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

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Solution

$98 %$ by weight means, $98 g m H_{2} S O_{4}$ in $100 g m$ solution $(M) 98 g H_{2} S O_{$}$ in $2 g$ water
No:- of moles of $H_{2} S O_{4} = 98 / 98 = 1 d e n s i t y = 1.8 g / L v o l u m e$
Volume of the solution $=$ Mass of $s o l^{n} / D e n s i t y$
$= 100 / 1.8 = 55.55 m l$
$= 0.055 L$
Applying $M_{1} V_{1} = M_{2} V_{2} = 18.18 \times V_{1} = 0.1 \times 1 V_{1}$
$= 0.0055 L$
$L = 5.5 m l$
Hence, volume of acid required $= 5.5 m l$ .

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