pH, pOH, pKa, and pKb
The symbol "p" means "the negative of the logrithm of." "p" is often used with very small or very large values.- Calculating pH
- Calculating hydronium ion concentration from pH
- Calculating pOH
- Calculating hydroxide ion concentration from pOH
- The relationship between pH and pOH
- Calculating pKa
- Calculating Ka from pKa
- Calculating pKb
- Calculating Kb from pKb
To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter (molarity). The pH is then calculated using the expression:
pH = - log [H3O+].
Example: Find the pH of a 0.0025 M HCl solution. The HCl is a strong acid and is 100% ionized in water. The hydronium ion concentration is 0.0025 M. Thus:
pH = - log (0.0025) = - ( - 2.60) = 2.60
Calculating the Hydronium Ion Concentration from pH
The hydronium ion concentration can be found from the pH by the reverse of the mathematical operation employed to find the pH.
[H3O+] = 10-pH or [H3O+] = antilog (- pH)
Example: What is the hydronium ion concentration in a solution that has a pH of 8.34?
- 8.34 = log [H3O+]
[H3O+] = 10-8.34 = 4.57 x 10-9 M
On a calculator, calculate 10-8.34, or "inverse" log ( - 8.34).
To calculate the pOH of a solution you need to know the concentration of the hydroxide ion in moles per liter (molarity). The pOH is then calculated using the expression:
pOH = - log [OH-]
Example: What is the pOH of a solution that has a hydroxide ion concentration of 4.82 x 10-5 M?
pOH = - log [4.82 x 10-5] = - ( - 4.32) = 4.32
Calculating the Hydroxide Ion Concentration from pOH
The hydroxide ion concentration can be found from the pOH by the reverse mathematical operation employed to find the pOH.
[OH-] = 10-pOH or [OH-] = antilog ( - pOH)
Example: What is the hydroxide ion concentration in a solution that has a pOH of 5.70?
5.70 = - log [OH-]
-5.70 = log[OH-]
[OH-] = 10-5.70 = 2.00 x 10-6 M
On a calculator calculate 10-5.70, or "inverse" log (- 5.70).
Relationship Between pH and pOH
The pH and pOH of a water solution at 25oC are related by the following equation.
pH + pOH = 14
If either the pH or the pOH of a solution is known, the other can be quickly calculated.
Example: A solution has a pOH of 11.76. What is the pH of this solution?
pH = 14 - pOH = 14 - 11.76 = 2.24
The pKa is calculated using the expression:
pKa = - log (Ka)
where "Ka" is the equilibrium constant for the ionization of the acid.
Example: What is the pKa of acetic acid, if Ka for acetic acid is 1.78 x 10-5?
pKa = - log (1.78 x 10-5) = - ( - 4.75) = 4.75
The Ka for an acid is calculated from the pKa by performing the reverse of the mathematical operation used to find pKa.
Ka = 10-pKa or Ka = antilog ( - pKa)
Example: Calculate the value of the ionization constant for the ammonium ion, Ka, if the pKa is 9.74.
9.74 = - log (Ka)
-9.74 = log (Ka)
Ka = 10-9.74 = 1.82 x 10-10
On a calculator calculate 10-9.74, or "inverse" log ( - 9.74).
The pKb is calculated using the expression:
pKb = - log (Kb)
where Kb is the equilibrium constant for the ionization of a base.
Example: What is the pKb for methyl amine, if the value of Kb for methyl amine is 4.4 x 10-4?
pKb = - log (4.4 x 10-4) = - ( - 3.36) = 3.36
The Kb for an acid is calculated from the pKb by performing the reverse of the mathematical operation used to find pKb.
Kb = 10-pKb or Kb = antilog ( - pKb)
Example: Calculate the value of the ionization constant, Kb, for aniline if the pKb is 9.38.
9.38 = - log (Kb)
-9.38 = log (Kb)
Kb = 10-9.38 = 4.17 x 10-10
On a calculator calculate 10-9.38, or "inverse" log ( - 9.38).
