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If 9g of aluminium reacts with 35.5g of chlorine, the empirical formula of the compound formed is A1C1₃

Analysing Substances - Quantitative

Measure how much of a substance is in a sample using titrations and instruments. This GCSE Chemistry quiz helps you calculate concentration, interpret graphs, and compare accuracy.

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Fascinating Fact:

Instrumental methods, like flame emission spectroscopy, can measure concentration using light intensity. A calibration curve is made from standards, then the unknown is read from the graph.

In GCSE Chemistry, quantitative analysis focuses on measuring amounts, not just identifying substances. You practise using data from experiments to calculate concentration, judge reliability, and decide which method gives the most useful results.

Key Terms

Concentration: How much solute is dissolved in a certain volume of solution, often measured in g/dm³ or mol/dm³.
Titration: A method where one solution is added to another until the reaction is complete, so you can calculate an unknown concentration.
Endpoint: The point in a test where a visible change happens, such as an indicator colour change showing the reaction has just finished.

Frequently Asked Questions (Click to see answers)

What is quantitative analysis in GCSE Chemistry?

Quantitative analysis in GCSE Chemistry is measuring how much of a substance is present, such as the concentration of a solution, using calculations and experimental results.

How do you calculate concentration from a titration?

To calculate concentration from a titration, you use the volumes and known concentration to find moles, apply the balanced equation, then divide moles by volume to get the unknown concentration.

Why do scientists repeat measurements in chemistry?

Scientists repeat measurements to reduce random error and spot anomalies. Repeats make results more reliable and help you calculate a better average value.

Try These Related Quizzes

1 .

What is the relative formula mass of copper sulfate CuSO₄?

160 amu

96 amu

128 amu

144 amu

amu = atomic mass units

2 .

What is the relative formula mass of MgF₂?

60 amu

62 amu

43 amu

64 amu

Mg = 24 amu, F = 19 amu, remember that there are 2 F atoms in the molecule of MgF₂

3 .

What % mass of magnesium oxide is magnesium?

60%

40%

30%

70%

First you work out the relative formula mass of magnesium oxide (MgO) then divide the relative atomic mass of magnesium by the relative formula mass and multiply by 100 for the percentage

4 .

What is the % mass of hydrogen in methane CH₄?

20%

25%

75%

12.5%

Use the same method as for the previous question

5 .

Calcium reacts with oxygen as shown by this reaction 2Ca + O₂ → 2CaO. What mass of oxygen will react with 60g of calcium?

12g

24g

14g

From the equation, you find that they react in a ratio of 2 moles to 1 mole. 60g of calcium is 1.5 moles so you will need 0.75 moles of oxygen molecules

6 .

Sodium hydroxide reacts with chlorine to make bleach as shown by this reaction. 2NaOH + Cl₂ → NaOCl + NaCl + H₂O. If we have a solution containing 100g of sodium hydroxide, how much chlorine gas should we pass through the solution to make bleach?

28.65g

82.45g

88.75g

86.57g

Ratio of sodium hydroxide to chlorine is 2 moles to1 mole

7 .

If 9g of aluminium reacts with 35.5g of chlorine, what is the empirical formula of the compound formed?

AlCl

AlCl₂

AlCl₃

Al₃Cl

Use moles! One third of a mole of aluminium atoms react with 1 mole of chlorine atoms therefore there are three times as many chlorine atoms involved. Remember, the mole is nothing more complicated than a measure of the number of particles in a reaction

8 .

A compound contains 13.5g of calcium, 10.8g of oxygen and 0.675g of hydrogen. What is its empirical formula?

CaOH

CaOH₂

CaO₂H

Ca(OH)₂

It's those moles again ...

9 .

A reaction that could theoretically produce 200g of product only produces 140g. What is its % yield?

70%

14.2%

142%

Divide the actual yield by the theoretical yield and multiply by 100

10 .

Ammonium nitrate NH₄NO₃ is used as a fertiliser. What is the % mass of nitrogen in it?

21%

37%

17.5%

35%

Divide the total relative atomic mass of the nitrogen in the formula by the relative formula mass and multiply by 100

You can find more about this topic by visiting BBC Bitesize - Analysing substances

Author: Kate Gardiner (Chemistry Educator & GCSE Quiz Writer)

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