Chapter 10 Acid-base (Proton Transfer) Reactions

Alkali

Bases which are soluble in water and neutralises acids

Acid

A donator of protons (hydrogen ions) to bases

Base

A reciever of protons (hydrogen ions) from acids

Amphiprotic

Being able to act as an acid and as a base depending on the reactant

Monoprotic Acid

An acid which only donates one proton

Diprotic Acid

An acid which can donate 2 protons

Triprotic Acid

An acid which can donate three protons

Polyprotic Acid

An acid which can donate more than one proton

Strong Acids

Acids that completely dissociate and ionise in solution.

Weak Acids

Acids that partially dissociate and ionise in solution

Acidic Proton

A hydrogen atom in a molecule that can be easily donated as a hydrogen ion

Conjugate

A pair of chemical species linked by the transfer of a proton and only differ by one proton

Conjugate Base

The chemical species formed after an acid loses a proton (H⁺) during a chemical reaction

Conjugate Acid

The chemical species formed after an base gains a proton (H⁺) during a chemical reaction

Strength

Substance’s willingness to ionise and dissociate

Concentration

Amount of an acid or base dissolved in a solute

Dissociate

To break down into smaller parts

Dilute

Reduce concentration of a solute in a solvent by increasing the amount of solvent

Brønsted-Lowry Theory

Definition of an acid as a chemical species which donates a proton to a base

Acid-base Reaction

Chemical reaction where a proton is transferred from an acid to a base

Deprotonation

Loss of a proton from an acid

Neutralise

React with an acid or base to produce water

Super Acid

An acid which has an acidity greater than the acidity of pure sulfuric acid

Antacid

Over-the-counter medications made of bases that provide fast, temporary relief from heartburn, indigestion, and mild acid reflux by neutralising excess stomach acid

Metal Carbonate

An ionic compound base which contains a positive metal ion and a negative carbonate ion (CO₃^2-).

Metal carbonates form the same products as metal hydrogencarbonates reacting with acids

Metal Hydrogencarbonates

Inorganic, amphoteric, ionic salts containing a metal cation and the bicarbonate anion (HCO₃^-)

Metal hydrogencarbonates form the same products as metal carbonates reacting with acids

Also known as bicarbonate

Metal Carbonates General Reaction

Acid + Metal Carbonate → Ionic Salt + CO₂ (g) + H₂O (l)

Metal Hydroxides General Reaction

Acid + Metal Hydroxide → Ionic Salt + H₂O (l)

Metal Carbonate Solubility

• It is soluble if it contains a group 1 metal

• When added to water, a soluble metal carbonate will dissociate into cations and carbonate ions

• Insoluble metal carbonates will remain solid when added to water

  though they still follow the same general reaction as soluble metal carbonates

Metal Hydroxides

An ionic compound base consisting of a metallic cation and the hydroxide (OH^-) anion

Metal Hydrogencarbonate General Reaction

Acid + Metal Hydrogencarbonate → Ionic Salt + CO₂ (g) + H₂O (l)

Metal Hydroxide Solubility

• Most metal hydroxides are soluble (e.g., NaOH and KOH)

• When added to water, a soluble metal hydroxide will dissociate into cations and hydroxide ions

• Insoluble metal hydroxides (e.g., MgCO₃) will remain solid when added to water though they still follow the same general reaction as soluble metal hydroxides