Question

The density in g $m{L}^{-1}$ of a 3.6 M sulphuric acid solution, that is $29\%H_{2}S{O}_4$ (molar mass = 98 g $mo{l}^{-1}$) by mass will be:

• A. 1.45
• B. 1.65
• C. 1.88
• D. 1.22

Answer 1

The correct option is D 1.22

$\begin{array}{c}\text{No of moles of}{H}_2{SO}_4\text{in acid}=3.6mol/L\\ \text{Volume of Solution,}V=1L=1000ml\\ \text{Mass of}{H}_2{SO}_4\text{in solution}\begin{array}{cc}& \\ & =3.6\times 98\\ & =352.8g\end{array}\end{array}$

$\begin{array}{c}\text{If density of solution is d then}\\ \text{Mass of}1L\text{solution}=1000ml\times d\\ \text{Mass}\%\text{of}{H}_2{SO}_4=\frac{352.8}{1000\times d}\times 100\end{array}$

$\begin{array}{cc}29& =\frac{35.28}{d}g/mL\\ d& =1.22g/ml\\ \text{Hence option}& \left(D\right)\text{is correct}\end{array}$