Question

• Using the dehydration equation of hydrated barium chloride, answer the following question:

a) If 3 moles of hydrated barium chloride was heated, how many moles of anhydrous barium chloride, and how many moles of water vapor will be produced?

b) 20 g of sand was mixed with 5 g of a hydrate. Calculate the percentage of the hydrate in this mixture.

c) If you know that the real percentage of the hydrated barium chloride was exactly 25% out of the total mixture in part (B) of this experiment. "our result was 38%"

- How did your result compare to this value?

- Describe an error that may have affected your data (weaknesses)

- How could you fix this error next time? (improvements)

Answer 1

Hi,

Generally Barium chloride exist as it dihydrate i,e BaCl₂ 2H₂O ( if this changes also we can follow same analysis)

Answer for a)

When 3 mole of BaCl2 heated you will get 3 mole of anHydrus BaCl2 and 6 moles of H2O

3.0 Moles BaCl₂ 2H₂O 3.0 Moles BaCl₂ + 6 Moles of 2H₂O evoperates

answer for b)

Its 20 g sand is mixed with 5 g Barium chloride dihydrate which result in 25 g of total weight

% of Barium chloride dihydrate = 5g/25g

= 25%

answer for c)

the error may be in calculation!

Next time it should be repeated with 2-3 times with careful observation in weighing and recording the values.