12.50 g of a hydrated form of copper(II) sulfate, CuSO4•x H2O (where x is unknown) is gently heated. When all the water has been driven off, the mass of the anhydrous copper(II) sulfate is found to be 7.99 g. What is the mass of the water that was lost as a result of the heating?
Convert this mass of water to moles of water.
Convert the mass of the anhydrous CuSO4 to moles.
Divide the answer to b by the answer to c. This is the value of x in the formula of the hydrate. Write the formula of hydrated copper(II) sulfate.

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Explanation:

please

Step 1. Calculate the mass of water in the sample

Mass of water = mass of hydrate - mass of anhydrous salt

= 3.94 g - 2.52 g = 1.42 g

Step 2. Calculate the mass of water that combines with 1 mol of  

CuSO

4

The molar mass of  

CuSO

4

is 159.61 g/mol.

Mass of water

=

159.61

g CuSO

4

×

1.42 g H

2

O

2.52

g CuSO

4

=

89.93 g H

2

O

Step 3. Calculate the moles of  

H

2

O

Moles of water

=

89.93

g H

2

O

×

1 mol H

2

O

18.02

g H

2

O

=

4.99 mol H

2

O

≈

5 mol H

2

O

Step 4. Determine the formula of the hydrate

1 mol of  

CuSO

4

combines with 5 mol of  

H

2

O

.

∴ The formula of the hydrate is  

CuSO

4

⋅

5H

2

O

.

Explanation: