Ionic EquilibriumHard

Question

A 0.1 mole of AgNO3 is dissolved in 1 L of 1 M-NH3. If 0.01 mole of NaCl is added to this solution, will AgCl(s) precipitate? The value of Ksp for AgCl = 1.8 × 10–10 and Kstab for Ag(NH3)2+ = 1.6 × 107.

Options

A.Yes
B.No
C.Addition of NaCl in any amount can never result in precipitation.
D.Addition of even smaller amount of NaCl may result in precipitation.

Solution

Ag+ + 2NH3 $\rightleftharpoons$ Ag(NH3)+2; Kstab = 1.6 × 107

0.1 M 1M 0

100% 0 (1 – 0.2) M 0.1 M = 0.8 M

Equ. xM 0.8 + 2x 0.1 – x

≈ 0.8 M ≈ 0.1 M

Now, $1.6 \times 10^{7} = \frac{0.1}{x \times (0.8)^{2}} \Rightarrow x = 9.76 \times 10^{- 9}\text{ M}$

Now, on adding NaCl, Q = [Ag+][Cl–] = 9.76 × 10–9 × 0.01 = 9.76 × 10–11 < Ksp

Hence, no precipitation of AgCl.

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