---
title: "A student prepares a saturated aqueous solution of silver chromate, \\(\\text{Ag}_2\\text{CrO}_4\\), by adding excess solid to pure distilled water at a constant temperature. The dissolution equilibrium and its solubility product constant, \\(K_{sp}\\), are represented below.  \\[ \\text{Ag}_2\\text{CrO}_4(s) \\rightleftharpoons 2\\text{Ag}^+(aq) + \\text{CrO}_4^{2-}(aq) \\quad\\quad K_{sp} = 4.0 \\times 10^{-12} \\]  Based on the information above, what is the molar solubility of \\(\\text{Ag}_2\\text{CrO}_4(s)\\) in pure water at this temperature?"
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url: "https://nerd-notes.com/ubq/119755/"
date_modified: "2026-08-21T08:12:13+00:00"
---

# A student prepares a saturated aqueous solution of silver chromate, \(\text{Ag}_2\text{CrO}_4\), by adding excess solid to pure distilled water at a constant temperature. The dissolution equilibrium and its solubility product constant, \(K_{sp}\), are represented below.

\[ \text{Ag}_2\text{CrO}_4(s) \rightleftharpoons 2\text{Ag}^+(aq) + \text{CrO}_4^{2-}(aq) \quad\quad K_{sp} = 4.0 \times 10^{-12} \]

Based on the information above, what is the molar solubility of \(\text{Ag}_2\text{CrO}_4(s)\) in pure water at this temperature?

A student prepares a saturated aqueous solution of silver chromate, \(\text{Ag}_2\text{CrO}_4\), by adding excess solid to pure distilled water at a constant temperature. The dissolution equilibrium and its solubility product constant, \(K_{sp}\), are represented below.

\[ \text{Ag}_2\text{CrO}_4(s) \rightleftharpoons 2\text{Ag}^+(aq) + \text{CrO}_4^{2-}(aq) \quad\quad K_{sp} = 4.0 \times 10^{-12} \]

Based on the information above, what is the molar solubility of \(\text{Ag}_2\text{CrO}_4(s)\) in pure water at this temperature?

- **A.** \(2.0 \times 10^{-6} \text{ M}\)
- **B.** \(1.0 \times 10^{-4} \text{ M}\)
- **C.** \(2.0 \times 10^{-4} \text{ M}\)
- **D.** \(3.0 \times 10^{-4} \text{ M}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119755/*