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# A sample of sulphuric acid is 98% $H_2SO_4$ by weight (density =$1.10gmL^{-1})$.Calculate Molarity

$\begin{array}{1 1}11.0M\\12.0M\\13.0M\\14.0M\end{array}$

98 % $H_2SO_4$ solution means that 98 g of $H_2SO_4$ are present in 100g of solution in water
Molarity =$\large\frac{\text{Moles of solute}}{\text{Volume of solution}}$
Moles of $H_2SO_4=\large\frac{98}{98}$$=1 Volume of solution =\large\frac{\text{Mass}}{\text{Density}} \Rightarrow \large\frac{100}{1.10}$$=90.9mL$
Molarity of $H_2SO_4=\large\frac{\text{Moles of }H_2SO_4}{\text{Volume of solution(mL)}}$$\times 1000 \Rightarrow \large\frac{1\times 1000}{90.9}$$=11.0M$