Question

Concentrated aqueous sulphuric acid is 98% $H_{2}S{O}_4$ by mass and has a density of 1.80 g.$m{L}^{-1}$. The volume of acid required to make 1 litre of 0.1 M $H_{2}S{O}_4$ solution is:

• A. $5.55ml$
• B. $11.10ml$
• C. $33.00ml$
• D. $22.20ml$

Answer 1

Answer: (A)

$5.55ml$

$9.8\%H_{2}S{O}_4$ by mass

Given, density =1.80 g/ml

1.80= $\frac{98}{Volume}$

$v=\frac{98}{1.80}$ $=54.44ml$

We know, M${}_1{V}_1$=M${}_2{V}_2$ ------(1)

Molarity of $98\%$ $H_{2}S{O}_4$= $\frac{98}{98}\times \frac{1000}{54.44}$ = 18.368M

Using equation (1)

$18.368$$\times$$V=0.1$ $\times$ $1$

$V=5.55ml$

Therefore, the correct option is $A$