The pH of NaOH solution is 12. Then the pH of H₂SO₄ solution having same molar concentration of NaOH solution is

            

Given data: It is given that the pH of NaOH solution is 12. Then the pH of $H_{2}S{O_{4 }}_{ }$solution having same molar concentration of $NaOH$ solution is:

Explanation: pH of any acid can be calculated by using the following formula:

$pH= -\log (H+) Here H+$ Here $H+$refers to the concentration of $H+$ ions or the Hydronium ions.

Firstly we need to see the dissociation of $H_{2}S{O}_4$ in water:

$H2SO4\left(aq\right)—\to 2H+\left(aq\right)+\left(SO\right(D{)}^2-\left(aq\right)$

Here it can be clearly observed that 1 moles of sulphuric acid gives rise to 2 moles of $H+$ ions.

Therefore, 0.01 moles of$H_{2}S{O}_4$ will give rise to 0.02 moles of$H+$ ions

Substituting the value of $H+$ in the formula,

$pH=-\log (0.0(B)$

which is equal to 1.698.

Hence the correct option is (C) 1.7