The wrong statement among the following is
Correct answer: D. Addition of sodium acetate to a buffer solution of sodium acetate and acetic acid does not affect its pH
- A. Buffer solutions have reserve pH
- B. An acidic buffer mixture can be prepare by mixing a solution of formic acid and sodium formate
- C. Buffer solution resist the change in pH by the addition of an acid or base
- D. Addition of sodium acetate to a buffer solution of sodium acetate and acetic acid does not affect its pH
Explanation
Adding sodium acetate to a buffer solution of sodium acetate and acetic acid will increase the pH of the solution. This is because sodium acetate is the conjugate base of acetic acid, and adding more conjugate base will shift the equilibrium towards the deprotonated form of the acid, which is the acetate ion. The acetate ion has a higher pH than the acetic acid molecule, so adding sodium acetate will increase the overall pH of the solution.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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