The ionization constant (K_a) of a certain we | vedclass

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(B) The Henderson-Hasselbalch equation for an acidic buffer is: $pH = pK_a + \log \frac{[salt]}{[acid]}$Given $K_a = 10^{-4}$,so $pK_a = - \log(10^{-4

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$10:1$

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(B) The Henderson-Hasselbalch equation for an acidic buffer is: $pH = pK_a + \log \frac{[salt]}{[acid]}$Given $K_a = 10^{-4}$,so $pK_a = - \log(10^{-4}) = 4$.Substituting the values into the equation: $5 = 4 + \log \frac{[salt]}{[acid]}$$\log \frac{[salt]}{[acid]} = 5 - 4 = 1$Taking the antilog on both sides: $\frac{[salt]}{[acid]} = 10^1 = 10$Therefore,the ratio of $[salt]$ to $[acid]$ is $10:1$.

The ionization constant $(K_a)$ of a certain weak acid is $10^{-4}$. What should be the $[salt]$ to $[acid]$ ratio if we have to prepare a buffer with $pH = 5$ using this acid and one of its salts?

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