What is the $pH$ of $0.005\left(M\right)H_{2}S{O}_4$ solutions?

The correct option is C $2$
$H_2{SO}_4$ is a strong, diprotic acid. The equation for its ionization is
$H_2{SO}_{4\left(aq\right)}⟶{2H}^{+}+{SO}_4^{2-}$
Since the equation tells us that each molecule of acid will produce $2$ hydrogen ions, the concentration of the $H^{+}$ ion must be $2$x$0.0050M$ or $0.010M$
Using the definition of $pH$=-log$H^{+}$=$-log\left(0.010M\right)$ =$2$