s This eqeation has a special name: Henderson-Hasselbalck equation. In its geñer

Question

s This eqeation has a special name: Henderson-Hasselbalck equation. In its geñeral form base acld] 6. Use the above equation to calculate the pH of the following mixtures. Use the accepted K, of 1.8x 10. Then make the solution and test the pH (the drop counter is not needed for this part). Volume of TAR Volume of 0.1 Calculated pH 0.1 M acetic M sodium [acetic acid] [sodium acetate] (base) (Henderson. Measured pH H m 50SA 50 25 75 75 Now let's use the Henderson-Hasselbalch equation to determine the amount of 0.1 M acetic acid and O.1 M acetate you need to make a mixture with a pH of 4.00. Use the accepted K, of 1.8 x 10. 7. 12

Explanation / Answer

I am solving the complete Q6 as per Chegg guidelines, post multiple question to get the remaining answers

Q6)

a) [CH3COO-] = [CH3COOH] = 0.05

Using hessley henderbach equation

pKa = -log(Ka) = -log(1.8 * 10^(-5)) = 5 - log(1.8) = 4.744

pH = pKa + log([CH3COO-]/[CH3COOH])

=> 4.744 + log(0.05/0.05) = 4.744 + log(1) = 4.744

b) [CH3COO-] = 0.075

[CH3COOH] = 0.025

Using hessley henderbach equation

pKa = -log(Ka) = -log(1.8 * 10^(-5)) = 5 - log(1.8) = 4.744

pH = pKa + log([CH3COO-]/[CH3COOH])

=> 4.744 + log(0.075/0.025) = 4.744 + log(3) = 5.221

c) [CH3COO-] = 0.025

[CH3COOH] = 0.075

Using hessley henderbach equation

pKa = -log(Ka) = -log(1.8 * 10^(-5)) = 5 - log(1.8) = 4.744

pH = pKa + log([CH3COO-]/[CH3COOH])

=> 4.744 + log(0.025/0.075) = 4.744 + log(1/3) = 4.267

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