Question

$2.5ml$ of $\frac{2}{5}M$ weak monoacidic base $(K_b={1\times 10}^{-12}$ at ${25}^{0}C)$ is titrated with $\frac{2}{5}M$ HCl in water at ${25}^{0}C$. The concentration of $H^{+}$ at equivalence point is: (${K_w=10}^{-14}$ at ${25}^{0}C$)

• A. ${3.7\times 10}^{-13}M$
• B. ${3.2\times 10}^{-7}M$
• C. ${3.2\times 10}^{-2}M$
• D. ${2.7\times 10}^{-2}M$

Answer 1

The correct option is D ${2.7\times 10}^{-2}M$

i.e $\left[H^{+}\right]=2.7\times {10}^{-2}$ Thus, option D is correct.