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A: Solubility of AgCI is more in NH3 tha...

A: Solubility of AgCI is more in `NH_3` than in pure water.
R : Common ion effect decreases the concentration of `CI^-` when `NH_3` is added to 0.1 m AgCI solution.

A

If both Assertion & Reason are true and the reason in the corret explanation of the assertion, then mark

B

If both assertion & Reason are true but the reason is not the correct explanation of the assertion, then mark

C

If Assertion is true statement but Reason is false then mark

D

If both Assertion and Reason are false statements , then mark

Text Solution

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The correct Answer is:
To solve the question, we need to analyze the statements provided regarding the solubility of AgCl in NH3 compared to pure water and the role of the common ion effect. ### Step-by-Step Solution: 1. **Understanding the Solubility of AgCl**: - AgCl (silver chloride) is a sparingly soluble salt. Its solubility in pure water is quite low due to the limited dissociation into Ag⁺ and Cl⁻ ions. 2. **Effect of NH3 on AgCl Solubility**: - When NH3 (ammonia) is added to a solution containing AgCl, it interacts with Ag⁺ ions to form a complex ion, [Ag(NH3)2]⁺. This complex formation increases the solubility of AgCl in the solution. 3. **Complex Formation**: - The reaction can be represented as: \[ Ag^+ + 2NH_3 \rightleftharpoons [Ag(NH_3)_2]^+ \] - The formation of this complex shifts the equilibrium, allowing more AgCl to dissolve as more Ag⁺ ions are removed from the solution. 4. **Common Ion Effect**: - The common ion effect states that the solubility of a sparingly soluble salt decreases in the presence of a common ion. In this case, if NH4Cl (which provides Cl⁻ ions) were added, it would decrease the solubility of AgCl due to the increased concentration of Cl⁻ ions. 5. **Conclusion on Statements**: - Statement A is true: The solubility of AgCl is indeed greater in NH3 than in pure water due to complex formation. - Statement R is false: The addition of NH3 does not decrease the concentration of Cl⁻ ions; rather, it facilitates the dissolution of AgCl by forming a complex with Ag⁺ ions. ### Final Answer: - A is true, and R is false.
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AAKASH INSTITUTE-EQUILIBRIUM-ASSIGNMENT (SECTION -D)
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  2. A : HCI, HNO3 and H2SO4 are equalty strong acids in water R : Water ...

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  3. A : Increasing the concentration of H2 will increases magnitude of e...

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  4. A : Increasing the temperature , increases [H^+] concentration in wat...

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  5. A : Solution of CH3COONH4 is a buffer solution R: H^+ ion added will...

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  6. A : K(sp) is a constant value for any salt at particular temperature ...

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  7. A : H3O^+ ion from water is also taken in consideration while calcula...

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  8. A : pH of 10^(-8) M HCI solution is approx 6.9 R : HCI is a strong a...

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  9. A : For equilibrium ice hArr water on increasing temperature and pres...

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  10. A : At equilibrium concentration of the reactant and product does not ...

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  11. A : pH of 0.1 M HCI solution is less than 0.1 M HCN solution R : In ...

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  12. A : A catalyst does not alter the equilibrium constant of a reaction ...

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  13. A : pH of equimolar solution of NH4 CI and NH4OH does not change when ...

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  14. A: The reaction 2NO(g) +O2(g) hArr 2NO2(g) is favoured in the forwar...

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  15. A : pH of 1 M NaCI solution is 7 at 25^@C. R : pH of this solution d...

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  16. A : CO2 is a Lewis acid. R : H2SO4 is Arrhenius acid as well as Bron...

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  17. A : For H2CO3 K(a1) lt K(a2). R : H2CO3 is weaker acid than HCO3^-

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  18. A : pH of mixture of 0.1 M HCN and 0.05 M NaOH is less than 7 . R : ...

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  19. A: Solubility of AgCI is more in NH3 than in pure water. R : Common ...

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  20. A : Precipitates formation takes place when K(ip) gt K(sp) . R : K...

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