im trying to work out the answer to this but i keep getting stuck..can you please explain it in a really *simple* way? The pH of a buffer solution made up of acetic acid (0.100 mol L-1) and sodium acetate (0.100 mol L-1) is 4.76. How much will the pH of this buffer change if 100 mL of 0.100 mol L-1 HCl is added to 1.00 L of the buffer solution?
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The added acid will protonate the acetate, thus lowering its concentration. The acetic acid concentration will rise. We needed to determine the moles of Ac- and HAc present before adding the HCl. Both are 0.1 mole. You may verify this. we added (0.1 L) (0.1 mol/L) = 0.01 mole of HCl. Therefore the HAc goes from 0.1 mol to 0.11 mole and the Ac- goes 0.1 mol to 0.09 mol. Notice that the total volume rises from 1 L to 1.1 liter. This will create new molarities, but I will ignore the molarity calculation. This is because the ratio portion of the H-H will work just fine with the mole amounts. pH = 4.76 + log (0.09/0.11) gives the answer.
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