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 12.2 Acid–base titrations Question Bank

[Maximum number: 1]

Name the process used to:

(a)

determine the volume of an acid required to neutralise a given volume of an alkali.

[ 1 ]

[Maximum number: 1]

Which piece of apparatus is used to measure variable quantities of liquid in a titration?

[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 experimental technique used when salts are made by reacting a dilute acid with an aqueous alkali.

[ 1 ]

[Maximum number: 2]

Calcium hydroxide, $\mathrm{Ca}(\mathrm{OH})_{2}$ , is slightly soluble in water.

(a)

A $25.0 \mathrm{~cm}^{3}$ sample of limewater is placed in a conical flask. The concentration of $\mathrm{Ca}(\mathrm{OH})_{2}$ in the limewater is determined by titration with dilute hydrochloric acid, HCl .

[ 2 ]

(i)

Name the item of apparatus used to measure the volume of acid in this titration.

[ 1 ]

(ii)

As well as limewater and dilute hydrochloric acid, state what other type of substance must be added to the conical flask.

[ 1 ]

[Maximum number: 2]

This question is about sodium and compounds of sodium.

(a)

A student determines the concentration of a solution of dilute sulfuric acid, $\mathrm{H}_{2} \mathrm{SO}_{4}$ , by titration with aqueous sodium hydroxide, NaOH .
step $125.0 \mathrm{~cm}^{3}$ of $0.200 \mathrm{~mol} / \mathrm{dm}^{3} \mathrm{NaOH}$ is transferred into a conical flask.
step 2 Three drops of methyl orange indicator are added to the conical flask.
step 3 A burette is filled with $\mathrm{H}_{2} \mathrm{SO}_{4}$ .
step 4 The acid in the burette is added to the conical flask until the indicator changes colour. The volume of acid is recorded. This process is known as titration.
step 5 The titration is repeated several times until a suitable number of results is obtained.

[ 2 ]

(i)

State the colour change of the methyl orange indicator in step 4. from to

[ 1 ]

(ii)

State how the student decides that a suitable number of results have been obtained.

[ 1 ]

[Maximum number: 1]

What is used to identify the end-point of an acid-base titration?

balance

measuring cylinder

indicator

volumetric pipette

(a)

Dilute sulfuric acid and aqueous sodium hydroxide can be used to prepare sodium sulfate crystals using a method that involves titration.

[ 2 ]

(i)

Suggest why universal indicator is not suitable for this titration.

[ 1 ]

(ii)

Name an indicator that can be used in this titration.
$20.0 \mathrm{~cm}^{3}$ of dilute sulfuric acid neutralises $25.0 \mathrm{~cm}^{3}$ of $1.00 \mathrm{~mol} / \mathrm{dm}^{3}$ aqueous sodium hydroxide. At the end of the titration the conical flask contains aqueous sodium sulfate with the dissolved indicator as an impurity.

[ 1 ]

[Maximum number: 1]

Dilute hydrochloric acid is titrated into a conical flask containing sodium hydroxide solution and a few drops of methyl orange indicator.

Which piece of apparatus is used to add the hydrochloric acid?

beaker

burette

measuring cylinder

pipette

[Maximum number: 1]

An acid-base titration is described.
- $25.0 \mathrm{~cm}^{3}$ of dilute aqueous alkali is put into a conical flask.
- Indicator is added to the flask.
- Dilute acid is added to the aqueous alkali until the indicator changes colour.
- The volume of acid used is then recorded.

Which use of apparatus is correct?

The $25.0 \mathrm{~cm}^{3}$ of aqueous alkali is measured using a volumetric pipette.

The $25.0 \mathrm{~cm}^{3}$ of aqueous alkali is measured using the lines on the conical flask.

The volume of acid is measured using a measuring cylinder.

The volume of acid is measured using a volumetric pipette.

[Maximum number: 1]

The concentration of acids and alkalis can be determined by titration.
Which pieces of equipment are needed to perform a titration?

1 and 2

1 and 3

2 and 3

2 and 4

0 selected

Question 1

Question 1(g)

Question 2

Question 2

Question 2(d)

Question 2(d)(iii)

Question 2

Question 2(d)

Question 2(d)(i)

Question 2(d)(iii)

Question 3

Question 3(c)

Question 3(c)(ii)

Question 3(c)(iii)

Question 37

Question 5

Question 5(a)

Question 5(a)(i)

Question 5(a)(ii)

Question 38

Question 39

Question 39