PH of resulting solution when equal volumes of 0.1, M, NaOH and 0.01, M, HCl are mixed?

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6-2.Equilibrium-II (Ionic Equilibrium)

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What is the $pH$ of the resulting solution when equal volumes of $0.1\, M\, NaOH$ and $0.01\, M\, HCl$ are mixed?

A

$2$

B

$7$

C

$1.04$

D

$12.65$

(NEET-2015)

Solution

One mole of $NaOH$ is completely neutralised by one mole of $HCL$.

Hence, $0.01$ mole of $NaOH$ will be completely neutralised by $0.01$ mole of $HCL$.

$\Rightarrow\; NaOH$ left unneutralised $=0.1-0.01=0.09$ mol As equal volumes of two solutions are mixed,

$[\mathrm{OH}]^{-}=\frac{0.09}{2}=0.045 \mathrm{M} $

$ \Rightarrow \mathrm{pOH}=-\log (0.045)=1.35 $

$\therefore \mathrm{pH}=14-1.35=12.65$

Standard 11

Chemistry

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