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title: "A student prepares an aqueous solution containing three different anions, each capable of forming an insoluble precipitate with silver ions. The initial concentration of each anion and the solubility product constant, \\(K_{sp}\\), of each corresponding precipitate are provided in the table below.  | Anion | Initial concentration (\\(\\text{M}\\)) | Precipitate formed | \\(K_{sp}\\) at \\(298\\text{ K}\\) | | :— | :— | :— | :— | | \\(\\text{Cl}^-\\) | \\(1.0 \\times 10^{-3}\\) | \\(\\text{AgCl}\\) | \\(1.8 \\times 10^{-10}\\) | | \\(\\text{Br}^-\\) | \\(2.0 \\times 10^{-6}\\) | \\(\\text{AgBr}\\) | \\(5.0 \\times 10^{-13}\\) | | \\(\\text{CrO}_4^{2-}\\) | \\(3.0 \\times 10^{-3}\\) | \\(\\text{Ag}_2\\text{CrO}_4\\) | \\(1.2 \\times 10^{-12}\\) |  As a concentrated solution of \\(\\text{AgNO}_3\\text{(aq)}\\) is slowly added dropwise to the mixture at \\(298\\text{ K}\\), assuming volume changes are negligible, in which order do the precipitates begin to form?"
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url: "https://nerd-notes.com/ubq/120309/"
date_modified: "2026-08-23T04:04:31+00:00"
---

# A student prepares an aqueous solution containing three different anions, each capable of forming an insoluble precipitate with silver ions. The initial concentration of each anion and the solubility product constant, \(K_{sp}\), of each corresponding precipitate are provided in the table below.

| Anion | Initial concentration (\(\text{M}\)) | Precipitate formed | \(K_{sp}\) at \(298\text{ K}\) |
| :— | :— | :— | :— |
| \(\text{Cl}^-\) | \(1.0 \times 10^{-3}\) | \(\text{AgCl}\) | \(1.8 \times 10^{-10}\) |
| \(\text{Br}^-\) | \(2.0 \times 10^{-6}\) | \(\text{AgBr}\) | \(5.0 \times 10^{-13}\) |
| \(\text{CrO}_4^{2-}\) | \(3.0 \times 10^{-3}\) | \(\text{Ag}_2\text{CrO}_4\) | \(1.2 \times 10^{-12}\) |

As a concentrated solution of \(\text{AgNO}_3\text{(aq)}\) is slowly added dropwise to the mixture at \(298\text{ K}\), assuming volume changes are negligible, in which order do the precipitates begin to form?

A student prepares an aqueous solution containing three different anions, each capable of forming an insoluble precipitate with silver ions. The initial concentration of each anion and the solubility product constant, \(K_{sp}\), of each corresponding precipitate are provided in the table below.

| Anion | Initial concentration (\(\text{M}\)) | Precipitate formed | \(K_{sp}\) at \(298\text{ K}\) |
| :--- | :--- | :--- | :--- |
| \(\text{Cl}^-\) | \(1.0 \times 10^{-3}\) | \(\text{AgCl}\) | \(1.8 \times 10^{-10}\) |
| \(\text{Br}^-\) | \(2.0 \times 10^{-6}\) | \(\text{AgBr}\) | \(5.0 \times 10^{-13}\) |
| \(\text{CrO}_4^{2-}\) | \(3.0 \times 10^{-3}\) | \(\text{Ag}_2\text{CrO}_4\) | \(1.2 \times 10^{-12}\) |

As a concentrated solution of \(\text{AgNO}_3\text{(aq)}\) is slowly added dropwise to the mixture at \(298\text{ K}\), assuming volume changes are negligible, in which order do the precipitates begin to form?

- **A.** \(\text{AgBr}\text{, then }\text{Ag}_2\text{CrO}_4\text{, then }\text{AgCl}\)
- **B.** \(\text{Ag}_2\text{CrO}_4\text{, then }\text{AgCl}\text{, then }\text{AgBr}\)
- **C.** \(\text{AgCl}\text{, then }\text{AgBr}\text{, then }\text{Ag}_2\text{CrO}_4\)
- **D.** \(\text{Ag}_2\text{CrO}_4\text{, then }\text{AgBr}\text{, then }\text{AgCl}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120309/*