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Q.
The density (in $g \,mL^{-1}$) of a $3.6\, M$ sulphuric acid solution that is $29\%\, H_2SO_4$ (Molar mass $= 98\, g\, mol^{-1})$ by mass will be :
Some Basic Concepts of Chemistry
Solution:
Let the density of solution be $'d'$
Molarity of solution given $= 3.6$
i.e., $1$ litre of solution contains $3.6$ moles of $H_2SO_4$ or $1$ litre
of solution contain $3.6 \times 98 \,g $ of $H_2SO_4$ Since, the solution
contains $29\%$ by mass.
$100 \,g$ solution contains $29 \,g \,H_2SO_4$
$\frac{100}{d}mL$ solution contains $29\, g$ of $H_2SO_4$
$1000 \,mL$ solution contains $3.6 \times 98\, g$ of $H_2SO_4$
$\therefore 3.6 \times 98 = \frac{29 \times d}{100} \times 1000$
$d = 1.22$