1. States of matter

1.1 Solids, liquids and gases

1.2 Diffusion

2. Atoms, elements and compounds

2.1 Elements, compounds and mixtures

2.2 Atomic structure and the Periodic Table

2.3 Isotopes

2.4 Ions and ionic bonds

2.5 Simple molecules and covalent bonds

2.6 Giant covalent structures

2.7 Metallic bonding

3. Stoichiometry

3.1 Formulae

3.2 Relative masses of atoms and molecules

3.3 The mole and the Avogadro constant

4. Electrochemistry

4.1 Electrolysis

4.2 Hydrogen–oxygen fuel cells

5. Chemical energetics

5.1 Exothermic and endothermic reactions

6. Chemical reactions

6.1 Physical and chemical changes

6.2 Rate of reaction

6.3 Reversible reactions and equilibrium

6.4 Redox

7. Acids, bases and salts

7.1 The characteristic properties of acids and bases

7.2 Oxides

7.3 Preparation of salts

8. The Periodic Table

8.1 Arrangement of elements

8.2 Group I properties

8.3 Group VII properties

8.4 Transition elements

8.5 Noble gases

9. Metals

9.1 Properties of metals

9.2 Uses of metals

9.3 Alloys and their properties

9.4 Reactivity series

9.5 Corrosion of metals

9.6 Extraction of metals

10. Chemistry of the environment

10.1 Water

10.2 Fertilisers

10.3 Air quality and climate

11. Organic chemistry

11.1 Formulae, functional groups and terminology

11.2 Naming organic compounds

11.3 Fuels

11.4 Alkanes

11.5 Alkenes

11.6 Alcohols

11.7 Carboxylic acids

11.8 Polymers

12. Experimental techniques and chemical analysis

12.1 Experimental design

12.2 Acid–base titrations

12.3 Chromatography

12.4 Separation and purification

12.5 Identification of ions and gases

IGCSE Chemistry 7.3 Preparation of salts Question Bank

[Maximum number: 1]

This question is about states of matter.

(a)

A solution is a mixture of a solute and a solvent.

[ 1 ]

(i)

Name the type of reaction when two solutions react to form an insoluble substance.

[ 1 ]

[Maximum number: 1]

Some symbol equations and word equations, A to J, are shown.

A $\mathrm{Fe}^{3+}+3 \mathrm{OH}^{-} \rightarrow \mathrm{Fe}(\mathrm{OH})_{3}$

B $\mathrm{H}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$

C ethane + chlorine → chloroethane + hydrogen chloride

D $\mathrm{C}_{12} \mathrm{H}_{26} \rightarrow \mathrm{C}_{8} \mathrm{H}_{18}+\mathrm{C}_{4} \mathrm{H}_{8}$

E ethene + steam → ethanol
F chlorine + aqueous potassium iodide → iodine + aqueous potassium chloride

G $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} \rightarrow 2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}+2 \mathrm{CO}_{2}$

H ethanoic acid + ethanol → ethyl ethanoate + water
I calcium carbonate → calcium oxide + carbon dioxide

J $6 \mathrm{CO}_{2}+6 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}+6 \mathrm{O}_{2}$

Use the equations to answer the questions that follow.
Each equation may be used once, more than once, or not at all.
Give the letter, A to J, for the equation that represents:

(a)

a precipitation reaction [1]

[ 1 ]

[Maximum number: 1]

Some symbol equations and word equations, A to J, are shown.

A $\mathrm{H}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$

B $\mathrm{Cr}^{3+}+3 \mathrm{OH}^{-} \rightarrow \mathrm{Cr}(\mathrm{OH})_{3}$

C methane + chlorine → chloromethane + hydrogen chloride
D propene + bromine → 1,2-dibromopropane

E $\quad \mathrm{C}_{10} \mathrm{H}_{22} \rightarrow \mathrm{C}_{8} \mathrm{H}_{18}+\mathrm{C}_{2} \mathrm{H}_{4}$

F chlorine + aqueous potassium bromide → bromine + aqueous potassium chloride
G methane + oxygen → carbon monoxide + water

H $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{OH} \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOCH}_{3}+\mathrm{H}_{2} \mathrm{O}$

I hydrogen + oxygen → water

J $6 \mathrm{CO}_{2}+6 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}+6 \mathrm{O}_{2}$

Use the equations to answer the questions that follow.
Each equation may be used once, more than once, or not at all.
Give the letter, A to J, for the equation which represents:

(a)

a precipitation reaction [1]

[ 1 ]

[Maximum number: 1]

Lead(II) iodide is insoluble in water.
Lead(II) iodide is made by adding aqueous lead(II) nitrate to aqueous potassium iodide.
Which pieces of apparatus are needed to obtain solid lead(II) iodide from $20 \mathrm{~cm}^{3}$ of aqueous lead(II) nitrate?

1, 2 and 4

1, 3 and 5

1, 4 and 5

2, 4 and 5

[Maximum number: 1]

The equation for the reaction between barium chloride and dilute sulfuric acid is shown.

\mathrm{BaCl}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{BaSO}_{4}+2 \mathrm{HCl}

Which row shows the state symbols for this equation?

$\mathrm{BaCl}_{2}$

$\mathrm{H}_{2} \mathrm{SO}_{4}$

$\mathrm{BaSO}_{4}$

2 HCl

$(\mathrm{aq})$

$(\mathrm{s})$

$(\mathrm{aq})$

$(\mathrm{I})$

$(\mathrm{s})$

$(\mathrm{aq})$

$(\mathrm{I})$

$(\mathrm{aq})$

$(\mathrm{s})$

$(\mathrm{I})$

$(\mathrm{aq})$

$(\mathrm{I})$

$(\mathrm{aq})$

$(\mathrm{I})$

[Maximum number: 1]

The equation for the reaction between barium chloride and dilute sulfuric acid is shown.

\mathrm{BaCl}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{BaSO}_{4}+2 \mathrm{HCl}

Which row shows the state symbols for this equation?

$\mathrm{BaCl}_{2}$

$\mathrm{H}_{2} \mathrm{SO}_{4}$

$\mathrm{BaSO}_{4}$

2 HCl

$(\mathrm{aq})$

$(\mathrm{s})$

$(\mathrm{aq})$

$(\mathrm{I})$

$(\mathrm{s})$

$(\mathrm{aq})$

$(\mathrm{I})$

$(\mathrm{aq})$

$(\mathrm{s})$

$(\mathrm{I})$

$(\mathrm{aq})$

$(\mathrm{I})$

$(\mathrm{aq})$

$(\mathrm{I})$

[Maximum number: 2]

Sodium is a reactive metal.

(a)

When NaOH(aq) is added to aqueous iron(III) chloride, $\mathrm{FeCl}_{3}(\mathrm{aq})$ , a solid product is formed.

[ 2 ]

(i)

Name the type of reaction where a solid is formed from two solutions.

[ 1 ]

(ii)

Name this solid product.

[ 1 ]

[Maximum number: 4]

Cobalt and copper are transition elements.

(a)

Both copper and cobalt can form coloured compounds. Some of these compounds contain water of crystallisation.

[ 4 ]

(i)

Define the term water of crystallisation.

[ 2 ]

(ii)

State the colour and formula of hydrated cobalt(II) chloride crystals.
colour
formula

[ 2 ]

[Maximum number: 1]

Potassium is a Group I element.

(a)

Aqueous potassium hydroxide reacts with a dilute acid to produce aqueous potassium chloride, KCl(aq), which is a salt.

[ 1 ]

(i)

Name the dilute acid used.

[ 1 ]

[Maximum number: 7]

Soluble salts can be made by adding a metal carbonate to a dilute acid.

(a)

A student wanted to make hydrated iron(II) sulfate crystals, $\mathrm{FeSO}_{4} \cdot x \mathrm{H}_{2} \mathrm{O}$ , by adding excess iron(II) carbonate to dilute sulfuric acid. The student followed the procedure shown.
step 1 Add dilute sulfuric acid to a beaker.
step 2 Add small amounts of iron(II) carbonate to the dilute sulfuric acid in the beaker until the iron(II) carbonate is in excess.
step 3 Filter the mixture formed in step 2.
step 4 Heat the filtrate until it is a saturated solution. Allow to cool.
step 5 Once cold, pour away the remaining solution. Dry the crystals between filter papers.

[ 5 ]

(i)

Why must the iron(II) carbonate be added in excess in step 2?

[ 1 ]

(ii)

State two observations in step 2 that would show that iron(II) carbonate was in excess. 1

2

[ 2 ]

(iii)

Describe what should be done during step 3 to ensure there is a maximum yield of crystals.

[ 1 ]

(iv)

Name a different compound that could be used instead of iron(II) carbonate to produce hydrated iron(II) sulfate crystals from dilute sulfuric acid.

[ 1 ]

(b)

Insoluble salts can be made by mixing solutions of two soluble salts.

A student followed the procedure shown to make silver bromide, an insoluble salt.
step 1 Add aqueous silver nitrate to a beaker. Then add aqueous potassium bromide and stir.
step 2 Filter the mixture formed in step 1.
step 3 Dry the residue.

[ 2 ]

(i)

State the term used to describe this method of making salts.

[ 1 ]

(ii)

Give the observation the student would make during step 1.

[ 1 ]

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Question 1

Question 1(d)

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Question 1(b)

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Question 1(c)

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Question 7

Question 7

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Question 2(d)(i)

Question 2(d)(iii)

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Question 2

Question 2(d)

Question 2(d)(i)

Question 2

Question 2(b)

Question 2(b)(i)

Question 2(b)(ii)

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Question 2(b)(v)

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