What is the pH at the equivalence point in the titration of a 22.4 mL sample of a 0.326 M aqueous hydrofluoric acid solution with a 0.484 M aqueous potassium hydroxide solution? pH = Submit Answer Retry Entire Group 2 more group attempts remaining

What is the pH at the equivalence point in the titration of a 22.4 mL sample of a 0.326 M aqueous hydrofluoric acid solution with a 0.484 M aqueous potassium hydroxide solution? pH = Submit Answer Retry Entire Group 2 more group attempts remaining

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.145E

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

What is the pH at the equivalence point in the titration of a 22.4 mL sample of a 0.326 M aqueous hydrofluoric acid
solution with a 0.484 M aqueous potassium hydroxide solution?
pH
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Step 2: Calculation of total volume

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Step 3: Calculation of F- concentration

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Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). 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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