---
title: "A student models a halide-exchange step that can occur when silver halide solids contact an aqueous sample. At \\(25^\\circ\\text{C}\\), the equilibrium constants for the dissolution reactions are given below.  | Equilibrium | Equilibrium constant | |—|—| | \\(\\text{AgCl(s)} \\rightleftharpoons \\text{Ag}^+\\text{(aq)} + \\text{Cl}^-\\text{(aq)}\\) | \\(K_1=2.0\\times10^{-10}\\) | | \\(\\text{AgBr(s)} \\rightleftharpoons \\text{Ag}^+\\text{(aq)} + \\text{Br}^-\\text{(aq)}\\) | \\(K_2=5.0\\times10^{-13}\\) |  The student combines the equilibria to represent the net reaction \\(\\text{AgCl(s)}+\\text{Br}^-\\text{(aq)}\\rightleftharpoons\\text{AgBr(s)}+\\text{Cl}^-\\text{(aq)}\\). What is the value of \\(K\\) for this net reaction at \\(25^\\circ\\text{C}\\)?"
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url: "https://nerd-notes.com/ubq/119513/"
date_modified: "2026-08-19T12:41:01+00:00"
---

# A student models a halide-exchange step that can occur when silver halide solids contact an aqueous sample. At \(25^\circ\text{C}\), the equilibrium constants for the dissolution reactions are given below.

| Equilibrium | Equilibrium constant |
|—|—|
| \(\text{AgCl(s)} \rightleftharpoons \text{Ag}^+\text{(aq)} + \text{Cl}^-\text{(aq)}\) | \(K_1=2.0\times10^{-10}\) |
| \(\text{AgBr(s)} \rightleftharpoons \text{Ag}^+\text{(aq)} + \text{Br}^-\text{(aq)}\) | \(K_2=5.0\times10^{-13}\) |

The student combines the equilibria to represent the net reaction \(\text{AgCl(s)}+\text{Br}^-\text{(aq)}\rightleftharpoons\text{AgBr(s)}+\text{Cl}^-\text{(aq)}\). What is the value of \(K\) for this net reaction at \(25^\circ\text{C}\)?

A student models a halide-exchange step that can occur when silver halide solids contact an aqueous sample. At \(25^\circ\text{C}\), the equilibrium constants for the dissolution reactions are given below.

| Equilibrium | Equilibrium constant |
|---|---|
| \(\text{AgCl(s)} \rightleftharpoons \text{Ag}^+\text{(aq)} + \text{Cl}^-\text{(aq)}\) | \(K_1=2.0\times10^{-10}\) |
| \(\text{AgBr(s)} \rightleftharpoons \text{Ag}^+\text{(aq)} + \text{Br}^-\text{(aq)}\) | \(K_2=5.0\times10^{-13}\) |

The student combines the equilibria to represent the net reaction \(\text{AgCl(s)}+\text{Br}^-\text{(aq)}\rightleftharpoons\text{AgBr(s)}+\text{Cl}^-\text{(aq)}\). What is the value of \(K\) for this net reaction at \(25^\circ\text{C}\)?

- **A.** \(1.0\times10^{-22}\)
- **B.** \(2.0\times10^{-10}\)
- **C.** \(2.5\times10^{-3}\)
- **D.** \(4.0\times10^2\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119513/*