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A buffer solution has equal volumes of 0.2 M `NH_(4)OH` and 0.02 M `NH_(4)Cl`. The `pK_(b)` of the base is 5. The pH is
A. 10
B. 9
C. 4
D. 7

1 Answer

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Correct Answer - A
`pOH = pK_(b) + log.(["salt"])/(["base"])`
`= 5 + log.(0.02)/(0.2) = 5 + log.(1)/(10) = 5 + (-1) = 4`
`pH = 14 - pOH = 14 - 4 = 10`.

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