The molarity of the solution prepared by dissolving 6.3 g of oxalic acid $\left(\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4 .2 \mathrm{H}_2 \mathrm{O}\right)$ in 250 mL of water in $\mathrm{mol} \mathrm{L}^{-1}$ is $\mathrm{x} \times 10^{-2}$. The value of x is $\_\_\_\_$ .
(Nearest integer) [Atomic mass : $\mathrm{H}: 1.0, \mathrm{C}: 12.0, \mathrm{O}: 16.0$ ]