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4.2.10Chemical Changes

Titration Calculations — AQA GCSE Combined Science Trilogy 8464 - Chemistry Revision Notes & Topical Questions

5 min read 11 parts Lesson 15 of 21

📚 AQA GCSE Combined Science Trilogy 8464 - Chemistry Hub / Topical Revision
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Part 1 of 11Metal and Acid

Core Concept
  • Core Concept Fundamental principles, definitions, and physical or chemical laws governing this topic.
Mechanism & Behavior
  • Mechanism & Behavior Key interactions, structural properties, and process dynamics observed in experiments.
Exam Applications
  • Exam Applications Quantitative relationships, key formulas, and criteria required by specification mark schemes.

Part 2 of 11Metal & Acid Reactions as Redox Reactions

1
Fundamental principles, definitions, and physical or chemical laws governing this topic.
2
Key interactions, structural properties, and process dynamics observed in experiments.
3
Quantitative relationships, key formulas, and criteria required by specification mark schemes.

Part 3 of 11Neutralisation of Acids and Salt Production

Neutralisation of Acids and Salt Production
Acid-base reactions
  • Acid-base reactions Acid-base reactions When an acid reacts with a base, a neutralisation reaction occurs A base is a chemical that neutralises acids Examples of bases include: Metal oxides, e.g
Copper(ii) oxide,
  • Copper(ii) oxide, copper(II) oxide, CuO Metal hydroxides, e.g
Sodium hydroxide,
  • Sodium hydroxide, sodium hydroxide, NaOH Metal carbonates, e.g
Therefore, the
  • Therefore, the Therefore, the reaction between an acid and a metal is not a neutralisation reaction
If an
  • If an If an acid-base reaction effervesces (fizzes), then the base must be a metal carbonate as carbon dioxide gas is produced

Part 4 of 11Soluble Salts

Core Concept
  • Core Concept Fundamental principles, definitions, and physical or chemical laws governing this topic.
Mechanism & Behavior
  • Mechanism & Behavior Key interactions, structural properties, and process dynamics observed in experiments.
Exam Applications
  • Exam Applications Quantitative relationships, key formulas, and criteria required by specification mark schemes.

Part 5 of 11Required Practical: Preparation of a Soluble Salt

1
The steps in the preparation of a soluble salt Practical Tip: The base is added in excess to use up all of the acid, which would become dangerously concentrated during the evaporation and crystallisation stages Method: 1
2
Add 50 cm dilute acid into a beaker and warm gently using a Bunsen burner 2
3
Add the insoluble oxide slowly to the hot dilute acid and stir until the base is in excess (i.e
4
until the base stops dissolving and a suspension of the base forms in the acid) 3
5
Filter the mixture into an evaporating basin to remove the excess base 4

Part 6 of 11The pH Scale & Neutralisation

The pH Scale & Neutralisation
Substance ph
  • Substance ph Substance pH lemon juice 2.2 limewater 10.5 saliva 6.3 milk of magnesia 10.1 1
Name the
  • Name the Name the strongest alkali 2
Name the
  • Name the Name the strongest acid 3
This
  • This is incorrect as a sharp colour change is required to identify the end-point, which cannot be achieved with Universal Indicator

Part 7 of 11Strong & Weak Acids

A dilute
  • A dilute A dilute solution of a strong acid can have a lower pH than a concentrated solution of a weak acid, due to the stronger acid undergoing complete dissociation
Examiner tips
  • Examiner tips Examiner Tips and Tricks Remember concentration describes the total number of acid molecules added to the solution but does not consider those that dissociated
This
  • This is measured using the pH scale

Part 8 of 11Titrations

1
Fundamental principles, definitions, and physical or chemical laws governing this topic.
2
Key interactions, structural properties, and process dynamics observed in experiments.
3
Quantitative relationships, key formulas, and criteria required by specification mark schemes.

Part 9 of 11Required Practical: Strong Acid & Strong Alkali Titration

Required Practical: Strong Acid & Strong Alkali Titration
Use the
  • Use the Use the pipette and pipette filler and place exactly 25 cm sodium hydroxide solution into the conical flask 2
Place the
  • Place the Place the conical flask on a white tile so the tip of the burette is inside the flask 3
Add a
  • Add a Add a few drops of a suitable indicator to the solution in the conical flask 4
Perform a
  • Perform a Perform a rough titration by taking the burette reading and running in the solution in 1 – 3 cm portions,
    • while swirling the flask vigorously 5
Quickly close
  • Quickly close Quickly close the tap when the end-point is reached (sharp colour change) and record the volume, placing your eye level with the meniscus 6

Part 10 of 11Titration Calculations

Calculate the
  • Calculate the Calculate the concentration of HNO that was used
Give your
  • Give your Give your answer to 2 decimal places
0128 =
  • 0128 = 0128 = 0.59 mol/dm to 2 dp Remember to convert cm to dm by dividing by 1000 3 3

Part 11 of 11Exam Checklist & Tips

Specification Mastery Checklist

  • Key Definitions Ensure precise recall of terms and units as required by examination mark schemes.
  • Equations & Formulas Double-check balanced state symbols, subscripts, and SI unit conversions.
  • Common Misconceptions Verify experimental conditions, controls, and comparative trends across groups.

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