Which of the following would NOT act as a buffer solution? A) A solution formed

Question

Which of the following would NOT act as a buffer solution?
A) A solution formed by adding 0.10 mol of acetic acid and and 0.10 mol of sodium acetate to 1.00 L of water
B) A solution formed by adding 0.10 mol of acetic acid and 0.10 mol of sodium hydroxide to 1.00 L of water
C) A solution formed by adding 0.10 mol of acetic acid and 0.050 mol of sodium acetate to 1.00 L of water
D) A solution formed by adding 0.10 mol of acetic acid and 0.050 mol of sodium hydroxide to 1.00 L of water
I am not sure how to answer this question, so I would really appreciate if you could explain this to me! I thought that buffers can only be formed by weak acid and it's conjugate base (answers A and C), so I thought that B) and D) are both incorrect but this question only has 1 correct answer. Plus then again I have no idea what mol values are there for. Thanks! Which of the following would NOT act as a buffer solution?
A) A solution formed by adding 0.10 mol of acetic acid and and 0.10 mol of sodium acetate to 1.00 L of water
B) A solution formed by adding 0.10 mol of acetic acid and 0.10 mol of sodium hydroxide to 1.00 L of water
C) A solution formed by adding 0.10 mol of acetic acid and 0.050 mol of sodium acetate to 1.00 L of water
D) A solution formed by adding 0.10 mol of acetic acid and 0.050 mol of sodium hydroxide to 1.00 L of water
I am not sure how to answer this question, so I would really appreciate if you could explain this to me! I thought that buffers can only be formed by weak acid and it's conjugate base (answers A and C), so I thought that B) and D) are both incorrect but this question only has 1 correct answer. Plus then again I have no idea what mol values are there for. Thanks!
A) A solution formed by adding 0.10 mol of acetic acid and and 0.10 mol of sodium acetate to 1.00 L of water
B) A solution formed by adding 0.10 mol of acetic acid and 0.10 mol of sodium hydroxide to 1.00 L of water
C) A solution formed by adding 0.10 mol of acetic acid and 0.050 mol of sodium acetate to 1.00 L of water
D) A solution formed by adding 0.10 mol of acetic acid and 0.050 mol of sodium hydroxide to 1.00 L of water
I am not sure how to answer this question, so I would really appreciate if you could explain this to me! I thought that buffers can only be formed by weak acid and it's conjugate base (answers A and C), so I thought that B) and D) are both incorrect but this question only has 1 correct answer. Plus then again I have no idea what mol values are there for. Thanks!

Explanation / Answer

C) A solution formed by adding 0.10 mol of acetic acid and 0.050 mol of sodium acetate to 1.00 L of water

Since the concentration of conjugate base is less than the weak acid which is almost half of the acid's concentration, the buffer capacity will be to low. The acid being a weak one is expected to have atleast equal concentration of its conjugate base. In case if the base is strong, lower concentration of base is acceptable since it would dissociate completely to give enough concentration of OH- to form a buffer with a weak acid.

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