Chemistry: Acids, Bases, and salts

Acids

Are substances that can donate H plus ions to bases to form salt and water, an acid is therefore defined as a PROTON DONOR.

Ionization of acids in Water

When an acid is added to water, the acid molecules ionize they Form ions.

Acids ionize to form hydrogen ions H^+ ions and negative anions.

The H^+ ions become attached to the polar water molecules forming hydronium ions.

Organic Acid

Contains the carboxyl group ( COOH). In these acids, it is the hydrogen at the end of the carboxyl group which forms H^+ ions when the acid dissolves in water

Inorganic Acids

Inorganic acids contains a non metallic element or polyatomic group as well as hydrogen.

Basicity

Acids can also be classified according to the of H^+ ions they produce per molecule when dissolved in water. The is known as their basicity.

Monobasic acid

A monobasic acid produces one H plus ion per molecule when it is dissolved in water example economic acid CH3COOH and hydrochloric acid HCL.

Dibasic acid

A dibasic acid produces two hydrogen plus ions per molecule when it is dissolved in water. e.g sulphuric acid, H2 SO4

Tribasic acid

A tribasic acid produces three (hydrogen plus ions) per molecule when it is dissolved in water, e.g. phosphoric acid H3PO4

Degree of ionization

An acid can be classified based on a degree of organization that occurs when the acid is dissolved in water.

Strong acid

A strong acid is fully ionized when they dissolve in water. There is therefore high concentration of hydrogen plus ions in the solution, example hydrochloric acid and sulfuric acid.

Weak acid

A weak acid is only partially ionized when it is dissolved in water. There is therefore a low concentration of hydrogen + ions in the solution. example a weak acid is ethanoic acid.

Concentration

Assets can be classified based on the quality of water present.

Dilute acid

Dilute acid is one that contains a lot of water example hydrochloric acid that has a concentration of 0.01 mole or DM cubed.

Concentrated

I concentrated acid is one that contains very little water example hydrochloric acid that has a concentration of 12 miles per DM cubed

Acid Anhydride

An acid anhydride is a compound which reacts with water to vitamin acid many acid anhydrides or acid oxide of non- metals example of acid anhydride are: carbon dioxide, sulphuric trioxide, and nitrogen dioxide.

Bases

Bases are usually metal oxide or metal hydroxide and they can accept hydrogen plus ions from acid to form salt and water. Therefore a a base is defined as a proton acceptor.

Soluble bases

Soluble bases are known as alkalis. An alkali is a base which dissolves in water to form a solution containing hydroxide ions..

Classification of oxide

Bases are oxide and hydroxide and oxide can be classified as acidic basic amphoteric, and neutral.

Acidic oxide

Acidic oxide or oxide of certain metals with react with alkali to form salt and water

Acid oxide also react with water to form an acid

Examples of acid oxide, carbon dioxide super dioxide, sulfur, trioxide, nitrogen dioxide

Basic oxide

Basic oxides are oxides of metal with react with acids to form assault and water. There are a few basic oxide that react with water to form a hydroxide. These are alkalis. Examples of basic oxide, magnesium oxide, iron two oxide and copper two oxide.

Amphoteric oxide

An amphoteric substance is one that can behave as both an acid or base so they react with both acids and strong alkalis.

Some metal oxides and hydroxides are termed as amphoteric hydroxide we will be studying.

Neutral Oxides

Neutral oxide or oxide of a certain nonmetal, which do not react with acids or alkalis.

Strength of an Alkali

When a little water and alkali ions for positive ions and hydrogen ions

Strong Alkali

A strong alkali is fully ionized when dissolved in water therefore, there is a high concentration of hydroxide ions in the solution, example sodium hydroxide and potassium hydroxide.

Weak alkali

A weak alkali is only partially ionized when it dissolves in water, there is therefore a low concentration of hydroxide ions in the solution example a weak alkali ammonia.

Indicators

An indicator also called an acid base indicator is a chemical that is indifferent colors in acid and basis some acid based indicators are obtained from organic material. A common indicator is litmus which is extracted from reaching lichen

Salt

Salts are ionic compounds formed when some are all the replaced hydrogen ions in an acid are replaced by metals or ammonium ions

Normal Salts

Normal salts are formed when all of the hydrogen ions in an acid are replaced by metals Ar ammonium ions

All acids can form normals salts.

Acids salt

An acid salt is formed when the hydrogen ions in an acid are only partially replaced a by metal or ammonium ions. Only dibasic and tribasic acids can form acid salts.

Water crystallization

Some salts contain a fixed amount of water molecules trapped between their ions in crystal lattice. This is known crystallization

Hydrated salts

Contain water of crystallization - hydrated copper two sulphate

Anhydrous salts

Do not contain water of crystallization - anhydrous copper two sulphate

Preparation of salts

To prepare a salt, you select a method based on the solubility of the salt you are trying to prepare

The method for preparing a soluble saltis different form method to propose an insoluble salt.

Preparing an insoluble salt

Insoluble salts can be prepared using ionic precipitation otherwise know double displacement reactions

Neutralization reaction

A neutralization reaction is a reaction between a base an acid to form salt and water

Neutralization point / end point

The neutralization point is the point in an acid alkali reaction where the reaction is complete and neither acid nor alkali is present in excess. The neutralization point is also known as the end point

Determine the Neutralization point

The neutralization point of an acid-alkali reaction can be determined during a titration by using an indication, a pH meter or temperature change

Titration

Is the show addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization.