Textbook Question
Pick the stronger base from each pair. c. NO2– or NO3–
17. Acid and Base Equilibrium
Ka and Kb
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Which Bronsted-Lowry acid has the weakest conjugate base?
A
HCNO (Ka = 2.0 x 10-4)
B
HF (Ka = 3.5 x 10-4)
C
HN3 (Ka = 2.5 x 10-5)
D
H2CO3 (Ka = 4.3 x 10-7)
Verified step by step guidance1
Understand 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 given acids and their acid dissociation constants (Ka): 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 of the acids. The larger the Ka value, the stronger the acid.
Determine which acid has the largest Ka value, as this will correspond to the weakest conjugate base.
Conclude that the acid with the largest Ka value has the weakest conjugate base, based on the comparison of the given Ka values.
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