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.
                                                    There are no AI answers yet. The ability to request AI answers is coming soon!
                                            
                Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.