Copper sulphate experiment
Copper sulphate experiment
Introduction
There are a number of different methods of making salts, such as the reaction of a metal with an acid. Copper metal, however, does not react with sulphuric acid and so another method must be used. In this experiment a basic copper compound (copper(II) oxide) will be reacted with sulphuric acid giving copper(II) sulphate as one of the products.
Method
1. Wear goggles and keep your face away from the beaker during the reaction
2. Place 20 cmm3 sulphuric acid into a 100 cm3 beaker
3. Add spatulas of copper carbonate carefully and stir the mixture (a lot) with a starring rod (not the spatula) to react all of the copper carbonate with acid.
4. Keep adding copper carbonate until no more will react and there is green copper carbonate left unreacted at the bottom of the beaker. This will ensure that all the acid is used up.
5. Filter the solution to remove unreacted copper carbonate
6. If there is time, concentrate the solution by evaporating a little of the water off over a Bunsen burner (slowly).
7. Leave the solution on the window sill with your name on a piece of paper to compere evaporation by next time the lesson will take place.
Results
Mass of:
Results:
Malachite/g
4.44
Filter paper/g
1.32
Paper + residue/g
3.96
CuSO4.5H2O/g
2.52
Theoretical yield
This is calculated from the moles of sulphuric acid used. n = cv
C= 1 mol v= 0.020 dm3 n=0.020 mol/dm3
Percentage yield
Actual mass = 2.52 g
Theoretical mass = 0.020 x [63.5+32.1+(4x16)+(5x18)]
0.020 x 249.6=4.992
Percentage yield = actual mass x 100 theoretical mass
=2.52 x100 4.992
=50.480%
Actual mass= (Paper + residue) – (filter paper)
= 3.96 – 1.32 =2.64
Atom economy
AE (%) = (Desired)/ (Total Products)
Desired mass ∑ (desire product)/ mass ∑ (all products)
Two ways to make copper sulphate
CuO(s) + H2SO4(aq) → CuSO4(aq) + H2O(l)
159.6 + 18= 177.6
159/177.6 x 100 =89.86486%
Copper
Introduction
There are a number of different methods of making salts, such as the reaction of a metal with an acid. Copper metal, however, does not react with sulphuric acid and so another method must be used. In this experiment a basic copper compound (copper(II) oxide) will be reacted with sulphuric acid giving copper(II) sulphate as one of the products.
Method
1. Wear goggles and keep your face away from the beaker during the reaction
2. Place 20 cmm3 sulphuric acid into a 100 cm3 beaker
3. Add spatulas of copper carbonate carefully and stir the mixture (a lot) with a starring rod (not the spatula) to react all of the copper carbonate with acid.
4. Keep adding copper carbonate until no more will react and there is green copper carbonate left unreacted at the bottom of the beaker. This will ensure that all the acid is used up.
5. Filter the solution to remove unreacted copper carbonate
6. If there is time, concentrate the solution by evaporating a little of the water off over a Bunsen burner (slowly).
7. Leave the solution on the window sill with your name on a piece of paper to compere evaporation by next time the lesson will take place.
Results
Mass of:
Results:
Malachite/g
4.44
Filter paper/g
1.32
Paper + residue/g
3.96
CuSO4.5H2O/g
2.52
Theoretical yield
This is calculated from the moles of sulphuric acid used. n = cv
C= 1 mol v= 0.020 dm3 n=0.020 mol/dm3
Percentage yield
Actual mass = 2.52 g
Theoretical mass = 0.020 x [63.5+32.1+(4x16)+(5x18)]
0.020 x 249.6=4.992
Percentage yield = actual mass x 100 theoretical mass
=2.52 x100 4.992
=50.480%
Actual mass= (Paper + residue) – (filter paper)
= 3.96 – 1.32 =2.64
Atom economy
AE (%) = (Desired)/ (Total Products)
Desired mass ∑ (desire product)/ mass ∑ (all products)
Two ways to make copper sulphate
CuO(s) + H2SO4(aq) → CuSO4(aq) + H2O(l)
159.6 + 18= 177.6
159/177.6 x 100 =89.86486%
Copper