Chemistry, 02.07.2020 16:01 jalynholden07
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).
Answers: 2
![ZnCO_3 _{(s)} + 4 OH^{-}_{(aq)} \to [Zn(OH)_4]^{2-} _{(aq)} + CO_3^{2-} _{(aq)}](/tpl/images/0699/8948/a1741.png)
⇔ 
The solubility product constant for stage is 
⇔ ![[Zn(OH_4)]^{2-} _{(aq)}](/tpl/images/0699/8948/a852d.png)
The formation constant for this step is given as 
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Consider the insoluble compound zinc carbonate , ZnCO3 . The zinc ion also forms a complex with hydr...
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