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title: "A student places \\(0.10 \\text{ mol}\\) of \\(\\text{AgCl}(s)\\) into \\(1.0 \\text{ L}\\) of distilled water at \\(298 \\text{ K}\\) and stirs until equilibrium is established. A noticeable amount of undissolved \\(\\text{AgCl}(s)\\) remains at the bottom of the flask. The relevant chemical equations and equilibrium constants at \\(298 \\text{ K}\\) are given below.  \\[\\text{AgCl}(s) \\rightleftharpoons \\text{Ag}^+(aq) + \\text{Cl}^-(aq) \\quad K_{sp} = 1.8 \\times 10^{-10}\\]  \\[\\text{Ag}^+(aq) + 2\\,\\text{NH}_3(aq) \\rightleftharpoons [\\text{Ag}(\\text{NH}_3)_2]^+(aq) \\quad K_f = 1.7 \\times 10^7\\]  The student then adds several drops of concentrated \\(\\text{NH}_3(aq)\\) to the mixture at constant temperature with negligible change in total volume. Which of the following correctly predicts and explains the effect of adding \\(\\text{NH}_3(aq)\\) on the amount of solid \\(\\text{AgCl}\\) in the flask?"
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url: "https://nerd-notes.com/ubq/123790/"
date_modified: "2026-09-28T12:30:18+00:00"
---

# A student places \(0.10 \text{ mol}\) of \(\text{AgCl}(s)\) into \(1.0 \text{ L}\) of distilled water at \(298 \text{ K}\) and stirs until equilibrium is established. A noticeable amount of undissolved \(\text{AgCl}(s)\) remains at the bottom of the flask. The relevant chemical equations and equilibrium constants at \(298 \text{ K}\) are given below.

\[\text{AgCl}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{Cl}^-(aq) \quad K_{sp} = 1.8 \times 10^{-10}\]

\[\text{Ag}^+(aq) + 2\,\text{NH}_3(aq) \rightleftharpoons [\text{Ag}(\text{NH}_3)_2]^+(aq) \quad K_f = 1.7 \times 10^7\]

The student then adds several drops of concentrated \(\text{NH}_3(aq)\) to the mixture at constant temperature with negligible change in total volume. Which of the following correctly predicts and explains the effect of adding \(\text{NH}_3(aq)\) on the amount of solid \(\text{AgCl}\) in the flask?

A student places \(0.10 \text{ mol}\) of \(\text{AgCl}(s)\) into \(1.0 \text{ L}\) of distilled water at \(298 \text{ K}\) and stirs until equilibrium is established. A noticeable amount of undissolved \(\text{AgCl}(s)\) remains at the bottom of the flask. The relevant chemical equations and equilibrium constants at \(298 \text{ K}\) are given below.

\[\text{AgCl}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{Cl}^-(aq) \quad K_{sp} = 1.8 \times 10^{-10}\]

\[\text{Ag}^+(aq) + 2\,\text{NH}_3(aq) \rightleftharpoons [\text{Ag}(\text{NH}_3)_2]^+(aq) \quad K_f = 1.7 \times 10^7\]

The student then adds several drops of concentrated \(\text{NH}_3(aq)\) to the mixture at constant temperature with negligible change in total volume. Which of the following correctly predicts and explains the effect of adding \(\text{NH}_3(aq)\) on the amount of solid \(\text{AgCl}\) in the flask?

- **A.** The amount of solid \(\text{AgCl}\) increases because \(\text{NH}_3\) acts as a Bronsted-Lowry base, generating \(\text{OH}^-(aq)\) that reacts with \(\text{Cl}^-(aq)\) to precipitate an additional solid.
- **B.** The amount of solid \(\text{AgCl}\) increases because the introduction of \(\text{NH}_3(aq)\) increases the total concentration of dissolved species, raising \(Q_{sp}\) above \(K_{sp}\).
- **C.** The amount of solid \(\text{AgCl}\) decreases because \(\text{NH}_3\) coordinates with \(\text{Ag}^+(aq)\) to form \([\text{Ag}(\text{NH}_3)_2]^+(aq)\), lowering \([\text{Ag}^+]\) so that \(Q_{sp} < K_{sp}\).
- **D.** The amount of solid \(\text{AgCl}\) decreases because the large magnitude of \(K_f\) increases the numerical value of \(K_{sp}\) for \(\text{AgCl}\), driving the dissolution of more solid.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123790/*