{"id":2827,"date":"2016-08-24T19:57:20","date_gmt":"2016-08-24T19:57:20","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=2827"},"modified":"2016-08-24T22:55:50","modified_gmt":"2016-08-24T22:55:50","slug":"buffers","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/buffers\/","title":{"raw":"Buffers","rendered":"Buffers"},"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 buffer.<\/li>\r\n \t<li>Define buffer capacity.<\/li>\r\n \t<li>Describe how a buffer controls pH.<\/li>\r\n \t<li>List some common buffer systems.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3><strong>How does insulin work? <\/strong><\/h3>\r\n<p id=\"x-ck12-YTYyYzc0NWZkY2QwMDQ1OTY3Zjg4OTc2MzhlYWI1MGU.-lno\">Diabetes mellitus is a disorder of glucose metabolism in which insulin production by the pancreas is impaired. Since insulin helps glucose enter the cells, a decrease of this hormone means that glucose cannot be used in its normal fashion. When this happens, the body begins to break down fats, producing a decrease in blood pH. Chemical systems in the body can balance this pH shift for a while, but excessive acid production can create serious problems if not corrected by administering insulin to restore normal glucose use.<\/p>\r\n<img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213420\/20140811155918015775.jpeg\" alt=\"One of the effects of diabetes is a decrease in blood pH\" width=\"250\" \/>\r\n\r\n<\/div>\r\n<p id=\"x-ck12-NGY5ZjI3MjFmYzgwNmM3ZGRjMmZhYjg1Njk4NWIwNjQ.-mho\">If only 1.0 mL of 0.10 M hydrochloric acid is added to 1.0 L of pure water the pH drops drastically from 7.0 to 4.0. This is a 1000-fold increase in the acidity of the solution. For many purposes, it is desirable to have a solution which is capable of resisting such large changes in pH when relatively small amounts of acid or base are added to them. Such a solution is called a buffer. A <strong> buffer <\/strong> is a solution of a weak acid or a base and its salt. Both components must be present for the system to act as a buffer to resist changes in pH. Commercial buffer solutions, which have a wide variety of pH values, can be obtained.<\/p>\r\n<p id=\"x-ck12-NTM1ZmY3MzFmZGZhNDAyN2Y1ZjcyNzFkNDJiYzA0OTk.-azf\">Some common buffer systems are listed in the <strong> Table <\/strong> below:<\/p>\r\n\r\n<table id=\"x-ck12-MTM2NzA0MTA1Njk4NQ..\" class=\"x-ck12-nofloat\" border=\"1\"><caption>Some Common Buffers<\/caption>\r\n<tbody>\r\n<tr>\r\n<td><strong> Buffer system <\/strong><\/td>\r\n<td><strong> Buffer components <\/strong><\/td>\r\n<td><strong> pH of buffer (equal molarities of both components) <\/strong><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Acetic acid \/ acetate ion<\/td>\r\n<td>CH <sub> 3 <\/sub> COOH \/ CH <sub> 3 <\/sub> COO <sup> \u2212 <\/sup><\/td>\r\n<td>4.74<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Carbonic acid \/ hydrogen carbonate ion<\/td>\r\n<td>H <sub> 2 <\/sub> CO <sub> 3 <\/sub> \/ HCO <sub> 3 <\/sub><sup> \u2212 <\/sup><\/td>\r\n<td>6.38<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>\r\n<p id=\"x-ck12-OThhNmM3Y2IwNDAzNzJmYjZiMThlY2MwYTU4MTc1NjY.-pxl\">Dihydrogen phosphate ion \/ hydrogen phosphate ion<\/p>\r\n<\/td>\r\n<td>H <sub> 2 <\/sub> PO <sub> 4 <\/sub><sup> \u2212 <\/sup> \/ HPO <sub> 4 <\/sub><sup> 2\u2212 <\/sup><\/td>\r\n<td>7.21<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Ammonia \/ ammonium ion<\/td>\r\n<td>NH <sub> 3 <\/sub> \/ NH <sub> 4 <\/sub><sup> + <\/sup><\/td>\r\n<td>9.25<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"x-ck12-NDQ0MzY1NmY5NjE3NGI5ZDVmNWZmMGJiYzM1MmJiZGM.-k9u\">One example of a buffer is a solution made of acetic acid (the weak acid) and sodium acetate (the salt). The pH of a buffer consisting of 0.50 M CH <sub> 3 <\/sub> COOH and 0.50 M CH <sub> 3 <\/sub> COONa is 4.74. If 10.0 mL of 1.0 M HCl is added to 1.0 L of the buffer, the pH only decreases to 4.73. This ability to \u201csoak up\u201d the additional hydrogen ions from the HCl that was added is due to the reaction below.<\/p>\r\n<p id=\"x-ck12-3ls\"><img id=\"x-ck12-MTM2ODczOTAxMDEzMA..\" 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\/19213421\/3a8e0b072107314d683a68cf2d0d4fcb.png\" alt=\"text{CH}_3text{COO}^-(aq)+text{H}^+(aq) rightarrow text{CH}_3text{COOH}(aq)\" width=\"342\" height=\"21\" \/><\/p>\r\n<p id=\"x-ck12-NTMxZjQwOTJiN2I0NWIwOTBkNmExZDEyYmYzNTc2M2M.-hqh\">Since both the acetate ion and the acetic acid were already present in the buffer, the only thing that changes is the ratio of one to the other. Small changes in that ratio have only very minor effects on the pH.<\/p>\r\n<p id=\"x-ck12-MDM0OWQyYWQzMmEwY2IxYjg0ZTlmN2VhN2I3ZWU3ZDE.-oqj\">If 10.0 mL of 1.0 M NaOH were added to another 1.0 L of the same buffer, the pH would only increase to 4.76. In this case the buffer takes up the additional hydroxide ions.<\/p>\r\n<p id=\"x-ck12-qds\"><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\/19213423\/9f730348f213e9bc8640147dd4c5ba10.png\" alt=\"text{CH}_3text{COOH}(aq)+text{OH}^-(aq) rightarrow text{CH}_3text{COO}^-(aq)+text{H}_2text{O}(l)\" width=\"432\" height=\"18\" \/><\/p>\r\n<p id=\"x-ck12-ZTVkNGYzNGEyYWQxNDc5ZGNjYmVkZjIwYzFjOTc0YjU.-hvs\">Again the ratio of acetate ion to acetic acid changes slightly, this time causing a very small increase in the pH.<\/p>\r\n<p id=\"x-ck12-ZTE5MTM1NWEwNDVhNDI0MzgyYTBmM2UyNzhkODJkZWQ.-acw\">It is possible to add so much acid or base to a buffer that its ability to resist a significant change in pH is overwhelmed. The <strong> buffer capacity <\/strong> is the amount of acid or base that can be added to a buffer solution before a large change in pH occurs. The buffer capacity is exceeded when the number of moles of H <sup> + <\/sup> or OH <sup> \u2212 <\/sup> that are added to the buffer exceeds the number of moles of the buffer components.<\/p>\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-ZGE4YjRiZTg0MWIzNGNkODZhMjhiZTlkMzkwMjQzMGM.-iry\">\r\n \t<li>Buffer is defined.<\/li>\r\n \t<li>Reactions showing how buffers regulate pH 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-ZDA1NTE4MmE3ZWNhMTc1ZjZmZjlhNTc2YTQzZWI5ZTg.-fca\">Read the material at the link below and answer the following questions:<\/p>\r\n<p id=\"x-ck12-ZmFmNDM3OTA3ZTExNmQzOTlhZWZlM2EyOTljMjE4MzM.-ogj\"><a href=\"http:\/\/chemcollective.org\/activities\/tutorials\/buffers\/buffers3\"> http:\/\/chemcollective.org\/activities\/tutorials\/buffers\/buffers3 <\/a><\/p>\r\n\r\n<ol id=\"x-ck12-MGFjMDBiNzhjMzgwZjczODY3NmQxNTI2NWVjYzM1ZTE.-hrq\">\r\n \t<li>What is a weak acid?<\/li>\r\n \t<li>What does a conjugate base rarely do?<\/li>\r\n \t<li>Write the generic equation for neutralization of a base by a weak acid.<\/li>\r\n \t<li>Write the generic equation for neutralization of an acid by a weak base.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-NmJmNTVkNGY2YWE2NmZiY2RmMzBkZmU3OTg5OTg3MTI.-deq\">\r\n \t<li>What is a buffer?<\/li>\r\n \t<li>How would the acetic acid\/acetate buffer system neutralize an added base?<\/li>\r\n \t<li>If acid is added to the carbonic acid\/carbonate buffer system, how is it neutralized?<\/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-ZjQ0M2JjMjgzMTA3OWI2YTZkOTBiM2JjZTE2OTU4NTY.-gbn\">\r\n \t<li><strong> buffer: <\/strong> A solution of a weak acid or a base and its salt.<\/li>\r\n \t<li><strong> buffer capacity: <\/strong> The amount of acid or base that can be added to buffer solution before a large change in pH occurs.<\/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 buffer.<\/li>\n<li>Define buffer capacity.<\/li>\n<li>Describe how a buffer controls pH.<\/li>\n<li>List some common buffer systems.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3><strong>How does insulin work? <\/strong><\/h3>\n<p id=\"x-ck12-YTYyYzc0NWZkY2QwMDQ1OTY3Zjg4OTc2MzhlYWI1MGU.-lno\">Diabetes mellitus is a disorder of glucose metabolism in which insulin production by the pancreas is impaired. Since insulin helps glucose enter the cells, a decrease of this hormone means that glucose cannot be used in its normal fashion. When this happens, the body begins to break down fats, producing a decrease in blood pH. Chemical systems in the body can balance this pH shift for a while, but excessive acid production can create serious problems if not corrected by administering insulin to restore normal glucose use.<\/p>\n<p><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19213420\/20140811155918015775.jpeg\" alt=\"One of the effects of diabetes is a decrease in blood pH\" width=\"250\" \/><\/p>\n<\/div>\n<p id=\"x-ck12-NGY5ZjI3MjFmYzgwNmM3ZGRjMmZhYjg1Njk4NWIwNjQ.-mho\">If only 1.0 mL of 0.10 M hydrochloric acid is added to 1.0 L of pure water the pH drops drastically from 7.0 to 4.0. This is a 1000-fold increase in the acidity of the solution. For many purposes, it is desirable to have a solution which is capable of resisting such large changes in pH when relatively small amounts of acid or base are added to them. Such a solution is called a buffer. A <strong> buffer <\/strong> is a solution of a weak acid or a base and its salt. Both components must be present for the system to act as a buffer to resist changes in pH. Commercial buffer solutions, which have a wide variety of pH values, can be obtained.<\/p>\n<p id=\"x-ck12-NTM1ZmY3MzFmZGZhNDAyN2Y1ZjcyNzFkNDJiYzA0OTk.-azf\">Some common buffer systems are listed in the <strong> Table <\/strong> below:<\/p>\n<table id=\"x-ck12-MTM2NzA0MTA1Njk4NQ..\" class=\"x-ck12-nofloat\">\n<caption>Some Common Buffers<\/caption>\n<tbody>\n<tr>\n<td><strong> Buffer system <\/strong><\/td>\n<td><strong> Buffer components <\/strong><\/td>\n<td><strong> pH of buffer (equal molarities of both components) <\/strong><\/td>\n<\/tr>\n<tr>\n<td>Acetic acid \/ acetate ion<\/td>\n<td>CH <sub> 3 <\/sub> COOH \/ CH <sub> 3 <\/sub> COO <sup> \u2212 <\/sup><\/td>\n<td>4.74<\/td>\n<\/tr>\n<tr>\n<td>Carbonic acid \/ hydrogen carbonate ion<\/td>\n<td>H <sub> 2 <\/sub> CO <sub> 3 <\/sub> \/ HCO <sub> 3 <\/sub><sup> \u2212 <\/sup><\/td>\n<td>6.38<\/td>\n<\/tr>\n<tr>\n<td>\n<p id=\"x-ck12-OThhNmM3Y2IwNDAzNzJmYjZiMThlY2MwYTU4MTc1NjY.-pxl\">Dihydrogen phosphate ion \/ hydrogen phosphate ion<\/p>\n<\/td>\n<td>H <sub> 2 <\/sub> PO <sub> 4 <\/sub><sup> \u2212 <\/sup> \/ HPO <sub> 4 <\/sub><sup> 2\u2212 <\/sup><\/td>\n<td>7.21<\/td>\n<\/tr>\n<tr>\n<td>Ammonia \/ ammonium ion<\/td>\n<td>NH <sub> 3 <\/sub> \/ NH <sub> 4 <\/sub><sup> + <\/sup><\/td>\n<td>9.25<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"x-ck12-NDQ0MzY1NmY5NjE3NGI5ZDVmNWZmMGJiYzM1MmJiZGM.-k9u\">One example of a buffer is a solution made of acetic acid (the weak acid) and sodium acetate (the salt). The pH of a buffer consisting of 0.50 M CH <sub> 3 <\/sub> COOH and 0.50 M CH <sub> 3 <\/sub> COONa is 4.74. If 10.0 mL of 1.0 M HCl is added to 1.0 L of the buffer, the pH only decreases to 4.73. This ability to \u201csoak up\u201d the additional hydrogen ions from the HCl that was added is due to the reaction below.<\/p>\n<p id=\"x-ck12-3ls\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-MTM2ODczOTAxMDEzMA..\" 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\/19213421\/3a8e0b072107314d683a68cf2d0d4fcb.png\" alt=\"text{CH}_3text{COO}^-(aq)+text{H}^+(aq) rightarrow text{CH}_3text{COOH}(aq)\" width=\"342\" height=\"21\" \/><\/p>\n<p id=\"x-ck12-NTMxZjQwOTJiN2I0NWIwOTBkNmExZDEyYmYzNTc2M2M.-hqh\">Since both the acetate ion and the acetic acid were already present in the buffer, the only thing that changes is the ratio of one to the other. Small changes in that ratio have only very minor effects on the pH.<\/p>\n<p id=\"x-ck12-MDM0OWQyYWQzMmEwY2IxYjg0ZTlmN2VhN2I3ZWU3ZDE.-oqj\">If 10.0 mL of 1.0 M NaOH were added to another 1.0 L of the same buffer, the pH would only increase to 4.76. In this case the buffer takes up the additional hydroxide ions.<\/p>\n<p id=\"x-ck12-qds\"><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\/19213423\/9f730348f213e9bc8640147dd4c5ba10.png\" alt=\"text{CH}_3text{COOH}(aq)+text{OH}^-(aq) rightarrow text{CH}_3text{COO}^-(aq)+text{H}_2text{O}(l)\" width=\"432\" height=\"18\" \/><\/p>\n<p id=\"x-ck12-ZTVkNGYzNGEyYWQxNDc5ZGNjYmVkZjIwYzFjOTc0YjU.-hvs\">Again the ratio of acetate ion to acetic acid changes slightly, this time causing a very small increase in the pH.<\/p>\n<p id=\"x-ck12-ZTE5MTM1NWEwNDVhNDI0MzgyYTBmM2UyNzhkODJkZWQ.-acw\">It is possible to add so much acid or base to a buffer that its ability to resist a significant change in pH is overwhelmed. The <strong> buffer capacity <\/strong> is the amount of acid or base that can be added to a buffer solution before a large change in pH occurs. The buffer capacity is exceeded when the number of moles of H <sup> + <\/sup> or OH <sup> \u2212 <\/sup> that are added to the buffer exceeds the number of moles of the buffer components.<\/p>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-ZGE4YjRiZTg0MWIzNGNkODZhMjhiZTlkMzkwMjQzMGM.-iry\">\n<li>Buffer is defined.<\/li>\n<li>Reactions showing how buffers regulate pH are described.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-ZDA1NTE4MmE3ZWNhMTc1ZjZmZjlhNTc2YTQzZWI5ZTg.-fca\">Read the material at the link below and answer the following questions:<\/p>\n<p id=\"x-ck12-ZmFmNDM3OTA3ZTExNmQzOTlhZWZlM2EyOTljMjE4MzM.-ogj\"><a href=\"http:\/\/chemcollective.org\/activities\/tutorials\/buffers\/buffers3\"> http:\/\/chemcollective.org\/activities\/tutorials\/buffers\/buffers3 <\/a><\/p>\n<ol id=\"x-ck12-MGFjMDBiNzhjMzgwZjczODY3NmQxNTI2NWVjYzM1ZTE.-hrq\">\n<li>What is a weak acid?<\/li>\n<li>What does a conjugate base rarely do?<\/li>\n<li>Write the generic equation for neutralization of a base by a weak acid.<\/li>\n<li>Write the generic equation for neutralization of an acid by a weak base.<\/li>\n<\/ol>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-NmJmNTVkNGY2YWE2NmZiY2RmMzBkZmU3OTg5OTg3MTI.-deq\">\n<li>What is a buffer?<\/li>\n<li>How would the acetic acid\/acetate buffer system neutralize an added base?<\/li>\n<li>If acid is added to the carbonic acid\/carbonate buffer system, how is it neutralized?<\/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-ZjQ0M2JjMjgzMTA3OWI2YTZkOTBiM2JjZTE2OTU4NTY.-gbn\">\n<li><strong> buffer: <\/strong> A solution of a weak acid or a base and its salt.<\/li>\n<li><strong> buffer capacity: <\/strong> The amount of acid or base that can be added to buffer solution before a large change in pH occurs.<\/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-2827\">\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>Insulin Application. <strong>Authored by<\/strong>: Mr Hyde. <strong>Provided by<\/strong>: Czech Wikipedia. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Insulin_Application.jpg\">https:\/\/commons.wikimedia.org\/wiki\/File:Insulin_Application.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":17,"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\":\"Insulin Application\",\"author\":\"Mr Hyde\",\"organization\":\"Czech Wikipedia\",\"url\":\"https:\/\/commons.wikimedia.org\/wiki\/File:Insulin_Application.jpg\",\"project\":\"\",\"license\":\"pd\",\"license_terms\":\"\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-2827","chapter","type-chapter","status-publish","hentry"],"part":2342,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2827","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/users\/17"}],"version-history":[{"count":3,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2827\/revisions"}],"predecessor-version":[{"id":3054,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2827\/revisions\/3054"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/parts\/2342"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2827\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=2827"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=2827"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=2827"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=2827"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}