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A 35.00 mL solution of 0.2500 M HF is titrated with a standardized 0.1978 M solution of NaOH at 25 C.
a) What is the pH of the HF solution before titrant is added?
b) How many milliliters of titrant are required to reach the equivalent point?
c) What is the pH and 0.50 mL before the equivalence point?
d) What is the pH at the equivalence point?
e) What is the pH at 0.50 mL after the equivalence point?
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Write a net ionic equation to explain why the pH didn't go up to about 10, as it would have if that amount of NaOH were added to distilled water or to 20ml 0.00040 M HCL, which also would have a pH of 3.40
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