Question

The density (in g $m{l}^{-1}$) of a $3.60$M sulphuric acid solution having $29\%$ $H_{2}S{O}_4$ [molar mass $=98$g $mo{l}^{-1}$] by mass, will be:

• A. $1.64$
• B. $1.88$
• C. $1.22$
• D. $1.45$

Answer 1

The correct option is C $1.22$

Let us consider the problem:

Mass % of $H_{2}S{O}_4=29\%$

Therefore $100g$ solution contains $29g{H}_{2}S{O}_4$

Let the density of solution $\left(ing/ml\right)$ is $d$

Molarity of solution $=\frac{\text{Moles of}{H}_{2}S{O}_4}{\text{Volume of solution(ml)}}\times 1000$

$\left(M=3.60\right)$

$\frac{\frac{29}{98}}{\frac{100}{d}}\times 1000=3.60$

Hence the answer is $d=1.22g/ml$.

Hence, the correct option is $C$