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How do you use the equilibrium constants to predict solubility? Do you just see which way the reaction favors, and if it is the side with (aq) you know it is going to be soluble but if it favors the other direction then it won’t?
Exactly. If a reaction has solid reactants and aqueous products, a larger equilibrium constant means the reactants are more soluble.
Yes, you essentially answered your own question -- just pay attention to the K value and the phases of the reactants/products and the answer should be clear, just as the previous answer stated.
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