A 10.0-mL sample of vinegar, which is an aqueous solution of acetic acid, CH3COOH, requires 16.5 XML of a 0.500M NaOH solution to reach the endpoint in a titration (where the moles of acid are equal to the moles of base). What is the molarity of the acetic acid solution
How many moles NaOH do you have? That is M x L = ??
How many moles acetic acid do you have? That will be the same thing; the problem tells you.
Concn acetic acid = moles/L soln. The problem gives you 10 mL which is 0.010 L so M = ??moles/0.010L = ??
To determine the molarity of the acetic acid solution, we can use the following equation based on the balanced chemical equation:
CH3COOH + NaOH → CH3COONa + H2O
According to the equation, one mole of acetic acid reacts with one mole of sodium hydroxide to produce one mole of sodium acetate and one mole of water.
First, we need to determine the number of moles of NaOH used in the titration.
Using the formula:
moles = concentration × volume
moles of NaOH = 0.500 M × 16.5 mL = 8.25 mmol
Since the balanced equation shows that one mole of acetic acid reacts with one mole of sodium hydroxide, the moles of acetic acid will also be 8.25 mmol.
Next, we calculate the molarity of the acetic acid solution:
Molarity = moles/volume
Molarity = 8.25 mmol / 10.0 mL = 0.825 M
Therefore, the molarity of the acetic acid solution is 0.825 M.