Concentrated aqueous sulphuric acid 98% $H_{2} {S O}_{4}$ by mass has a density of 1.80 g $m L^{- 1} .$ Volume of acid required to make one litre of 0.1 M $m L^{- 1} .$ solution is

16.65 mL

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22.20 mL

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5.55 ml

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11.10 mL

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Solution

The correct option is D 5.55 ml
Given :
Concentrated aqueous sulphuric acid is $98 % H_{2} S_{2} O_{4}$ by mass
Density $- 1.80 g m / L$
Number of moles in $H_{2} S O_{4}$ of concentration in $0.1 M$ and volume $1 L$
$n = M \times V$
$\Rightarrow 0.1 \times 1 = 0.1 m o l$
Molecular mass of $H_{2} S O_{4} = 99 g$
Therefore ,
Mass of $0.1$ mole $H_{2} S O_{4} = 0.1 \times 98 = 9.8 g$
As we know that
density = $\frac{m a s s}{v o l u m e}$
$\Rightarrow$ Volume $= \frac{9.8}{1.80} = 5.44 m L$
Given that the solution is $98 %$ pure.
Therefore,
Volume required $= \frac{5.44}{98} \times 100 = 5.55 m L$ c
Hence the volume of acid required to make $1$ liter of $0.1\
M\ H_{2} SO_{4} $s o l u t i o n i s$ 5.55\ ml $

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