Problem 16.63
Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook).
Part A
0.388 M .
Express your answer using two significant figures.


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Part B
0.117 M .
Express your answer using two significant figures.


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Part C
3.61×10^{−2} M .
Express your answer using two significant figures.


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Ka = Cα^{2} α= percent ionization
α = (Ka/C)^{1/2}
Ka of hydrazoic acid (HN3) = 1.9 x10^{5}
A) C= 0.388 M
α = (Ka/C)^{1/2}
= ( 1.9 x10^{5} / 0.388)^{1/2}
= 0.007
= 0.7 %
Therefore, percent ionization = 0.7 %
B)
C= 0.117 M
α = (Ka/C)^{1/2}
= ( 1.9 x10^{5} / 0.117)^{1/2}
= 0.012
= 1.2 %
Therefore, percent ionization =1.2 %
C)
C= 3.61×10^{−2} M
α = (Ka/C)^{1/2}
= ( 1.9 x10^{5} / 3.61×10^{−2} )^{1/2}
= 0.023
= 2.3 %
Therefore, percent ionization = 2.3 %
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