When a 28.1 mL sample of a 0.465 M aqueous acetic acid solution is titrated with a 0.419 M aqueouspotassium hydroxide solution, what is the pH at the midpoint in the titration?pH =35.9 mL sample of a 0.576 M aqueous hypochlorous acid solution is titrated with a 0.329 M aqueous sodiumhydroxide solution. What is the pH after 42.9 mL of base have been added? Ka for HC1O is 3.5 × 10-8.pH =A 26.3 mL sample of 0.296 M ethylamine, C₂H5NH₂, is titrated with 0.246 M perchloric acid.At the titration midpoint, the pH isA 20.0 mL sample of 0.369 M diethylamine, (C₂H5)₂NH, is titrated with 0.320 M perchloric acid.After adding 8.88 mL of perchloric acid, the pH is

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Answered: When a 28.1 mL sample of a 0.465 M…

When a 28.1 mL sample of a 0.465 M aqueous acetic acid solution is titrated with a 0.419 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration? pH =

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.102E

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The weak base ethanolamine. HOCH2CH2NH2, can be titrated with HCl. HOCH2CH2NH2(aq)+H3O+(aq)HOCH2CH2NH3+(aq)+H2O(l) Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 107.) (a) What is the pH of the ethanolamine solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 would be the best choice to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 10.0, 20.0, and 30.0 mL of the acid. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.
A buffer solution was prepared by adding 4.95 g of sodium acetate, NaCH3CO2, to 2.50 102 mL of 0.150 M acetic acid, CH3CO2H. (a) What is the pH of the buffer? (b) What is the pH of 1.00 102 mL of the buffer solution if you add 82 mg of NaOH to the solution?
You require 36.78 mL of 0.0105 M HCl to reach the equivalence point in the titration of 25.0 mL of aqueous ammonia. (a) What was the concentration of NH3 in the original ammonia solution? (b) What are the concentrations of H3O+, OH, and NH4+ at the equivalence point? (c) What is the pH of the solution at the equivalence point?
1) What is the pH at the equivalence point in the titration of a 29.1 mL sample of a 0.450 M aqueous acetic acid solution with a 0.400 M aqueous sodium hydroxide solution?pH = 2) When a 26.8 mL sample of a 0.420 M aqueous hypochlorous acid solution is titrated with a 0.383 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration?pH =
What is the pH at the equivalence point in the titration of a 20.7 mL sample of a 0.452 M aqueous hypochlorous acid solution with a 0.443 M aqueous potassium hydroxide solution? You must also determine: A 41.0 mL sample of a 0.399 M aqueous hypochlorous acid solution is titrated with a 0.349 M aqueous barium hydroxide solution. What is the pH after 7.85 mL of base have been added?
7.) A.) A 20.2 mL sample of a 0.422 M aqueous hydrofluoric acid solution is titrated with a 0.426 M aqueous potassium hydroxide solution. What is the pH at the start of the titration, before any potassium hydroxide has been added? B.) What is the pH at the equivalence point in the titration of a 22.7 mL sample of a 0.336 M aqueous hypochlorous acid solution with a 0.383 M aqueous potassium hydroxide solution?
When a 16.0 mL sample of a 0.469 M aqueous nitrous acid solution is titrated with a 0.460 M aqueous potassium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 24.5 mL of potassium hydroxide have been added
Consider a titration where 0.215 M potassium hydroxide is added from a burette to 10.00 mL of hydrochloric acid in an Erlenmeyer flask under the burette. A few drops of phenolphthalein are added to the acid in the Erlenmeyer flask. Discuss how the pH of the solution in the Erlenmeyer flask changes as the titration is carried out. Your response should focus on the pH at the beginning of the titration (before the addition of any base), the pH at the equivalence point, and the pH past the equivalence point.
What is the pH at the equivalence point in the titration of a 19.3 mL sample of a 0.316 M aqueous acetic acid solution with a 0.448 M aqueous sodium hydroxide solution?pH =
a. A 24.4 mL sample of a 0.487 M aqueous hydrocyanic acid solution is titrated with a 0.409 M aqueous barium hydroxide solution. What is the pH at the start of the titration, before any barium hydroxide has been added?pH = b. What is the pH at the equivalence point in the titration of a 26.9 mL sample of a 0.401 M aqueous hydrofluoric acid solution with a 0.366 M aqueous sodium hydroxide solution?pH = ? c. When a 19.3 mL sample of a 0.459 M aqueous acetic acid solution is titrated with a 0.496 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration?pH = ?
What is the pH at the equivalence point in the titration of a 15.2 mL sample of a 0.316 M aqueous nitrous acid solution with a 0.337 M aqueous sodium hydroxide solution?pH =
What is the pH at the equivalence point in the titration of a 22.9 mL sample of a 0.351 M aqueous acetic acid solution with a 0.445 M aqueous potassium hydroxide solution? pH =

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