Given Ag^+(NH3)2 ⇌ Ag^+ + 2NH3 , Kc = 8.2 × 10^–8 and Ksp(AgCl) = 2.378 × 10^–10 at 298 K. Calculate the concentration of the complex

Question 1

Given Ag+(NH3)2 ⇌ Ag+ + 2NH3 , Kc = 8.2 × 10–8 and Ksp(AgCl) = 2.378 × 10–10 at 298 K. Calculate the concentration of the complex in 1.0 M aqueous ammonia.

Question 2

In case of simultaneous solubility, Ag+ *** same in both the equilibrium

[Ag(NH3)2]+ = [Cl–] = y because Ag+ obtained from AgCl passes in [Ag(NH3)2]+ state.

kratos · Answer 1 · 2020-03-27T10:55:45+0000

In case of simultaneous solubility, Ag+ *** same in both the equilibrium

[Ag(NH3)2]+ = [Cl–] = y because Ag+ obtained from AgCl passes in [Ag(NH3)2]+ state.

Given Ag^+(NH3)2 ⇌ Ag^+ + 2NH3 , Kc = 8.2 × 10^–8 and Ksp(AgCl) = 2.378 × 10^–10 at 298 K. Calculate the concentration of the complex

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Given Ag^+(NH3)2 ⇌ Ag^+ + 2NH3 , Kc = 8.2 × 10^–8 and Ksp(AgCl) = 2.378 × 10^–10 at 298 K. Calculate the concentration of the complex

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