Dissolving $120 \mathrm{g}$ of a compound of relative molar mass $60$ in $1000 \mathrm{g}$ of water gave a solution of density $1.12 \mathrm{g}/\mathrm{mL}.$The molarity of the solution is

Total mass of the solution$= 120 \mathrm{g} + 1000 \mathrm{g} = 1120 \mathrm{g}$

Volume of the solution, $V=\frac{m}{\rho }=\frac{1120\mathrm{g}}{1.12\mathrm{g}{\mathrm{mL}}^{-1}}=1000\mathrm{mL}=1.0\mathrm{L}$

Amount of compound, $n=\frac{m}{M}=\frac{120\mathrm{g}}{60\mathrm{g}{\mathrm{mol}}^{-1}}=2.0\mathrm{mol}$

 molarity of solution $M=\frac{n}{V}=\frac{2.0\mathrm{mol}}{1.0\mathrm{L}}=2.0\mathrm{M}$