If the ka of a monoprotic weak acid is 5.4 × 10-6, what is the ph of a 0.14 m solution of this acid?

pH = 2.1

Let resembles the acid; as a weak acid (a small value of ) would partially dissociate to produce protons and , its conjugate base. Let the final proton concentration (i.e., ) be . (Apparently ) Construct the following RICE table:

By definition, (all concentrations are under equilibrium condition)

It is given that

Equating and simplifying the two expressions gives a quadratic equation; solve the equation for gives:

The pH of a solutions equals the opposite of the logarithm of its proton concentration to base 10; thus for this particular solution

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