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CuSO4 * 5H2O

Formula for a Hydrate

Chan Chan Cheng

Date published: Nov. 10th

Lab partner: Emi Ushida

 

Purpose / Goal

To determine the formula of the hydrate and to find the percentage of water in a hydrated copper sulfate.

 

Materials

Apparatus

*   Porcelain crucible

*   Clay triangle

*   Safety goggles

*   Lab apron

*   Ring Stand

*   Iron Ring

*   Laboratory Burner

*   Scale

*   Tongs

Procedure

Data / Observation

 

Target

Mass in grams

Crucible

13.55g

Crucible with hydrate

15.84g

hydrate

2.29g

Crucible and dehydrated copper sulfate

14.99g

Dehydrated copper sulfate

1.44g

Water

0.047g

 

Before we heated copper sulfate, it was blue. Then it turned to white when it was dehydrated.

 

Calculation

CuSO4          63.55g + 32g + 4*16g = 159.45g

1.44g CuSO4 ( 1 mole CuSO4 / 159.45g CuSO4 ) = 0.009 moles of CuSO4

0.009 moles of CuSO4 ( 6.022*1023 / 1 mole) = 5.42*1021 molecules of CuSO4

H2O          2*1.008g + 16 = 18g

0.85g H2O ( 1 mole H2O / 18g H2O ) = 0.047 moles of H2O

0.047 moles of H2O ( 6.022*1023 molecules of H2O / 1 mole H2O )                                                           = 2.83*1022 molecules H2O

5.42*1021 / 2.83*1022 = 5 (approximately)

 

Conclusion

Therefore the formula is CuSO4 * 5H2O. There are five water molecules per one copper sulfate.