A 0.185 M solution of a weak acid (HA) has

Roger Smith

Roger Smith

Answered question


A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (K3) for the acid.

Answer & Explanation



Beginner2022-01-10Added 31 answers

Step 1
Use the definition of pH to compute the equilibrium hydronium concentration of this solution.
Step 2
Create an ICE Table based on the given values, where I ''stands for the initial concentrations, C' stands for the changes in concentration, and'' E' stands for the equilibrium concentrations. Use multiples of z based on the stoichiometric coefficients in the balanced equilibrium equation to represent the changes in concentration in terms of x. Reactants decrease, so their changes are given negative values. Products increase, so their changes are given positive values. Keep in mind that the concentrations of liquids are never included in an ICE table. Note that the initial concentration of hydronium is 1.0×107 which is approximated to 0M.
Step 3
Sum the column under H3O+ to solve for x.
Step 4
Determine the equilibrium concentrations for all substances.
Step 5
Calculate the equilibrium constant from the equilibrium constant expression.

Gerald Lopez

Gerald Lopez

Beginner2022-01-11Added 29 answers

Step 1
The amount of acid present HA is 0.185M.
The pH of the given acid is 2.95
Step 2
The formula for the answer is,
Change the pH value in the formula above.
The following is the ICE table for the acid's dissociation reaction:
 HA+H2OH3O++AInitial concentration(M)0.185  0 0Change in concentration(M)x  +x +xEquilibrium(M)0.185x  x x
Step 3
The expression for Ka is shown below.
It is seen from the ICE table that [H3O+]=[A]=x=1.122×103
Replace the values in the equation above.
The Ka of given acid is 6.8×106

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