 I now have a solution that is 0.01 molar in acetic acid and 0.01 molar in sodium acetate. Notice that the pH of this buffer solution is very close to the pH of the 0.1 molar buffer solution. Remember that diluting the buffer does not change the pH of the buffer. I will now add one molar HCl to the buffer. Notice that I have added five drops of one molar HCl. Notice that the pH of the buffer has dropped very rapidly. The two buffers have the same initial pH, but the 0.01 molar buffer has a much lower buffer capacity. It will not neutralize nearly as much added acid or base. It only takes five drops of the one molar HCl solution to destroy the buffer. I have a new sample of the 0.01 molar acetic acid, 0.01 molar sodium acetate buffer mixture. I'm now going to add one molar sodium hydroxide to the solution. I've added five drops of the one molar sodium hydroxide. Notice that the pH of the solution has risen rapidly. Again, the buffer capacity of the more dilute buffer solution is a lot lower. After adding ten drops of the one molar sodium hydroxide, we have completely destroyed the buffer and the pH has risen very rapidly.