a)
HIO dissociates as:
HIO
-----> H+ + IO-
0.146
0 0
0.146-x
x x
Ka = [H+][IO-]/[HIO]
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 ((2.3*10^-11)*0.146) = 1.832*10^-6
since c is much greater than x, our assumption is correct
so, x = 1.832*10^-6 M
% dissociation = (x*100)/c
= 1.832*10^-6*100/0.146
= 1.255*10^-3 %
Answer: 1.26*10^-3 %
b)
HIO dissociates as:
HIO
-----> H+ + IO-
0.564
0 0
0.564-x
x x
Ka = [H+][IO-]/[HIO]
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 ((2.3*10^-11)*0.564) = 3.602*10^-6
since c is much greater than x, our assumption is correct
so, x = 3.602*10^-6 M
% dissociation = (x*100)/c
= 3.602*10^-6*100/0.564
= 6.386*10^-4 %
Answer: 6.39*10^-4 %
c)
HIO dissociates as:
HIO
-----> H+ + IO-
0.797
0 0
0.797-x
x x
Ka = [H+][IO-]/[HIO]
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 ((2.3*10^-11)*0.797) = 4.281*10^-6
since c is much greater than x, our assumption is correct
so, x = 4.281*10^-6 M
% dissociation = (x*100)/c
= 4.281*10^-6*100/0.797
= 5.372*10^-4 %
Answer: 5.37*10^-4 %
Calculate the percent ionization of hypolodous acid (HIO) in solutions of each of the following concentrations...
23. + -/0.1 points 0/4 Submissions Used Calculate the percent ionization of hypoiodous acid (HIO) in solutions of each of the following concentrations (Ka = 2.3e-11.) (a) 0.235 M % (b) 0.401 M % (C) 0.791 M %
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 %
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 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 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 %
Calculate the percent ionization of carbonic acid (H2CO3) in solutions of each of the following concentrations (Ka = 4.3e-07.) (a) 0.193 M (b) 0.371 M (c) 0.783 M
Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook). -7.96
23. Calculate the percent ionization of hydrosulfuric acid (H2S) in solutions of each of the following concentrations (Ka = 9.5e-08.) (a) 0.171 M ________ % (b) 0.454 M _______ % (c) 0.809 M ______ %