An aqueous KCI solution of density


An aqueous $\mathrm{KCl}$ solution of density $1.20 \mathrm{~g} \mathrm{~mL}^{-1}$ has a molality of $3.30 \mathrm{~mol} \mathrm{~kg}^{-1}$. The molarity of the solution in $\mathrm{mol} \mathrm{L}^{-1}$ is (Nearest integer)

$[$ Molar mass of $\mathrm{KCl}=74.5]$


$1000 \mathrm{~kg}$ solvent has $3.3$ moles of $\mathrm{KCl}$

$1000 \mathrm{~kg}$ solvent $\longrightarrow 3.3 \times 74.5 \mathrm{gm} \mathrm{KCl}$

$\longrightarrow \quad 245.85$

Weight of solution $=1245.85 \mathrm{gm}$

Volume of solution $=\frac{1245.85}{1.2} \mathrm{ml}$

So molarity $=\frac{3.3 \times 1.2}{1245.85} \times 1000=3.17$

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