{"id":1274,"date":"2016-04-29T20:28:13","date_gmt":"2016-04-29T20:28:13","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/biologyxwaymakerxmaster\/?post_type=chapter&#038;p=1274"},"modified":"2024-04-26T18:38:25","modified_gmt":"2024-04-26T18:38:25","slug":"reading-buffers","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/wm-biology1\/chapter\/reading-buffers\/","title":{"raw":"Buffers","rendered":"Buffers"},"content":{"raw":"<div class=\"textbox learning-objectives\">\r\n<h3>Learning Outcomes<\/h3>\r\n<ul>\r\n \t<li>Define \u201cbuffers\u201d and discuss the role they play in human biology<\/li>\r\n<\/ul>\r\n<\/div>\r\nSo how can organisms whose bodies require a near-neutral pH ingest acidic and basic substances (a human drinking orange juice, for example) and survive?\u00a0<strong>Buffers<\/strong> are the key. Buffers readily absorb excess H<sup>+<\/sup> or OH<sup>\u2013<\/sup>, keeping the pH of the body carefully maintained in the narrow range required for survival. Maintaining a constant blood pH is critical to a person's well-being. The buffer maintaining the pH of human blood involves carbonic acid (H<sub>2<\/sub>CO<sub>3<\/sub>), bicarbonate ion (HCO<sub>3<\/sub><sup>\u2013<\/sup>), and carbon dioxide (CO<sub>2<\/sub>). When bicarbonate ions combine with free hydrogen ions and become carbonic acid, hydrogen ions are removed, moderating pH changes. Similarly, as shown in Figure\u00a01, excess carbonic acid can be converted to carbon dioxide gas and exhaled through the lungs. This prevents too many free hydrogen ions from building up in the blood and dangerously reducing the blood's pH. Likewise, if too much OH<sup>\u2013<\/sup> is introduced into the system, carbonic acid will combine with it to create bicarbonate, lowering the pH. Without this buffer system, the body's pH would fluctuate enough to put survival in jeopardy.\r\n\r\n[caption id=\"attachment_1543\" align=\"aligncenter\" width=\"800\"]<img class=\"size-full wp-image-1543\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/110\/2016\/05\/02211648\/Figure_02_02_08.jpg\" alt=\"An H2O molecule can combine with a CO2 molecule to form H2CO3, or carbonic acid. A proton may dissociate from H2CO3, forming bicarbonate, or HCO3-, in the process. The reaction is reversible so that if acid is added protons combined with bicarbonate to form carbonic acid.\" width=\"800\" height=\"87\" \/> Figure 1. This diagram shows the body's buffering of blood pH levels. The blue arrows show the process of raising pH as more CO<sub>2<\/sub> is made. The purple arrows indicate the reverse process: the lowering of pH as more bicarbonate is created.[\/caption]\r\n\r\nOther examples of buffers are antacids used to combat excess stomach acid. Many of these over-the-counter medications work in the same way as blood buffers, usually with at least one ion capable of absorbing hydrogen and moderating pH, bringing relief to those that suffer \"heartburn\" after eating. The unique properties of water that contribute to this capacity to balance pH\u2014as well as water's other characteristics\u2014are essential to sustaining life on Earth.\r\n<div class=\"textbox learning-objectives\">\r\n<h3>In Summary: Buffers<\/h3>\r\nThe pH scale is a measure of acidity\/alkalinity and provides information about how substances tend to act in aqueous solutions. All living processes occur in an ideal pH range. Buffers act together to keep the pH within a certain range, based off the release or absorption of hydrogen ions.\r\n\r\n<\/div>\r\n<div class=\"textbox tryit\">\r\n<h3>Try It<\/h3>\r\nhttps:\/\/assess.lumenlearning.com\/practice\/53fd909a-da14-4f4d-9e7a-129eb60dcea0\r\n<\/div>","rendered":"<div class=\"textbox learning-objectives\">\n<h3>Learning Outcomes<\/h3>\n<ul>\n<li>Define \u201cbuffers\u201d and discuss the role they play in human biology<\/li>\n<\/ul>\n<\/div>\n<p>So how can organisms whose bodies require a near-neutral pH ingest acidic and basic substances (a human drinking orange juice, for example) and survive?\u00a0<strong>Buffers<\/strong> are the key. Buffers readily absorb excess H<sup>+<\/sup> or OH<sup>\u2013<\/sup>, keeping the pH of the body carefully maintained in the narrow range required for survival. Maintaining a constant blood pH is critical to a person&#8217;s well-being. The buffer maintaining the pH of human blood involves carbonic acid (H<sub>2<\/sub>CO<sub>3<\/sub>), bicarbonate ion (HCO<sub>3<\/sub><sup>\u2013<\/sup>), and carbon dioxide (CO<sub>2<\/sub>). When bicarbonate ions combine with free hydrogen ions and become carbonic acid, hydrogen ions are removed, moderating pH changes. Similarly, as shown in Figure\u00a01, excess carbonic acid can be converted to carbon dioxide gas and exhaled through the lungs. This prevents too many free hydrogen ions from building up in the blood and dangerously reducing the blood&#8217;s pH. Likewise, if too much OH<sup>\u2013<\/sup> is introduced into the system, carbonic acid will combine with it to create bicarbonate, lowering the pH. Without this buffer system, the body&#8217;s pH would fluctuate enough to put survival in jeopardy.<\/p>\n<div id=\"attachment_1543\" style=\"width: 810px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" aria-describedby=\"caption-attachment-1543\" class=\"size-full wp-image-1543\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/110\/2016\/05\/02211648\/Figure_02_02_08.jpg\" alt=\"An H2O molecule can combine with a CO2 molecule to form H2CO3, or carbonic acid. A proton may dissociate from H2CO3, forming bicarbonate, or HCO3-, in the process. The reaction is reversible so that if acid is added protons combined with bicarbonate to form carbonic acid.\" width=\"800\" height=\"87\" \/><\/p>\n<p id=\"caption-attachment-1543\" class=\"wp-caption-text\">Figure 1. This diagram shows the body&#8217;s buffering of blood pH levels. The blue arrows show the process of raising pH as more CO<sub>2<\/sub> is made. The purple arrows indicate the reverse process: the lowering of pH as more bicarbonate is created.<\/p>\n<\/div>\n<p>Other examples of buffers are antacids used to combat excess stomach acid. Many of these over-the-counter medications work in the same way as blood buffers, usually with at least one ion capable of absorbing hydrogen and moderating pH, bringing relief to those that suffer &#8220;heartburn&#8221; after eating. The unique properties of water that contribute to this capacity to balance pH\u2014as well as water&#8217;s other characteristics\u2014are essential to sustaining life on Earth.<\/p>\n<div class=\"textbox learning-objectives\">\n<h3>In Summary: Buffers<\/h3>\n<p>The pH scale is a measure of acidity\/alkalinity and provides information about how substances tend to act in aqueous solutions. All living processes occur in an ideal pH range. Buffers act together to keep the pH within a certain range, based off the release or absorption of hydrogen ions.<\/p>\n<\/div>\n<div class=\"textbox tryit\">\n<h3>Try It<\/h3>\n<p>\t<iframe id=\"assessment_practice_53fd909a-da14-4f4d-9e7a-129eb60dcea0\" class=\"resizable\" src=\"https:\/\/assess.lumenlearning.com\/practice\/53fd909a-da14-4f4d-9e7a-129eb60dcea0?iframe_resize_id=assessment_practice_id_53fd909a-da14-4f4d-9e7a-129eb60dcea0\" frameborder=\"0\" style=\"border:none;width:100%;height:100%;min-height:300px;\"><br \/>\n\t<\/iframe>\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-1274\">\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>Biology 2e. <strong>Provided by<\/strong>: OpenStax. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/cnx.org\/contents\/185cbf87-c72e-48f5-b51e-f14f21b5eabd@10.8\">http:\/\/cnx.org\/contents\/185cbf87-c72e-48f5-b51e-f14f21b5eabd@10.8<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY: Attribution<\/a><\/em>. <strong>License Terms<\/strong>: Access for free at https:\/\/openstax.org\/books\/biology-2e\/pages\/1-introduction<\/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":14,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Biology 2e\",\"author\":\"\",\"organization\":\"OpenStax\",\"url\":\"http:\/\/cnx.org\/contents\/185cbf87-c72e-48f5-b51e-f14f21b5eabd@10.8\",\"project\":\"\",\"license\":\"cc-by\",\"license_terms\":\"Access for free at https:\/\/openstax.org\/books\/biology-2e\/pages\/1-introduction\"}]","CANDELA_OUTCOMES_GUID":"bc6a0466-8565-43d1-98bb-05b98d2dd2d2, 9e8e7647-df7f-4272-bbe7-c06de04880b3","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-1274","chapter","type-chapter","status-publish","hentry"],"part":43,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/pressbooks\/v2\/chapters\/1274","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/wp\/v2\/users\/17"}],"version-history":[{"count":13,"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/pressbooks\/v2\/chapters\/1274\/revisions"}],"predecessor-version":[{"id":5865,"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/pressbooks\/v2\/chapters\/1274\/revisions\/5865"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/pressbooks\/v2\/parts\/43"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/pressbooks\/v2\/chapters\/1274\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/wp\/v2\/media?parent=1274"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/pressbooks\/v2\/chapter-type?post=1274"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/wp\/v2\/contributor?post=1274"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/wm-biology1\/wp-json\/wp\/v2\/license?post=1274"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}