Hi, everyone. I need help regarding buffers. Using the Henderson-Hasselbach equa

Question

Hi, everyone. I need help regarding buffers. Using the Henderson-Hasselbach equation, calculate how much acetic acid (1M) and sodium acetate should be required, and prepare the buffers accordingly. Be sure to bring the final volume to 100mL. 1) 100mM acetate buffer, pH 4.5. Hi, everyone. I need help regarding buffers. Using the Henderson-Hasselbach equation, calculate how much acetic acid (1M) and sodium acetate should be required, and prepare the buffers accordingly. Be sure to bring the final volume to 100mL. 1) 100mM acetate buffer, pH 4.5. Hi, everyone. I need help regarding buffers. Using the Henderson-Hasselbach equation, calculate how much acetic acid (1M) and sodium acetate should be required, and prepare the buffers accordingly. Be sure to bring the final volume to 100mL. 1) 100mM acetate buffer, pH 4.5.

Explanation / Answer

100mM acetate buffer and volume = 100 mL

millimols of buffer = 100 x 10^-3 * 100 = 10 millimol

So,

miilimol of conjugate base + millimol of acid = 10

Again,

pH = pKa + log ( [conjugate base] / [acid] )

4.5 = 4.74 + log ( [conjugate base] / [acid] )

[conjugate base] / [acid] = 0.575

[conjugate base] = 0.575 * [acid]

millimoles of conjugate base = millimoles of acid * 0.575

millimoles of acid * 0.575 + millimoles of acid = 10

millimoles of acid * 1.575 = 10

millimoles of acid = 6.35 millimol

Millimol of Conjugate base = 3.65 millimol

Molarity * Volume of acetic acid = 6.35

1 * V = 6.35

V = 6.35 mL

Millimol of sodium acetate = 3.65

Moles of sodium acetate = 0.00365 mol

Mass of sodium acetate = 0.00365 * Molar mass = 0.00365 * 82 = 0.2993 g

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