Question

Step 1. Procedure Obtain a weighted amount of the Copper (II) Sulfate hydrate (say 30 g), place in an 100 ml beaker

Step 2. Heat compound with bunsen burner until all of the water is driven-off (you can verify this be weighing the beaker while heating it, when the weight stops declining you’ve removed all the water.

Step 3. Weigh final compound. write your observations Observations:

Initial Weight:

Final Weight:

Weight of Water driven off (Initial weight - final weight) :

moles of water loss: Weight of water / GMW H2O (18.016 )
moles of CuSO4: final weight/ GMW CuSO4 (159.61)

X = moles of water loss/ moles of CuSO4

Given that hydrate is: CuSO4 (XH2O)

Formula of hydrate:

Answer 1

Given mass of the hydrated sample , m = 30 g

mass of the anhydrous sample , m'

mass of the water , m" = m - m"

No . of moles of water , n ' = mass / Molar mass

                                          = m" / 18                    

No . of moles of anhydrous salt , n = m' / Molar mass of CuSO₄

ration to the no . of moles of water to the anhydrous salt is x = n'/n

This is the process

If they give the mass of anhydrate sample we can find out x