/sup><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-YmIzNzJhNjE3OGU4MjA5OTc2NGYxZTFjNjcyM2ZkZTI.-jff\">\r\n \t<li>The solubility product constant is defined.<\/li>\r\n \t<li>Calculations using solubility product constants are illustrated.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-ZjZmM2IwMWMyODg5N2U3YmUxNDE0NDA3ZDJmY2JhY2U.-yaw\">\r\n \t<li>What does the<i>\u00a0<\/i>[latex]K_{sp}[\/latex]\u00a0tell us?<\/li>\r\n \t<li>Which of the lead salts listed in the table above is the most soluble?<\/li>\r\n \t<li>What is the exponent for an ion in the equation?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<h3 class=\"x-ck12-data-problem-set\">Glossary<\/h3>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-MWYxYmFlYzg2YWZmMDcwMmM3NGNmZGNmYWUxYjNlYWE.-xti\">\r\n \t<li><strong> solubility product constant, [latex]\\left(K_{sp}\\right)[\/latex]: <\/strong> The mathematical product of the ions each raised to the power of the coefficient of the ion in the dissociation equation.<\/li>\r\n<\/ul>\r\n[reveal-answer q=\"836080\"]Show References[\/reveal-answer]\r\n[hidden-answer a=\"836080\"]\r\n<h2>References<\/h2>\r\n<ol>\r\n \t<li>User:Ebultoof\/Wikipedia. <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Analytical_Balance.JPG\">http:\/\/commons.wikimedia.org\/wiki\/File:Analytical_Balance.JPG <\/a>.<\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n\r\n<\/div>","rendered":"<div class=\"x-ck12-data-objectives\">\n<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<ul>\n<li>Define solubility product constant.<\/li>\n<li>Perform calculations involving solubility product constants.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3><strong style=\"line-height: 1.5;\">No more weighing<\/strong><\/h3>\n<p id=\"x-ck12-NmQxNDk4NGUwMWI0MzI2NjJlYTIyN2M1ZjM0M2Y1MzI.-edu\"><img decoding=\"async\" class=\"alignright\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213024\/20140811155758396743.jpeg\" alt=\"Gravimetric analysis used to be used to determine the amount of ion present in a solution\" width=\"200\" \/>At one time, a major analytical technique was gravimetric analysis. An ion would be precipitated out of solution, purified, and weighed to determine the amount of that ion in the original material. As an example, measurement of Ca <sup> 2+ <\/sup> involved dissolving the sample in water, precipitating the calcium as calcium oxalate, purifying the precipitate, drying it, and weighing the final product. Although this approach can be very accurate (atomic weights for many elements were determined this way), the process is slow, tedious, and prone to a number of errors in technique. Newer methods are now available that measure minute amounts of calcium ions in solution without the long, involved gravimetric approach.<\/p>\n<\/div>\n<h2>Solubility Product Constant<\/h2>\n<p id=\"x-ck12-NGMyNjU5MDRkZDg2MmM3YzNiNWNkOGUxMjE2YmRiOGU.-zdm\">Ionic compounds have widely differing solubilities. Sodium chloride has a solubility of about 360 g per liter of water at 25\u00b0C. Salts of alkali metals tend to be quite soluble. On the other end of the spectrum, the solubility of zinc hydroxide is only 4.2\u00a0\u00d7\u00a010 <sup> -4 <\/sup> \u00a0g\/L of water at the same temperature. Many ionic compounds containing hydroxide are relatively insoluble.<\/p>\n<p id=\"x-ck12-M2UzNjZiMGE5MWYzY2I3N2I1Yjc2MmQ3NmNkZjEyMjU.-mop\">Most ionic compounds that are considered to be insoluble will still dissolve to a small extent in water. These \u201cmostly insoluble\u201d compounds are considered to be strong electrolytes because whatever portion of the compound that dissolved also dissociates. As an example, silver chloride dissociates to a small extent into silver ions and chloride ions upon being added to water.<\/p>\n<p id=\"x-ck12-knz\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-MTM2Nzk0OTA2MzU4Ng..\" class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213025\/b27955a80662145f0f100ed79b3cf1d6.png\" alt=\"text{AgCl}(s) rightleftarrows text{Ag}^+(aq)+text{Cl}^-(aq)\" width=\"238\" height=\"21\" \/><\/p>\n<p id=\"x-ck12-MGQzNzAxM2NjZjUxMGNmMjQ5ZmYzMjZkMWQyMzc5NmQ.-dkt\">The process is written as an equilibrium because the dissociation occurs only to a small extent. Therefore, an equilibrium expression can be written for the process. Keep in mind that the solid silver chloride does not have a variable concentration and so is not included in the expression.<\/p>\n<p id=\"x-ck12-3tz\"><img loading=\"lazy\" decoding=\"async\" class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213026\/07159934c562b92cb9d4db2e0612b31e.png\" alt=\"K_{sp}=[text{Ag}^+][text{Cl}^-]\" width=\"132\" height=\"23\" \/><\/p>\n<p id=\"x-ck12-YWZlZjA4NmMxNzQyMDlkNGI2MWUyYjkyNmFlMDRkMzA.-uob\">This equilibrium constant is called the <strong> solubility product constant [latex]\\left(K_{sp}\\right)[\/latex]<\/strong>\u00a0and is equal to the mathematical product of the ions each raised to the power of the coefficient of the ion in the dissociation equation.<\/p>\n<p id=\"x-ck12-NjQwNzhkZWViNTRjNmY3YWQ3MGIzMjYyZTkxMzdmMDM.-gwh\">The stoichiometry of the formula of the ionic compound dictates the form of the \u00a0[latex]K_{sp}[\/latex]\u00a0expression. For example the formula of calcium phosphate is Ca <sub> 3 <\/sub> (PO <sub> 4 <\/sub> ) <sub> 2 <\/sub> . The dissociation equation and\u00a0 [latex]K_{sp}[\/latex]\u00a0expression are shown below:<\/p>\n<p id=\"x-ck12-3gx\"><img loading=\"lazy\" decoding=\"async\" class=\"x-ck12-block-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213027\/66dee2776086f9a3aa068c44d536608c.png\" alt=\"text{Ca}_3(text{PO}_4)_2(s) rightleftarrows 3text{Ca}^{2+}(aq)+2text{PO}^{3-}_4(aq) quad K_{sp}=[text{Ca}^{2+}]^3[text{PO}^{3-}_4]^2\" width=\"507\" height=\"23\" \/><\/p>\n<p id=\"x-ck12-NDY1NDUyMDAxYzI0Yjc5NDFkZDJmOTAyYjM3MDc2ZmE.-jt2\">The <strong> Table <\/strong> below lists solubility product constants for some common nearly insoluble ionic compounds.<\/p>\n<table id=\"x-ck12-ZWFhYzllOGJkMWMzYWRhY2YwODU0NWEwNjY3NmFiOWU.-aqx\" class=\"x-ck12-nofloat\">\n<caption>Solubility Product Constants (25\u00b0C)<\/caption>\n<tbody>\n<tr>\n<td><strong> Compound <\/strong><\/td>\n<td>[latex]K_{sp}[\/latex]<\/td>\n<td>\u00a0 <strong> Compound <\/strong><\/td>\n<td>[latex]K_{sp}[\/latex]<\/td>\n<\/tr>\n<tr>\n<td>AgBr<\/td>\n<td>5.0 \u00d7 10 <sup> -13 <\/sup><\/td>\n<td>CuS<\/td>\n<td>8.0 \u00d7 10 <sup> -37 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>AgCl<\/td>\n<td>1.8 \u00d7 10 <sup> -10 <\/sup><\/td>\n<td>Fe(OH) <sub> 2 <\/sub><\/td>\n<td>7.9 \u00d7 10 <sup> -16 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>Al(OH) <sub> 3 <\/sub><\/td>\n<td>3.0 \u00d7 10 <sup> -34 <\/sup><\/td>\n<td>Mg(OH) <sub> 2 <\/sub><\/td>\n<td>7.1 \u00d7 10 <sup> -12 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>BaCO <sub> 3 <\/sub><\/td>\n<td>5.0 \u00d7 10 <sup> -9 <\/sup><\/td>\n<td>PbCl <sub> 2 <\/sub><\/td>\n<td>1.7 \u00d7 10 <sup> -5 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>BaSO <sub> 4 <\/sub><\/td>\n<td>1.1 \u00d7 10 <sup> -10 <\/sup><\/td>\n<td>PbCO <sub> 3 <\/sub><\/td>\n<td>7.4 \u00d7 10 <sup> -14 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>CaCO <sub> 3 <\/sub><\/td>\n<td>4.5 \u00d7 10 <sup> -9 <\/sup><\/td>\n<td>PbI <sub> 2 <\/sub><\/td>\n<td>7.1 \u00d7 10 <sup> -9 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>Ca(OH) <sub> 2 <\/sub><\/td>\n<td>6.5 \u00d7 10 <sup> -6 <\/sup><\/td>\n<td>PbSO <sub> 4 <\/sub><\/td>\n<td>6.3 \u00d7 10 <sup> -7 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>Ca <sub> 3 <\/sub> (PO <sub> 4 <\/sub> ) <sub> 2 <\/sub><\/td>\n<td>1.2 \u00d7 10 <sup> -26 <\/sup><\/td>\n<td>Zn(OH) <sub> 2 <\/sub><\/td>\n<td>3.0 \u00d7 10 <sup> -16 <\/sup><\/td>\n<\/tr>\n<tr>\n<td>CaSO <sub> 4 <\/sub><\/td>\n<td>2.4 \u00d7 10 <sup> -5 <\/sup><\/td>\n<td>ZnS<\/td>\n<td>3.0 \u00d7 10 <sup> -23 <\/sup><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-YmIzNzJhNjE3OGU4MjA5OTc2NGYxZTFjNjcyM2ZkZTI.-jff\">\n<li>The solubility product constant is defined.<\/li>\n<li>Calculations using solubility product constants are illustrated.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-ZjZmM2IwMWMyODg5N2U3YmUxNDE0NDA3ZDJmY2JhY2U.-yaw\">\n<li>What does the<i>\u00a0<\/i>[latex]K_{sp}[\/latex]\u00a0tell us?<\/li>\n<li>Which of the lead salts listed in the table above is the most soluble?<\/li>\n<li>What is the exponent for an ion in the equation?<\/li>\n<\/ol>\n<\/div>\n<h3 class=\"x-ck12-data-problem-set\">Glossary<\/h3>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-MWYxYmFlYzg2YWZmMDcwMmM3NGNmZGNmYWUxYjNlYWE.-xti\">\n<li><strong> solubility product constant, [latex]\\left(K_{sp}\\right)[\/latex]: <\/strong> The mathematical product of the ions each raised to the power of the coefficient of the ion in the dissociation equation.<\/li>\n<\/ul>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q836080\">Show References<\/span><\/p>\n<div id=\"q836080\" class=\"hidden-answer\" style=\"display: none\">\n<h2>References<\/h2>\n<ol>\n<li>User:Ebultoof\/Wikipedia. <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Analytical_Balance.JPG\">http:\/\/commons.wikimedia.org\/wiki\/File:Analytical_Balance.JPG <\/a>.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n\n\t\t\t <section class=\"citations-section\" role=\"contentinfo\">\n\t\t\t <h3>Candela Citations<\/h3>\n\t\t\t\t\t <div>\n\t\t\t\t\t\t <div id=\"citation-list-2748\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Shared previously<\/div><ul class=\"citation-list\"><li>Chemistry Concepts Intermediate. <strong>Authored by<\/strong>: Calbreath, Baxter, et al.. <strong>Provided by<\/strong>: CK12.org. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/\">http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc\/4.0\/\">CC BY-NC: Attribution-NonCommercial<\/a><\/em><\/li><\/ul><\/div>\n\t\t\t\t\t\t <\/div>\n\t\t\t\t\t <\/div>\n\t\t\t <\/section>","protected":false},"author":17,"menu_order":11,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Chemistry Concepts Intermediate\",\"author\":\"Calbreath, Baxter, et 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