| Define an acid (according to the Brønsted–Lowry definition) | Acids are substances that act as proton donors in a chemical reaction. |
| Define a base (according to the Brønsted–Lowry definition) | Bases are substances that act as proton receivers in a chemical reaction. |
| Define the term monoprotic | "Monoprotic" refers to an acid or base that can donate or accept only one proton (H+) in a chemical reaction. |
| Define the term polyprotic | "Polyprotic" refers to an acid or base that can donate or accept more than one proton (H+) in a chemical reaction. |
| Distinguish between strong and weak acids and bases in terms of the extent of dissociation, reaction with water and electrical conductivity. | Strong acids and bases dissociate completely in water, leading to a high degree of ionization, strong reaction with water, and high electrical conductivity. Weak acids and bases partially dissociate, resulting in lower ionization, weaker reaction with water, and lower electrical conductivity. |
| Define what a 'strong' acid and base is. | Strong acids and bases fully ionize or dissociate in water, resulting in high concentrations of hydrogen ions (H+) for strong acids and hydroxide ions (OH-) for strong bases |
| Define what is meant by 'concentrated acids and bases'. | Concentrated acids and bases refer to solutions with a large amount of acid or base dissolved in water regardless of their ionization or dissociation properties. |
