For a buffer with a pKa of 4.76, if the pH equals the pKa, what is the ratio of salt to weak acid?

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Multiple Choice

For a buffer with a pKa of 4.76, if the pH equals the pKa, what is the ratio of salt to weak acid?

Explanation:
The key idea is the Henderson–Hasselbalch relationship, which links pH to the ratio of conjugate base to weak acid: pH = pKa + log([A-]/[HA]). If pH equals pKa, the log term must be zero, so [A-]/[HA] = 1. That means the salt (conjugate base form) and the weak acid form are present in equal amounts, giving a 1:1 ratio.

The key idea is the Henderson–Hasselbalch relationship, which links pH to the ratio of conjugate base to weak acid: pH = pKa + log([A-]/[HA]). If pH equals pKa, the log term must be zero, so [A-]/[HA] = 1. That means the salt (conjugate base form) and the weak acid form are present in equal amounts, giving a 1:1 ratio.

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