Multiple Choice
Identify which of the compounds is the strongest species.
10. Acids and Bases
Ka and Kb
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Identify a Bronsted-Lowry acid with weakest conjugate base.
A
H3BO3 Ka = 5.4 × 10−10
B
HF Ka = 3.5 × 10−4
C
HNO2 Ka = 4.6 × 10−4
D
HClO Ka = 2.9 × 10−8
Verified step by step guidance1
Understand that a Bronsted-Lowry base is a substance that can accept a proton (H+). In aqueous solutions, these bases will react with water to produce hydroxide ions (OH-).
The strength of a base in water is indicated by its base dissociation constant, Kb. A larger Kb value means the base is stronger and will produce more hydroxide ions in solution.
Compare the given Kb values for each base: C2H8N2 (Kb = 8.3 x 10^-5), C5H5N (Kb = 1.7 x 10^-9), (CH3)3N (Kb = 1.0 x 10^-6), C3H7NH2 (Kb = 3.5 x 10^-4), and C6H5NH2 (Kb = 3.9 x 10^-10).
Identify the base with the largest Kb value, as this base will have the greatest concentration of hydroxide ions in solution.
Conclude that C3H7NH2, with a Kb of 3.5 x 10^-4, has the greatest concentration of hydroxide ions among the given options.
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