HClO(aq)+H2O(l)⇄H3O+(aq)+ClO−(aq)Ka=3.98×10−8The acid ionization equilibrium for HClO at 25°C is shown above. A 0.100M aqueous solution of this acid has a pH of about 4.2. If a solution with an initial concentration of HClO of 0.200M is allowed to reach equilibrium at the same temperature, which of the following correctly predicts its pH, and why?AThe pH will be higher than 4.2 because increasing the concentration of the weak acid decreases the percent ionization.BThe pH will be higher than 4.2 because, for weak acid solutions, the pH is directly proportional to the initial concentration of the weak acid.CThe pH will be lower than 4.2 because increasing the concentration of the weak acid produces more H3O+ to establish equilibrium.DThe pH will be lower than 4.2 because the Ka of the weak acid is inversely proportional to the initial concentration of the weak acid.

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