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Concept explainers
Follow the directions of Question 64. Consider two beakers:
Beaker A has a weak acid (Ka=1×10−5).
Beaker B has HCI.
The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH.
(a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B.
(b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the
pH of the solution in Beaker B.
(c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B.
(d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
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Chapter 14 Solutions
Chemistry: Principles and Reactions
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