Consider the insoluble compound silver hydroxide , AgOH. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3),*, Kç= 1.6×107 . Be sure to specify states such as (aq) or (s). + K =
Consider the insoluble compound silver hydroxide , AgOH. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3),*, Kç= 1.6×107 . Be sure to specify states such as (aq) or (s). + K =
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 61QAP
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Transcribed Image Text:Consider the insoluble compound silver hydroxide , AgOH. The silver ion also forms a complex with ammonia. Write a
balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of ammonia and calculate the
equilibrium constant for this reaction.
For Ag(NH3),*, Kç= 1.6×107 . Be sure to specify states such as (aq) or (s).
+
K =
Transcribed Image Text:values if needed for this question.
In the laboratory you are given the task of separating Ag* and Ba* ions in aqueous solution.
2+.
For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent
CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No"
Y or N Reagent Formula of Precipitate if YES
1. NaBr
2. Na,CO3
3. NaOH
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