OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)

5th Edition

ISBN: 9781285460420

Author: John W. Moore; Conrad L. Stanitski

Publisher: Cengage Learning US

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Textbook Question

Chapter 15, Problem 19QRT

Select from Table 15.1 a conjugate acid-base pair that is suitable for preparing a buffer solution whose concentration (molarity) of hydronium ions is

(a) 3.55 × 10⁻⁴.
(b) 3.31 × 10⁻⁶.
(c) 4.79 × 10⁻⁹.
(d) 7.08 × 10⁻¹¹.

Explain your choices.

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Chapter 15, Problem 18QRT

Chapter 15, Problem 20QRT

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Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a)The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b)The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.

Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4 and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a) The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b) The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.

4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂

Chapter 15 Solutions

OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)

Ch. 15.1 - Predict whether 1.0 L of each solution is a...Ch. 15.1 - Calculate the pH of blood containing 0.0020-M...Ch. 15.1 - Prob. 15.2E Ch. 15.1 - Calculate the ratio of [] to [] in blood at a...Ch. 15.1 - Use the data in Table 15.1 to select a conjugate...Ch. 15.1 - Calculate the mole ratio of sodium acetate and...Ch. 15.1 - Calculate the pH of these buffers. Ch. 15.1 - If an abnormally high CO2 concentration is present...Ch. 15.1 - Calculate the minimum mass (g) of KOH that would...Ch. 15.2 - For the titration of 50.0 mL of 0.100-M HCl with...

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Select from Table 15.1 a conjugate acid-base pair that is suitable for preparing a buffer solution whose concentration (molarity) of hydronium ions is (a) 3.55 × 10 −4 . (b) 3.31 × 10 −6 . (c) 4.79 × 10 −9 . (d) 7.08 × 10 −11 . Explain your choices.

Solution Summary: The author explains that the conjugate acid-base pair that would be required to make a buffer solution with 3.55times 10-4

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Chapter 15 Solutions