Find the pH of an aqueous solution formed on mixing equal volumes of $0.05M{H}_{2}S{O}_4$ and $0.1MHCl$ solution.

The correct option is A 1
Number of moles of $H^{+}$ coming from $H_{2}S{O}_4$ are,
$n_{H^{+}}=2\times 0.05\times V$
Number of moles of $H^{+}$ coming from $HCl$ are,
$n_{H^{+}}=0.1\times V$
Here final volume is $V_f=V+V=2VL$
So, final concentration of $H^{+}$ will be:

$C_f=\frac{(2\times 0.05\times V)+(0.1\times V)}{2V}=0.1MpH=-{\log }_{10}\left[0.1\right]pH=1$