Ionic EquilibriumHard
Question
The solubility of Ag2CO3 in water at 25oC is 1 × 10-4 mole/litre. What is its solubility in 0.01 M Na2CO3 solution? Assume no hydrolysis of CO32- ion.
Options
A.6 × 10-6 mole/litre
B.4 × 10-5 mole/litre
C.10-5 mole /litre
D.2 × 10-5 mole/litre
Solution
Na2CO3 ⇋ 2Na+ + CO32-
2 × 0.01 0.01
Ag2CO3 ⇋ 2 Ag+ + CO32-
2x (x + 0.01) 0.01
Ksp = 4x2 (0.01)
Ksp = 4s3 = 4 × 10-12 = 4x2 (0.01) ⇒ x = 10-5
2 × 0.01 0.01
Ag2CO3 ⇋ 2 Ag+ + CO32-
2x (x + 0.01) 0.01
Ksp = 4x2 (0.01)
Ksp = 4s3 = 4 × 10-12 = 4x2 (0.01) ⇒ x = 10-5
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