Arrange the following solutions in the decreasing order of pOH: (A) 0.01 M HCl (B) 0.01 M NaOH (C) 0.01 M CH3COONa (D)…
Ionic Equilibrium · Class 11 · JEE Main Previous Year Question
Arrange the following solutions in the decreasing order of pOH:
(A) 0.01 M HCl (B) 0.01 M NaOH (C) 0.01 M (D) 0.01 M NaCl
- a
(A) > (C) > (D) > (B)
- b✓
(A) > (D) > (C) > (B)
- c
(B) > (C) > (D) > (A)
- d
(B) > (D) > (C) > (A)
(A) > (D) > (C) > (B)
pOH = 14 − pH. Higher pOH = lower pH = more acidic.
Step 1 — Determine pH of each:
(A) 0.01 M HCl: Strong acid, pH = 2 pOH = 12 (highest pOH)
(B) 0.01 M NaOH: Strong base, pH = 12 pOH = 2 (lowest pOH)
(C) 0.01 M : Salt of weak acid + strong base basic, pH ≈ 8.4 pOH ≈ 5.6
(D) 0.01 M NaCl: Neutral salt, pH = 7 pOH = 7
Step 2 — Decreasing order of pOH:
Answer: Option (2) — (A) > (D) > (C) > (B)
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