Part a: What volume of 10.0 M NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCl?
answer : 6.7ml
Part B: The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0200 mol of hydrogen ions without changing the volume. What is the pH of the final solution?
answer : pH 7.28
Part C: What additional volume of 10.0 M HCl would be needed to exhaust the remaining capacity of the buffer after the reaction described in Part B? In other words, how much more of this HCl solution is required to consume the remaining Tris in the buffer?
1.8 is not the answer
HELP ME FOR PART C PLEASE!!!
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