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Preparation of copper(II)sulfate crystals.

Measure 50 cm3 of dil.H2SO4 into a beaker and heat it on a tripod and gauze using a Bunsen burner.

Add a spatula full of black copper(II)oxide and continue heating. If Copper oxide disappears, and more until all the acid has reacted. So, this means you should add excess copper oxide until the solution is neutralized.

Drain the solution through a filter to get rid of the excess copper and contain the solution in an evaporating basin.

The solution you have in the evaporating basin is copper sulfate  which is blue. Heat this solution in order to boil off the water and concentrate the solution. Keep heating until you get a saturated solution. If you want to know if the solution is saturated, you will have to dip a glass rod in the solution and check if crystals are present. If they are present, then the solution is saturated.

Stop heating the solution and allow it to cool down at room temperature so that large crystals can form. Remove the blue crystals from the reaction mixture by filtration. The crystals can then be dried by blotting them with paper towel or by placing them in a dry oven.

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Procedure for preparation of soluble and insoluble 

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Procedure for preparation of soluble and insoluble 

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a) dynamic equilibrium are the rate of forward and backword reaction are equal

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Question 7:
a. Dynamic equilibrium: The condition that exists in a sealed container when the rate of the forward and backward reactions in a reversible reaction mixture are equal.
b.i- When pressure is increases, equilibrium shifts to the side with fewer moles which is NO2.
ii- As equilibrium is now shifted towards NO2, the colour appears to be darker.
c.i- The combustion of gasoline in vehicles produce nitrogen oxides.
ii- Oxides of nitrogen are irritant gas which can cause inflammation in airways (lungs).
iii- NO + CO-----> CO2 + N2

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7) a- dynamic equilibrium is a state where the the rate of the forward reaction is equal to the rate of the reverse reaction.
b-