According to the experiment
procedure, given that the NaOH
solution has a concentration of
0.100M, and that the vinegar
(acetic acid) has a concentration of
5.0%m/m (mass percent), what
volume(mL) of titrant would be
required to reach the "equivalence
point", if you place 2.500g of
vinegar in the flask (show
calculations) ?
Vinegar is acetic acid (CH3COOH) but I will shorten that to HAc.
5.0% w/w means 5g HAc in 100 g solution.
g HAc in 2.5g vinegar is 0.05 x 2.5 = about 0.125
mols HAc = g/molar mass = ?
mols KOH = mols HAc
M KOH needed = mols KOH/L KOH. You know mols and M, solve for L and convert to mL.
To calculate the volume (in mL) of the titrant required to reach the equivalence point, we need to use the given concentrations of the NaOH solution and vinegar (acetic acid), along with the mass of vinegar placed in the flask.
Step 1: Convert the mass percent concentration of vinegar to molarity:
Since the vinegar concentration is given as 5.0% m/m (mass percent), we need to convert it to molarity (M). The molar mass of acetic acid (CH3COOH) is 60.052 g/mol.
First, calculate the mass of acetic acid in the given 2.500g of vinegar:
Mass of acetic acid = (5.0 g/100g) x 2.500g = 0.125g
Next, convert the mass of acetic acid to moles:
Moles of acetic acid = Mass of acetic acid / Molar mass of acetic acid
Moles of acetic acid = 0.125g / 60.052 g/mol
Step 2: Calculate the moles of NaOH required for the reaction:
In a balanced chemical equation representing the neutralization reaction between NaOH and acetic acid (CH3COOH), the stoichiometric ratio is 1:1. It means that one mole of NaOH will react with one mole of acetic acid.
Therefore, the moles of NaOH required for the reaction are also equal to the moles of acetic acid calculated in Step 1.
Step 3: Calculate the volume of the titrant (NaOH solution):
The concentration of the NaOH solution is given as 0.100M, which means it contains 0.100 moles of NaOH in every 1 liter of solution.
Since we know the moles of NaOH required for the reaction from Step 2, we can use the formula:
Volume (in liters) = Moles / Concentration
First, convert the moles of NaOH to liters:
Volume of NaOH in liters = Moles of NaOH / Concentration of NaOH
Volume of NaOH in liters = Moles of NaOH / 0.100 M
Finally, convert the volume from liters to milliliters (mL) by multiplying by 1000:
Volume of NaOH in mL = Volume of NaOH in liters x 1000
By following these steps and substituting the calculated values, you can find the volume (in mL) of the NaOH titrant required to reach the equivalence point.