Multiple Choice
Calculate the pH of a 0.500 M pyridine (C5H5N) solution. Kb value for pyridine is 1.7 × 10−9.
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17. Acid and Base Equilibrium
Ka and Kb
Multiple 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
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 acid donates a proton (H+) and forms a conjugate base. The strength of the acid is inversely related to the strength of its conjugate base.
Recognize that the acid dissociation constant (Ka) is a measure of the strength of an acid in solution. A larger Ka value indicates a stronger acid, which means a weaker conjugate base.
Compare the given Ka values for each acid: H3BO3 (Ka = 5.4 × 10^−10), HF (Ka = 3.5 × 10^−4), HNO2 (Ka = 4.6 × 10^−4), and HClO (Ka = 2.9 × 10^−8).
Identify the acid with the largest Ka value, as this will have the weakest conjugate base. In this case, compare the Ka values to determine which is the largest.
Conclude that the acid with the largest Ka value is the strongest acid and therefore has the weakest conjugate base. Based on the comparison, identify HNO2 as the acid with the weakest conjugate base.
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