A weak acid (HA) has a pKa of 4.679. If a solution of this acid has a pH of 4.876, what percentage of the acid is not ionized? (Assume all H in solution came from the ionization of HA.)
Problem is based on the concept of chemical equilibrium. Equilibrium is attained by a reaction if rate of change of concentration of reactant is equal to rate of change of concentration of product.
For a solution, pH is the measure of acidity/basicity of a compound in that solution.
Percentage ionization is the extent of dissociated form of an acid/base in a solution.
For a solution, pH is equal to the negative of log of concentration of ions in a solution.
For acid HA,
Acid dissociation constant is calculated as follows:
Here, is concentration of hydrogen ion, is concentration of anion and is concentration of undissociated acid in solution.
Percentage ionization is calculated as follows:
Here, is concentration of hydrogen ion and is concentration of undissociated acid in solution.
For an acid,
Substitute, thus,
Or,
Calculate the concentration of ions from pH as follows:
Substitute, 4.876 for pH thus,
Or,
The dissociation reaction of acid is as follows;
Concentration of ions is. ICE table for this reaction is as follows:
Now,
Substitute, for , for , for and for
Rearrange,
Or,
Calculate the percentage ionization as follows:
Substitute,for and for thus,
Calculate unionized percent of acidas follows:
Substitute, for thus,
Ans:
The unionized percent of acid is 39 %
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