Ch.16 - Aqueous Equilibria: Acids & Bases
Chapter 16, Problem 13
Consider the reaction: SO2 + OH- S HSO3 -. Which reaction scheme shows the correct use of the curved arrow notation representing the donation of an electron pair and the correct labeling of the Lewis acid and Lewis base? (LO 16.14) (a) (b) (c) (d)
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Related Practice
Textbook Question
What is the pH of an aqueous solution of Ca1OH22 at 25.0 °C
with a concentration of 6.3 * 10-5 M? (LO 16.7)
(a) 4.20 (b) 10.10
(c) 11.36 (d) 9.80
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Textbook Question
An acid solution with a concentration of 0.500 M has a
pH = 3.21. What is the Ka of the acid? (LO 16.8)
(a) 1.2 * 10-5 (b) 1.7 * 10-6
(c) 7.6 * 10-7 (d) 5.4 * 10-3
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Textbook Question
Ammonia 1NH32 has base dissociation constant 1Kb2 of
1.8 * 10-5. What is the concentration of an aqueous ammonia
solution that has a pH of 11.68? (LO 16.11)
(a) 0.28 M (b) 3.6 M
(c) 9.0 * 10-3 M (d) 1.3 M
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Textbook Question
What is the pH and the principal source of H3O+ ions in 1.0 * 10-10 M HCl? (Hint: The pH of an acid solution can’t exceed 7.) What is the pH of 1.0 * 10-7 M HCl?
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Textbook Question
Calculate the pH of solutions prepared by:
(d) Mixing equal volumes of 0.20 M HCl and 0.50 M HNO3.
(Assume that volumes are additive.)
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Textbook Question
The acidity of lemon juice is derived primarily from citric acid (H3Cit), a triprotic acid. What are the concentrations of H3Cit, H2Cit-, HCit2-, and Cit3- in a sample of lemon juice that has a pH of 2.37 and a total concentration of the four citrate-containing species of 0.350 M?
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