$x \mathrm{mg}$ of pure HCl was used to make an aqueous solution. 25.0 mL of $0.1 \mathrm{M} \mathrm

Question

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

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