Consider the titration of 35.0 mL of 0.260 M HF with 0.215 MNaOH. Calculate the pH...

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Chemistry

Consider the titration of 35.0 mL of 0.260 M HF with 0.215MNaOH. Calculate the pH at each of the following points.
Part A.)
How many milliliters of base are required to reach theequivalence point?
Express your answer using three significant figures.
Part B.)
Calculate the pH after the addition of 8.75 mL of base
Express your answer using two decimal places.
Part C.)
Calculate the pH at halfway to the equivalence point.
Express your answer using two decimal places.
Part D.)
Calculate the pH at the equivalence point.
Express your answer using two decimal places.
Part E.)
Calculate the pH after the addition of 70.0 mL of base.
Express your answer using two decimal places.

Answer & Explanation Solved by verified expert

3.9 Ratings (743 Votes)

Part A Reaction of HF and NaOH HF NaOH NaF H2O Moles of HF 0035 L 0260 M 91103 mol HF Moles of NaOH 91103 mol because 1 mole HF reacts with 1 mol NaOH Volume moles molarity 91103 mol 0215 molL 00423 L or 423 mL Part B Calculate the pH after the addition of 875 mL of base Express your answer using two See Answer

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