A solution was prepared by dissolving 0.8 mole of acetic acid, 0.7 mole of sodium acetate and 0.3 mole of NaOH . The pH of resultant solution would be
[Given : $K_{a} (C H_{3} COO H) = 2 \times 1 0^{- 5}$ ]

Question

A solution was prepared by dissolving 0.8 mole of acetic acid, 0.7 mole of sodium acetate and 0.3 mole of NaOH . The pH of resultant solution would be

[Given : $K_{a} (C H_{3} COO H) = 2 \times 1 0^{- 5}$ ]

TestHub · Accepted Answer

C H 3 ​ COO H + N a O H → C H 3 ​ COON a + H 2 ​ O 0.80.30.7 0.501 pH = pKa + lo g 0.5 1 ​ = pKa + lo g 2 pH = 5 − lo g 2 + lo g 2 pH = 5

Chemistry - Ionic Equilibrium Question with Solution | TestHub

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