You are working on a project to recycle nickel and cadmium from old nickel–cadmium batteries that have an iron casing. The batteries are dissolved in aqueous nitric acid, producing a solution containing primarily Ni 2+ , Cd 2+ , and Fe 3+ cations. One idea is to add sodium hydroxide to neutralize the acid and cause precipitation of Ni(OH) 2 , Cd(OH) 2 , and Fe(OH) 3 . Assume the concentration of each of the cations is 0.100 M before the sodium hydroxide is added. The pH increases as the sodium hydroxide is added. Which compound will precipitate first, and what is the pH at that point? ### Solubility Product Constants (Ksp) for Various HydroxidesThis table displays the solubility product constants (\(K_{sp}\)) for three different metal hydroxides. The \(K_{sp}\) value is an indicator of the solubility of a compound; the smaller the \(K_{sp}\), the less soluble the compound.| **Salt** | **\(K_{sp}\)** ||-------------|----------------------|| Ni(OH)\(_2\) | \(2.8 \times 10^{-16}\) || Cd(OH)\(_2\) | \(1.2 \times 10^{-14}\) || Fe(OH)\(_3\) | \(6.3 \times 10^{-38}\) |- **Ni(OH)\(_2\)** (Nickel(II) hydroxide) has a solubility product constant of \(2.8 \times 10^{-16}\).- **Cd(OH)\(_2\)** (Cadmium(II) hydroxide) has a solubility product constant of \(1.2 \times 10^{-14}\).- **Fe(OH)\(_3\)** (Iron(III) hydroxide) has a solubility product constant of \(6.3 \times 10^{-38}\).The significantly lower \(K_{sp}\) of Fe(OH)\(_3\) indicates it is much less soluble compared to Ni(OH)\(_2\) and Cd(OH)\(_2\). These values are crucial in predicting the formation of precipitates in aqueous solutions and are used in various chemical calculations and applications.

Given : Concentration of Ni2+, [Ni2+ ] = Concentration of Cd2+, [Cd2+ ] = concentration of Fe3+,…

Answered: You are working on a project to recycle…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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You are working on a project to recycle nickel and cadmium from old nickel–cadmium batteries that have an iron casing. The batteries are dissolved in aqueous nitric acid, producing a solution containing primarily Ni 2+ , Cd 2+ , and Fe 3+ cations. One idea is to add sodium hydroxide to neutralize the acid and cause precipitation of Ni(OH) 2 , Cd(OH) 2 , and Fe(OH) 3 . Assume the concentration of each of the cations is 0.100 M before the sodium hydroxide is added. The pH increases as the sodium hydroxide is added. Which compound will precipitate first, and what is the pH at that point?

### Solubility Product Constants (Ksp) for Various Hydroxides

This table displays the solubility product constants (\(K_{sp}\)) for three different metal hydroxides. The \(K_{sp}\) value is an indicator of the solubility of a compound; the smaller the \(K_{sp}\), the less soluble the compound.

| **Salt** | **\(K_{sp}\)** |
|-------------|----------------------|
| Ni(OH)\(_2\) | \(2.8 \times 10^{-16}\) |
| Cd(OH)\(_2\) | \(1.2 \times 10^{-14}\) |
| Fe(OH)\(_3\) | \(6.3 \times 10^{-38}\) |

- **Ni(OH)\(_2\)** (Nickel(II) hydroxide) has a solubility product constant of \(2.8 \times 10^{-16}\).
- **Cd(OH)\(_2\)** (Cadmium(II) hydroxide) has a solubility product constant of \(1.2 \times 10^{-14}\).
- **Fe(OH)\(_3\)** (Iron(III) hydroxide) has a solubility product constant of \(6.3 \times 10^{-38}\).

The significantly lower \(K_{sp}\) of Fe(OH)\(_3\) indicates it is much less soluble compared to Ni(OH)\(_2\) and Cd(OH)\(_2\). These values are crucial in predicting the formation of precipitates in aqueous solutions and are used in various chemical calculations and applications.

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