High School Chemistry : Using Acid Dissociation Constant (Ka)
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Example Questions
Example Question #1 : Using Acid Dissociation Constant (Ka)
What is the concentration of hydronium ions in a solution if the hydroxide ion concentration is 
For every acidic or basic solution, the product of the hydroxide ion concentration and the hydronium ion concentration will be equal to 
Since we are given the hydroxide ion concentration, we can determine the hydronium ion concentration using this equation.
Example Question #1 : Using Acid Dissociation Constant (Ka)
A student has a 0.50M solution of acetic acid. She adds solid sodium acetate until the concentration of sodium acetate is 0.050M. What is the final pH of the solution?
The 
Acetic acid is a weak acid, and its dissociation reaction is written as:
Using an ICE table, we can find the pH of the solution when the sodium acetate is added:
I: There is initially a 0.50M concentration of acetic acid. Because sodium acetate will dissolve completely, there will be a 0.050M concentration of acetate ions in the solution.
C: As acetic acid dissociates, the concentrations of acetate ions and hydronium ions will increase by an unknown concentration 
E: By setting the equilibrium expression equal to the acid equilibrium constant, we can solve for the value of 
*Because the value for 
Keep in mind that 
Use this value in the equation for pH:
Example Question #2 : Using Acid Dissociation Constant (Ka)
What property distinguishes a strong acid from a weak acid?
A weak acid will fail to dissociate completely in water and have a high Ka value
There is no difference between a strong acid and a weak acid based on their properties in water
A strong acid will dissociate completely in water and have a high Ka value
A strong acid will dissociate completely in water and have a low Ka value
A weak acid will dissociate completely in water and have a low Ka value
A strong acid will dissociate completely in water and have a high Ka value
The acid dissociation constant (Ka) is used to distinguish strong acids from weak acids. Strong acids have exceptionally high Ka values.
The Ka value is found by looking at the equilibrium constant for the dissociation of the acid. The higher the Ka, the more the acid dissociates. Thus, strong acids must dissociate more in water. In contrast, a weak acid is less likely to ionize and release a hydrogen ion, thus resulting in a less acidic solution.
This equation makes it clear that the more the acid converts from its original form to its ionzied, dissociated form, the higher the Ka value will be.
Example Question #3 : Using Acid Dissociation Constant (Ka)
Which of the following is what determines the strength of an acid?
The Ka
How many bonds the central atom makes
The Kb
Electronegativity values
Its physical state
The Ka
The Ka is the acid dissociation constant, and thus it is what determines how strong the acid is. Stronger acids dissociate to a greater extent and produce lower pH values.
Example Question #2 : Using Acid Dissociation Constant (Ka)
Determine the equilibrium concentration of 
The definition of 
Set up an "ICE" table:
Plug in values:
Use the quadratic formula to solve:
Example Question #33 : Acid Base Chemistry
Determine the equilibrium concentration of 
Set up an "ICE" table
Plug in values:
Use the quadratic formula:
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