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Given, Ka = 1 × 10⁻⁴ pKa = -log (1 × 10⁻⁴) = 4 From Henderson equation: pH = pKa + log [Salt]/[Acid] Putting the values: 5 = 4 + log [Salt]/[Acid] log [Salt]/[Acid] = 5 - 4 = 1 Taking antilog [Salt]/[Acid] = 10 = 10 : 1

1. 10 : 1
2. 1 : 10
3. 1 : 1
4. None of these

Correct answer: 10 : 1

Solution

Using the Henderson-Hasselbalch equation, the given pH and pKa values lead to a log ratio of 1, which corresponds to a [Salt]/[Acid] ratio of 10:1 after taking the antilog.

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