DATA TABLE Trial 3 Trial 1 Equivalence point (mL) Mass ter paper precipitate (go

Question

DATA TABLE Trial 3 Trial 1 Equivalence point (mL) Mass ter paper precipitate (go 5.Hly Mass of filter paper (g) Mass of precipitate (g) Molarity of H2SO. (M) DATA ANALYSIS 1. Use the titration results to calculate the moles of H,so, that were used to reach the equivalence point in each trial. 2 Use your titration results to calculate the molar concentration (molarity) of the Ba(OH) solution using the molar amount of H2Sou used in each 3. Convert the mass of the barium sulfate precipitate, formed in each trial, to moles. 237.3% Basae mohr mass 5 Compare the results of your calculations from 2 and 4 above with the actual molarity of the Ba(OH2 solution. Which method of analysis, equivalence point or gravimetric determination, was more accurate in your experiment? Why?

Explanation / Answer

1. Molarity of sol = 0.1 M, volume used = 9.18 ml

so moles required for the equivalence point = 0.1 *9.18= 0.918 millimoles

2. at equivalence poitn both reactants completely react with each other so

moles of BA(OH)2 = moles of H2SO4

0.918 = 10ml * M

M is molarity of BA(OH)2

M= .0918 Molar

3.

0.181 g of BASO4= 7.76 *10-4 mol

4.

7.76 *10-4 mol of BASO4= 7.76 *10-4 mol of BA(OH)2

in 10 ml volume

so concentration= 7.76 *10-4/ .01

= .076 Molar

5.

Equivalence point method gives molarity of BA(OH)2 = .0918

Gravimetric method gives molarity of BA(OH)2 = = .076

Gravimetric method can have error due to inefficient weight measurement of the precipitate. Since sources of erro are less in equivalence point Gravimetric method is more prone to errors.

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