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Which of the following would decrease the solubility of a 0.10 M solution of Ag2CO3 the most? (Ksp of Ag2CO; is 8.1 x 10 12) A) adding 0.10 M H* B) adding 0.10 M CO3- C) adding 0.10 MAg*

Which of the following would decrease the solubility of a 0.10 M solution of Ag2CO3 the most? (Ksp of Ag2CO; is 8.1 x 10 12) A) adding 0.10 M H* B) adding 0.10 M CO3- C) adding 0.10 MAg*

Chemistry
Chemistry
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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
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**Question:** Which of the following would decrease the solubility of a 0.10 M solution of Ag₂CO₃ the most? (Ksp of Ag₂CO₃ is 8.1 x 10⁻¹²) **Options:** A) Adding 0.10 M H⁺ B) Adding 0.10 M CO₃²⁻ C) Adding 0.10 M Ag⁺ **Explanation:** This question asks which addition will most significantly reduce the solubility of silver carbonate (Ag₂CO₃) in solution by common ion effect or shifting of equilibrium. The Ksp value indicates the solubility product constant, which is a measure of the solubility of a compound under equilibrium conditions. - **Option A:** Adding H⁺ could potentially react with the carbonate ion (CO₃²⁻) forming HCO₃⁻ or CO₂ and H₂O, which might increase solubility due to removal of CO₃²⁻ ions. - **Option B:** Adding CO₃²⁻ will increase the concentration of carbonate ions, shifting the equilibrium to favor the formation of more Ag₂CO₃ precipitate, thus decreasing solubility. - **Option C:** Adding Ag⁺ will increase the concentration of silver ions, also shifting the equilibrium towards the formation of more solid Ag₂CO₃ precipitate, decreasing solubility. This is likely the most effective way to decrease solubility due to the common ion effect.
Transcribed Image Text:**Question:** Which of the following would decrease the solubility of a 0.10 M solution of Ag₂CO₃ the most? (Ksp of Ag₂CO₃ is 8.1 x 10⁻¹²) **Options:** A) Adding 0.10 M H⁺ B) Adding 0.10 M CO₃²⁻ C) Adding 0.10 M Ag⁺ **Explanation:** This question asks which addition will most significantly reduce the solubility of silver carbonate (Ag₂CO₃) in solution by common ion effect or shifting of equilibrium. The Ksp value indicates the solubility product constant, which is a measure of the solubility of a compound under equilibrium conditions. - **Option A:** Adding H⁺ could potentially react with the carbonate ion (CO₃²⁻) forming HCO₃⁻ or CO₂ and H₂O, which might increase solubility due to removal of CO₃²⁻ ions. - **Option B:** Adding CO₃²⁻ will increase the concentration of carbonate ions, shifting the equilibrium to favor the formation of more Ag₂CO₃ precipitate, thus decreasing solubility. - **Option C:** Adding Ag⁺ will increase the concentration of silver ions, also shifting the equilibrium towards the formation of more solid Ag₂CO₃ precipitate, decreasing solubility. This is likely the most effective way to decrease solubility due to the common ion effect.
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