Question:
What is the pH of 0.365% (w/V) HCl aqueous solution? (HCl=36.5 u), (log 0.365=−0.4377)
What is the pH of 0.365% (w/V) HCl aqueous solution? (HCl=36.5 u), (log 0.365=−0.4377)
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w/V to M: (g/100 mL) × 10 / MM for M. Strong acids: pH = -log M. Ignore distractor logs. Assume dilute for activity ≈ concentration.
Updated On: Mar 6, 2026
- 1.301
- 1.0
- 2.699
- 0.4377
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The Correct Option is B
Solution and Explanation
1. w/V % = 0.365 g HCl per 100 mL solution.
2. Concentration = 0.365 g / 0.1 L = 3.65 g/L.
3. Molarity M = 3.65 / 36.5 = 0.1 M.
4. HCl is strong acid, fully dissociates: [H$^+$] = 0.1 M.
5. pH = -log [H$^+$] = -log 0.1 = 1.0.
6. Given log 0.365 not needed; perhaps distractor. Therefore, the correct option is (2) 1.0.
2. Concentration = 0.365 g / 0.1 L = 3.65 g/L.
3. Molarity M = 3.65 / 36.5 = 0.1 M.
4. HCl is strong acid, fully dissociates: [H$^+$] = 0.1 M.
5. pH = -log [H$^+$] = -log 0.1 = 1.0.
6. Given log 0.365 not needed; perhaps distractor. Therefore, the correct option is (2) 1.0.
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