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Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.165 M in propanoic acid and 0.110 M in potassium propionate. Express your answer using two decimal places. Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.16 M in C5H5N and 0.13 M in C5H5NCI. Express your answer using two decimal places. Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 11.5g of HF and 24.0g of NaF in 125 mL of solution Express your answer using two decimal places.

Solution

part A :
pKa = 4.74
pH = 4.74 + log 0.110 / 0.165

partc:
Moles HF = 11.5 g /20.0 g/mol=0.575
[HF]= 0.575 mol/ 0.125 L= 4.60 M

moles NaF = 22.5 g / 41.9882 g/mol=0.536
[F-]= 0.536/ 0.125 L=4.29 M

pKa of HF = - log 6.7 x 10^-4 = 3.17

pH = 3.17 + log 4.29/ 4.60=3.14