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A 6.90 M solution of KOH in water contains 30% by mass of KOH.Calculate the density of the KOH solution ?[Molar mass of KOH=$56g mol^{-1}$]

$\begin{array}{1 1}1.288gcm^{-3}\\2.288gcm^{-3}\\3.288gcm^{-3}\\4.288gcm^{-3}\end{array} $

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A 6.90M solution contains 6.90 mol KOH in 1000 $cm^3$ of the solution
Mass of 6.90 mol of KOH =$6.90\times 56$
$\Rightarrow 386.4g$
A 30% solution contains 30g of KOH present in 100g of solution.
$\therefore 386.4$ g of KOH is present in = $\large\frac{100\times 386.4}{30}$
$\Rightarrow 1288g$ of solution
Density of KOH solution =$\large\frac{\text{Mass}}{\text{Volume}}$
$\Rightarrow \large\frac{1288g}{1000cm^3}$
$\Rightarrow 1.288g cm^{-3}$
answered Aug 8, 2014 by sreemathi.v
 

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