Languages: English

Examines and evaluates uses of acids and bases in the food and pharmaceutical industries. Shows how acids, produced directly or indirectly, can lead to environmental problems such as acid rain.

The two reactions involved in the production of methanol form the basis for a review of the factors which favour methanol production. Provides an example of a calculation using a quadratic equation to solve for equilibrium concentrations.

Empirical definitions of acidic, basic and neutral solutions are derived by performing diagnostic tests. Students examine real-life applications of acids and bases, and an analogy is used to present the historical development of acid-base theories.

Studies evidence for the shifting of equilibrium in pure water when acids or bases are added. Examines the inverse relationship between hydrogen and hydroxide ions in all solutions, and sample calculations are worked out with Kw.

Provides a definition of pH and how it is calculated. Explains a pH/pOH scale and the mathematical relationship between pH and pOH. Demonstrates the use of pH metres and examines the significance of pH in biological systems.

The topic of acid deposition leads to a calculation of hydronium and hydroxide ion concentrations, pH and pOH using Kw. These calculations demonstrate what happens to pH and pOH during a series of dilutions.

An experiment comparing acidic solutions in relationship to their pH and conductivity leads to a definition of strong and weak acids. A similar procedure is followed for bases.

Various real-life contexts are used to present the different calculations involving Ka, Kb, pH, pOH, hydronium ion, hydroxide ion, and the percentage of a reaction. Shows the relationship between Kw, Ka and Kb.

Shows how the Brønsted-Lowry Theory explains the limitations of Arrhenius’ Theory. Demonstrates the five-step method for writing Brønsted-Lowry equations using the acid-base table from the data booklet.

Reactions involving polyprotic and anions of polyprotic acids can be predicated by adding the proton transfer equations together. Students test and evaluate these predictions through laboratory activities.