Question

A sample of $H_{2}S{O}_4$ (density $=1.4g/ml)$ is labelled as $49$% by weight. What volume of acid has to be used to make $1.0L$ of $0.2M{H}_{2}S{O}_4$ solution?

• A. $2000ml$
• B. $28.57ml$
• C. $13.6L$
• D. $1.12L$

Answer 1

The correct option is B $28.57ml$

Density =$1.4g/ml$

$100ml$ weight $1400g$

mass of $H_{2}S{O}_4=1400\times \frac{49}{100}=686g$

male of $H_{2}S{O}_4$=$\frac{686}{98}=7$

therefore molarity of stock solution $7M$

To prepare $1000ml$ of $0.2m$ solution :-

$M_1{V}_1=M_2{V}_2$

$7\times V_1=0.2\times 1000$

$V_1=28.57ml$

So option $B$ is correct.