Seeing solubility in various cases
A is wrong. $\ce{AgBr}$ is one of the least soluble compounds of $\ce{Ag}$. Why don't you have a look in the table of solubility products to be convinced? Further more, $\ce{AgBr}$ will never react with $\ce{H_2O}$ to produce a strong acid like $\ce{HBr}$ and a base like $\ce{AgOH}$. The reaction goes the other way round. Strong acids react with hydroxydes to produce a salt and water. 

C is wrong, because of the Le Chatelier's principle. Try to get the reason your self.

To solve D, you must know that $\ce{Zn(OH)_2}$ is soluble in an excess of $\ce{OH^-}$ ions