{"id":2825,"date":"2016-08-24T19:46:26","date_gmt":"2016-08-24T19:46:26","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=2825"},"modified":"2016-08-24T22:51:20","modified_gmt":"2016-08-24T22:51:20","slug":"hydrolysis-of-salts-equations","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/hydrolysis-of-salts-equations\/","title":{"raw":"Hydrolysis of Salts: Equations","rendered":"Hydrolysis of Salts: Equations"},"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 salt hydrolysis.<\/li>\r\n \t<li>Write equations for salts that form basic solutions.<\/li>\r\n \t<li>Write equations for salts that form acidic solutions.<\/li>\r\n \t<li>Write equations for salts that form neutral solutions.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>Baking better biscuits<\/h3>\r\n<p id=\"x-ck12-OGYxNjA3OWY2NWMxOGFjODFmOTQ4NTU0YzVjZDc5OTE.-ve9\"><span class=\"x-ck12-img-inline\"><img class=\"alignright\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213401\/20140811155917678711.jpeg\" alt=\"Baking often requires the formation of carbon dioxide to make dough more puffy\" width=\"200\" \/><\/span><\/p>\r\n<p id=\"x-ck12-Njg4YTM4ZGJlNzU3ZDY2YjZlZWZjZmQ5ODViMWJmNTA.-se7\">Baking seems easy with all the boxed mixes that are\u00a0available (\u201cjust add water and stir\u201d). However, baking involves a lot of chemistry\u2014whether you're working with a box or with ingredients that you measure out.<\/p>\r\nOne important component of any biscuit\u00a0is <strong>sodium bicarbonate<\/strong> (more commonly known as baking powder). If you have a yeast-free recipe, any fluffiness in the final biscuit is usually due to carbon dioxide formed from baking powder. One popular brand of boxed mix\u00a0uses a combination\u00a0of sodium bicarbonate and sodium aluminum sulfate to produce the CO<sub>2<\/sub>. The reaction is seen below:\r\n<p id=\"x-ck12-tqc\"><img id=\"x-ck12-MTM2NzA0OTA0NzI5MA..\" class=\"x-ck12-block-math aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213403\/b2712e2aea65c0078918010cddab4c6c.png\" alt=\"3 text{NaHCO}_3+text{NaAl(SO}_4)_2 rightarrow text{Al(OH)}_3+2text{Na}_2text{SO}_4+3text{CO}_2\" width=\"445\" height=\"19\" \/><\/p>\r\n<p id=\"x-ck12-NDYwMTEzZGYzNDkzZDM3MWFiMjdjNzhjOGVmNmIwYjY.-w2t\">If all goes well, the biscuits rise, the pancakes are fluffy, and everybody is happy.<\/p>\r\n\r\n<\/div>\r\n<h2>Hydrolysis of Salts: Equations<\/h2>\r\n<p id=\"x-ck12-ZjhlZjNhNDAzMDViNzlkZTU1YTc0YTI4YjRiZTk4MmQ.-ryx\">A salt is an ionic compound that is formed when an acid and a base neutralize each other. While it may seem that salt solutions would always be neutral, they can frequently be either acidic or basic.<\/p>\r\n<p id=\"x-ck12-NDhhMTY4MGRkOGI2ZjgxZjYyODk1YjkxODI3MzlkNTI.-1cq\">Consider the salt formed when the weak acid hydrofluoric acid is neutralized by the strong base sodium hydroxide. The molecular and net ionic equations are shown below.<\/p>\r\n<p id=\"x-ck12-opm\"><img id=\"x-ck12-MTM2NzA0OTA0NzI5MQ..\" 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\/19213404\/84e54a8b425a9c97da791a949cf27c08.png\" alt=\"&amp; text{HF}(aq)+text{NaOH}(aq) rightarrow text{NaF}(aq)+text{H}_2text{O}(l) \\&amp; text{HF}(aq)+text{OH}^-(aq) rightarrow text{F}^-(aq)+text{H}_2text{O}(l)\" width=\"330\" height=\"44\" \/><\/p>\r\n<p id=\"x-ck12-OTVmYThmYzdiMzIyMTEwMWU1NzI3OWRkODQ2ZWY0NzE.-76s\">Since sodium fluoride is soluble, the sodium ion is a spectator ion in the neutralization reaction. The fluoride ion is capable of reacting, to a small extent, with water, accepting a proton.<\/p>\r\n<p id=\"x-ck12-sfu\"><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\/19213406\/c65fd3e30e6550028e01c8d42203a384.png\" alt=\"text{F}^-(aq)+text{H}_2text{O}(l) rightleftarrows text{HF}(aq)+text{OH}^-(aq)\" width=\"307\" height=\"18\" \/><\/p>\r\n<p id=\"x-ck12-NWI4NmI3Y2Y0YWFkYTEwZDE5ZWNlYjI4MWI3MTk2NTk.-wtf\">The fluoride ion is acting as a weak Br\u00f8nsted-Lowry base. The hydroxide ion that is produced as a result of the above reaction makes the solution slightly basic. <strong> Salt hydrolysis <\/strong> is a reaction in which one of the ions from a salt reacts with water, forming either an acidic or basic solution.<\/p>\r\n\r\n<h3>Salts That Form Basic Solutions<\/h3>\r\n<p id=\"x-ck12-Zjk5ZDBiY2ExNTA3YmE3MDE2NmI4YjcxMzczZmI2ZWY.-hbj\">When solid sodium fluoride is dissolved into water, it completely dissociates into sodium ions and fluoride ions. The sodium ions do not have any capability of hydrolyzing, but the fluoride ions hydrolyze to produce a small amount of hydrofluoric acid and hydroxide ion.<\/p>\r\n<p id=\"x-ck12-5ks\"><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\/19213406\/c65fd3e30e6550028e01c8d42203a384.png\" alt=\"text{F}^-(aq)+text{H}_2text{O}(l) rightleftarrows text{HF}(aq)+text{OH}^-(aq)\" width=\"307\" height=\"18\" \/><\/p>\r\n<p id=\"x-ck12-ODYwNmQxMTc0ZDk2MjRiMmU1ZTgxNDQ5MjFjN2FmNjg.-t3s\">Salts that are derived from the neutralization of a weak acid (HF) by a strong base (NaOH) will always produce salt solutions that are basic.<\/p>\r\n\r\n<h3>Salts That Form Acidic Solutions<\/h3>\r\n<p id=\"x-ck12-YzEyZTc3NWM2NWZhYzI2YzVlNmVlZjI4MGY2NTk3ZTc.-6sp\">Ammonium chloride (NH <sub> 4 <\/sub> Cl) is a salt that is formed when the strong acid HCl is neutralized by the weak base NH <sub> 3 <\/sub> . Ammonium chloride is soluble in water. The chloride ion produced is incapable of hydrolyzing because it is the conjugate base of the strong acid HCl. In other words, the Cl <sup> \u2212 <\/sup> ion cannot accept a proton from water to form HCl and OH <sup> \u2212 <\/sup> , as the fluoride ion did in the previous section. However, the ammonium ion is capable of reacting slightly with water, donating a proton and so acting as an acid.<\/p>\r\n<p id=\"x-ck12-j7k\"><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\/19213407\/1743ae28a10d891d2fdfa56eba5bc031.png\" alt=\"text{NH}^+_4(aq)+text{H}_2text{O}(l) rightleftarrows text{H}_3text{O}^+(aq)+text{NH}_3(aq)\" width=\"339\" height=\"21\" \/><\/p>\r\n\r\n<h3>Salts That Form Neutral Solutions<\/h3>\r\n<p id=\"x-ck12-NGFjZDJhZDEwMWEzMjE1MWZiODU3YTdkM2UyMzNiNjQ.-7pk\">A salt that is derived from the reaction of a strong acid with a strong base forms a solution that has a pH of 7. An example is sodium chloride, formed from the neutralization of HCl by NaOH. A solution of NaCl in water has no acidic or basic properties, since neither ion is capable of hydrolyzing. Other salts that form neutral solutions include potassium nitrate (KNO <sub> 3 <\/sub> ) and lithium bromide (LiBr). The <strong>Table<\/strong> below summarizes how to determine the acidity or basicity of a salt solution.<\/p>\r\n\r\n<table id=\"x-ck12-OWJkNjliNTU4ZjljZmQzNWY3YjBhMzUxMzM3MmZlMTA.-ifo\" class=\"x-ck12-nofloat\" border=\"1\">\r\n<tbody>\r\n<tr>\r\n<td><strong> Salt formed from: <\/strong><\/td>\r\n<td><strong> Salt Solution <\/strong><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Strong acid + Strong base<\/td>\r\n<td>Neutral<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Strong acid + Weak base<\/td>\r\n<td>Acidic<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Weak acid + Strong base<\/td>\r\n<td>Basic<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"x-ck12-ZDdkMzk1NTdhOWI3MGZiMzMwMTJkYWJmZGFhYjMzMzg.-ty1\">Salts formed from the reaction of a weak acid and a weak base are more difficult to analyze because of competing hydrolysis reactions between the cation and the anion. These salts will not be considered in this concept.<\/p>\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-M2YxNTExODhhNTYwNTc1OTIxNTBiMmM2OTE0N2E4NmE.-yl4\">\r\n \t<li>Salt hydrolysis is defined.<\/li>\r\n \t<li>Salt hydrolysis reactions resulting in acidic, basic, or neutral solutions are described.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Practice<\/h3>\r\n<p id=\"x-ck12-OTZiMTY0ODUxMzY3M2MwMWYwYzJhYzA0MWZmNmY1M2U.-73o\"><a href=\"http:\/\/chemwiki.ucdavis.edu\/Physical_Chemistry\/Physical_Properties_of_Matter\/Solubilty\/Hydrolysis%3A_With_Respect_to_Acids,_Bases,_and_Salt_Solutions\" target=\"_blank\">Do problems 1, 2, 3, and 5 at\u00a0ChemWiki.<\/a><\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-YTMzYjhiMjU4MDk0YmYyN2E1NjZjZDE2YjgwODIyMDk.-hqz\">\r\n \t<li>How does F <sup> \u2212 <\/sup> produce a basic solution?<\/li>\r\n \t<li>How does the ammonium ion produce an acidic solution?<\/li>\r\n \t<li>Why does dissolved NaCl produce a neutral solution?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<h2 class=\"x-ck12-data-problem-set\">Glossary<\/h2>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-YTY3OGFhMjg4YzRiMGVlNmMxODY2OGY1NjU0OGE1Mjc.-div\">\r\n \t<li><strong> salt hydrolysis: <\/strong> A reaction in which one of the ions from a salt reacts with water, forming either an acidic or basic solution.<\/li>\r\n<\/ul>\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 salt hydrolysis.<\/li>\n<li>Write equations for salts that form basic solutions.<\/li>\n<li>Write equations for salts that form acidic solutions.<\/li>\n<li>Write equations for salts that form neutral solutions.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3>Baking better biscuits<\/h3>\n<p id=\"x-ck12-OGYxNjA3OWY2NWMxOGFjODFmOTQ4NTU0YzVjZDc5OTE.-ve9\"><span class=\"x-ck12-img-inline\"><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\/19213401\/20140811155917678711.jpeg\" alt=\"Baking often requires the formation of carbon dioxide to make dough more puffy\" width=\"200\" \/><\/span><\/p>\n<p id=\"x-ck12-Njg4YTM4ZGJlNzU3ZDY2YjZlZWZjZmQ5ODViMWJmNTA.-se7\">Baking seems easy with all the boxed mixes that are\u00a0available (\u201cjust add water and stir\u201d). However, baking involves a lot of chemistry\u2014whether you&#8217;re working with a box or with ingredients that you measure out.<\/p>\n<p>One important component of any biscuit\u00a0is <strong>sodium bicarbonate<\/strong> (more commonly known as baking powder). If you have a yeast-free recipe, any fluffiness in the final biscuit is usually due to carbon dioxide formed from baking powder. One popular brand of boxed mix\u00a0uses a combination\u00a0of sodium bicarbonate and sodium aluminum sulfate to produce the CO<sub>2<\/sub>. The reaction is seen below:<\/p>\n<p id=\"x-ck12-tqc\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-MTM2NzA0OTA0NzI5MA..\" class=\"x-ck12-block-math aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213403\/b2712e2aea65c0078918010cddab4c6c.png\" alt=\"3 text{NaHCO}_3+text{NaAl(SO}_4)_2 rightarrow text{Al(OH)}_3+2text{Na}_2text{SO}_4+3text{CO}_2\" width=\"445\" height=\"19\" \/><\/p>\n<p id=\"x-ck12-NDYwMTEzZGYzNDkzZDM3MWFiMjdjNzhjOGVmNmIwYjY.-w2t\">If all goes well, the biscuits rise, the pancakes are fluffy, and everybody is happy.<\/p>\n<\/div>\n<h2>Hydrolysis of Salts: Equations<\/h2>\n<p id=\"x-ck12-ZjhlZjNhNDAzMDViNzlkZTU1YTc0YTI4YjRiZTk4MmQ.-ryx\">A salt is an ionic compound that is formed when an acid and a base neutralize each other. While it may seem that salt solutions would always be neutral, they can frequently be either acidic or basic.<\/p>\n<p id=\"x-ck12-NDhhMTY4MGRkOGI2ZjgxZjYyODk1YjkxODI3MzlkNTI.-1cq\">Consider the salt formed when the weak acid hydrofluoric acid is neutralized by the strong base sodium hydroxide. The molecular and net ionic equations are shown below.<\/p>\n<p id=\"x-ck12-opm\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-MTM2NzA0OTA0NzI5MQ..\" 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\/19213404\/84e54a8b425a9c97da791a949cf27c08.png\" alt=\"&amp; text{HF}(aq)+text{NaOH}(aq) rightarrow text{NaF}(aq)+text{H}_2text{O}(l) \\&amp; text{HF}(aq)+text{OH}^-(aq) rightarrow text{F}^-(aq)+text{H}_2text{O}(l)\" width=\"330\" height=\"44\" \/><\/p>\n<p id=\"x-ck12-OTVmYThmYzdiMzIyMTEwMWU1NzI3OWRkODQ2ZWY0NzE.-76s\">Since sodium fluoride is soluble, the sodium ion is a spectator ion in the neutralization reaction. The fluoride ion is capable of reacting, to a small extent, with water, accepting a proton.<\/p>\n<p id=\"x-ck12-sfu\"><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\/19213406\/c65fd3e30e6550028e01c8d42203a384.png\" alt=\"text{F}^-(aq)+text{H}_2text{O}(l) rightleftarrows text{HF}(aq)+text{OH}^-(aq)\" width=\"307\" height=\"18\" \/><\/p>\n<p id=\"x-ck12-NWI4NmI3Y2Y0YWFkYTEwZDE5ZWNlYjI4MWI3MTk2NTk.-wtf\">The fluoride ion is acting as a weak Br\u00f8nsted-Lowry base. The hydroxide ion that is produced as a result of the above reaction makes the solution slightly basic. <strong> Salt hydrolysis <\/strong> is a reaction in which one of the ions from a salt reacts with water, forming either an acidic or basic solution.<\/p>\n<h3>Salts That Form Basic Solutions<\/h3>\n<p id=\"x-ck12-Zjk5ZDBiY2ExNTA3YmE3MDE2NmI4YjcxMzczZmI2ZWY.-hbj\">When solid sodium fluoride is dissolved into water, it completely dissociates into sodium ions and fluoride ions. The sodium ions do not have any capability of hydrolyzing, but the fluoride ions hydrolyze to produce a small amount of hydrofluoric acid and hydroxide ion.<\/p>\n<p id=\"x-ck12-5ks\"><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\/19213406\/c65fd3e30e6550028e01c8d42203a384.png\" alt=\"text{F}^-(aq)+text{H}_2text{O}(l) rightleftarrows text{HF}(aq)+text{OH}^-(aq)\" width=\"307\" height=\"18\" \/><\/p>\n<p id=\"x-ck12-ODYwNmQxMTc0ZDk2MjRiMmU1ZTgxNDQ5MjFjN2FmNjg.-t3s\">Salts that are derived from the neutralization of a weak acid (HF) by a strong base (NaOH) will always produce salt solutions that are basic.<\/p>\n<h3>Salts That Form Acidic Solutions<\/h3>\n<p id=\"x-ck12-YzEyZTc3NWM2NWZhYzI2YzVlNmVlZjI4MGY2NTk3ZTc.-6sp\">Ammonium chloride (NH <sub> 4 <\/sub> Cl) is a salt that is formed when the strong acid HCl is neutralized by the weak base NH <sub> 3 <\/sub> . Ammonium chloride is soluble in water. The chloride ion produced is incapable of hydrolyzing because it is the conjugate base of the strong acid HCl. In other words, the Cl <sup> \u2212 <\/sup> ion cannot accept a proton from water to form HCl and OH <sup> \u2212 <\/sup> , as the fluoride ion did in the previous section. However, the ammonium ion is capable of reacting slightly with water, donating a proton and so acting as an acid.<\/p>\n<p id=\"x-ck12-j7k\"><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\/19213407\/1743ae28a10d891d2fdfa56eba5bc031.png\" alt=\"text{NH}^+_4(aq)+text{H}_2text{O}(l) rightleftarrows text{H}_3text{O}^+(aq)+text{NH}_3(aq)\" width=\"339\" height=\"21\" \/><\/p>\n<h3>Salts That Form Neutral Solutions<\/h3>\n<p id=\"x-ck12-NGFjZDJhZDEwMWEzMjE1MWZiODU3YTdkM2UyMzNiNjQ.-7pk\">A salt that is derived from the reaction of a strong acid with a strong base forms a solution that has a pH of 7. An example is sodium chloride, formed from the neutralization of HCl by NaOH. A solution of NaCl in water has no acidic or basic properties, since neither ion is capable of hydrolyzing. Other salts that form neutral solutions include potassium nitrate (KNO <sub> 3 <\/sub> ) and lithium bromide (LiBr). The <strong>Table<\/strong> below summarizes how to determine the acidity or basicity of a salt solution.<\/p>\n<table id=\"x-ck12-OWJkNjliNTU4ZjljZmQzNWY3YjBhMzUxMzM3MmZlMTA.-ifo\" class=\"x-ck12-nofloat\">\n<tbody>\n<tr>\n<td><strong> Salt formed from: <\/strong><\/td>\n<td><strong> Salt Solution <\/strong><\/td>\n<\/tr>\n<tr>\n<td>Strong acid + Strong base<\/td>\n<td>Neutral<\/td>\n<\/tr>\n<tr>\n<td>Strong acid + Weak base<\/td>\n<td>Acidic<\/td>\n<\/tr>\n<tr>\n<td>Weak acid + Strong base<\/td>\n<td>Basic<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"x-ck12-ZDdkMzk1NTdhOWI3MGZiMzMwMTJkYWJmZGFhYjMzMzg.-ty1\">Salts formed from the reaction of a weak acid and a weak base are more difficult to analyze because of competing hydrolysis reactions between the cation and the anion. These salts will not be considered in this concept.<\/p>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-M2YxNTExODhhNTYwNTc1OTIxNTBiMmM2OTE0N2E4NmE.-yl4\">\n<li>Salt hydrolysis is defined.<\/li>\n<li>Salt hydrolysis reactions resulting in acidic, basic, or neutral solutions are described.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-OTZiMTY0ODUxMzY3M2MwMWYwYzJhYzA0MWZmNmY1M2U.-73o\"><a href=\"http:\/\/chemwiki.ucdavis.edu\/Physical_Chemistry\/Physical_Properties_of_Matter\/Solubilty\/Hydrolysis%3A_With_Respect_to_Acids,_Bases,_and_Salt_Solutions\" target=\"_blank\">Do problems 1, 2, 3, and 5 at\u00a0ChemWiki.<\/a><\/p>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-YTMzYjhiMjU4MDk0YmYyN2E1NjZjZDE2YjgwODIyMDk.-hqz\">\n<li>How does F <sup> \u2212 <\/sup> produce a basic solution?<\/li>\n<li>How does the ammonium ion produce an acidic solution?<\/li>\n<li>Why does dissolved NaCl produce a neutral solution?<\/li>\n<\/ol>\n<\/div>\n<h2 class=\"x-ck12-data-problem-set\">Glossary<\/h2>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-YTY3OGFhMjg4YzRiMGVlNmMxODY2OGY1NjU0OGE1Mjc.-div\">\n<li><strong> salt hydrolysis: <\/strong> A reaction in which one of the ions from a salt reacts with water, forming either an acidic or basic solution.<\/li>\n<\/ul>\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-2825\">\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 class=\"license-attribution-dropdown-subheading\">Public domain content<\/div><ul class=\"citation-list\"><li>Runny hunny. <strong>Authored by<\/strong>: Scott Bauer. <strong>Provided by<\/strong>: USDA, ARS. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Runny_hunny.jpg\">https:\/\/commons.wikimedia.org\/wiki\/File:Runny_hunny.jpg<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/about\/pdm\">Public Domain: No Known Copyright<\/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":15,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Chemistry Concepts Intermediate\",\"author\":\"Calbreath, Baxter, et al.\",\"organization\":\"CK12.org\",\"url\":\"http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/\",\"project\":\"\",\"license\":\"cc-by-nc\",\"license_terms\":\"\"},{\"type\":\"pd\",\"description\":\"Runny hunny\",\"author\":\"Scott Bauer\",\"organization\":\"USDA, 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