Question

Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 10.5 g of HC2H3O2 and 11.5 g of NaC2H3O2 in 150.0 mL of solution.

Answer 1

We know that Henderson-Hasselbalch Equation that

We have the salt form of Acetic acid CH₃COONa is 11.5 g in 150 mL

And acid form CH₃COOH is 10.5g in 150 mL

Now we have to calculate the number of moles/L that means the concentration , But we have same volume of solvent, Henece it is sufficient to calculate the moles.

Number of moles can be calculated from

Now for the salt part CH₃COONa is 11.5 g in 150 mL

Again for the Acetic acid part CH₃COOH is 10.5g in 150 mL

We have the

Now apply Henderson-Hasselbalch Equation to get the pH as

Hence the pH is 4.67.

Answer.