1. The problem statement, all variables and given/known data A buffer is prepared by dissolving 1.00 mole HLac (with a ka=8.0x10-3) and 1.00 mole of sodium lactate (NaLac) in enough water to form one (1) liter of solution. Calculate the [H+] and the pH of the buffer. 36 minutes ago - 3 days left to answer. Additional Details 12 minutes ago There is another part to this and it says Using the information from that problem: supposed we add a strong acid or base to the buffer; calculate the following: a. [HLac], [Lac], [H+] and the pH after adding 1L of 0.15 M-HCl b. [HLac], [Lac], [H+], and the pH after adding 1L of 0.15M-NaOH 2. Relevant equations pH=pka-log[HA]/[A-] 3. The attempt at a solution I know the answer to the first part is found to be pH=2.1 I just have no idea how to find the part a and b for the second half.