acetic acid, CH3COOH is a commercially weak acid with a value of Ka = 1.8 x 10 ^ -5. In an erlenmeyer, you titrate 50 mL of this acid with 0.103 M NaOH and the phenolphtalein indicator duplo. The volume of NaOH needed to reach the equivalence point in both experiments was 48.96 mL and 49.11 mL. a. Write down the equilibrium reaction of dissolving vinegar in water, then write down the equation that reflects the acidic equilibrium constant! b. Calculate the average volume of NaOH needed to reach the equivalence point! c. Calculate the acidity of the vinegar in this sample!
acetic acid, CH3COOH is a commercially weak acid with a value of Ka = 1.8 x 10 ^ -5. In an erlenmeyer, you titrate 50 mL of this acid with 0.103 M NaOH and the phenolphtalein indicator duplo. The volume of NaOH needed to reach the equivalence point in both experiments was 48.96 mL and 49.11 mL.
a. Write down the equilibrium reaction of dissolving vinegar in water, then write down the equation that reflects the acidic equilibrium constant!
b. Calculate the average volume of NaOH needed to reach the equivalence point!
c. Calculate the acidity of the vinegar in this sample!
d. Calculate the initial pH of the vinegar solution before titrating!
e. Calculate the pH at the equivalence point
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
