{"id":7693,"date":"2024-12-05T16:18:04","date_gmt":"2024-12-05T21:18:04","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/pathology\/chapter\/acids-bases-and-buffers-gj-betts-clone\/"},"modified":"2025-11-11T23:44:56","modified_gmt":"2025-11-12T04:44:56","slug":"acids-bases-and-buffers-gj-betts-clone","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/pathology\/chapter\/acids-bases-and-buffers-gj-betts-clone\/","title":{"raw":"Acids, Bases, and Buffers","rendered":"Acids, Bases, and Buffers"},"content":{"raw":"<div class=\"textbox textbox--learning-objectives\"><header class=\"textbox__header\">\r\n<p class=\"textbox__title\">Learning Objectives<\/p>\r\n\r\n<\/header>\r\n<div class=\"textbox__content\">\r\n\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Identify the most powerful buffer system in the body.<\/li>\r\n \t<li>Explain the way in which the respiratory system affects blood pH.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<span style=\"text-align: initial;font-size: 1em\">Proper physiological functioning depends on a very tight balance between the concentrations of acids and bases in the blood. Acid-balance balance is measured using the pH scale, as shown in <\/span><a href=\"#pHscale\">The pH scale<\/a><span style=\"text-align: initial;font-size: 1em\">. A variety of buffering systems permits blood and other bodily fluids to maintain a narrow pH range, even in the face of perturbations. A buffer is a chemical system that prevents a radical change in fluid pH by dampening the change in hydrogen ion concentrations in the case of excess acid or base. Most commonly, the substance that absorbs the ions is either a weak acid, which takes up hydroxyl ions, or a weak base, which takes up hydrogen ions.<\/span>\r\n\r\n[caption id=\"attachment_9607\" align=\"aligncenter\" width=\"497\"]<img class=\" wp-image-9607\" src=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-597x1024.jpg\" alt=\"This table gives examples of solutions from PH of zero to 14. Examples of solutions with a PH of zero include battery acid and strong hydrofluoric acid. An example of a solution with a pH of one is the hydrochloric acid secreted by the stomach lining. Examples of solutions with a PH of two include lemon juice and vinegar. Examples of solutions with a PH of three include grapefruit juice, orange juice and soda. Examples of solutions with a PH of four include tomato juice and acid rain. Examples of solutions with a PH of five include soft drinking water and black coffee. Examples of solutions with a PH of six include urine and saliva. An example of a solution with a PH of seven is pure water. An example of a solution with a PH of eight is sea water. An example of a solution with a PH of nine is baking soda. Examples of solutions with a PH of ten include saline lake water and milk of magnesia. An example of a solution with a PH of eleven is an ammonia solution. An example of a solution with a PH of twelve is soapy water. Examples of solutions with a PH of thirteen include bleach and oven cleaner. An example of a solution with a PH of fourteen is liquid drain cleaner.\" width=\"497\" height=\"852\" \/> <strong>The pH Scale<\/strong> - This chart shows where many common substances fall on the pH scale.[\/caption]\r\n\r\n<section id=\"fs-id2143807\" data-depth=\"1\">\r\n<h2 data-type=\"title\">Buffer Systems in the Body<\/h2>\r\n<p id=\"fs-id1638084\">The buffer systems in the human body are extremely efficient, and different systems work at different rates. It takes only seconds for the chemical buffers in the blood to make adjustments to pH. The respiratory tract can adjust the blood pH upward in minutes by exhaling CO<sub>2<\/sub>\u00a0from the body. The renal system can also adjust blood pH through the excretion of hydrogen ions (H<sup>+<\/sup>) and the conservation of bicarbonate, but this process takes hours to days to have an effect.<\/p>\r\n<p id=\"fs-id1272927\">The buffer systems functioning in blood plasma include plasma proteins, phosphate, and bicarbonate and carbonic acid buffers. The kidneys help control acid-base balance by excreting hydrogen ions and generating bicarbonate that helps maintain blood plasma pH within a normal range. Protein buffer systems work predominantly inside cells.<\/p>\r\n\r\n<section id=\"fs-id1971620\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Protein Buffers in Blood Plasma and Cells<\/h3>\r\n<p id=\"fs-id1918574\">Nearly all proteins can function as buffers. Proteins are made up of amino acids, which contain positively charged amino groups and negatively charged carboxyl groups. The charged regions of these molecules can bind hydrogen and hydroxyl ions, and thus function as buffers. Buffering by proteins accounts for two-thirds of the buffering power of the blood and most of the buffering within cells.<\/p>\r\n\r\n<\/section><section id=\"fs-id2059524\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Hemoglobin as a Buffer<\/h3>\r\n<p id=\"fs-id1373424\">Hemoglobin is the principal protein inside of red blood cells and accounts for one-third of the mass of the cell. During the conversion of CO<sub>2<\/sub>\u00a0into bicarbonate, hydrogen ions liberated in the reaction are buffered by hemoglobin, which is reduced by the dissociation of oxygen. This buffering helps maintain normal pH. The process is reversed in the pulmonary capillaries to re-form CO<sub>2<\/sub>, which then can diffuse into the air sacs to be exhaled into the atmosphere. This process is discussed in detail in the chapter on the respiratory system.<\/p>\r\n\r\n<\/section><section id=\"fs-id1615929\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Phosphate Buffer<\/h3>\r\n<p id=\"fs-id1882970\">Phosphates are found in the blood in two forms: sodium dihydrogen phosphate (<span id=\"MathJax-Span-84\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-85\" class=\"mrow\"><span id=\"MathJax-Span-86\" class=\"mtext\">NaH<\/span><\/span><sub><span id=\"MathJax-Span-87\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-88\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-89\" class=\"mrow\"><span id=\"MathJax-Span-90\" class=\"mtext\">PO<\/span><\/span><sub><span id=\"MathJax-Span-91\" class=\"mtext\">4<\/span><\/sub><\/span>), which is a weak acid, and sodium monohydrogen phosphate (<span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-15\" class=\"math\"><span id=\"MathJax-Span-16\" class=\"mrow\"><span id=\"MathJax-Span-17\" class=\"semantics\"><span id=\"MathJax-Span-18\" class=\"mrow\"><span id=\"MathJax-Span-19\" class=\"mrow\"><span id=\"MathJax-Span-24\" class=\"msub\"><span id=\"MathJax-Span-27\" class=\"mrow\"><span id=\"MathJax-Span-28\" class=\"mtext\">),<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span> which is a weak base. When <span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><span style=\"font-size: 1em\"> comes into contact with a strong acid, such as HCl, the base picks up a second hydrogen ion to form the weak acid <span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><\/span><span style=\"font-size: 1em\">\u00a0and sodium chloride, NaCl. When <\/span><span id=\"MathJax-Span-57\" class=\"math\"><span id=\"MathJax-Span-58\" class=\"mrow\"><span id=\"MathJax-Span-59\" class=\"semantics\"><span id=\"MathJax-Span-60\" class=\"mrow\"><span id=\"MathJax-Span-61\" class=\"mrow\"><span id=\"MathJax-Span-62\" class=\"mrow\"><span id=\"MathJax-Span-63\" class=\"mtext\">Na<\/span><\/span><span id=\"MathJax-Span-64\" class=\"msub\"><span id=\"MathJax-Span-65\" class=\"mrow\"><span id=\"MathJax-Span-66\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-67\" class=\"mrow\"><span id=\"MathJax-Span-68\" class=\"mtext\">4<\/span><\/span><\/sub><\/span><\/span><\/span><\/span><\/span><\/span><span style=\"font-size: 1em\"> (the weak acid) comes into contact with a strong base, such as sodium hydroxide (NaOH), the weak acid reverts back to the weak base and produces water. Acids and bases are still present, but they hold onto the ions.<\/span><\/p>\r\n<p style=\"text-align: center\"><span id=\"MathJax-Span-74\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-75\" class=\"mrow\"><span id=\"MathJax-Span-76\" class=\"mtext\">HCl + Na<\/span><\/span><sub><span id=\"MathJax-Span-77\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-78\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-79\" class=\"mrow\"><span id=\"MathJax-Span-80\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-81\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-82\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-83\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-84\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-85\" class=\"mrow\"><span id=\"MathJax-Span-86\" class=\"mtext\">NaH<\/span><\/span><sub><span id=\"MathJax-Span-87\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-88\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-89\" class=\"mrow\"><span id=\"MathJax-Span-90\" class=\"mtext\">PO<\/span><\/span><sub><span id=\"MathJax-Span-91\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-92\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\"> + NaCl<\/span><\/p>\r\n\r\n<div id=\"eip-177\" data-type=\"equation\">\r\n<div class=\"MathJax_Display\" style=\"text-align: center\"><span style=\"font-size: 1em\">(strong acid) + (weak base)<\/span><span style=\"font-size: 1em\">\u2192<\/span><span style=\"font-size: 1em\">(weak\u00a0acid)\u00a0+\u00a0(salt)<\/span><\/div>\r\n<\/div>\r\n<div id=\"eip-75\" style=\"text-align: center\" data-type=\"equation\"><\/div>\r\n<div id=\"eip-714\" data-type=\"equation\">\r\n<div style=\"text-align: center\"><span id=\"MathJax-Span-107\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-108\" class=\"mrow\"><span id=\"MathJax-Span-109\" class=\"mtext\">NaOH + NaH<\/span><\/span><sub><span id=\"MathJax-Span-110\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-111\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-112\" class=\"mrow\"><span id=\"MathJax-Span-113\" class=\"mtext\">PO<\/span><\/span><sub><span id=\"MathJax-Span-114\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-115\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-116\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-125\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-126\" class=\"mrow\"><span id=\"MathJax-Span-127\" class=\"mtext\">\u00a0+\u00a0H<\/span><\/span><sub><span id=\"MathJax-Span-128\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-129\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">O<\/span><\/div>\r\n<div class=\"MathJax_Display\" style=\"text-align: center\"><span id=\"MathJax-Span-130\" class=\"math\"><span id=\"MathJax-Span-131\" class=\"mrow\"><span id=\"MathJax-Span-132\" class=\"semantics\"><span id=\"MathJax-Span-133\" class=\"mrow\"><span id=\"MathJax-Span-134\" class=\"mrow\"><span id=\"MathJax-Span-135\" class=\"mtext\">(strong\u00a0base)\u00a0+\u00a0(weak\u00a0acid)\u00a0<\/span><span id=\"MathJax-Span-136\" class=\"mrow\"><span id=\"MathJax-Span-137\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-138\" class=\"mtext\"> (weak\u00a0base)\u00a0+\u00a0(water)<\/span><\/span><\/span><\/span><\/span><\/span><\/div>\r\n<\/div>\r\n<\/section><section id=\"fs-id1689764\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Bicarbonate-Carbonic Acid Buffer<\/h3>\r\n<p id=\"fs-id2029316\">The bicarbonate-carbonic acid buffer works in a fashion similar to phosphate buffers. The bicarbonate is regulated in the blood by sodium, as are the phosphate ions. When sodium bicarbonate (NaHCO<sub>3<\/sub>), comes into contact with a strong acid, such as HCl, carbonic acid (H<sub>2<\/sub>CO<sub>3<\/sub>), which is a weak acid, and NaCl are formed. When carbonic acid comes into contact with a strong base, such as NaOH, bicarbonate and water are formed.<\/p>\r\n\r\n<div id=\"eip-515\" data-type=\"equation\">\r\n<div class=\"MathJax_Display\" style=\"text-align: center\">\r\n<p style=\"text-align: center\"><span id=\"MathJax-Span-139\" class=\"math\"><span id=\"MathJax-Span-140\" class=\"mrow\"><span id=\"MathJax-Span-141\" class=\"semantics\"><span id=\"MathJax-Span-142\" class=\"mrow\"><span id=\"MathJax-Span-143\" class=\"mrow\"><span id=\"MathJax-Span-148\" class=\"mtext\">NaHCO<sub>3<\/sub> + HCl\u00a0<\/span><span id=\"MathJax-Span-149\" class=\"mrow\"><span id=\"MathJax-Span-150\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-151\" class=\"msub\"><span id=\"MathJax-Span-152\" class=\"mrow\"><span id=\"MathJax-Span-153\" class=\"mtext\"> H<sub>2<\/sub>CO<sub>3<\/sub><\/span><\/span><\/span><span id=\"MathJax-Span-159\" class=\"mtext\">+NaCl<\/span><\/span><\/span><\/span><\/span><\/span><\/p>\r\n<p style=\"text-align: center\"><span id=\"MathJax-Span-160\" class=\"math\"><span id=\"MathJax-Span-161\" class=\"mrow\"><span id=\"MathJax-Span-162\" class=\"semantics\"><span id=\"MathJax-Span-163\" class=\"mrow\"><span id=\"MathJax-Span-164\" class=\"mrow\"><span id=\"MathJax-Span-165\" class=\"mtext\">(sodium bicarbonate) + (strong acid)\u00a0<\/span><span id=\"MathJax-Span-166\" class=\"mrow\"><span id=\"MathJax-Span-167\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-168\" class=\"mtext\"> (weak acid) + (salt)<\/span><\/span><\/span><\/span><\/span><\/span><\/p>\r\n<p style=\"text-align: center\"><span id=\"MathJax-Span-181\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">H<sub>2<\/sub>CO<sub>3<\/sub> + NaOH<\/span><span id=\"MathJax-Span-182\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-183\" class=\"mo\">\u2192NaHCO<sub>3<\/sub><\/span><\/span><span id=\"MathJax-Span-189\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-190\" class=\"mrow\"><span id=\"MathJax-Span-191\" class=\"mtext\">\u00a0+\u00a0H<\/span><\/span><sub><span id=\"MathJax-Span-192\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-193\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">O<\/span><\/p>\r\n\r\n<\/div>\r\n<div class=\"MathJax_Display\" style=\"text-align: center\"><span id=\"MathJax-Span-199\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">(weak acid) + (strong base)<\/span><span id=\"MathJax-Span-200\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-201\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-202\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">(sodium bicarbonate) + (water)<\/span><\/div>\r\n<\/div>\r\n<p id=\"fs-id1353864\">As with the phosphate buffer, a weak acid or weak base captures the free ions, and a significant change in pH is prevented. Bicarbonate ions and carbonic acid are present in the blood in a 20:1 ratio if the blood pH is within the normal range. With 20 times more bicarbonate than carbonic acid, this capture system is most efficient at buffering changes that would make the blood more acidic. This is useful because most of the body\u2019s metabolic wastes, such as lactic acid and ketone bodies, are acids. Carbonic acid levels in the blood are controlled by the expiration of CO<sub>2<\/sub>\u00a0through the lungs. In red blood cells, carbonic anhydrase forces the dissociation of the acid, rendering the blood less acidic. Because of this acid dissociation, CO<sub>2<\/sub>\u00a0is exhaled (see equations above). The level of bicarbonate in the blood is controlled through the renal system, where bicarbonate ions in the renal filtrate are conserved and passed back into the blood. However, the bicarbonate buffer is the primary buffering system of the IF surrounding the cells in tissues throughout the body.<\/p>\r\n\r\n<\/section><\/section>\r\n<h2 data-type=\"title\">Respiratory Regulation of Acid-Base Balance<\/h2>\r\nThe respiratory system contributes to the balance of acids and bases in the body by regulating the blood levels of carbonic acid (<a href=\"#BloodpHRespiratoryRegulation\">Respiratory Regulation of Blood pH<\/a>). CO<sub>2\u00a0<\/sub>in the blood readily reacts with water to form carbonic acid, and the levels of CO<sub>2\u00a0<\/sub>and carbonic acid in the blood are in equilibrium. When the CO<sub>2\u00a0<\/sub>level in the blood rises (as it does when you hold your breath), the excess CO<sub>2<\/sub>\u00a0reacts with water to form additional carbonic acid, lowering blood pH. Increasing the rate and\/or depth of respiration (which you might feel the \u201curge\u201d to do after holding your breath) allows you to exhale more CO<sub>2<\/sub>. The loss of CO<sub>2<\/sub>\u00a0from the body reduces blood levels of carbonic acid and thereby adjusts the pH upward, toward normal levels. As you might have surmised, this process also works in the opposite direction. Excessive deep and rapid breathing (as in hyperventilation) rids the blood of CO<sub>2<\/sub>\u00a0and reduces the level of carbonic acid, making the blood too alkaline. This brief alkalosis can be remedied by rebreathing air that has been exhaled into a paper bag. Rebreathing exhaled air will rapidly bring blood pH down toward normal.<a id=\"BloodpHRespiratoryRegulation\"><\/a>\r\n\r\n[caption id=\"attachment_9608\" align=\"aligncenter\" width=\"424\"]<img class=\" wp-image-9608\" src=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2714_Respiratory_Regulation_of_Blood.jpg\" alt=\"This top to bottom flowchart describes the regulation of PH in the blood. The left branch shows acidosis, which is when the PH of the blood drops. Acidosis stimulates brain and arterial receptors, triggering an increase in respiratory rate. This causes a drop in blood CO two and H two CO three. A drop in these two acidic compounds causes the blood PH to rise back to homeostatic levels. The right branch shows alkalosis which is when the PH of the blood rises. Alkalosis also stimulates brain and arterial receptors, but these now trigger a decrease in respiratory rate. This causes an increase in blood CO two and H two CO three, which lowers the PH of the blood back to homeostatic levels.\" width=\"424\" height=\"773\" \/> <strong>Respiratory Regulation of Blood pH\u00a0<\/strong>- The respiratory system can reduce blood pH by removing CO<sub>2<\/sub> from the blood.[\/caption]\r\n\r\nThe chemical reactions that regulate the levels of CO<sub>2<\/sub>\u00a0and carbonic acid occur in the lungs when blood travels through the lung\u2019s pulmonary capillaries. Minor adjustments in breathing are usually sufficient to adjust the pH of the blood by changing how much CO<sub>2<\/sub>\u00a0is exhaled. In fact, doubling the respiratory rate for less than 1 minute, removing \u201cextra\u201d CO<sub>2<\/sub>, would increase the blood pH by 0.2. This situation is common if you are exercising strenuously over a period of time. To keep up the necessary energy production, you would produce excess CO<sub>2<\/sub>\u00a0(and lactic acid if exercising beyond your aerobic threshold). In order to balance the increased acid production, the respiration rate goes up to remove the CO<sub>2<\/sub>. This helps to keep you from developing acidosis.\r\n\r\nThe body regulates the respiratory rate by the use of chemoreceptors, which primarily use CO<sub>2<\/sub>\u00a0as a signal. Peripheral blood sensors are found in the walls of the aorta and carotid arteries. These sensors signal the brain to provide immediate adjustments to the respiratory rate if CO<sub>2\u00a0<\/sub>levels rise or fall. Yet other sensors are found in the brain itself. Changes in the pH of CSF affect the respiratory center in the medulla oblongata, which can directly modulate breathing rate to bring the pH back into the normal range.\r\n\r\n<span id=\"term-00001\" data-type=\"term\">Hypercapnia<\/span>, or abnormally elevated blood levels of CO<sub>2<\/sub>, occurs in any situation that impairs respiratory functions, including pneumonia and congestive heart failure. Reduced breathing (hypoventilation) due to drugs such as morphine, barbiturates, or ethanol (or even just holding one\u2019s breath) can also result in hypercapnia.\u00a0<span id=\"term-00002\" data-type=\"term\">Hypocapnia<\/span>, or abnormally low blood levels of CO<sub>2<\/sub>, occurs with any cause of hyperventilation that drives off the CO<sub>2<\/sub>, such as salicylate toxicity, elevated room temperatures, fever, or hysteria.\r\n<h2 data-type=\"title\">Renal Regulation of Acid-Base Balance<\/h2>\r\nThe renal regulation of the body\u2019s acid-base balance addresses the metabolic component of the buffering system. Whereas the respiratory system (together with breathing centers in the brain) controls the blood levels of carbonic acid by controlling the exhalation of CO<sub>2<\/sub>, the renal system controls the blood levels of bicarbonate. A decrease of blood bicarbonate can result from the inhibition of carbonic anhydrase by certain diuretics or from excessive bicarbonate loss due to diarrhea. Blood bicarbonate levels are also typically lower in people who have Addison\u2019s disease (chronic adrenal insufficiency), in which aldosterone levels are reduced, and in people who have renal damage, such as chronic nephritis. Finally, low bicarbonate blood levels can result from elevated levels of ketones (common in unmanaged diabetes mellitus), which bind bicarbonate in the filtrate and prevent its conservation.\r\n\r\nBicarbonate ions, HCO<sub>3<\/sub><sup>-<\/sup>, found in the filtrate, are essential to the bicarbonate buffer system, yet the cells of the tubule are not permeable to bicarbonate ions. The steps involved in supplying bicarbonate ions to the system are seen in <a href=\"#KidneyBicarbonateConservation\">Conservation of Bicarbonate in the kidney <\/a>and are summarized below:\r\n<ul id=\"fs-id1414107\">\r\n \t<li>Step 1: Sodium ions are reabsorbed from the filtrate in exchange for H<sup>+<\/sup>\u00a0by an antiport mechanism in the apical membranes of cells lining the renal tubule.<\/li>\r\n \t<li>Step 2: The cells produce bicarbonate ions that can be shunted to peritubular capillaries.<\/li>\r\n \t<li>Step 3: When CO<sub>2<\/sub>\u00a0is available, the reaction is driven to the formation of carbonic acid, which dissociates to form a bicarbonate ion and a hydrogen ion.<\/li>\r\n \t<li>Step 4: The bicarbonate ion passes into the peritubular capillaries and returns to the blood. The hydrogen ion is secreted into the filtrate, where it can become part of new water molecules and be reabsorbed as such, or removed in the urine.<a id=\"KidneyBicarbonateConservation\"><\/a><\/li>\r\n<\/ul>\r\n<div id=\"fig-ch27_04_03\" class=\"os-figure\">\r\n<figure data-id=\"fig-ch27_04_03\"><\/figure>\r\n<figure data-id=\"fig-ch27_04_03\">\r\n\r\n[caption id=\"attachment_9610\" align=\"aligncenter\" width=\"824\"]<img class=\" wp-image-9610\" src=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-1024x602.jpg\" alt=\"This diagram depicts a cross section of the left wall of a kidney proximal tubule. The wall is composed of two block-shaped cells arranged vertically one on top of each other. The lumen of the proximal tubule is to the left of the two cells. Yellow-colored urine is flowing through the lumen. There is a small strip of blue interstitial fluid to the right of the two cells. To the right of the interstitial fluid is a cross section of a blood vessel. A loop of chemical reactions is occurring in the diagram. Within the lumen of the proximal tubule, HCO three minus is combining with an H plus ion that enters the lumen from a proximal tubule cell. This reaction forms H two CO three. H two CO three then breaks into H two O and CO two, a reaction catalyzed by the enzyme carbonic anhydrase. The CO two then moves from the lumen of the proximal tubule into one of the proximal tubule cells. There, the reaction runs in reverse, with CO two combining with H two O to form H two CO three. The H two CO three then splits into H plus and HCO three minus. The H plus moves into the lumen, reinitiating the first step of the loop. The HCO three minus leaves the proximal tubule cell and enters the blood stream.\" width=\"824\" height=\"484\" \/> <strong>Conservation of Bicarbonate in the Kidney<\/strong> - Tubular cells are not permeable to bicarbonate; thus, bicarbonate is conserved rather than reabsorbed. Steps 1 and 2 of bicarbonate conservation are indicated.[\/caption]<\/figure>\r\n<\/div>\r\nIt is also possible that salts in the filtrate, such as sulfates, phosphates, or ammonia, will capture hydrogen ions. If this occurs, the hydrogen ions will not be available to combine with bicarbonate ions and produce CO<sub>2<\/sub>. In such cases, bicarbonate ions are not conserved from the filtrate to the blood, which will also contribute to a pH imbalance and acidosis.\r\n\r\nThe hydrogen ions also compete with potassium to exchange with sodium in the renal tubules. If more potassium is present than normal, potassium, rather than the hydrogen ions, will be exchanged, and increased potassium enters the filtrate. When this occurs, fewer hydrogen ions in the filtrate participate in the conversion of bicarbonate into CO<sub>2<\/sub>\u00a0and less bicarbonate is conserved. If there is less potassium, more hydrogen ions enter the filtrate to be exchanged with sodium and more bicarbonate is conserved.\r\n\r\nChloride ions are important in neutralizing positive ion charges in the body. If chloride is lost, the body uses bicarbonate ions in place of the lost chloride ions. Thus, lost chloride results in an increased reabsorption of bicarbonate by the renal system.\r\n<div id=\"fs-id1473396\" class=\"anatomy disorders ui-has-child-title\" data-type=\"note\"><header>\r\n<h2 data-type=\"title\">DISORDERS OF THE...<\/h2>\r\n<\/header><section>\r\n<div class=\"os-note-body\">\r\n<h3 class=\"os-subtitle\" data-type=\"title\"><span class=\"os-subtitle-label\">Acid-Base Balance: Ketoacidosis<\/span><\/h3>\r\nDiabetic acidosis, or ketoacidosis, occurs most frequently in people with poorly controlled diabetes mellitus. When certain tissues in the body cannot get adequate amounts of glucose, they depend on the breakdown of fatty acids for energy. When acetyl groups break off the fatty acid chains, the acetyl groups then non-enzymatically combine to form ketone bodies, acetoacetic acid, beta-hydroxybutyric acid, and acetone, all of which increase the acidity of the blood. In this condition, the brain isn\u2019t supplied with enough of its fuel\u2014glucose\u2014to produce all of the ATP it requires to function. Ketoacidosis can be severe and, if not detected and treated properly, can lead to diabetic coma, which can be fatal. A common early symptom of ketoacidosis is deep, rapid breathing as the body attempts to drive off CO<sub>2<\/sub> and compensate for the acidosis. Another common symptom is fruity-smelling breath, due to the exhalation of acetone. Other symptoms include dry skin and mouth, a flushed face, nausea, vomiting, and stomach pain. Treatment for diabetic coma is ingestion or injection of sugar; its prevention is the proper daily administration of insulin. A person who is diabetic and uses insulin can initiate ketoacidosis if a dose of insulin is missed. Among people with type 2 diabetes, those of Hispanic and African-American descent are more likely to go into ketoacidosis than those of other ethnic backgrounds, although the reason for this is unknown.\r\n<h1>Adaption<\/h1>\r\nThis chapter was adapted by Carter Allen from the following text:<a href=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\" target=\"_blank\" rel=\"noopener\">Acid Base Balance<\/a>\u00a0<strong>in\u00a0<\/strong><a href=\"https:\/\/openstax.org\/books\/anatomy-and-physiology\/\">Anatomy and Physiology<\/a>\u00a0by\u00a0OSCRiceUniversity\u00a0is licensed under a\u00a0<a href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">Creative Commons Attribution 4.0 International License<\/a>\r\n\r\n<\/div>\r\n<\/section><\/div>","rendered":"<div class=\"textbox textbox--learning-objectives\">\n<header class=\"textbox__header\">\n<p class=\"textbox__title\">Learning Objectives<\/p>\n<\/header>\n<div class=\"textbox__content\">\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Identify the most powerful buffer system in the body.<\/li>\n<li>Explain the way in which the respiratory system affects blood pH.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<p><span style=\"text-align: initial;font-size: 1em\">Proper physiological functioning depends on a very tight balance between the concentrations of acids and bases in the blood. Acid-balance balance is measured using the pH scale, as shown in <\/span><a href=\"#pHscale\">The pH scale<\/a><span style=\"text-align: initial;font-size: 1em\">. A variety of buffering systems permits blood and other bodily fluids to maintain a narrow pH range, even in the face of perturbations. A buffer is a chemical system that prevents a radical change in fluid pH by dampening the change in hydrogen ion concentrations in the case of excess acid or base. Most commonly, the substance that absorbs the ions is either a weak acid, which takes up hydroxyl ions, or a weak base, which takes up hydrogen ions.<\/span><\/p>\n<figure id=\"attachment_9607\" aria-describedby=\"caption-attachment-9607\" style=\"width: 497px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-9607\" src=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-597x1024.jpg\" alt=\"This table gives examples of solutions from PH of zero to 14. Examples of solutions with a PH of zero include battery acid and strong hydrofluoric acid. An example of a solution with a pH of one is the hydrochloric acid secreted by the stomach lining. Examples of solutions with a PH of two include lemon juice and vinegar. Examples of solutions with a PH of three include grapefruit juice, orange juice and soda. Examples of solutions with a PH of four include tomato juice and acid rain. Examples of solutions with a PH of five include soft drinking water and black coffee. Examples of solutions with a PH of six include urine and saliva. An example of a solution with a PH of seven is pure water. An example of a solution with a PH of eight is sea water. An example of a solution with a PH of nine is baking soda. Examples of solutions with a PH of ten include saline lake water and milk of magnesia. An example of a solution with a PH of eleven is an ammonia solution. An example of a solution with a PH of twelve is soapy water. Examples of solutions with a PH of thirteen include bleach and oven cleaner. An example of a solution with a PH of fourteen is liquid drain cleaner.\" width=\"497\" height=\"852\" srcset=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-597x1024.jpg 597w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-175x300.jpg 175w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-768x1317.jpg 768w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-896x1536.jpg 896w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-65x111.jpg 65w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-225x386.jpg 225w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale-350x600.jpg 350w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2713_pH_Scale.jpg 1069w\" sizes=\"auto, (max-width: 497px) 100vw, 497px\" \/><figcaption id=\"caption-attachment-9607\" class=\"wp-caption-text\"><strong>The pH Scale<\/strong> &#8211; This chart shows where many common substances fall on the pH scale.<\/figcaption><\/figure>\n<section id=\"fs-id2143807\" data-depth=\"1\">\n<h2 data-type=\"title\">Buffer Systems in the Body<\/h2>\n<p id=\"fs-id1638084\">The buffer systems in the human body are extremely efficient, and different systems work at different rates. It takes only seconds for the chemical buffers in the blood to make adjustments to pH. The respiratory tract can adjust the blood pH upward in minutes by exhaling CO<sub>2<\/sub>\u00a0from the body. The renal system can also adjust blood pH through the excretion of hydrogen ions (H<sup>+<\/sup>) and the conservation of bicarbonate, but this process takes hours to days to have an effect.<\/p>\n<p id=\"fs-id1272927\">The buffer systems functioning in blood plasma include plasma proteins, phosphate, and bicarbonate and carbonic acid buffers. The kidneys help control acid-base balance by excreting hydrogen ions and generating bicarbonate that helps maintain blood plasma pH within a normal range. Protein buffer systems work predominantly inside cells.<\/p>\n<section id=\"fs-id1971620\" data-depth=\"2\">\n<h3 data-type=\"title\">Protein Buffers in Blood Plasma and Cells<\/h3>\n<p id=\"fs-id1918574\">Nearly all proteins can function as buffers. Proteins are made up of amino acids, which contain positively charged amino groups and negatively charged carboxyl groups. The charged regions of these molecules can bind hydrogen and hydroxyl ions, and thus function as buffers. Buffering by proteins accounts for two-thirds of the buffering power of the blood and most of the buffering within cells.<\/p>\n<\/section>\n<section id=\"fs-id2059524\" data-depth=\"2\">\n<h3 data-type=\"title\">Hemoglobin as a Buffer<\/h3>\n<p id=\"fs-id1373424\">Hemoglobin is the principal protein inside of red blood cells and accounts for one-third of the mass of the cell. During the conversion of CO<sub>2<\/sub>\u00a0into bicarbonate, hydrogen ions liberated in the reaction are buffered by hemoglobin, which is reduced by the dissociation of oxygen. This buffering helps maintain normal pH. The process is reversed in the pulmonary capillaries to re-form CO<sub>2<\/sub>, which then can diffuse into the air sacs to be exhaled into the atmosphere. This process is discussed in detail in the chapter on the respiratory system.<\/p>\n<\/section>\n<section id=\"fs-id1615929\" data-depth=\"2\">\n<h3 data-type=\"title\">Phosphate Buffer<\/h3>\n<p id=\"fs-id1882970\">Phosphates are found in the blood in two forms: sodium dihydrogen phosphate (<span id=\"MathJax-Span-84\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-85\" class=\"mrow\"><span id=\"MathJax-Span-86\" class=\"mtext\">NaH<\/span><\/span><sub><span id=\"MathJax-Span-87\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-88\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-89\" class=\"mrow\"><span id=\"MathJax-Span-90\" class=\"mtext\">PO<\/span><\/span><sub><span id=\"MathJax-Span-91\" class=\"mtext\">4<\/span><\/sub><\/span>), which is a weak acid, and sodium monohydrogen phosphate (<span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-15\" class=\"math\"><span id=\"MathJax-Span-16\" class=\"mrow\"><span id=\"MathJax-Span-17\" class=\"semantics\"><span id=\"MathJax-Span-18\" class=\"mrow\"><span id=\"MathJax-Span-19\" class=\"mrow\"><span id=\"MathJax-Span-24\" class=\"msub\"><span id=\"MathJax-Span-27\" class=\"mrow\"><span id=\"MathJax-Span-28\" class=\"mtext\">),<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span> which is a weak base. When <span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><span style=\"font-size: 1em\"> comes into contact with a strong acid, such as HCl, the base picks up a second hydrogen ion to form the weak acid <span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><\/span><span style=\"font-size: 1em\">\u00a0and sodium chloride, NaCl. When <\/span><span id=\"MathJax-Span-57\" class=\"math\"><span id=\"MathJax-Span-58\" class=\"mrow\"><span id=\"MathJax-Span-59\" class=\"semantics\"><span id=\"MathJax-Span-60\" class=\"mrow\"><span id=\"MathJax-Span-61\" class=\"mrow\"><span id=\"MathJax-Span-62\" class=\"mrow\"><span id=\"MathJax-Span-63\" class=\"mtext\">Na<\/span><\/span><span id=\"MathJax-Span-64\" class=\"msub\"><span id=\"MathJax-Span-65\" class=\"mrow\"><span id=\"MathJax-Span-66\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-67\" class=\"mrow\"><span id=\"MathJax-Span-68\" class=\"mtext\">4<\/span><\/span><\/sub><\/span><\/span><\/span><\/span><\/span><\/span><span style=\"font-size: 1em\"> (the weak acid) comes into contact with a strong base, such as sodium hydroxide (NaOH), the weak acid reverts back to the weak base and produces water. Acids and bases are still present, but they hold onto the ions.<\/span><\/p>\n<p style=\"text-align: center\"><span id=\"MathJax-Span-74\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-75\" class=\"mrow\"><span id=\"MathJax-Span-76\" class=\"mtext\">HCl + Na<\/span><\/span><sub><span id=\"MathJax-Span-77\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-78\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-79\" class=\"mrow\"><span id=\"MathJax-Span-80\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-81\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-82\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-83\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-84\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-85\" class=\"mrow\"><span id=\"MathJax-Span-86\" class=\"mtext\">NaH<\/span><\/span><sub><span id=\"MathJax-Span-87\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-88\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-89\" class=\"mrow\"><span id=\"MathJax-Span-90\" class=\"mtext\">PO<\/span><\/span><sub><span id=\"MathJax-Span-91\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-92\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\"> + NaCl<\/span><\/p>\n<div id=\"eip-177\" data-type=\"equation\">\n<div class=\"MathJax_Display\" style=\"text-align: center\"><span style=\"font-size: 1em\">(strong acid) + (weak base)<\/span><span style=\"font-size: 1em\">\u2192<\/span><span style=\"font-size: 1em\">(weak\u00a0acid)\u00a0+\u00a0(salt)<\/span><\/div>\n<\/div>\n<div id=\"eip-75\" style=\"text-align: center\" data-type=\"equation\"><\/div>\n<div id=\"eip-714\" data-type=\"equation\">\n<div style=\"text-align: center\"><span id=\"MathJax-Span-107\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-108\" class=\"mrow\"><span id=\"MathJax-Span-109\" class=\"mtext\">NaOH + NaH<\/span><\/span><sub><span id=\"MathJax-Span-110\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-111\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-112\" class=\"mrow\"><span id=\"MathJax-Span-113\" class=\"mtext\">PO<\/span><\/span><sub><span id=\"MathJax-Span-114\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-115\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-116\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-117\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-118\" class=\"mrow\"><span id=\"MathJax-Span-119\" class=\"mtext\">Na<\/span><\/span><sub><span id=\"MathJax-Span-120\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-121\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-122\" class=\"mrow\"><span id=\"MathJax-Span-123\" class=\"mtext\">HPO<\/span><\/span><sub><span id=\"MathJax-Span-124\" class=\"mtext\">4<\/span><\/sub><\/span><span id=\"MathJax-Span-125\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-126\" class=\"mrow\"><span id=\"MathJax-Span-127\" class=\"mtext\">\u00a0+\u00a0H<\/span><\/span><sub><span id=\"MathJax-Span-128\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-129\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">O<\/span><\/div>\n<div class=\"MathJax_Display\" style=\"text-align: center\"><span id=\"MathJax-Span-130\" class=\"math\"><span id=\"MathJax-Span-131\" class=\"mrow\"><span id=\"MathJax-Span-132\" class=\"semantics\"><span id=\"MathJax-Span-133\" class=\"mrow\"><span id=\"MathJax-Span-134\" class=\"mrow\"><span id=\"MathJax-Span-135\" class=\"mtext\">(strong\u00a0base)\u00a0+\u00a0(weak\u00a0acid)\u00a0<\/span><span id=\"MathJax-Span-136\" class=\"mrow\"><span id=\"MathJax-Span-137\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-138\" class=\"mtext\"> (weak\u00a0base)\u00a0+\u00a0(water)<\/span><\/span><\/span><\/span><\/span><\/span><\/div>\n<\/div>\n<\/section>\n<section id=\"fs-id1689764\" data-depth=\"2\">\n<h3 data-type=\"title\">Bicarbonate-Carbonic Acid Buffer<\/h3>\n<p id=\"fs-id2029316\">The bicarbonate-carbonic acid buffer works in a fashion similar to phosphate buffers. The bicarbonate is regulated in the blood by sodium, as are the phosphate ions. When sodium bicarbonate (NaHCO<sub>3<\/sub>), comes into contact with a strong acid, such as HCl, carbonic acid (H<sub>2<\/sub>CO<sub>3<\/sub>), which is a weak acid, and NaCl are formed. When carbonic acid comes into contact with a strong base, such as NaOH, bicarbonate and water are formed.<\/p>\n<div id=\"eip-515\" data-type=\"equation\">\n<div class=\"MathJax_Display\" style=\"text-align: center\">\n<p style=\"text-align: center\"><span id=\"MathJax-Span-139\" class=\"math\"><span id=\"MathJax-Span-140\" class=\"mrow\"><span id=\"MathJax-Span-141\" class=\"semantics\"><span id=\"MathJax-Span-142\" class=\"mrow\"><span id=\"MathJax-Span-143\" class=\"mrow\"><span id=\"MathJax-Span-148\" class=\"mtext\">NaHCO<sub>3<\/sub> + HCl\u00a0<\/span><span id=\"MathJax-Span-149\" class=\"mrow\"><span id=\"MathJax-Span-150\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-151\" class=\"msub\"><span id=\"MathJax-Span-152\" class=\"mrow\"><span id=\"MathJax-Span-153\" class=\"mtext\"> H<sub>2<\/sub>CO<sub>3<\/sub><\/span><\/span><\/span><span id=\"MathJax-Span-159\" class=\"mtext\">+NaCl<\/span><\/span><\/span><\/span><\/span><\/span><\/p>\n<p style=\"text-align: center\"><span id=\"MathJax-Span-160\" class=\"math\"><span id=\"MathJax-Span-161\" class=\"mrow\"><span id=\"MathJax-Span-162\" class=\"semantics\"><span id=\"MathJax-Span-163\" class=\"mrow\"><span id=\"MathJax-Span-164\" class=\"mrow\"><span id=\"MathJax-Span-165\" class=\"mtext\">(sodium bicarbonate) + (strong acid)\u00a0<\/span><span id=\"MathJax-Span-166\" class=\"mrow\"><span id=\"MathJax-Span-167\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-168\" class=\"mtext\"> (weak acid) + (salt)<\/span><\/span><\/span><\/span><\/span><\/span><\/p>\n<p style=\"text-align: center\"><span id=\"MathJax-Span-181\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">H<sub>2<\/sub>CO<sub>3<\/sub> + NaOH<\/span><span id=\"MathJax-Span-182\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-183\" class=\"mo\">\u2192NaHCO<sub>3<\/sub><\/span><\/span><span id=\"MathJax-Span-189\" class=\"msub\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-190\" class=\"mrow\"><span id=\"MathJax-Span-191\" class=\"mtext\">\u00a0+\u00a0H<\/span><\/span><sub><span id=\"MathJax-Span-192\" class=\"mtext\">2<\/span><\/sub><\/span><span id=\"MathJax-Span-193\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">O<\/span><\/p>\n<\/div>\n<div class=\"MathJax_Display\" style=\"text-align: center\"><span id=\"MathJax-Span-199\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">(weak acid) + (strong base)<\/span><span id=\"MathJax-Span-200\" class=\"mrow\" style=\"text-align: initial;font-size: 1em\"><span id=\"MathJax-Span-201\" class=\"mo\">\u2192<\/span><\/span><span id=\"MathJax-Span-202\" class=\"mtext\" style=\"text-align: initial;font-size: 1em\">(sodium bicarbonate) + (water)<\/span><\/div>\n<\/div>\n<p id=\"fs-id1353864\">As with the phosphate buffer, a weak acid or weak base captures the free ions, and a significant change in pH is prevented. Bicarbonate ions and carbonic acid are present in the blood in a 20:1 ratio if the blood pH is within the normal range. With 20 times more bicarbonate than carbonic acid, this capture system is most efficient at buffering changes that would make the blood more acidic. This is useful because most of the body\u2019s metabolic wastes, such as lactic acid and ketone bodies, are acids. Carbonic acid levels in the blood are controlled by the expiration of CO<sub>2<\/sub>\u00a0through the lungs. In red blood cells, carbonic anhydrase forces the dissociation of the acid, rendering the blood less acidic. Because of this acid dissociation, CO<sub>2<\/sub>\u00a0is exhaled (see equations above). The level of bicarbonate in the blood is controlled through the renal system, where bicarbonate ions in the renal filtrate are conserved and passed back into the blood. However, the bicarbonate buffer is the primary buffering system of the IF surrounding the cells in tissues throughout the body.<\/p>\n<\/section>\n<\/section>\n<h2 data-type=\"title\">Respiratory Regulation of Acid-Base Balance<\/h2>\n<p>The respiratory system contributes to the balance of acids and bases in the body by regulating the blood levels of carbonic acid (<a href=\"#BloodpHRespiratoryRegulation\">Respiratory Regulation of Blood pH<\/a>). CO<sub>2\u00a0<\/sub>in the blood readily reacts with water to form carbonic acid, and the levels of CO<sub>2\u00a0<\/sub>and carbonic acid in the blood are in equilibrium. When the CO<sub>2\u00a0<\/sub>level in the blood rises (as it does when you hold your breath), the excess CO<sub>2<\/sub>\u00a0reacts with water to form additional carbonic acid, lowering blood pH. Increasing the rate and\/or depth of respiration (which you might feel the \u201curge\u201d to do after holding your breath) allows you to exhale more CO<sub>2<\/sub>. The loss of CO<sub>2<\/sub>\u00a0from the body reduces blood levels of carbonic acid and thereby adjusts the pH upward, toward normal levels. As you might have surmised, this process also works in the opposite direction. Excessive deep and rapid breathing (as in hyperventilation) rids the blood of CO<sub>2<\/sub>\u00a0and reduces the level of carbonic acid, making the blood too alkaline. This brief alkalosis can be remedied by rebreathing air that has been exhaled into a paper bag. Rebreathing exhaled air will rapidly bring blood pH down toward normal.<a id=\"BloodpHRespiratoryRegulation\"><\/a><\/p>\n<figure id=\"attachment_9608\" aria-describedby=\"caption-attachment-9608\" style=\"width: 424px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-9608\" src=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2714_Respiratory_Regulation_of_Blood.jpg\" alt=\"This top to bottom flowchart describes the regulation of PH in the blood. The left branch shows acidosis, which is when the PH of the blood drops. Acidosis stimulates brain and arterial receptors, triggering an increase in respiratory rate. This causes a drop in blood CO two and H two CO three. A drop in these two acidic compounds causes the blood PH to rise back to homeostatic levels. The right branch shows alkalosis which is when the PH of the blood rises. Alkalosis also stimulates brain and arterial receptors, but these now trigger a decrease in respiratory rate. This causes an increase in blood CO two and H two CO three, which lowers the PH of the blood back to homeostatic levels.\" width=\"424\" height=\"773\" srcset=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2714_Respiratory_Regulation_of_Blood.jpg 495w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2714_Respiratory_Regulation_of_Blood-164x300.jpg 164w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2714_Respiratory_Regulation_of_Blood-65x119.jpg 65w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2714_Respiratory_Regulation_of_Blood-225x410.jpg 225w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2714_Respiratory_Regulation_of_Blood-350x638.jpg 350w\" sizes=\"auto, (max-width: 424px) 100vw, 424px\" \/><figcaption id=\"caption-attachment-9608\" class=\"wp-caption-text\"><strong>Respiratory Regulation of Blood pH\u00a0<\/strong>&#8211; The respiratory system can reduce blood pH by removing CO<sub>2<\/sub> from the blood.<\/figcaption><\/figure>\n<p>The chemical reactions that regulate the levels of CO<sub>2<\/sub>\u00a0and carbonic acid occur in the lungs when blood travels through the lung\u2019s pulmonary capillaries. Minor adjustments in breathing are usually sufficient to adjust the pH of the blood by changing how much CO<sub>2<\/sub>\u00a0is exhaled. In fact, doubling the respiratory rate for less than 1 minute, removing \u201cextra\u201d CO<sub>2<\/sub>, would increase the blood pH by 0.2. This situation is common if you are exercising strenuously over a period of time. To keep up the necessary energy production, you would produce excess CO<sub>2<\/sub>\u00a0(and lactic acid if exercising beyond your aerobic threshold). In order to balance the increased acid production, the respiration rate goes up to remove the CO<sub>2<\/sub>. This helps to keep you from developing acidosis.<\/p>\n<p>The body regulates the respiratory rate by the use of chemoreceptors, which primarily use CO<sub>2<\/sub>\u00a0as a signal. Peripheral blood sensors are found in the walls of the aorta and carotid arteries. These sensors signal the brain to provide immediate adjustments to the respiratory rate if CO<sub>2\u00a0<\/sub>levels rise or fall. Yet other sensors are found in the brain itself. Changes in the pH of CSF affect the respiratory center in the medulla oblongata, which can directly modulate breathing rate to bring the pH back into the normal range.<\/p>\n<p><span id=\"term-00001\" data-type=\"term\">Hypercapnia<\/span>, or abnormally elevated blood levels of CO<sub>2<\/sub>, occurs in any situation that impairs respiratory functions, including pneumonia and congestive heart failure. Reduced breathing (hypoventilation) due to drugs such as morphine, barbiturates, or ethanol (or even just holding one\u2019s breath) can also result in hypercapnia.\u00a0<span id=\"term-00002\" data-type=\"term\">Hypocapnia<\/span>, or abnormally low blood levels of CO<sub>2<\/sub>, occurs with any cause of hyperventilation that drives off the CO<sub>2<\/sub>, such as salicylate toxicity, elevated room temperatures, fever, or hysteria.<\/p>\n<h2 data-type=\"title\">Renal Regulation of Acid-Base Balance<\/h2>\n<p>The renal regulation of the body\u2019s acid-base balance addresses the metabolic component of the buffering system. Whereas the respiratory system (together with breathing centers in the brain) controls the blood levels of carbonic acid by controlling the exhalation of CO<sub>2<\/sub>, the renal system controls the blood levels of bicarbonate. A decrease of blood bicarbonate can result from the inhibition of carbonic anhydrase by certain diuretics or from excessive bicarbonate loss due to diarrhea. Blood bicarbonate levels are also typically lower in people who have Addison\u2019s disease (chronic adrenal insufficiency), in which aldosterone levels are reduced, and in people who have renal damage, such as chronic nephritis. Finally, low bicarbonate blood levels can result from elevated levels of ketones (common in unmanaged diabetes mellitus), which bind bicarbonate in the filtrate and prevent its conservation.<\/p>\n<p>Bicarbonate ions, HCO<sub>3<\/sub><sup>&#8211;<\/sup>, found in the filtrate, are essential to the bicarbonate buffer system, yet the cells of the tubule are not permeable to bicarbonate ions. The steps involved in supplying bicarbonate ions to the system are seen in <a href=\"#KidneyBicarbonateConservation\">Conservation of Bicarbonate in the kidney <\/a>and are summarized below:<\/p>\n<ul id=\"fs-id1414107\">\n<li>Step 1: Sodium ions are reabsorbed from the filtrate in exchange for H<sup>+<\/sup>\u00a0by an antiport mechanism in the apical membranes of cells lining the renal tubule.<\/li>\n<li>Step 2: The cells produce bicarbonate ions that can be shunted to peritubular capillaries.<\/li>\n<li>Step 3: When CO<sub>2<\/sub>\u00a0is available, the reaction is driven to the formation of carbonic acid, which dissociates to form a bicarbonate ion and a hydrogen ion.<\/li>\n<li>Step 4: The bicarbonate ion passes into the peritubular capillaries and returns to the blood. The hydrogen ion is secreted into the filtrate, where it can become part of new water molecules and be reabsorbed as such, or removed in the urine.<a id=\"KidneyBicarbonateConservation\"><\/a><\/li>\n<\/ul>\n<div id=\"fig-ch27_04_03\" class=\"os-figure\">\n<figure data-id=\"fig-ch27_04_03\"><\/figure>\n<figure data-id=\"fig-ch27_04_03\">\n<figure id=\"attachment_9610\" aria-describedby=\"caption-attachment-9610\" style=\"width: 824px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-9610\" src=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-1024x602.jpg\" alt=\"This diagram depicts a cross section of the left wall of a kidney proximal tubule. The wall is composed of two block-shaped cells arranged vertically one on top of each other. The lumen of the proximal tubule is to the left of the two cells. Yellow-colored urine is flowing through the lumen. There is a small strip of blue interstitial fluid to the right of the two cells. To the right of the interstitial fluid is a cross section of a blood vessel. A loop of chemical reactions is occurring in the diagram. Within the lumen of the proximal tubule, HCO three minus is combining with an H plus ion that enters the lumen from a proximal tubule cell. This reaction forms H two CO three. H two CO three then breaks into H two O and CO two, a reaction catalyzed by the enzyme carbonic anhydrase. The CO two then moves from the lumen of the proximal tubule into one of the proximal tubule cells. There, the reaction runs in reverse, with CO two combining with H two O to form H two CO three. The H two CO three then splits into H plus and HCO three minus. The H plus moves into the lumen, reinitiating the first step of the loop. The HCO three minus leaves the proximal tubule cell and enters the blood stream.\" width=\"824\" height=\"484\" srcset=\"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-1024x602.jpg 1024w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-300x176.jpg 300w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-768x452.jpg 768w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-65x38.jpg 65w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-225x132.jpg 225w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney-350x206.jpg 350w, https:\/\/pressbooks.bccampus.ca\/pathology\/wp-content\/uploads\/sites\/1260\/2025\/08\/2715_Conservation_of_Bicarbonate_in_Kidney.jpg 1471w\" sizes=\"auto, (max-width: 824px) 100vw, 824px\" \/><figcaption id=\"caption-attachment-9610\" class=\"wp-caption-text\"><strong>Conservation of Bicarbonate in the Kidney<\/strong> &#8211; Tubular cells are not permeable to bicarbonate; thus, bicarbonate is conserved rather than reabsorbed. Steps 1 and 2 of bicarbonate conservation are indicated.<\/figcaption><\/figure>\n<\/figure>\n<\/div>\n<p>It is also possible that salts in the filtrate, such as sulfates, phosphates, or ammonia, will capture hydrogen ions. If this occurs, the hydrogen ions will not be available to combine with bicarbonate ions and produce CO<sub>2<\/sub>. In such cases, bicarbonate ions are not conserved from the filtrate to the blood, which will also contribute to a pH imbalance and acidosis.<\/p>\n<p>The hydrogen ions also compete with potassium to exchange with sodium in the renal tubules. If more potassium is present than normal, potassium, rather than the hydrogen ions, will be exchanged, and increased potassium enters the filtrate. When this occurs, fewer hydrogen ions in the filtrate participate in the conversion of bicarbonate into CO<sub>2<\/sub>\u00a0and less bicarbonate is conserved. If there is less potassium, more hydrogen ions enter the filtrate to be exchanged with sodium and more bicarbonate is conserved.<\/p>\n<p>Chloride ions are important in neutralizing positive ion charges in the body. If chloride is lost, the body uses bicarbonate ions in place of the lost chloride ions. Thus, lost chloride results in an increased reabsorption of bicarbonate by the renal system.<\/p>\n<div id=\"fs-id1473396\" class=\"anatomy disorders ui-has-child-title\" data-type=\"note\">\n<header>\n<h2 data-type=\"title\">DISORDERS OF THE&#8230;<\/h2>\n<\/header>\n<section>\n<div class=\"os-note-body\">\n<h3 class=\"os-subtitle\" data-type=\"title\"><span class=\"os-subtitle-label\">Acid-Base Balance: Ketoacidosis<\/span><\/h3>\n<p>Diabetic acidosis, or ketoacidosis, occurs most frequently in people with poorly controlled diabetes mellitus. When certain tissues in the body cannot get adequate amounts of glucose, they depend on the breakdown of fatty acids for energy. When acetyl groups break off the fatty acid chains, the acetyl groups then non-enzymatically combine to form ketone bodies, acetoacetic acid, beta-hydroxybutyric acid, and acetone, all of which increase the acidity of the blood. In this condition, the brain isn\u2019t supplied with enough of its fuel\u2014glucose\u2014to produce all of the ATP it requires to function. Ketoacidosis can be severe and, if not detected and treated properly, can lead to diabetic coma, which can be fatal. A common early symptom of ketoacidosis is deep, rapid breathing as the body attempts to drive off CO<sub>2<\/sub> and compensate for the acidosis. Another common symptom is fruity-smelling breath, due to the exhalation of acetone. Other symptoms include dry skin and mouth, a flushed face, nausea, vomiting, and stomach pain. Treatment for diabetic coma is ingestion or injection of sugar; its prevention is the proper daily administration of insulin. A person who is diabetic and uses insulin can initiate ketoacidosis if a dose of insulin is missed. Among people with type 2 diabetes, those of Hispanic and African-American descent are more likely to go into ketoacidosis than those of other ethnic backgrounds, although the reason for this is unknown.<\/p>\n<h1>Adaption<\/h1>\n<p>This chapter was adapted by Carter Allen from the following text:<a href=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\" target=\"_blank\" rel=\"noopener\">Acid Base Balance<\/a>\u00a0<strong>in\u00a0<\/strong><a href=\"https:\/\/openstax.org\/books\/anatomy-and-physiology\/\">Anatomy and Physiology<\/a>\u00a0by\u00a0OSCRiceUniversity\u00a0is licensed under a\u00a0<a href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">Creative Commons Attribution 4.0 International License<\/a><\/p>\n<\/div>\n<\/section>\n<\/div>\n<div class=\"media-attributions clear\" prefix:cc=\"http:\/\/creativecommons.org\/ns#\" prefix:dc=\"http:\/\/purl.org\/dc\/terms\/\"><h2>Media Attributions<\/h2><ul><li about=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\"><a rel=\"cc:attributionURL\" href=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\" property=\"dc:title\">2713_pH_Scale<\/a>  &copy;  OSCRiceUniversity    is licensed under a  <a rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY (Attribution)<\/a> license<\/li><li about=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\"><a rel=\"cc:attributionURL\" href=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\" property=\"dc:title\">2714_Respiratory_Regulation_of_Blood<\/a>  &copy;  OSCRiceUniversity    is licensed under a  <a rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY (Attribution)<\/a> license<\/li><li about=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\"><a rel=\"cc:attributionURL\" href=\"https:\/\/openstax.org\/books\/anatomy-and-physiology-2e\/pages\/26-4-acid-base-balance\" property=\"dc:title\">2715_Conservation_of_Bicarbonate_in_Kidney<\/a>  &copy;  OSCRiceUniversity    is licensed under a  <a rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY (Attribution)<\/a> license<\/li><\/ul><\/div>","protected":false},"author":1076,"menu_order":4,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":["j-gordon-betts-xthrkeeivi-8fx5ggejmj","kelly-a-young-oshuupwjvs","james-a-wise-d1yrtemlzk","eddie-johnson-ljviofnjlc-pdgaajcn0a","brandon-poe-ahwkqiu5bv-wmotbmjnbo","dean-h-kruse-fjrrkqc7wi","oksana-korol-wz71t6zrpc-kgysk8vqqd","jody-e-johnson-gmyqec8nhu","mark-womble-9aswiv74hr-r7kvbmoxfk","peter-desaix-fikwt3tlhg"],"pb_section_license":""},"chapter-type":[],"contributor":[252,97,297,314,132,137,131,403,453,149],"license":[],"class_list":["post-7693","chapter","type-chapter","status-publish","hentry","contributor-brandon-poe-ahwkqiu5bv-wmotbmjnbo","contributor-dean-h-kruse-fjrrkqc7wi","contributor-eddie-johnson-ljviofnjlc-pdgaajcn0a","contributor-j-gordon-betts-xthrkeeivi-8fx5ggejmj","contributor-james-a-wise-d1yrtemlzk","contributor-jody-e-johnson-gmyqec8nhu","contributor-kelly-a-young-oshuupwjvs","contributor-mark-womble-9aswiv74hr-r7kvbmoxfk","contributor-oksana-korol-wz71t6zrpc-kgysk8vqqd","contributor-peter-desaix-fikwt3tlhg"],"part":7690,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/pressbooks\/v2\/chapters\/7693","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/wp\/v2\/users\/1076"}],"version-history":[{"count":16,"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/pressbooks\/v2\/chapters\/7693\/revisions"}],"predecessor-version":[{"id":9805,"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/pressbooks\/v2\/chapters\/7693\/revisions\/9805"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/pressbooks\/v2\/parts\/7690"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/pressbooks\/v2\/chapters\/7693\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/wp\/v2\/media?parent=7693"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/pressbooks\/v2\/chapter-type?post=7693"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/wp\/v2\/contributor?post=7693"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/pathology\/wp-json\/wp\/v2\/license?post=7693"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}