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# The density (in $gml^{-1}$) of a 3.60M sulphuric acid solution that is 29% $H_2SO_4$.(Molar mass=98$gmol^{-1}$) by mass will be

$(a)\;1.64\qquad(b)\;1.88\qquad(c)\;1.22\qquad(d)\;1.45$

Mass % of $H_2SO_4=29\%$
(i.e) 100g solution contains 29g $H_2SO_4$
Let the density of solution (in g/ml) is d
Molarity of solution=$\large\frac{\text{Moles of }H_2SO_4}{\text{Volume of solution(ml)}}$$\times 1000 (M=3.60) \large\frac{\Large\frac{29}{98}}{\Large\frac{100}{d}}$$\times 1000=3.60$
$d=1.22g/ml$
Hence (c) is the correct answer.