What is the [ch3co2-]/[ch3co2h] ratio necessary to make a buffer solution with a ph of 4.34? ka = 1.8 × 10-5 for ch3co2h?

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11-04-2018
Chemistry

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What is the [ch3co2-]/[ch3co2h] ratio necessary to make a buffer solution with a ph of 4.34? ka = 1.8 × 10-5 for ch3co2h?

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transitionstate transitionstate · Answer 1 · 2018-04-20T14:53:06+02:00

According to Henderson–Hasselbalch Equation,

pH = pKa + log [Acetate] / [Acetic Acid]

As,
pKa = -log Ka
pKa = -log (1.8 × 10⁻⁵)
pKa = 4.74
So,
pH = 4.74 + log [Acetate] / [Acetic Acid]

4.34 = 4.74 + log [Acetate] / [Acetic Acid]

4.34 - 4.74 = log [Acetate] / [Acetic Acid]

-0.40 = log [Acetate] / [Acetic Acid]

Taking Antilog on both sides,

[Acetate] / [Acetic Acid] = 0.398

aliasger2709 aliasger2709 · Answer 2 · 2022-04-13T09:29:29+02:00

pH is the measure of the hydrogen ion concentration to determine the acidity of the solution. 0.398 is the ratio of the acetate to acetic acid for a buffer solution.

What is Henderson–Hasselbalch Equation?

Henderson–Hasselbalch Equation is used to determine the acidity of the solution by the acid dissociation constant, the concentration of acid, and the concentration of the conjugate base.

The Henderson–Hasselbalch Equation is given as,

[tex]\rm pH = \rm pKa + log \dfrac{[Acetate]}{[Acetic\; acid]}[/tex]

The negative log of acid disassociation constant is determined as:

[tex]\begin{aligned}\rm pKa &= \rm -log Ka\\\\&= \rm - log (1.8 \times 10^{-5})\\\\&= 4.74\end{aligned}[/tex]

Now the ratio of the concentration is calculated as:

[tex]\begin{aligned} \rm pH &= \rm 4.74+ log \dfrac{[Acetate]}{[Acetic\; acid]}\\\\4.34 - 4.74 &= \rm log \dfrac{[Acetate]}{[Acetic\; acid]}\\\\-0.40 &= \rm log \dfrac{[Acetate]}{[Acetic\; acid]} \end{aligned}[/tex]

Solving further by taking antilog on both sides:

[tex]\rm \dfrac{[Acetate]}{[Acetic\; acid]} \end{aligned} = 0.398[/tex]

Therefore, the ratio of the concentration is 0.398.

Learn more about Henderson–Hasselbalch Equation here:

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