Answer:
pH = 1.62
Explanation:
We can solve this problem using Henderson-Hasselbach's equation:
- pH = pKa + log[tex]\frac{[A^-]}{[HA]}[/tex]
Where
Now we convert 132.8 g of NaC₇H₅O₂ into moles, using its molar mass:
- 132.8 ÷ 144.11 g/mol = 0.921 moles
Then we calculate [NaC₇H₅O₂]:
- 0.921 moles / 300.0 mL = 0.003 M
Now we can proceed to calculate the pH of the solution:
- pH = 4.20 + log[tex]\frac{0.003}{1.17}[/tex]
