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pH of a Solution

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Question

Calculate the pH of a solution which is 0.1 M in HA and 0.5M in NaA. Ka for HA is $1.8 \times 10^{- 6}$ ?

A

3

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B

4

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C

6.4

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D

10

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Solution

The correct option is C 6.4
$P N = P k a + log \frac{s a l t}{a c i d}$
$P n = - {log}_{10} (1.8 \times 10^{- 6}) + (\frac{0.5}{0.1})$
$= 5.74 + 0.6989$
$P N = 6.44$

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