Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka = 1.9e-05.)
(a) 0.267 M %
(b) 0.530 M %
(c) 0.768 M %
a)
HN3 dissociates as:
HN3 -----> H+ + N3-
0.267 0 0
0.267-x x x
Ka = [H+][N3-]/[HN3]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((1.9*10^-5)*0.267) = 2.252*10^-3
since c is much greater than x, our assumption is correct
so, x = 2.252*10^-3 M
% dissociation = (x*100)/c
= 2.252*10^-3*100/0.267
= 0.8436 %
Answer: 0.844 %
b)
HN3 dissociates as:
HN3 -----> H+ + N3-
0.53 0 0
0.53-x x x
Ka = [H+][N3-]/[HN3]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((1.9*10^-5)*0.53) = 3.173*10^-3
since c is much greater than x, our assumption is correct
so, x = 3.173*10^-3 M
% dissociation = (x*100)/c
= 3.173*10^-3*100/0.53
= 0.5987 %a
Answer: 0.599 %
c)
HN3 dissociates as:
HN3 -----> H+ + N3-
0.768 0 0
0.768-x x x
Ka = [H+][N3-]/[HN3]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((1.9*10^-5)*0.768) = 3.82*10^-3
since c is much greater than x, our assumption is correct
so, x = 3.82*10^-3 M
% dissociation = (x*100)/c
= 3.82*10^-3*100/0.768
= 0.4974 %
Answer: 0.497 %
Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations...
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). 1.9 * 10^-5 Part A: 0.372 M Express your answer using two significant figures. Part B: 0.112 M Express your answer using two significant figures. Part C: 4.31×10−2 M . Express your answer using two significant figures.
Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (K, is given in Appendix D in the textbook). Part A 0.430 M Express your answer using two significant figures. PO AEO ? Submit Request Answer Part B 0.112 M Express your answer using two significant figures. ΡΟ ΑΣφ ? % Submit Request Answer Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (K, is given in...
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 0.406 M . Express your answer using two significant figures. TemplatesSymbols undoredoresetkeyboard shortcutshelp nothing % % SubmitRequest Answer Part B 0.118 M . Express your answer using two significant figures. TemplatesSymbols undoredoresetkeyboard shortcutshelp nothing % % SubmitRequest Answer Part C 4.03×10−2 M . Express your answer using two significant figures.
roblem 16.63 Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (K, is given in Appendix D in the textbook). Part A 0.430 M Express your answer using two significant figures. VE ΑΣφ ? Submit Request Answer Part B 0.112 M Express your answer using two significant figures. VO ΑΣφ ? Submit Request Answer Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (K, is given...
1.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). 0.435 M . 0.111 M . 3.79×10−2 M . 2.Consider two solutions, solution A and solution B. [H+] in solution A is 290 times greater than that in solution B. What is the difference in the pH values of the two solutions? Express your answer using two decimal places. 3.What volume of CO2 at 25...
Calculate the percent ionization of benzoic acid (HC2H5O2) in solutions of each of the following concentrations (Ka = 6.3e-05.) (a) 0.242 M % (b) 0.556 M % (C) 0.883 M
Calculate the percent ionization of ascorbic acid (HC6H7O6) in solutions of each of the following concentrations (Ka = 8.0e-05.) (a) 0.185 M % (b) 0.575 M % (c) 0.740 M %
Calculate the percent ionization of boric acid (H3BO3) in solutions of each of the following concentrations (Ka = 5.8e-10.) ( a) 0.269 M _____% (b) 0.324 M _____% (c) 0.737 M _____%
Calculate the percent ionization of hypobromous acid (HBrO) in solutions of each of the following concentrations (Ka = 2.5e-09.) (a) 0.271 M % (b) 0.388 M % (c) 0.794 M %
Calculate the percent ionization of hypochlorous acid (HClO) in solutions of each of the following concentrations (Ka = 3.0e-08.) (a) 0.144 M % (b) 0.568 M % (c) 0.896 M %