Consider the insoluble compound zinc carbonate , ZnCO3 . The zinc ion also forms a complex with hydroxide ions . Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)42- , Kf = 2.9×1015 . Use the pull-down boxes to specify states such as (aq) or (s).

The net ionic equation is  

The equilibrium constant is  

Explanation:

From the question we are that

      The  

The ionic equation is chemical represented as

    Step 1

           ⇔     The  solubility product constant for stage is    

 Step 2

           ⇔    The formation constant for this step is given as

 The net reaction is  

The equilibrium constant is mathematically evaluated as

substituting values