Which of the following mixtures would be described as buffer solution ?

A buffer solution is usually formed by mixing a weak acid and its conjugate base, or a weak base and its conjugate acid.

(A) is wrong because NaOH is a STRONG BASE & HCl is a STRONG ACID. At equal concentration, this reaction will not form a buffer solution, but a salt.

http://en.wikipedia.org/wiki/Acid-base

(B) is wrong because you mixing a WEAK ACID with a STRONG ACID. This won't create a Buffer solution because acetic acid's conjugate base will not appear this way.

(C) is wrong because the concentration of the STRONG BASE (0.1M) is of equal amount with the WEAK ACID (0.1). At this concentration, because NaOH is so strong, it will completely consume the acetic acid.

(E) is wrong because the concentration of the STRONG BASE is TOO SMALL. Its effect on the acetic acid will be negligible.

(D) is correct because you have the STRONG BASE at a concentration that is just right. It won't consume the acetic acid, but instead create a reaction that is in equilibrium.

A is a solution of 0.1 M NaCl not a buffer cannot neutralize acids or bases

B " " " " acetic acid and hydrochloric acid cannot neutralize acids = and has no buffer ability

C is a solution of 0.1M sodium acetate which will have a basic pH due to hydrolysis but cannot neutralize any added base..no buffer

D is a mixture of a weak acid and its conjugate base therefore it will possess buffer activity and have a starting pH of 4.76( = pKa of acetic acid ) since you have equal amounts of both forms good buffer capacity

E technically this is a mixture of a weak acid and its salt as well..The amount of base form ( acetate ) present is so small that the buffer capacity is so low that it would not functionally adequately as a useful buffer

A is not a buffer because there is no weak acid or weak base - both are strong.

B is not a buffer because there is no conjugate base for the (weak) acetic acid.

C is not a buffer because the moles of sodium hydroxide equals the moles of acetic acid - each component will be neutralized.

D IS a buffer because the concentration of sodium hydroxide is HALF that of the acetic acid. Half of the acetic acid is neutralized to form sodium acetate - the conjugate base of acetic acid.

E is not a buffer because there is not nearly enough sodium hydroxide to produce sufficient amounts of sodium acetate - there will be virtually no buffering capacity.

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