.To determine the number of moles of the water of crystallization (n) of a hydrated salt, a student took a sample of 5.94 g of a Cobalt(II)chloride hydrate. The student heated the sample over a burner until constant mass. After cooling, he found that the mass of the remaining dehydrated salt was 4.65 g. i. Determine the mass of water lost by the sample. (0.5 mark) and Determine the number of moles of anhydrous Cobalt(II)chloride and water. ii. Calculate the number of moles of water of crystallization(n). iv. Write the molecular formula for the hydrated salt. How can the student make sure that all of the water of hydration has been removed?
. In the gravimetric analysis of determination of loss of water molecules of hydration from a
hydrated salt, identify any one possible mistake, and one proper way to fix it.
b.To determine the number of moles of the water of crystallization (n) of a hydrated salt, a
student took a sample of 5.94 g of a Cobalt(II)chloride hydrate. The student heated the sample
over a burner until constant mass. After cooling, he found that the mass of the remaining
dehydrated salt was 4.65 g.
i. Determine the mass of water lost by the sample. (0.5 mark)
and Determine the number of moles of anhydrous Cobalt(II)chloride and water.
ii. Calculate the number of moles of water of crystallization(n).
iv. Write the molecular formula for the hydrated salt.
How can the student make sure that all of the water of hydration has been removed?
Step by step
Solved in 3 steps with 1 images
