At a constant temperature,if the molarity (M) | vedclass

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(C) Given that molarity $(M)$ = molality $(m)$.Formula for molarity: $M = \frac{n_2 	imes 1000}{V_{sol} (mL)}$Formula for molality: $m = \frac{n_2

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$d = \frac{50 + 3M}{50}$

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(C) Given that molarity $(M)$ = molality $(m)$.Formula for molarity: $M = \frac{n_2 	imes 1000}{V_{sol} (mL)}$Formula for molality: $m = \frac{n_2 	imes 1000}{W_1 (g)}$Since $M = m$,it implies $V_{sol} (mL) = W_1 (g)$,where $W_1$ is the mass of the solvent (water).The mass of the solution $(W_{sol})$ = $W_1 + W_2$,where $W_2$ is the mass of urea ($NH_2CONH_2$,molar mass = $60 \ g/mol$).$W_2 = M 	imes 60 	imes \frac{V_{sol}}{1000} = \frac{60M 	imes V_{sol}}{1000} = 0.06M 	imes V_{sol}$.Density $(d)$ = $\frac{W_{sol}}{V_{sol}} = \frac{W_1 + W_2}{V_{sol}} = \frac{V_{sol} + 0.06M 	imes V_{sol}}{V_{sol}} = 1 + 0.06M$.$d = 1 + \frac{6M}{100} = 1 + \frac{3M}{50} = \frac{50 + 3M}{50}$.

At a constant temperature,if the molarity $(M)$ and molality $(m)$ of an aqueous solution of urea are equal,which of the following options is correct for the density $(d)$ of the solution?

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