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Ionic Equilibrium question

2022 · 29 Jun · Shift 1 · Q3
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  5. /2022 · 29 Jun · Shift 1 · Q3

Ionic Equilibrium question

2022 · 29 Jun · Shift 1 · Q3

JEE MainChemistryIonic EquilibriumMCQ+4 / −1
The solubility of AgCl will be maximum in which of the following?
  1. A
    0.01 M KCl
  2. B
    0.01 M HCl
  3. C
    0.01 M AgNO3AgNO_3AgNO3​
  4. D
    Deionised water
View written solutionFree

Correct answer: D

  1. Write the solubility equilibrium of AgClAgClAgCl

    AgCl(s)⇌Ag++Cl−AgCl(s) \rightleftharpoons Ag^+ + Cl^-AgCl(s)⇌Ag++Cl−

    Its solubility product is Ksp=[Ag+][Cl−]K_{sp} = [Ag^+][Cl^-]Ksp​=[Ag+][Cl−]

  2. Use common ion effect

    The solubility of a sparingly soluble salt decreases in the presence of a common ion.

    Here, common ions are Ag+Ag^+Ag+ or Cl−Cl^-Cl−.

  3. Check each option

    A: 0.01 M KCl0.01\,M\ KCl0.01M KCl

    • Provides Cl−Cl^-Cl−, which is a common ion.
    • So solubility of AgClAgClAgCl decreases.

    B: 0.01 M HCl0.01\,M\ HCl0.01M HCl

    • HCl is a strong acid and gives Cl−Cl^-Cl− completely.
    • Again, Cl−Cl^-Cl− is a common ion.
    • So solubility decreases.

    C: 0.01 M AgNO30.01\,M\ AgNO_30.01M AgNO3​

    • Provides Ag+Ag^+Ag+, also a common ion.
    • So solubility decreases.

    D: Deionised water

    • No common ion is present.
    • Therefore, there is no suppression of solubility by common ion effect.
    • Hence solubility is maximum here.

  4. Conclusion

    Among all the given media, AgClAgClAgCl has the maximum solubility in deionised water.

  5. Comparison with stored answer

    Derived answer: D

    Stored correct answer: D

    They match.

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