Question

At 30°C, In which of the one litre solution, the solubility of Ag2CO3 (Solubility product = 8 × 10^-12) will be maximum :-
(a) 0.05M Na2CO3
(b) Pure water
(c) 0.05M AgNO3
(d) 0.05M NH3
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• Proper steps required.
• Full explanation required.​

Answer 1

Answer:

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(d) 0.05M NH3

Explanation:

Ag₂CO₃ ↔ 2Ag + CO$\frac{2}{3}$ -

Due to the common ion effect the solubility decreases so the solubility of Ag₂CO₃ would be greatest in 1 L of 0.05 M NH₃ due to the absence of common ion either Ag or CO$\frac{2}{3}$ -

Answer 2

Answer:-

We know,

The effect on ​equilibrium that occurs when a common ion (an ion that is already contained in the solution) is added to a solution is described by the common ion effect.

→The common ion effect generally decreases ​solubility of a solute.

In 0.05M Na₂CO₃:-

Due to common ion effect of CO₃⁻² ion,the solubility of Ag₂CO₃ will be less.

In pure water:-

Ag₂CO₃ ⇌ 2Ag⁺ + CO₃⁻²

In 0.05M NH₃:-

Ag₂CO₃ ⇌ 2Ag⁺ + CO₃⁻²

2Ag⁺ + 4NH₃⇌ 2Ag(NH₃)₂⁺

Overall reaction:

Ag₂CO₃ + NH₃⇌2Ag(NH₃)₂⁺  + CO₃⁻²  

We can see,a complex is formed.Due to the formation of this complex between the ammonium and silver ions,the solubility equilibrium is shifted in the forward direction.This increases the solubility of silver carbonate.

Hence,Ag₂CO₃  is maximum soluble in 0.05M NH₃.

Option(D) is correct.

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