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Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their solubility to be more, less, or about the same as in a pure water solution ? Clear All More soluble than in pure zinc carbonate water. Similar solubility as in pure cobalt(II) hydroxide water. Less soluble than in pure silver bromide water.

Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their solubility to be more, less, or about the same as in a pure water solution ? Clear All More soluble than in pure zinc carbonate water. Similar solubility as in pure cobalt(II) hydroxide water. Less soluble than in pure silver bromide water.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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### Solubility of Insoluble Salts in 0.10 M Hydrobromic Acid Solution Below are three insoluble salts. We will analyze their solubility when placed into a 0.10 M hydrobromic acid (HBr) solution and determine if their solubility increases, decreases, or remains the same compared to their solubility in pure water. **Insoluble Salts:** - Zinc carbonate - Cobalt(II) hydroxide - Silver bromide **Solubility Comparison:** 1. **Zinc Carbonate** - **More soluble than in pure water.** 2. **Cobalt(II) Hydroxide** - **Similar solubility as in pure water.** 3. **Silver Bromide** - **Less soluble than in pure water.** ### Explanation: **1. Zinc Carbonate (ZnCO3)** - In acidic solutions, the carbonate ion reacts with hydrogen ions (H⁺) from the acid to form carbonic acid, which decomposes into carbon dioxide and water. This shift in equilibrium increases the solubility of zinc carbonate in the acidic solution compared to pure water. **2. Cobalt(II) Hydroxide (Co(OH)₂)** - Cobalt(II) hydroxide has limited reactivity in acidic solutions, hence its solubility remains relatively unchanged when placed in 0.10 M HBr solution compared to pure water. **3. Silver Bromide (AgBr)** - Silver bromide is less soluble in a hydrobromic acid solution due to the common ion effect; the presence of bromide ions (Br⁻) from both AgBr and HBr decreases the solubility of AgBr in the solution. Analyzing solubility changes in different chemical environments, such as acidic solutions, can enhance our understanding of chemical equilibria, reaction mechanisms, and the properties of compounds.
Transcribed Image Text:### Solubility of Insoluble Salts in 0.10 M Hydrobromic Acid Solution Below are three insoluble salts. We will analyze their solubility when placed into a 0.10 M hydrobromic acid (HBr) solution and determine if their solubility increases, decreases, or remains the same compared to their solubility in pure water. **Insoluble Salts:** - Zinc carbonate - Cobalt(II) hydroxide - Silver bromide **Solubility Comparison:** 1. **Zinc Carbonate** - **More soluble than in pure water.** 2. **Cobalt(II) Hydroxide** - **Similar solubility as in pure water.** 3. **Silver Bromide** - **Less soluble than in pure water.** ### Explanation: **1. Zinc Carbonate (ZnCO3)** - In acidic solutions, the carbonate ion reacts with hydrogen ions (H⁺) from the acid to form carbonic acid, which decomposes into carbon dioxide and water. This shift in equilibrium increases the solubility of zinc carbonate in the acidic solution compared to pure water. **2. Cobalt(II) Hydroxide (Co(OH)₂)** - Cobalt(II) hydroxide has limited reactivity in acidic solutions, hence its solubility remains relatively unchanged when placed in 0.10 M HBr solution compared to pure water. **3. Silver Bromide (AgBr)** - Silver bromide is less soluble in a hydrobromic acid solution due to the common ion effect; the presence of bromide ions (Br⁻) from both AgBr and HBr decreases the solubility of AgBr in the solution. Analyzing solubility changes in different chemical environments, such as acidic solutions, can enhance our understanding of chemical equilibria, reaction mechanisms, and the properties of compounds.
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