Question

The density (in $gm{L}^{-1}$ ) of a $3.60M$ sulphuric acid solution that is $29\%H_{2}S{O}_4$ (molar mass $=98gmo{l}^{-1}$ ) by mass, will be

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

Answer 1

Answer: (D)

$3.6M$ solution means $3.6$ moles of $H_{2}S{O}_4$ is present in $1000mL$ of solution.

$\Rightarrow$ Mass of $3.6$ moles of $H_{2}S{O}_4=3.6\times 98g=352.8g$

$\Rightarrow$ Mass of $H_{2}S{O}_4$ in $1000mL$ of solution $=352.8g$

Given, $29g$ of $H_{2}S{O}_4$ is present in $100g$ of solution $(29\%H_{2}S{O}_4$ by mass)

$\Rightarrow 352.8g$ of $H_{2}S{O}_4$ is present in $\frac{100}{29}\times 352.8=1216g$ of solution

Now, density $=\frac{\text{ Mass }}{\text{ Volume }}$

$=\frac{1216}{1000}=1.216g/mL=1.22g/mL$