Open Question
Rearrange the equation you wrote in Problem 10.50 to solve for [H₃O⁺] in terms of Kₐ.
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10. Acids and Bases
Ka and Kb
Struggling with GOB Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
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 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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