Question

When 100 ml of $\frac{M}{10}{H}_2{SO}_4$ is mixed with 500 ml of $\frac{M}{10}$ NaOH then nature of resulting solution and normality of excess of reactant left is

• A. Acidic, $\frac{N}{5}$
• B. Basic, $\frac{N}{5}$
• C. Basic, $\frac{N}{20}$
• D. Acidic, $\frac{N}{10}$

Answer 1

The correct option is C Basic, $\frac{N}{20}$

Gram equivalent of $H_{2}S{O}_4$ = normality $\times$ volume (L)

=$\frac{\frac{1}{5}\times 100}{\frac{1000}{1}}=\frac{100}{5000}$

Gram equivalent of NaOH =$\frac{\frac{1}{10}\times 500}{1000}$

=0.05

nature of the solution will be basic as gram equivalent of NaOH are more

so after uses of 0.02 eq $H_{2}S{O}_4$ , eq left = 0.05 - 0.02

= 0.03(600ml/0.62)

so normality of excess react ant left is = $\frac{gramequivalent}{volume\left(L\right)}$

so option c is correct = $\frac{0.03}{0.6}$ = 0.05 N