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# A 6.90M solution of KOH in water has 30% by weight of KOH. Calculate the density of the solution.

$(a)\;1.5g/ml\qquad(b)\;1.288g/ml\qquad(c)\;2.3g/ml\qquad(d)\;2.64g/ml$

KOH solution is 30% by weight
Weight of KOH=30g
Weight of the solution=100g
$\therefore$ Volume of the solution=$\large\frac{100}{d}$ ; where, $d$ is density of the solution.
Molarity = 6.90 = $\large\frac{30}{56\times \Large\frac{100}{1000\times d}}$
By solving, we obtain, d = 1.288g/ml
Hence (b) is the correct answer.
edited Mar 18, 2014