Multiple Choice
Hypobromous acid (Ka = 2.8 × 10−9) and hydrocyanic acid (Ka = 4.9 × 10−10) are both weak acids. Determine if reactants or products are favored in the following reaction.
HBrO (aq) + CN− (aq) ⇌ BrO− (aq) + HCN (aq)
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10. Acids and Bases
Ka and Kb
Multiple Choice
Identify which of the compounds is the strongest species.
A
Iodic acid pKa = 0.80
B
Acetic acid pKb = 9.24
C
Formic acid pKa = 3.75
D
Ammonium pKb = 4.75
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Verified step by step guidance1
Understand that in the Bronsted-Lowry theory, an acid donates a proton (H+) and forms its conjugate base.
Recognize that the strength of a conjugate base is inversely related to the strength of its acid. A stronger acid has a weaker conjugate base.
Identify the acid dissociation constant (Ka) for each acid given: HCNO (Ka = 2.0 x 10^-4), HF (Ka = 3.5 x 10^-4), HN3 (Ka = 2.5 x 10^-5), and H2CO3 (Ka = 4.3 x 10^-7).
Compare the Ka values: a larger Ka value indicates a stronger acid. Therefore, the acid with the largest Ka value will have the weakest conjugate base.
Determine which acid has the largest Ka value from the list, as this will indicate the acid with the weakest conjugate base.
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