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11–12Chemistry 11–12 Syllabus (2025)

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Implementation from 2028
Expand for detailed implementation advice
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Year 12

Acid–base reactions

Relevant Working scientifically outcomes and content must be integrated with each focus area. All the Working scientifically outcomes and content must be addressed by the end of Year 12.

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Properties of acids and bases

  • Identify the common name and International Union of Pure and Applied Chemistry (IUPAC) nomenclature of inorganic acids and bases

  • Describe chemical properties of common inorganic acids and bases

  • Conduct a laboratory experiment to prepare a natural indicator and compare it to a universal indicator in terms of its effectiveness in identifying a variety of acids and bases

  • Conduct a scientific investigation to compare the accuracy of digital pH probes and indicators when identifying strong and weak acids and bases

  • Explain how limitations in Arrhenius’s theory led to the development of the Brønsted–Lowry theory of acids and bases

Using Brønsted–Lowry theory

  • Use Brønsted–Lowry theory to recognise conjugate acid–base pairs and amphiprotic substances

  • Use Brønsted–Lowry theory to explain the difference between monoprotic, diprotic and triprotic acids using balanced chemical equations

  • Conduct a practical investigation to compare the pH of a strong acid and a strong base in a variety of concentrations

  • Analyse the relationship between pH and hydrogen ion concentration ([H+])
  • Calculate the pH, pOH, hydrogen ion concentration ([H+]) and hydroxide ion concentration ([OH-]) of solutions
  • Solve dilution problems using C1V1=C2V2 and pH=-log10⁡H3O+
  • Describe the relationship between ionisation constant for water (Kw), hydrogen ion concentration ([H+]) and hydroxide ion concentration ([OH-]) in solutions

  • Calculate the pH of a resultant solution when solutions of acids and bases are mixed

  • Conduct a practical investigation to compare the pH of a variety of acids and bases with the same concentration

  • Use models and equilibrium principles to demonstrate the difference between strong and weak acids, including polyprotic acids

  • Use ionic equations to explain the ionisation or dissociation of acids and bases in water, conjugate acid–base pairs, and the amphiprotic natures of some salts

  • Use balanced equations to predict the acidic or basic nature of the salt produced by neutralisation reactions

  • Calculate and apply the dissociation constants Ka and Kb, and pKa and pKb to compare the strengths of acids and bases

  • Conduct a laboratory experiment to determine the Ka of a weak acid

  • Solve problems to relate Ka, Kb and Kw

  • Discuss the use of buffers in equilibrium systems

  • Conduct a practical investigation to prepare a buffer and demonstrate its properties

  • Conduct a secondary-source investigation to describe the role of buffers in a natural system

Quantitative analysis

  • Conduct a laboratory experiment to prepare a primary standard solution

  • Discuss the relationship between the equivalence point and endpoint, in determining the choice of an indicator for a titration

  • Conduct laboratory experiments to analyse the concentration of a strong acid and a strong base by titration

  • Analyse titration curves and conductivity graphs for monoprotic acids

  • Solve problems using titration curves and titration data to determine the concentration of strong and weak acids and bases

  • Analyse the use of limiting reagents in back titrations

  • Conduct a practical investigation using back titrations to determine the concentration of an unknown substance

  • Conduct a scientific investigation to analyse acid–base analysis techniques used in household digital probes and instruments

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