a)
State why chemists use a pH of 5.6 in the classification of acid rain.
[1]
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b)
Carbonic acid, H2 CO3 , is formed when CO2 dissolves in rainwater.
i)
Formulate an equation to show how carbonic acid is formed in rainwater. [1]
ii)
Formulate an equation to show the dissociation of carbonic acid. [1]
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c)
Two samples of rainwater, A and B, are pH 4.8 and pH 3.8, respectively. What is the relative acidity of sample A compared to sample B, in terms of [H+ ] concentration?
[1]
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d)
State two examples of wet acid deposition.
[1]
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a)
State the names of four acids that contribute to the formation of acid deposition.
[1]
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b)
Show, by means of balanced equations, the formation of sulfuric acid starting from sulfur.
[3]
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c)
Identify the changes in oxidation state for sulfur in part b).
[3]
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d)
Write a balanced equation to show the formation of nitric acid, from nitrogen dioxide, oxygen and water.
[1]
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a)
State two man-made sources of the oxides of sulfur and nitrogen.
[2]
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b)
State two natural sources of the oxides of sulfur and nitrogen.
[2]
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c)
State, giving a suitable equation, the effect of acid deposition, from sulfuric or nitric acids, on an iron bridge.
[2]
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a)
State the two ways by which emissions of sulfur oxides are reduced.
[1]
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b)
State a disadvantage of removing all the sulfur found in petroleum.
[1]
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c)
Explain the meaning of the term hydrodesulfurisation .
[1]
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d)
Compare and contrast two approaches to reducing sulfur oxide emissions.
[2]
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