Reactions of Acids (AQA GCSE Chemistry: Combined Science)

Exam Questions

2 hours16 questions
1a1 mark

This question is about the reactions of metals with acid.

Complete the general word equation for the reaction of a metal with an acid.

Metal + acid → __________ + hydrogen

1b2 marks

When metals react with acid, hydrogen gas is formed.

Describe the test for hydrogen, including the expected observation for a positive test.

Test: ______________________________________

Positive result: ______________________________

1c1 mark

Magnesium sulfate can be produced by the reaction of magnesium with an acid.

Which acid should the student use to produce magnesium sulfate?

Tick () one box.

Hydrochloric acid  
Nitric acid  
Sulfuric acid  
1d1 mark

Magnesium sulfate is made from the magnesium ion, Mg2+, and the sulfate ion, SO42–.

Write the chemical formula for magnesium sulfate.

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2a1 mark

This question is about acids, bases and salts.

A student reacts zinc carbonate with nitric acid.

Which salt is formed during this reaction? 

Tick () one box.

Zinc   
Zinc chloride   
Zinc nitrate  
Zinc oxide  
2b2 marks

Complete the sentences.

Choose answers from the box.

a colour change electrolysis a pungent smell
decomposition fizzing neutralisation oxidation


__________________ can be observed when zinc carbonate reacts with nitric acid.

This is due to the __________________ reaction releasing carbon dioxide gas.

2c1 mark

The reaction of zinc carbonate with nitric acid can be represented with a balanced symbol equation.

Balance the symbol equation for this reaction.

ZnCO3 + ___ HNO3 → Zn(NO3)2 + ___ H2O + CO2

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3a1 mark

Copper oxide reacts with hydrochloric acid to form a salt and water.

What is the name of the salt that is formed?

Copper ________________

3b1 mark

What type of reaction happens when copper oxide reacts with hydrochloric acid?

Draw a circle around the correct reaction type.

Combustion Precipitation Thermal decomposition Neutralisation
3c1 mark

A student added an excess of copper oxide to warm dilute hydrochloric acid.

Describe how the student removed any unreacted solid copper oxide.

3d3 marks

Complete the sentences.

Choose answers from the box.

boiling  salt  water
melting  crystallisation


The student extracts the _______________ from the aqueous salt solution by _______________ .

This involves heating the solution until it is _______________ .

The solution is then left until only the salt remains.

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4a1 mark

This question is about acids, bases and the pH scale.

Which ions make a solution alkaline?

4b3 marks

Match the pH value to the description.

Draw one line from each pH value to the correct description.

aqa-gcse-4-2e-q4b-ph-value-match-

4c2 marks

pH can be measured in different ways.

What do each of the following sentences describe?

One way of measuring pH involves a chemical that changes colour: _______________

Another way of measuring pH involves a piece of equipment that gives a more accurate pH reading: _______________

4d4 marks

A student has three unlabelled bottles containing clear liquids.

The liquids are known to be dilute nitric acid, dilute sodium hydroxide and water.

Explain how the student could use universal indicator to determine the contents of each bottle?

Your answer should include expected observations. 

   Method: ____________________

   Dilute nitric acid: ____________________

   Dilute sodium hydroxide: ____________________

   Water: ____________________

4e2 marks

In a neutralisation reaction, H+ ions react with OH ions to produce water.

Write the ionic equation of neutralisation.

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5a3 marks

This question is about strong and weak acids.

Use the information in Table 1 to help you answer all questions.

Table 1

  Nitric acid Sodium hydroxide
Type Strong acid Strong alkali
Ions in solution H+        NO3 Na+        OH
pH 1 14
Colour with universal indicator Red Purple


Complete the sentences.

The __________ ions in nitric acid make it acidic.

The __________ ions in sodium hydroxide make it alkaline.

Acids have a pH value that is __________ the pH value of alkalis.

5b1 mark

Draw a ring around the correct answer to complete this sentence.

Strong acids and strong alkalis are

completely

not

partially

           ionised in water.
5c1 mark

Draw a ring around the correct answer to complete this sentence.

Weak acids and weak alkalis are

completely

not

partially

           ionised in water.

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1a1 mark

Figure 1 shows a bottle of vinegar which is used to flavour food. 

Vinegar is an aqueous solution of ethanoic acid, CH3COOH.

Figure 1 

4-2-reactions-of-acids-medium-q1a

Ethanoic acid is described as a weak acid.

What is the ion present in aqueous solutions of all acids?

1b5 marks

Discuss the difference in pH between a weak acid and a strong acid of the same concentration.

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2a2 marks

The balanced chemical equation between iron and hydrochloric acid is:

Fe (s) + 2 HCl (aq) → FeCl2 (aq) + _____ (g)

What is the name and symbol of the missing product?

2b1 mark

What class of compound is the other product in the reaction?

2c6 marks

Describe a suitable method for separating the FeCl2.

2d4 marks

State what type of reaction this is and explain, using appropriate half equations the species being oxidised and those being reduced.

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3a2 marks

This question is about alkalis and bases.

Give the name and formula of the ion present in aqueous solutions of all alkalis.

3b3 marks

Explain the difference between the terms base, alkali and alkaline solution.

3c1 mark

Metals, metal hydroxides and metal oxides can neutralise acids.

Name one other type of compound that can neutralise an acid.

3d1 mark

Write the simplest ionic equation which represents a neutralisation reaction.

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4a2 marks

This question is about acids and alkalis.

A dilute solution of hydrochloric acid is considered a strong acid.

Justify how an acid can be described as both strong and dilute.

4b2 marks

A 1.0 × 10−4 mol/dm3 solution of HCl has a pH of 4.0

What is the pH of a 1.0 × 10−6 mol/dm3 solution of the same acid? 

Explain your answer.

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5a4 marks

Sodium hydroxide neutralises sulfuric acid in the following reaction:

2NaOH + H2SO4 → Na2SO4 + 2H2O

Sulfuric acid is a strong acid.

Explain what the term “strong acid” means, discussing how the strength of an acid is linked to its pH value.

5b2 marks

Write down the ionic equation for this neutralisation reaction and include the state symbols.

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6a2 marks

Soluble salts can be formed by reacting metals with acids.

Give two other types of substances that can react with an acid to form a soluble salt.

6b1 mark

Magnesium chloride is a soluble salt.

Give the formula of magnesium chloride.

6c2 marks

Calcium sulfate is another soluble salt that can be formed by the reaction between calcium and dilute sulfuric acid.

Ca (s)  +  H2SO4 (aq)   →   CaSO4 (aq)  +  H2 (g)

State two observations that could be made during this reaction.

6d
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3 marks

A student wanted to investigate the volume of hydrogen produced when different masses of calcium were reacted with dilute sulfuric acid.

They use the equipment shown in Figure 1

Figure 1

 

collecting-gas-experiment
The student made an error when setting up the apparatus.

State what the error is and describe what would happen if the student used the equipment.

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1a1 mark

This question is about the reactivity of metals.

One method that can be used to determine the order of reactivity of metals is to add the metals to cold water and to dilute hydrochloric acid.

The observations made when strips of four metals are added separately to cold water and to dilute hydrochloric acid are shown in Table 1.

Table 1

Metal Observation with cold water Observation with dilute hydrochloric acid
Magnesium Bubbles very slowly Bubbles very quickly
Platinum No change Not done
Potassium Bubbles very quickly, catches fire Not done
Zinc No change Bubbles very slowly


One reason for not completing the reaction of platinum with dilute hydrochloric acid is the high cost of platinum (roughly £25 per gram).

Suggest how the reaction of platinum with dilute hydrochloric acid could be completed without increasing the cost of the experiment.

1b2 marks

Explain why the experiment with potassium and dilute hydrochloric was not completed.

1c2 marks

Explain why it is not possible to produce a reactivity series using just the observations with cold water.

1d4 marks

Magnesium reacts slowly with cold water but quickly with dilute hydrochloric acid.

Explain two reasons why the reaction with cold water is slower than the reaction with hydrochloric acid.

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2a4 marks

This question is about chemical analysis.

Two students have solid powders of three metal compounds, X, Y and Z.

  • Compound is a black powder.
  • Compound Y is a grey powder.
  • Compound Z is a white powder.

The students both use the same method for their first experiment.

  1. Measure 1.0 g of each powder into a separate test tube
  2. Add 5.0 cm3 of dilute sulfuric acid into each test tube
  3. Record any observations

The observation of both students are shown in Table 1.

Table 1

Sulfuric acid test Student 1 observation Student 2 observation
Compound X Goes black Produces a blue solution
Compound Y Lots of fizzing and gets hot Effervescence 
Compound Z Lots of fizzing Very effervescent

 

Both student's observations for compound X are correct, however student 1 did not leave the reaction to stand for enough time to see the blue solution.

Suggest the identity of compound X. Justify your answer, including a balanced equation.

2b2 marks

Student 1 concludes that compounds and Z are metal carbonates because they fizz lots.

Evaluate student 1's conclusion.

2c3 marks

Both students agree that compound Z contains sodium. 

Student 1 thinks that it is sodium carbonate while student 2 thinks it is sodium hydrogen carbonate.

Sodium carbonate and sodium hydrogen carbonate are both basic.

Explain how the students could use universal indicator solution to determine the identity of compound Z.

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3a2 marks

Sodium hydroxide is a strong alkali.

Explain what is meant by a strong alkali.

3b1 mark

Sodium hydroxide can be neutralised with citric acid.

Write the word equation for this reaction.

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4a3 marks

This question is about hydrochloric acid.

Hydrochloric acid has some domestic uses such as cleaning tiles and rust.

It is recommended that dilute hydrochloric acid is used in these situations.

What is the difference between the pH of dilute hydrochloric acid compared to the pH of concentrated hydrochloric acid?

Give a reason for your answer. 

4b
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2 marks

A solution of hydrochloric acid, with a concentration of 1.5 g / dm3, has a pH value of 1.45.

Predict the pH value when it is diluted to make a solution with a concentration of 0.015 g / dm3. Explain your reasoning.

4c1 mark

The reaction of hydrochloric acid with sodium carbonate solution is an example of a neutralisation reaction.

Write the ionic equation, including state symbols, for neutralisation.

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5a3 marks

This question is about the preparation of magnesium sulfate.

A group of students are asked to prepare a sample of magnesium sulfate.

The students suggest four possible ways to do this:

  1. Magnesium + sulfuric acid
  2. Magnesium carbonate + sulfuric acid
  3. Magnesium hydroxide + sulfuric acid
  4. Magnesium oxide + sulfuric acid

Which of the student's suggestions can be classed as a redox reaction? Justify your choice including relevant equations.

5b1 mark

Explain which reaction produces the most hazardous products.

5c6 marks

Describe how to prepare a sample of magnesium sulfate using suggestion 2.

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