Consider the insoluble compound silver bromide , AgBr . The silver ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of AgBr (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)2+ , Kf = 1.6×107 . Use the pull-down boxes to specify states such as (aq) or (s).

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Explanation:

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In this case, by considering the dissolution of silver bromide:

And the formation of the complex:

We obtain the balanced net ionic equation by adding the aforementioned equations:

Now, the equilibrium constant is obtained by writing the law of mass action for the non-simplified net ionic equation:

So we notice that the equilibrium constant contains the solubility constant and formation constant for the initial reactions:

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explanation: