1) Consider the insoluble compound cobalt(II) carbonate , CoCO3. The cobalt(II) ion also forms a complex...

1) Consider the insoluble compound cobalt(II) carbonate , CoCO₃. The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of CoCO₃(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.

For Co(NH₃)₆²⁺, K_f = 1.3×10⁵. Use the pull-down boxes to specify states such as (aq) or (s).
K_net =

2) Consider the insoluble compound nickel(II) carbonate, NiCO₃. The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of NiCO₃(s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.

For Ni(CN)₄^2-(aq), K_f = 2.0×10³¹. Use the pull-down boxes to specify states such as (aq) or (s).

K_net =

3) Consider the insoluble compound zinc sulfide, ZnS. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnS(s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction.

For Zn(OH)₄^2-, K_f = 4.6×10¹⁷. Use the pull-down boxes to specify states such as (aq) or (s).

K_net =

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queen_honey_blossom answered 1 year ago

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