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Home  >>  AIMS  >>  Class12  >>  Chemistry  >>  Liquid Solutions
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$8.0575 × 10^{–2}$ kg of Glauber’s salt ($Na_2SO_4.10H_2O$) is dissolved in water to obtain 1 $dm^3$ of a solution of density $1077.2 kgm^{–3}$. Calculate the molarity fraction of $Na_2SO_4$ in the solution.

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Wt. of Glauber’s salt $(w_1) = 8.057 \times 10^{–2} kg = 80.575 g$
Density of solution (d) = $1077.2 kg m^{–3} =$$\large\frac{1077.22\times 1000gm}{10^6cm^3}$
Volume (V) 1L=1000ml
Molarity of $Na_2SO_4 ⋅10H_2O =\large\frac{w}{M}\times \frac{1000}{V(in\;ml}$
$\Rightarrow \large\frac{80.575}{322}$$\times \frac{1000}{1000}$
$\Rightarrow 0.25ml\;lit^{-1}$
$\Rightarrow 0.25ml\;dm^{-3}$
$\Rightarrow 0.25M$
Hence (A) is the correct answer.
answered Jun 6, 2014 by sreemathi.v
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