Question

Consider an aqueous solution, $0.1$M each in HOCN, HCCOH, $(COOH{)}_2$ and $H_{3}P{O}_4$, for HOCN, we can write $K_a\left(HOCN\right)=\frac{\left[H^{+}\right]\left[OC{N}^{-}\right]}{\left[HOCN\right]}$. $\left[H^{+}\right]$ in this expression refers to:

• A. $H^{+}$ ions released by HOCN
• B. sum of $H^{+}$ ions released by all monoprotic acids
• C. sum of $H^{+}$ ions released only the first dissociation of all the acids
• D. overall $H^{+}$ ion concentration in the solution

Answer 1

The correct option is D overall $H^{+}$ ion concentration in the solution

Since all are in same aqueous solution

hence $H^{+}$ in this expression refer to overall $H^{+}$ ion concentration in solution.

Hence option D is correct option