Question

For numbers 6-10, refer to the question below Ms. Everything is about to analyze the %S03 in her 0.9682 g sulfate containing sample. She reacted the sample with BaCl2, hot concentrated HCI, and allowed the digestion process to take place overnight. The next morning, she filtered out some of the precipitate and ignited it in a constant weighted crucible with a mass of 30.6842 g. After ignition, the mass of the crucible and the precipitate is about 31.0246 g. 6. What is the mass of the precipitate? a. 0.9682 b. 0.3404 C. 0.4681 d. 0.2987 7. What is the experimental mass of S03? a. 0.1168 b. 0.9922 c. 0.3322 d. 0.1974 8. What is the experimental %S03? a. 10.68 b. 13.98 c. 12.06 d. 11.68 9. If the true %SO3 is 13.98%, what is the percent error of her analysis a. 23.61 b. 13.73 c. 0.00 d. 16.45 10. Which could be the possible reason for Ms. Everything's percent error? a. The calibration of crucible b. The filtration of the sample c. The ignition the sample d. The calculation of data she obtained

Answer 1

Answer:

Mass of empty crucible = m = 30.6842 g

Mass of precipitate and crucible = M = 31.0246 g

Mass of precipitate = m'

M = m + m'

31.0246 g = 30.6842 g + m'

m' = 31.0246 g - 30.6842 g = 0.3404 g

The mass of the precipitate is 0.3404 grams , that is option b is a correct answer.