Acids

Recall that acids in solution provide hydrogen ions, while alkalis in solution provide hydroxide ions.

Recall that neutral solutions have a pH of 7, acidic solutions have pH values below 7, and alkaline solutions have pH values above 7.

Recall the specific colour changes of indicators, including litmus, methyl orange, and phenolphthalein, when exposed to acids and alkalis.

Understand the inverse relationship between hydrogen ion concentration and pH in acidic solutions, and the direct relationship between hydroxide ion concentration and pH in alkaline solutions.

Recall that a tenfold increase in hydrogen ion concentration corresponds to a decrease of 1 on the pH scale.

Investigate the change in pH when adding powdered calcium hydroxide or calcium oxide to a fixed volume of dilute hydrochloric acid.

Explain the terms dilute and concentrated concerning the amount of solute in a solution.

Explain the difference between weak and strong acids based on their degree of dissociation into ions in solution.

Understand that a base is a substance that reacts with an acid to produce only a salt and water.

Recall that alkalis are defined as soluble bases.

Explain the general reactions of aqueous acids with metals, metal oxides, metal hydroxides, and metal carbonates to produce specific salts.

Describe the standard chemical tests for hydrogen gas and carbon dioxide gas (using limewater).

Describe a neutralisation reaction as the chemical interaction between an acid and a base.

Explain acid-alkali neutralisation as the reaction where hydrogen ions from the acid combine with hydroxide ions from the alkali to form water.

Explain the steps and reasoning for preparing soluble salts from an acid and an insoluble reactant, including adding excess reactant, removing the excess, and isolating the salt and water.

Explain the steps and reasoning for preparing soluble salts from an acid and a soluble reactant using titration methods.

Investigate the preparation of pure, dry hydrated copper sulfate crystals from copper oxide, utilizing a water bath.

Describe the procedure for conducting an acid-alkali titration using a burette, pipette, and indicator to prepare a pure, dry salt.

Recall the general solubility rules for common substances in water, covering sodium, potassium, ammonium salts, nitrates, chlorides, sulfates, carbonates, and hydroxides.

Predict the formation of a precipitate when specific solutions are mixed, using solubility rules, and identify the resulting precipitate.

Describe the experimental method required to prepare a pure, dry sample of an insoluble salt.