Ionic EquilibriumHard

Question

Ag+ + NH3 $\rightleftharpoons$­ [Ag(NH3)+]; K1 = 1.6 × 103

[Ag(NH3)+] + NH3­ $\rightleftharpoons$ [Ag(NH3)2+]; K2 = 6.8 × 103

The formation constant of [Ag(NH3)2+] is

Options

A.1.08 × 107
B.6.08 × 106
C.1.08 × 103
D.1.08 × 105

Solution

$K_{f} = K_{f_{1}}.K_{f_{2}} = 1.6 \times 10^{3} \times 6.8 \times 10^{3} = 1.08 \times 10^{7}$

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