Part A Consider the titration of 36.4 mL of 0.260 M HF ( K = 3.5 x 10) with 0.220 M NaOH. Calculate the pH at each of the following points. How many milliliters of base are required to reach the equivalence point? Express your answer using three significant figures. VNaOH = mL Submit Previous Answers Bequest Answer X Incorrect; Try Again; 5 attempts remaining Part B Calculate the pH after the addition of 9.10 mL of base Express your answer using two decimal places. pH
Part A Consider the titration of 36.4 mL of 0.260 M HF ( K = 3.5 x 10) with 0.220 M NaOH. Calculate the pH at each of the following points. How many milliliters of base are required to reach the equivalence point? Express your answer using three significant figures. VNaOH = mL Submit Previous Answers Bequest Answer X Incorrect; Try Again; 5 attempts remaining Part B Calculate the pH after the addition of 9.10 mL of base Express your answer using two decimal places. pH
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...
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