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A solution contains 0.25 M Cd2+ ions. At what pH will Cd(OH)2 begin to precipitate? O 6.66 O 0.68 07.34 O 13.32

A solution contains 0.25 M Cd2+ ions. At what pH will Cd(OH)2 begin to precipitate? O 6.66 O 0.68 07.34 O 13.32

Chemistry
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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**Question 15** A solution contains 0.25 M Cd²⁺ ions. At what pH will Cd(OH)₂ begin to precipitate? - ○ 6.66 - ○ 0.68 - ○ 7.34 - ○ 13.32 *Note: The question involves determining the pH level at which cadmium hydroxide, Cd(OH)₂, starts to precipitate from a solution containing cadmium ions, Cd²⁺, at a concentration of 0.25 M. Knowledge of the solubility product constant (Ksp) for Cd(OH)₂ is needed to calculate the precise pH at which precipitation begins.*
Transcribed Image Text:**Question 15** A solution contains 0.25 M Cd²⁺ ions. At what pH will Cd(OH)₂ begin to precipitate? - ○ 6.66 - ○ 0.68 - ○ 7.34 - ○ 13.32 *Note: The question involves determining the pH level at which cadmium hydroxide, Cd(OH)₂, starts to precipitate from a solution containing cadmium ions, Cd²⁺, at a concentration of 0.25 M. Knowledge of the solubility product constant (Ksp) for Cd(OH)₂ is needed to calculate the precise pH at which precipitation begins.*
**Solubility Product Constants (25°C)** | Compound (s) | \( K_{sp} \) | |--------------|-----------------------| | BaF\(_2\) | 2.4 x 10\(^{-5}\) | | CuCl(s) | 1.9 x 10\(^{-7}\) | | PbF\(_2\) | 4.0 x 10\(^{-8}\) | | AgCl(s) | 1.6 x 10\(^{-10}\) | | FeCO\(_3\) | 2.1 x 10\(^{-11}\) | | Mn(OH)\(_2\) | 2.0 x 10\(^{-13}\) | | AuCl(s) | 2.0 x 10\(^{-13}\) | | Cd(OH)\(_2\) | 1.2 x 10\(^{-14}\) | This table presents the solubility product constants (\( K_{sp} \)) for various compounds at 25°C. The \( K_{sp} \) value indicates the extent to which a compound will dissolve in water. Lower \( K_{sp} \) values signify lower solubility, while higher \( K_{sp} \) values indicate higher solubility.
Transcribed Image Text:**Solubility Product Constants (25°C)** | Compound (s) | \( K_{sp} \) | |--------------|-----------------------| | BaF\(_2\) | 2.4 x 10\(^{-5}\) | | CuCl(s) | 1.9 x 10\(^{-7}\) | | PbF\(_2\) | 4.0 x 10\(^{-8}\) | | AgCl(s) | 1.6 x 10\(^{-10}\) | | FeCO\(_3\) | 2.1 x 10\(^{-11}\) | | Mn(OH)\(_2\) | 2.0 x 10\(^{-13}\) | | AuCl(s) | 2.0 x 10\(^{-13}\) | | Cd(OH)\(_2\) | 1.2 x 10\(^{-14}\) | This table presents the solubility product constants (\( K_{sp} \)) for various compounds at 25°C. The \( K_{sp} \) value indicates the extent to which a compound will dissolve in water. Lower \( K_{sp} \) values signify lower solubility, while higher \( K_{sp} \) values indicate higher solubility.
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