What is the pH of the resulting solution when equal volumes of $0.1 M N a O H$ and $0.01 M H C l$ are mixed?

7.0

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1.04

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12.65

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2.0

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Solution

The correct option is C 12.65
When equal volumes of $0.1 M N a O H$ and $0.01 M H C l$ are mixed, the hydroxide ion concentration is
$\frac{0.1 - 0.01}{2} = 0.045 M$

The pOH of the solution is
$p O H = - l o g [O H^{-}] = - l o g 0.045 = 1.35$
The pH of the solution is
$p H = 14 - p O H = 14 - 1.35 = 12.65$

Hence, option (c) is correct.

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