Question

Calculate the pH value of $0.01M$ $H_2{SO}_4$ solution.

($log2=0.3010$)

• A. $0.45$
• B. $0.55$
• C. $0.64$
• D. $1.699$

Answer 1

The correct option is D $1.699$

One mole of $H_{2}S{O}_4$ gives $2$ mole $H^{+}$ ions.

$\left[H^{+}\right]$ ion concentration in $0.01M{H}_{2}S{O}_4=0.01\times 2=0.02mole/l$

$pH=-log[2\times {10}^{-2}]=1.699$