A positively charged ion formed when a hydrogen atom loses an electron (H⁺).

The measure of the hydrogen ion (H⁺) concentration of a solution.

The amount of solute dissolved in a certain volume of solution.

An acid which fully dissociates to form H⁺ ions in aqueous solution.

An acid which partially dissociates to form H⁺ ions in aqueous solution.

Comparing concentration with strength

Chemistry

Describing salts

Hazard symbols and equipment

Acid-base reactions (carbonates as bases)

Chemical reactions of acids with metals and metal carbonates

Concentration of solutions

Concentration of solutions: using moles (RAM 1 d.p.)

Making a pure dry sample of a soluble salt

pH scale and indicators

Solubility rules

Ionic equations: salt formation

Adapting a multistep chemical procedure for making a pure dry salt

Change in pH: practical

Titrations: making soluble salts

Titrations: analytical technique

Titrations: calculating an unknown concentration (RAM 1 d.p.)

In the Electrolysis unit, pupils will build on their understanding of chemical reactions to explore the process of electrolysis and its applications.

In the Acids and Bases unit, pupils learned about the properties of acids, bases, and alkalis, and the reactions between them to form salts and water.

This unit explores empirical formulae, balanced chemical and ionic equations, gas identification, acid reactions, and pH as a measure of hydrogen ion concentration. It covers separation techniques and focuses on planning experiments, accurate measurements, safety, and communicating findings.

Making salts

a positive ion formed when a hydrogen atom loses an electron

the measure of hydrogen ion concentration in a solution

the amount of solute dissolved in a certain volume of solution

an acid that fully dissociates to form H⁺ ions in aqueous solution

an acid that partially dissociates to form H⁺ ions in aqueous solution

Match the following key terms to their definitions.

Which of the following statements about a strong acid in an aqueous solution is correct?

Why do strong acids have a lower pH than weak acids of the same concentration?

What happens to the pH of a solution if the hydrogen ion concentration increases by a factor of 10?

they measure the temperature of a reaction

they show the colour change in the solution

they allow chemists to pinpoint an accurate end point

the pH changes quickly after the end point is reached

What happens during the neutralisation of a weak acid?

the process of dissolving a substance in water

the formation of ions by gaining or losing electrons

What does it mean if an acid is completely ionised in an aqueous solution?

What does a weak acid do in an aqueous solution?

they show the temperature change during a reaction

they graph pH changes to find neutralisation points

What is the significance of titration curves?

Starter Quiz

What is the pH scale used to measure?