In addition to the acid-dissociation constant, K_a. another characteristic of so

Question

In addition to the acid-dissociation constant, K_a. another characteristic of solutions of acids is percent ionization, determined by the following formula: Percent ionization = [HA] ionized/[HA] initial times 100% Percent ionization increases with increasing K_a. Strong acids, for which K_a is very large, ionize completely (100%). For weak acids, the percent ionization changes with concentration. The more diluted the acid is, the greater percent ionization. A convenient way to keep track of changing concentrations is through what is often called an I.C.E table, where I stands for " Initial Concentration" C stands for "Change" and E stands for "Equilibrium Concentration". To create such a table, write the reaction across the top, creating the columns, and write the rows I.C.E on the left-hand side. Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. Calculate the percent ionization of HA in a 0 010 Af solution. Express your answer to two ignescent figures, and Include the appropriate units.

Explanation / Answer

HA <==> H+ + A-

Ka = [H+][A-]/[HA]

Ka = x^2/0.1-x

4.1*10^-7 = x^2/0.1-x

or, 4.1 * 10^-8 - 4.1 *10^-7 x -x^2 = 0

x = 0.002 M

[A-] = 0.002 M

% ionization = (0.002/0.1) * 100 =2 %

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HA H+ A- inital 0.1 0 0 change -x +x +x equilibrium 0.1-x x x

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