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KengaRu [80]
3 years ago
7

Suppose you want to prepare a buffer with a pH of 4.59 using formic acid. What ratio of [sodium formate]/[formic acid) do you ne

ed to make this buffer? Formic acid has a K, of 1.8x10 4 Enter your answer to three significant figures.
Chemistry
1 answer:
katrin [286]3 years ago
3 0

Answer:

7.08

Explanation:

To solve this problem we'll use the <em>Henderson-Hasselbach equation</em>:

  • pH = pka + log\frac{[A^-]}{[HA]}

Where \frac{[A^-]}{[HA]} is the ratio of [sodium formate]/[formic acid] and pka is equal to -log(Ka), meaning that:

  • pka = -log (1.8x10⁻⁴) = 3.74

We<u> input the data</u>:

  • 4.59 = 3.74 + log\frac{[A^-]}{[HA]}

And<u> solve for </u>\frac{[A^-]}{[HA]}:

  • 0.85 = log\frac{[A^-]}{[HA]}
  • 10^{(0.85)}=\frac{[A^-]}{[HA]}
  • \frac{[A^-]}{[HA]} = 7.08
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