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Silver (1) ions form a precipitate with chromate ions. Ksp = 9.0 x 10-¹2. a. Write the balanced chemical equation of the reaction. Indicate physical states of all reaction components. 4 Agcaq) + Croucags + Ag₂ (rO4(s) b. Calculate the solubility of the precipitate in pure water. c. Calculate the solubility of the precipitate in a solution containing 0.100 M potassium nitrate.

Silver (1) ions form a precipitate with chromate ions. Ksp = 9.0 x 10-¹2. a. Write the balanced chemical equation of the reaction. Indicate physical states of all reaction components. 4 Agcaq) + Croucags + Ag₂ (rO4(s) b. Calculate the solubility of the precipitate in pure water. c. Calculate the solubility of the precipitate in a solution containing 0.100 M potassium nitrate.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.98QE
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23. Silver (1) ions form a precipitate with chromate ions. Ksp = 9.0 x 10-¹2. a. Write the balanced chemical equation of the reaction. Indicate physical states of all reaction components. 4 Agcag) + Croucags + Ay₂ CrO4(s) t b. Calculate the solubility of the precipitate in pure water. C. Calculate the solubility of the precipitate in a solution containing 0.100 M potassium nitrate.
Transcribed Image Text:23. Silver (1) ions form a precipitate with chromate ions. Ksp = 9.0 x 10-¹2. a. Write the balanced chemical equation of the reaction. Indicate physical states of all reaction components. 4 Agcag) + Croucags + Ay₂ CrO4(s) t b. Calculate the solubility of the precipitate in pure water. C. Calculate the solubility of the precipitate in a solution containing 0.100 M potassium nitrate.
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