In each of two flasks, a solution is prepared by placing 0.25 mol acetic acid, C

Question

In each of two flasks, a solution is prepared by placing 0.25 mol acetic acid, CH3COOH, 0.25 mol acetate ions, CH3COO-, in sufficient water to prepare 1.00 liter of solution. These two solutions are used for the experiments described in parts B. and C. below:

A) What is the buffer solution? What characteristics make this solution a buffer solution?

B) Added to the solution in one flask is 0.15 mol KHSO4 (s). What is the effect on [CH3COOH] and [CH3COO-]? Account for your answer in terms of numbers of moles of protons transferred. Has the capacity of the buffer been exceeded? Explain.

C.) Added to the solution in one flask is 0.40 mol NaOH (s). What is the effect on [CH3COOOH] and [CH3COOH-]? Account for your answer in terms of moles of protons transferred. Has the capacity of the buffer been exceeded? Explain.

Explanation / Answer

A) Buffer solution is the solution which resists change in pH. yes it forms buffer.

B) [CH3COOH] increase and [CH3COO-] decreases, since H+(proton) increase acid concentration and neutralises bases.

Buffer capacity is decreased since concentration of conjugate base [CH3COO-] is decreased

C) [CH3COOH] decreases since OH- reacts with H+ and [CH3COO-] concetration increases.

Buffer capacity is increased due to increase in conjugate base concetration.

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