Acid/Base Balance
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| show | a logarithmic scale from 0-14; low end => acidic => high H+ concentration; ph 7 = neutral; pH = -log (H+) = log 1/(H+)
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| what is the normal pH of arterial blood? | show 🗑
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| what is the normal pH of urine? | show 🗑
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| what is the most powerful regulator of pH? | show 🗑
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| show | when cells make ATP, they produce CO2; CO2 can combine with water from red blood cells to produce carbonic acid (H2CO3)
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| what is the chemical equation for the formation of carbonic acid? | show 🗑
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| what is a volatile acid? | show 🗑
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| show | in the lungs, the carbonic acid reaction reverses; carbonic acid reforms into H2O & CO2; the CO2 will be removed and exhaled
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| show | volatile acids; specifically carbonic acid which dissociates into water and CO2, which is then exhaled
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| what is non-volatile acid? | show 🗑
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| how prevalent are non-volatile acids? | show 🗑
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| show | 1) buffers 2) kidneys, 3) respiratory system
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| how do buffers regulate free H+ concentrations? | show 🗑
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| how does the respiratory system regulate H+ concentration? | show 🗑
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| how do the kidneys regulate free H+ concentrations? | show 🗑
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| show | 2 chemical components; a weak acid and a weak base
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| show | to minimize potential pH changes that would result from the addition of strong acids/bases to body fluids
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| show | any molecule that can REVERSIBLY bind or release free H+
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| show | X + H+ <=> XH, where X is the buffer
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| where can free H+ bind with buffers? | show 🗑
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| show | phosphates (primary buffer in urine) and proteins (primary buffer inside cells; hemoglobin primary buffer inside RBC)
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| show | bicarbonate
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| show | carbonic acid (H2CO3) is the weak acid; sodium bicarbonate (NaHCO3) is the weak base
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| show | NaHCO3 + HCl => H2CO3 + NaCl
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| show | H2CO3 + NaOH => NaHCO3 + H2O
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| show | its weak acid component is regulated by the lungs and its weak base component is regulated by the kidneys
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| why do buffer systems work in pairs? | show 🗑
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| what is acidosis? | show 🗑
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| show | there is an increase of CO2 in the blood (which is a weak acid)
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| what is the catalyst that acts to dissociate carbonic acid, as well as to recombine its components back to carbonic acid? | show 🗑
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| what occurs during metabolic acidosis? | show 🗑
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| show | most important - loss of bicarbonate in diarrhea; also, kidney failure, formation of excess metabolic acids in body, ingestion of acids (such as aspirin, methyl alcohol)
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| show | alkalosis is the presence of excess base; the weak acid of the buffer system must be able to release H+ ions; in respiratory alkalosis there is a decrease of CO2 in the blood; in metabolic alkalosis there is an increase of bicarbonate in the blood
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| what are the causes of metabolic alkalosis? | show 🗑
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| how does hemoglobin function as a buffer? | show 🗑
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| why is CO2 considered a weak acid or a potential acid? | show 🗑
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| how is CO2 detected in the blood? | show 🗑
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| what happens if the chemoreceptors detect a rise in CO2 in the blood? | show 🗑
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| show | response to acidosis is increase in respiratory rate (to expel CO2); response to alkalosis is to decrease respirator rate (to retain CO2)
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| how do the respiratory and renal systems work together during alkalosis? | show 🗑
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| what is the role of carbonic anhydrase in the respiratory system? | show 🗑
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| show | by secreting H+ or by reabsorbing HCO3-
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| what happens in the renal system during acidosis? | show 🗑
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| what happens in the renal system during alkalosis? | show 🗑
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| show | for every bicarbonate ion absorbed by the blood, there must be one H+ secreted into the renal tubule
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| what is the role of ammonia in the renal system? | show 🗑
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| show | HPO4 is the weak base, which accepts hydrogen ions to become H2PO4 (and then combines with sodium to become NaH2CO4) which is excreted; H2PO4 is the weak acid component, as it will donate its H+
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