1. The problem statement, all variables and given/known data Predict whether an aqueous solution of KBr will be acidic, basic, or neutral. 2. Relevant equations KBr(s) → K+(aq) + Br-(aq) Br-(aq) + H2O(l) ← HBr(aq) + H3O+(aq) 3. The attempt at a solution The solution will be neutral. I know that this is the correct answer. I just don't know how they got there. What I am thinking is: We first dissociate KBr, which will give us the 1st reaction, then we discard the K+ since it's a salt and doesn't affect the pH, and then we see what the reactants are going to be if we dissociate the other product (Br-) in H2O. Apparently, the products of the second reaction are supposed to tell us what the pH of the KBr solution will be. How? I know that HBr is a strong acid. I would have thought that the solution is acidic, not neutral. What makes it neutral? Thank you, Joanna.