Consider the K_a values for the following acids:
Cyanic acid,HOCN,3.5 $\times$ 10^-4
Formic acid,HCHO₂,1.7 $\times$ 10^-4
Lactic acid,HC₃H₅O₃,1.3 $\times$ 10^-4
Propionic acid,HC₃H₅O₂,1.3 $\times$ 10^-5
Benzoic acid,HC₇H₅O₂,6.3 $\times$ 10^-5
Given initially equimolar solutions of each weak acid,which solution will have the highest pH once equilibrium is established?

Question

Consider the K_a values for the following acids:
Cyanic acid,HOCN,3.5

\times

10^-4
Formic acid,HCHO₂,1.7

\times

10^-4
Lactic acid,HC₃H₅O₃,1.3

\times

10^-4
Propionic acid,HC₃H₅O₂,1.3

\times

10^-5
Benzoic acid,HC₇H₅O₂,6.3

\times

10^-5
Given initially equimolar solutions of each weak acid,which solution will have the highest pH once equilibrium is established?

Quizplus · Accepted Answer

The Answer of Consider the K_a values for the following acids: Cyanic acid,HOCN,3.5 $\times$ 10^-4 Formic acid,HCHO₂,1.7 $\times$ 10^-4 Lactic acid,HC₃H₅O₃,1.3 $\times$ 10^-4 Propionic acid,HC₃H₅O₂,1.3 $\times$ 10^-5 Benzoic acid,HC₇H₅O₂,6.3 $\times$ 10^-5 Given initially equimolar solutions of each weak acid,which solution will have the highest pH once equilibrium is established?

Consider the Ka Values for the Following Acids: Cyanic Acid,HOCN,3 ×\times×

Consider the K_a Values for the Following Acids:
Cyanic Acid,HOCN,3 $\times$