A building clad in marble is exposed to $3700\mathrm{L}$ of acid rain containing $\mathrm{H}{}_2\mathrm{SO}{}_4$ at $2.5\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}$ and $\mathrm{HNO}{}_3$ at $1.0\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}$. Assume both acids are fully dissociated (both protons of $\mathrm{H}{}_2\mathrm{SO}{}_4$) and all the acid reacts with $\mathrm{CaCO}{}_3$ according to $\mathrm{CaCO}{}_3+2\mathrm{H}{}^{+}\to \mathrm{Ca}{}^{2+}+\mathrm{H}{}_2\mathrm{O}+\mathrm{CO}{}_2$. Using molar mass of $\mathrm{CaCO}{}_3$ = 100 g/mol, calculate the mass of $\mathrm{CaCO}{}_3$ dissolved, in grams, to the nearest integer.

Numerical answer type, answer in g, tolerance 0.5.