A. contains approximately equal amounts of a weak acid and its conjugate base.
B. increases its properties with an increase in the concentrations of the two buffer components.
C. resists changes in pH.
D. all of the above
This one is D right
I agree D is right but ONLY if you tell me what "approximately" in A means. Both B and C are correct. If this question has only ONE answer, then A must be true which makes D true. But I see buffer solutions on this board all the time with (Base) = 0.2(Acid) which makes the ratio about 5:1. That doesn't sound like approximately equal to me.
Yes, that's correct! The answer is D, all of the above. A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added to it. It achieves this by containing approximately equal amounts of a weak acid and its conjugate base. The weak acid can donate a proton (H+) to neutralize any added base, while the conjugate base can accept a proton to neutralize any added acid. The concentrations of the weak acid and its conjugate base determine the buffering capacity of the solution. If you increase the concentrations of both buffer components, the buffer solution will be able to resist larger changes in pH.
