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18 Nov 2019
A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift also results in a pH shift of the system. It is the presence of the common ion in the system that results in buffering behaviour, because both added H^+ or OH^- ions can be neutralized. What is the pH change of a 0.300 mol L^-1 solution of citric acid (pK_a = 4.77) if citrate is added to a concentration of 0.170 mol L^-1 with no change in volume? Express the difference in pH numerically to two decimal places.
A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift also results in a pH shift of the system. It is the presence of the common ion in the system that results in buffering behaviour, because both added H^+ or OH^- ions can be neutralized. What is the pH change of a 0.300 mol L^-1 solution of citric acid (pK_a = 4.77) if citrate is added to a concentration of 0.170 mol L^-1 with no change in volume? Express the difference in pH numerically to two decimal places.
Jamar FerryLv2
1 Sep 2019