What will be the pH value of $0.02 M$ $H_{2} S O_{4}$ solution.

1.7

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1.4

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Solution

The correct option is B 1.4
$H_{2} S O_{4}$ dissociates into $2 H^{+}$ and $S O_{4}^{2 -}$ . Thus each $H_{2} S O_{4}$ molecule gives two $H^{+}$ ions.
So, $0.02 M$ of $H_{2} S O_{4}$ will give $2 \times 0.02 M$ $H^{+}$ ions.
Hence pH of the solution is given as-
$p H$ $=$ $- l o g [2 \times 0.02]$
$p H$ $=$ $- l o g [0.04]$
Hence $p H$ $=$ $1.4$

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