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
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
Fear or excitement, generally cause on to breathe rapidly and it results in the decrease of CO2 concentration in blood. ...Silver nitrate solution is gradually added to an aqueous solution containing 0.01 M each of chloride, bromide and iodide...A saturated solution of silver benzoate (AgOCOC6H5) has pH of 8.6. Ka for benzoic acid is 5.0 × 10–5. The value of Ksp f...The species present in solution when CO2 is dissolved in water are...Liquid ammonia ionizes to slight extent. At −50°C, its self-ionization constant, K = [NH4+] [NH2−] = 10–30 M2. How many ...