Given this data: Determine the number of moles of sulfate which should be in the

Question

Given this data:

Determine the number of moles of sulfate which should be in the sample of Alum which you weighed in Part III. How well does it compare to the moles of sulfate which you obtained from the precipitation of barium sulfate? Provide an explanation for possible sources of error.

We used 43.0mL of 0.20M Ba(NO3)2 solution.

11/11/13 Date : DATA TABLE Part I- Melting Temperature Test Results Melting Temperature Range Part II- Water of Hydration Test Results Mass of Crucible and Cover (g) Mass of Crucible, Cover, and Alum before heating (g) Mass of Alum before heating (g) Mass of Crucible, Cover, and Alum after final heating (2) 2 Mass of Alum after heating (g) 22.awa a0131 Mass of Water lost (g) Part III - Percent Sulfate Test Results Mass of Filter Paper and Watch Glass (g) Mass of Filter Paper, Watch Glass, and Precipitate (g) G4. 093a

Explanation / Answer

Molar mass of BaSO4 = 233.4 g/mol

Molar mass of sulfate = 96.07 g/mol

Mass of BaSO4 (from part 3)= 54.093-52.987 =1.106 g

Now, 1.106 g BaSO4/ 233.4 = 0.0047 Mol BaSO4

0.0047 x 96.07 g/mol SO4 = 0.455 g

0.455/1.106 = 41.16 % sulfate

The theoretical yield of sulfate can be calculated as,

Molar mass of Alum =474.2 g/mol

2 mol sulfate/1 mol alum = 40.5% which is comparable to the experimental value.

The possible sources of error in this experiment are insufficient heating and the formation of water droplets in the precipitate during the cooling process

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