Question

Concentrated aqueous sulphuric acid is $98 \% \,H _{2} SO _{4}$ by mass and has a density of $1.80 \,g .\, mL ^{-1}$ Volume of acid required to make $1$ litre of $0.1\, M \,H _{2} SO _{4}$ solution is:

• A. 11.10 mL
• B. 5.55 mL
• C. 16.65 mL
• D. 22.20 mL

Answer 1

Answer: (B)

$w_2=98 \,g , w_1=100\, g , d=1 . 8 \,g\, mL$
Volume of solution $=\frac{\text { Mass }}{\text { Density }}=\frac{100}{1 \cdot 8}=55 . 55 \,ML$
Molarity $=\frac{ w _2 \times 1000}{ M _2 \times V ( in\, mL )}$
$=\frac{98 \times 1000}{98 \times 55.55}=18 \,M$
Now, $M_1 V_1=M_2 V_2$
$18 \times V_1=0.1 \times 1000$
$\Rightarrow V_1=\frac{0.1 \times 1000}{18}=5.55\, mL$