NEET Chemistry Ionic Equilibrium Match the Following Question
Match Column-I with Column-II.
| Column-I | Column-II |
|---|---|
| (a) Ionization of water | (i) K = [H3O+][OH–] |
| (b) Common ion effect | (ii) Shift in equilibrium |
| (c) pH calculation | (iii) –log[H+] |
| (d) Weak base reaction | (iv) Produces OH– in solution |
a-i, b-ii, c-iii, d-iv
a-ii, b-i, c-iv, d-iii
a-iii, b-iv, c-i, d-ii
a-iv, b-iii, c-ii, d-i
Correct Answer
Detailed Explanation
The ionization of water is represented by the equation K = [H3O+][OH–], where water acts as both an acid and a base. The common ion effect leads to a shift in equilibrium, affecting the concentrations of ions. The pH calculation is done using the formula –log[H+], and weak bases like ammonia produce OH– in solution.
Found an issue with this question?
Related Questions
More from Ionic Equilibrium
More from
Assertion (A): For a dibasic acid H2X, the equilibrium constant for the first ionization step (Ka1) is generally greater than that for the second ioni...
Assertion (A): The solubility of a sparingly soluble salt is affected by the presence of a common ion. | Reason (R): The solubility product constant (...
Match Column-I with Column-II. Column-I Column-II (a) K c for H 2 + I 2 2HI (i) 57.0 (b) K c for N 2 + O 2 2NO (ii) 4.8 × 10 –31 (c) K...