Titrations (weak acid/strong base) When a 18.4 mL sample of a 0.355 M aqueous hydrofluoric acid solution is titrated with a 0.462 M aqueous barium hydroxide solution, whatis the pH at the midpoint in the titration?pH = What is the pH at the equivalence point in the titration of a 15.6 mL sample of a 0.442 M aqueous hydrofluoric acid solution with a 0.319 Maqueous sodium hydroxide solution?pH =

2 HF (aq) + Ba(OH)2 (aq) -----> BaF2 (aq) + 2 H2O (l) Ka for HF =7.2 × 10–4pKa = – logKa = –…

Answered: When a 18.4 mL sample of a 0.355 M…

When a 18.4 mL sample of a 0.355 M aqueous hydrofluoric acid solution is titrated with a 0.462 M aqueous barium hydroxide solution, what is the pH at the midpoint in the titration? pH =

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

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Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.101E

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Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.
You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.
Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?
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.
Three students titrate different samples of the same solution of HCI to obtain its molarity. Below are their data. Student A: 20.00mLHCl+20.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student B: 20.00mLHCl+40.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student C: 20.00mLHCl+20.00mLH2O 0.100 M Ba(OH)2 used to titrate to the equivalence point. All the students calculated the molarities correctly. Which (if any) of the following statements are true? (a) The molarity calculated by A is half that calculated by B. (b) The molarity calculated by A is equal to that calculated by C. (c) The molarity calculated by B is twice that calculated by C. (d) The molarity calculated by A is twice that calculated by B. (e) The molarity calculated by A is equal to that calculated by B.
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.
A 5.36-g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L.. (a) What is the pH of this buffer solution?. (b) Is the solution acidic or basic?. (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?
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?
What is the pH at the equivalence point in the titration of a 23.9 mL sample of a 0.387 M aqueous hydrofluoric acid solution with a 0.496 M aqueous potassium hydroxide solution?
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 20.3 mL sample of a 0.386 M aqueous acetic acid solution with a 0.472 M aqueous potassium hydroxide solution?
What is the pH at the equivalence point in the titration of a 16.3 mL sample of a 0.497 M aqueous hypochlorous acid solution with a 0.446 M aqueous sodium hydroxide solution?

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