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(NH),*, K = 1.6x10. Be sure to specify states such as (aq) or (s). + K= Consider the insoluble compound nickel(II) hydroxide, Ni(OH), . The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Ni(OH), (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN),, K, = 1.0x101. 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(NH),*, K = 1.6x10. Be sure to specify states such as (aq) or (s). + K= Consider the insoluble compound nickel(II) hydroxide, Ni(OH), . The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Ni(OH), (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN),, K, = 1.0x101. Be sure to specify states such as (aq) or (s). K=

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 92QRT

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Similar questions

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