A 1.0-L buffer solution is 0.10 M in HF and 0.050 M in NaF. Which action destroys the buffer? (a) adding 0.050 mol of HCl (b) adding 0.050 mol of NaOH (c) adding 0.050 mol of NaF (d) none of the above

Question

Addyson Hughes

Chemistry

13 August, 05:23

A 1.0-L buffer solution is 0.10 M in HF and 0.050 M in NaF. Which action destroys the buffer? (a) adding 0.050 mol of HCl (b) adding 0.050 mol of NaOH (c) adding 0.050 mol of NaF (d) none of the above

+5

Answers (1)

Know the Answer?

Casey Banks · Answer 1

(a) adding 0.050 mol of HCl

Explanation:

A buffer is defined as the mixture of a weak acid and its conjugate base - or vice versa-.

In the buffer:

1.0L * (0.10 mol / L) = 0.10 moles of HF - Weak acid-

1.0L * (0.050 mol / L) = 0.050 moles of NaF - Conjugate base-

-The weak acid reacts with bases as NaOH and the conjugate base reacts with acids as HCl-

Thus:

(a) adding 0.050 mol of HCl: The addition of 0.050moles of HCl produce the reaction of 0.050 moles of NaF producing HF. That means after the reaction, all NaF is consumed and you will have in solution just the weak acid destroying the buffer.

(b) adding 0.050 mol of NaOH: The NaOH reacts with HF producing more NaF. Would be consumed just 0.050 moles of HF - remaining 0.050 moles of HF-. Thus, the buffer wouldn't be destroyed.

(c) adding 0.050 mol of NaF: The addition of conjugate base doesn't destroy the buffer