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

3.8 Ratings (628 Votes)

Answer We are given 350 mL of 0260 M HF NaOH 0215 M Part A Milliliters of base are required to reach the equivalence point We know at equivalence point moles of acid and base are equal Moles of HF 0260 M 00350 L 00091 moles So moles of NaOH 00091 moles So volume of NaOH 00091 moles 0215 M 00423 L 423 mL So 423 milliliters of base are required to reach the equivalence point Part B the pH after the addition See Answer

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