A student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwent precipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected in an ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible, the obtained mass was 30.3375 g.

- What is the mass of BaSO4
- Compute for the % error of the student in his analysis.

30.3375 = mass xble + ppt

-29.9442 = mass xble
-----------------
00.3933 = mass ppt
You don't give any information on the % BaSO4 in the sample; therefore, we can't calculate a % error.

hmmm, here are the other question though.

Compute for the experimental mass (g) of SO3 in grams obtained by the student. my answer = 0.1349

Compute for the experimental % SO3 obtained by the student. my answer = 17.89

Compute for the theoretical % SO3 obtained by the student, my answer =17.89

Compute for the theoretical mass (g) of SO3 that should be obtained by the student using his weighed sample. my answer = 0.1134

then finally the Compute for the % error of the student in his analysis my answer is round about 47.86% but it is not in the choices given.

The answers to the additional questions are correct; however, I don't have any way to check the last two (shown below). I can't calculate theoretical mass if I don't know the correct % mass. Likewise, I can't calculate a % error if I don't know what it was supposed to be.

Compute for the theoretical mass (g) of SO3 that should be obtained by the student using his weighed sample. my answer = 0.1134

then finally the Compute for the % error of the student in his analysis my answer is round about 47.86% but it is not in the choices given.

Ohhh, okaay thank youuu. :)

To find the mass of BaSO4, we need to determine the mass of BaSO4 formed from the difference in mass before and after burning the sample in the crucible.

1. Start by finding the mass of the white crystalline precipitate (BaSO4) collected on the ashless filter paper.
- Subtract the mass of the crucible before burning from the mass after burning. This will give the mass of the precipitate.
- Mass of BaSO4 (precipitate) = Mass after burning - Mass of crucible before burning
= 30.3375 g - 29.9442 g

2. Calculate the mass of BaSO4:
- Mass of BaSO4 = 0.3933 g

3. To compute the percent error in the student's analysis, we need to compare the experimental value (mass of BaSO4 obtained) with the theoretical value (expected mass based on stoichiometry).

4. Calculate the theoretical mass of BaSO4:
- Determine the molar mass of BaSO4, which consists of one Ba atom (137.33 g/mol) and one SO4 group (96.06 g/mol).
- The molar mass of BaSO4 is 137.33 g/mol + 96.06 g/mol = 233.39 g/mol.
- Use the molar mass to calculate the theoretical mass of BaSO4 from the number of moles:
Theoretical mass of BaSO4 = Number of moles * Molar mass of BaSO4
- First, find the number of moles of BaSO4 by dividing the mass by the molar mass:
Number of moles = Mass of BaSO4 / Molar mass of BaSO4
= 0.3933 g / 233.39 g/mol

5. Calculate the percent error:
- Percent error = |Theoretical mass - Experimental mass| / Theoretical mass * 100
= |(0.3933 g - Theoretical mass) / Theoretical mass| * 100

By following these steps, you can find the mass of BaSO4 and compute the percent error in the student's analysis.