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pH = 7.40 (initial buffer pH)
HCl (strong acid) will react with HCO3- (base).
HCO3-(aq) + HCl(aq) →H2CO3(aq) + Cl-(aq)
If x = concentration of HCl
Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3– and 0.0012 M H2CO3 (pKa1 for H2 CO3 at body temperature is 6.1). If the volume of blood in a normal adult is 5.0 L, what mass of HCl could be neutralized by the buffering system in blood before the pH fell below 7.0 (which would result in death)?
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Based on our data, we think this problem is relevant for Professor Ansari's class at PASADENA.