Y4 Revision for EOY

Acids, Bases, Salts &

Qualitative analysis ​

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Multiple Choice

Which solutions, when mixed together, form an insoluble salt?

• dilute nitric acid and aqueous magnesium chloride

• aqueous potassium hydroxide and aqueous iron(II) chloride

• dilute hydrochloric acid and aqueous ammonium carbonate

• aqueous potassium sulfate and aqueous calcium nitrate

Multiple Choice

Element J reacts with oxygen to form oxide of J. Oxide of J is soluble in water and forms a solution which turns Universal Indicator orange.

 

Based on the information, deduce the nature of oxide of J.

• Basic

• Acidic

• Neutral

• Amphoteric

Multiple Choice

What are the possible ions present in the colourless solution R?

• aluminium ions, lead(II) ions and sulfate ions

• aluminium ions, zinc ions and nitrate ions

• lead(II) ions, zinc ions and nitrate ions

• zinc ions, ammonium ions and iodide ions

Multiple Choice

What are the two metals present in the alloy?

• Copper and iron

• Zinc and iron

• Zinc and lead

• Copper and calcium

Redox Reactions ​

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Metals ​

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Multiple Choice

The coatings on four strips of iron were scratched to expose the iron. The strips were placed in salt solution. Which iron strip rusted most quickly?

• Plastic coated strip

• Zinc coated strip

• Tin coated strip

• Painted strip

Multiple Choice

Element U displaces element V from the

aqueous nitrate of V.

Element W reacts with cold water to give hydrogen.

Element U gives hydrogen only when heated with steam.

• A

• B

• C

• D

Open Ended

Explain why the pH of the solution increases when sodium is added to aqueous copper(II) chloride. 

Multiple Choice

Metal X reacts more vigorously with water than Metal Y.

Which statement is incorrect?

• The oxide of Y is more difficult to reduce than the oxide of X.

• X would displace Y from a solution containing ions of Y.

• X would react more readily with dilute hydrochloric acid than Y.

• The carbonate of Y is less thermally stable than that of X.

Open Ended

A piece of zinc was added to aqueous iron(II) sulfate. State and explain the observations.

​Periodic table

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Open Ended

Describe and explain the observations when chlorine gas is bubbled into a test tube of aqueous magnesium iodide.

​Electrochemistry

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Fill in the Blanks

Open Ended

Identify the electrolyte,  $$XSO_4$$  

Multiple Choice

Which is true about the set-up? 

• The pH of the electrolyte increases

• Electrons flow from the pure copper electrode through the wire to the impure copper electrode

• A gas is formed at the pure copper electrode 

• The impure copper electrode decreases in size 

Open Ended

Explain why the pure copper block increases in size.

Open Ended

Explain why the blue colour of the electrolyte will not fade over time. 

Speed of reaction ​

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Open Ended

Excess hydrochloric acid was added to 1 g of MgCO₃

producing MgCl₂, CO₂ and H₂O.

If the hydrochloric acid was replaced with sulfuric acid of the same concentration, describe and explain how the rate of reaction would change.

Open Ended

Excess hydrochloric acid was added to 1 g of MgCO₃

producing MgCl₂, CO₂ and H₂O. 

If the hydrochloric acid was replaced with sulfuric acid of the same concentration, would there be any change in the volume of CO₂? Explain. 

Open Ended

In terms of collisions between reacting particles, explain the effect of increasing the concentration of an aqueous reactant on the rate of reaction. 

Open Ended

In terms of collisions between reacting particles, explain the effect of increasing the temperature on the rate of reaction.

Open Ended

In terms of collisions between reacting particles, explain the effect of adding a catalyst on the rate of reaction.