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ignment/takeCovalentActivity.do?locator-assignment-take&takeAssignmentSessionLocator-assignment-t; 17 References INTERACTIVE EXAMPLE Determining Ka from the Solution pH A weak acid, HA, is a monoprotic acid. A solution that is 0.100 Min HA has a pH of 1.970 at 25°c HA(aq) + H20 Ho (a) +A (aq) What is the acid-ionization constant, Ka. for this acid? What is the degree of ionization of the acid in this solution? Degree of ionization = Submit Show Tutor Steps Submit Answer 10 item attempts remaining

Explanation / Answer

Weak acid dissociates as

HA +H2O A- + H3O+

Ka = [A-][H3O+] / [AH]

[HA] = 0.100 M

[H3O+] = 10-pH = 10-1.970 = 0.010715 M

Acid is monoprotic therefore [A-] = [H3O+] = 0.010715 M

substitute value

Ka= (0.010715) (0.010715) / 0.100 = 0.001148 = 1.148 X 10-3

Ka= 1.148 X 10-3

Degree of ionization = [H3O+] / [HA] = (0.010715) / (0.100) = 0.10715

Degree of ionization = 0.10715

some time we express degree of ionization in percent

percent ionization =  [H3O+] X 100 / [HA] = (0.010715) X(100) / (0.100) = 10.715 %

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