x mg of pure HCl was used to make an aqueous solution. 25.0 mL of 0.1 M Ba ( OH )_2 solution is used when the HCl solution was titrated against it.…

$\displaystyle x \mathrm{mg}$ of pure HCl was used to make an aqueous solution. $\displaystyle 25.0$ mL of $\displaystyle 0.1 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_2$ solution is used when the HCl solution was titrated against it. The numerical value of $\displaystyle x$ is $\displaystyle \_\_\_\_$ $\displaystyle \times 10^{-1}$. (Nearest integer) Given : Molar mass of HCl and $\displaystyle \mathrm{Ba}(\mathrm{OH})_2$ are $\displaystyle 36.5$ and $\displaystyle 171.0 \mathrm{~g} \mathrm{~mol}^{-1}$ respectively.