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Question

One of the buffer systems used to control the pH of blood involves the equilibrium between H2PO4\mathrm{H}_2 \mathrm{PO}_4{ }^{-}and HPO42\mathrm{HPO}_4{ }^{2-}. The pKa\mathrm{p} K_{\mathrm{a}} for H2PO4\mathrm{H}_2 \mathrm{PO}_4^{-}is 7.21. (a) Write the Henderson-Hasselbalch equation for this buffer system. (b) What HPO42\mathrm{HPO}_4{ }^{2-} to H2PO4\mathrm{H}_2 \mathrm{PO}_4{ }^{-}ratio is needed to maintain the optimum blood pH of 7.40?

Solution

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Answered 2 years ago
Answered 2 years ago
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a) Dissociation of H2_2PO4_4^- in this system is as follows

H2_2PO4_4^- \rightarrow HPO42_4^{-2} + H+^+

From this equation we can right the Henderson-Hasselbalch equation as follows

pH=pKa+log[HPO42][H2PO4]\begin{align*} \text{pH} = \text{pKa} + \text{log} \frac{[\text{HPO}_4^{-2}]}{[\text{H}_2\text{PO}_4^{-}]}\\ \end{align*}

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