How To Calculate Ka From Ph

Every acid has a characteristic dissociation constant (K_a), which is a measure of its ability to donate hydrogen ions in solution. In other words, K_a provides a way to gauge the strength of an acid. Larger values signify stronger acids. The pH (power of hydrogen) of a solution is a measure of the concentration of hydrogen ions and is also a measure of acidity, but it isn't the same as K_a. There's a relationship between the two, though, and you can calculate K_a for an acid if you know the concentration of acid and the pH of the solution.

A compound is acidic if it can donate hydrogen ions to an aqueous solution, which is equivalent to saying the compound is capable of creating hydronium ions (H₃0⁺). The general equation describing what happens to an acid (HA) in solution is:

HA + H₂0 <--> H₃0⁺ + A^-, where A^- is the conjugate base.

Some acids are strong and dissociate completely while others are weak and only partially dissociate. You can measure the strength of an acid by its dissociation constant K_a, which is a ratio formed by dividing the concentration of products by the concentration of reactants:

K_a = [H30+] [A-]/[HA]

All the reactions happen in water, so it it's usually deleted from the equation.

The pH of an aqueous acid solution is a measure of the concentration of free hydrogen (or hydronium) ions it contains: pH = -log [H⁺] or pH = -log [H₃0⁺]. The last equation can be rewritten:

[ H₃0⁺] = 10^-pH

It you know the molar concentration of an acid solution and can measure its pH, the above equivalence allows you to calculate the relative concentration of acid to conjugate base and derive the dissociation constant K_a. To do this, it helps to set up a table that delineates the Initial concentrations of reactants and products, the Change in concentrations and the concentrations at Equilibrium. This is an ICE table. Rather than setting one up in a general way, it's more instructive to illustrate the procedure with a specific example.

Acetic acid, the acid that gives vinegar its sour taste, is a weak acid that dissociates into acetate and hydronium ions in solution.

CH₃CO₂H + H₂O <--> CH₃CO₂⁻ + H₃O⁺

Typical household vinegar is a 0.9 M solution with a pH of 2.4. Using the data, it's possible to calculate the dissociation constant:

1. Set Up the ICE Table for Concentrations

Acetic Acid (CH₃CO₂₎H) Hydronium Ions (H3O⁺) Acetate Ions ( CH₃CO₂^-)

Initial 0.9 M 0 0

Change -x M +x M +x M

Equilibrium (0.9 – x) M x M x M

2. Write Ka as Ratio of Conjugate Base to Acid

The dissociation constant K_a is [H3O+] [CH₃CO₂^-] / [CH₃CO₂₎H].

3. Plug in Values from the Table

K_a = x²/(0.9 – x)

4. Note that x is Related to pH and Calculate Ka

As noted above, [H3O+] = 10^-pH. Since x = [H3O⁺] and you know the pH of the solution, you can write x = 10^-2.4. It is now possible to find a numerical value for Ka.

Ka = (10^-2.4)² /(0.9 – 10^-2.4) = 1.8 x 10^-5.