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Home  >>  JEEMAIN and AIPMT  >>  Chemistry  >>  Solutions
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A sample of $H_2SO_4$ solution is labeled 98% by weight. What is the normality of acid, given that the density of $H_2SO_4$ solution is 1.8g/ml.

$\begin{array}{1 1}(a)\;16N\\(b)\;26N\\(c)\;36N\\(d)\;46N\end{array}$

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Answer: 36 N
Molarity (M) is defined as number of moles of solute dissolved in one litre (or one cubic decimetre) of solution, $M = \large\frac{\text{ Moles of solute }}{\text{Molarity Volume of solution in litre}}$
Normality is the product of the molarity of the solution times the number of valences taking place in a reaction.
Let the Volume be $ V = 1\;L = 1000\;mL$ Therefore mass of the solution $ = 1.8 \times 1000 = 1800\;g$
Mass of the solute $= 98\; \%\; \text{of}\; 1800 = 1764\;g$ and Molarity volume of solution in liter $= 98\;L$
$\Rightarrow$ Molarity $M = \large\frac{1764}{98}$$ = 18M$
Valence of $H_2SO_4 = 2$
$\Rightarrow$ Normality $ = 2 \times 18 = 36\;N$
answered Feb 12, 2014 by sreemathi.v
edited Jul 16, 2014 by balaji.thirumalai
 

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