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The pH of a solution containing an acid can be determined using its acid dissociation constant and initial concentration. If a solution contains two different acids, then its pH can be determined using one of several methods depending on the relative strength of the acids and their dissociation constants.
In a strong and weak acid mixture, the strong acid dissociates completely and becomes a source of almost all the hydronium ions present in the solution. In contrast, the weak acid shows partial dissociation and produces a negligible concentration of hydronium ions. The high concentration of hydronium ions produced by the strong acid further reduces the dissociation of the weak acid. According to Le Chatelier's principle, this happens: "When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance." The excess hydronium ions produced by the strong acid disturb the equilibrium, and thus, the reaction will move in the reverse direction until the equilibrium is established. This leads to a decrease in the dissociation of the weak acid. Because of this decrease, the pH of a strong and weak acid mixture can be calculated from the concentration of the strong acid only. For example, the pH of a mixture with an equal concentration of hydrochloric acid (HCl), a strong acid, and formic acid (HCHO2), a weak acid, can be determined from the concentration of HCl only. If the concentration of the HCl in the mixture is 0.0020 M, its pH can be calculated as follows.
pH = −log(0.002) = 2.7
Here, the concentration of hydronium ions produced by HCHO2 and the autoionization of water is negligible and thus can be ignored.
A Mixture of Two Weak Acids with Different Dissociation Constants
In a mixture of two weak acids, the pH of a mixture will be determined by the stronger acid if its dissociation constant is significantly higher than the weaker acid. For example, in a mixture with an equal concentration of nitrous acid (HNO2) and hypochlorous acid (HClO), the HNO2 will be the main determinant of the pH of the mixture as its Ka (4.6 × 10−4) is approximately 10,000 times higher than the Ka (2.9 × 10−8) of HClO. According to Le Chatelier's principle, HClO shows decreased dissociation in the presence of HNO2.
