Consider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+ , K = 6.8x10¹2. Be sure to specify states such as (aq) or (s). K= + ?
Consider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+ , K = 6.8x10¹2. Be sure to specify states such as (aq) or (s). K= + ?
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![Consider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with
ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of
ammonia and calculate the equilibrium constant for this reaction.
For Cu(NH3)42+, K = 6.8x1012. Be sure to specify states such as (aq) or (s).
K =
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Transcribed Image Text:Consider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with
ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of
ammonia and calculate the equilibrium constant for this reaction.
For Cu(NH3)42+, K = 6.8x1012. Be sure to specify states such as (aq) or (s).
K =
[Review Topics]
[References]
Use the References to access important values if needed for this question.
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![A
Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with cyanide ions.
Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of cyanide ions
and calculate the equilibrium constant for this reaction.
For Ag (CN)₂, K = 5.6x1018. Be sure to specify states such as (aq) or (s).
K=
+
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[References]
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Transcribed Image Text:A
Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with cyanide ions.
Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of cyanide ions
and calculate the equilibrium constant for this reaction.
For Ag (CN)₂, K = 5.6x1018. Be sure to specify states such as (aq) or (s).
K=
+
[Review Topics]
[References]
Use the References to access important values if needed for this question.
Submit Answer
+
Retry Entire Group 9 more group attempts remaining
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