Find out molarity of $H^{+}$ ions in $2$M, $500$ml of $H_{2}S{O}_4$ solution.

The correct option is B 4 M

$H_{2}S{O}_4\rightleftharpoons 2H^{+}+S{O}_4^{-}$

$1$ $:$ $2$

$500mL$ of $2M$ solution contains $1M{H}_{2}S{O}_4$ molecules. We see from dissociation reaction that $H_{2}S{O}_4:H^{+}$ ratio is $1:2$

Therefore, $2moles{H}^{+}$ ions are present in $500mL$ solution.

$500mLsolution\to 2moles{H}^{+}ions$

$1000mLsolution\to 4moles{H}^{+}ions$

$\therefore$ Molarity of $H^{+}$ ions is $4M$