Calculate the molarity of each of the following solutions: (a) $30 g$ of $C o (N O_{3})_{2} . 6 H_{2} O$ in $4.3 L$ of solution (b) $30 m L$ of $0.5 M H_{2} S O_{4}$ diluted to $500 m L$ .

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Solution

(a) Molarity $= \frac{M a s s o f s o l u t e}{M o l e c u l a r m a s s} \times \frac{1000}{V o l u m e o f s o l u t i o n (m L)}$

$= \frac{30}{291} \times \frac{1000}{4300}$

$= 0.024 M$

(b) $M_{1} V_{1} = M_{2} V_{2}$

$\Rightarrow (0.5) (30 m L) = (M_{2}) (500)$

$\Rightarrow M_{2} = 0.03 M$

Molarity of $H_{2} S O_{4} = 0.03 M$

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