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Using Henderson-Hasselbalch equation, calculate the volume of 0.20 M Acetic Acid and 0.2 M Sodium Acetate needed to prepare 50 mL of 0.1 M Acetate Buffer solution (pH = 4.5). pKa of Acetic Acid is 4.74?

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Volume of 0.20 M sodium acetate is calculated to be 0.82g. Sodium acetate can  be used as additives in food, industry and in buffer solutions.

What is Henderson-Hasselbalch equation?

To determine  pH of a buffer is by using the Henderson–Hasselbalch equation is pH = pKₐ + log([A⁻]/[HA]).

As we know that, pH = pKa + log [salt]/[acid]  

Given pH (4.75) and  pKa (4.75).

Given [acid] = 0.20 M

When the pH = pKa, ratio of [salt]/[acid] =1 because log 1 = 0

Hence,[sodium acetate] = 0.20 M.  

4.75 = 4.75 + log [sodium acetate]/[0.20]

0 = log x/0.2

Hence, x = 0.2 M

To calculate the "amount" in grams, convert 0.20 M to grams using the volume of 50 ml (0.05 L)

0.20 mole/L x 0.05 L = 0.01 moles moles sodium acetate

0.01 moles sodium acetate x 82 g/mole

Volume of 0.20 M sodium acetate= 0.82g

To know more about Henderson-Hasselbalch equation, refer

https://brainly.com/question/26746644

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