1. % acetic acid = (Weight of acetic acid in sample / Total weight of sample) * 100
CH3COOH + NaOH CH3COONa + H2O
Hence number of moles of CH3COOH = number of moles of NaOH
Given, V = 20.72 mL = 0.02072 L
M = 0.125 M
Number of moles of NaOH = 0.125 mol/L x 0.02072 L
= 0.00259 mol
Hence number of moles of CH3COOH = 0.00259 mol
Molar mass of CH3COOH = 60.052 g/mol
Hence mass of CH3COOH = Molar mass x Number of moles
= 60.052 g/mol x 0.00259 mol
= 0.155 g
Weight of sample = 3.281 g
Hence % mass = (0.155 / 3.281) * 100 = 4.72 %
2. H3PO4 + 3 KOH K3PO4 + 3 H2O
Here we will use the formulae M1V1 = M2V2
where M1 = 0.220 M
V1 = Unknown
M2 = 0.816 M
V2 = 85 mL = 0.085 L
Substituting the values in the above equation, we get
V1 x 0.220 = 0.816 x 0.085
V1 = 0.315 L = 315 mL
Hence 315 mL of KOH will be required.
DATA SHEE Calculate the mass percent acetic acid present in a sample of balsamic vinegar if...
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acetic acid is an important ingredient of vinegar. a sample of 50.0 ml of a commercial vinegar is titrated against a 1.00 M NaOH solution. What is the molarity of acetic acid present in the vinegar if 5.75 ml of the base are needed for the titration?
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