Asked by Jordan
Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations
A) 0.377 M
B) 0.107 M
C) 4.16*10^-2 M
Ka= 1.9*10^-5
A) 0.377 M
B) 0.107 M
C) 4.16*10^-2 M
Ka= 1.9*10^-5
Answers
Answered by
DrBob222
..........HN3 ==> H^+ + N3^-
I.........0.377....0.....0
C.........-x.......x......x
E........0.377-x....x.....x
Ka = (H^)(N3^-)/(HN3)
Subtitute and solve for x = (H^+). Then % ion = [(H^+)/(HN3)]*100 = ?
Watch the lower cncns; they may require solving a qudratic.
I.........0.377....0.....0
C.........-x.......x......x
E........0.377-x....x.....x
Ka = (H^)(N3^-)/(HN3)
Subtitute and solve for x = (H^+). Then % ion = [(H^+)/(HN3)]*100 = ?
Watch the lower cncns; they may require solving a qudratic.
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