Introduction to acids and bases

1. INTRODUCTIONINTRODUCTION

2. Acids
Is a substance that produce hydrogen ions when
dissolved in water
All acids contains hydrogen. But not all substances
with hydrogen contains acida (water)
The hydorgen ions produced are responsible for the
properties of an acid

3. Some common acids
Man-made:
Hydrochloric Acid (HCl)
Sulphuric Acid (H2SO4)
Nitric Acid (HNO3)
Natural Acids:
Ethanoic acids (Found in vinegar)

4. Properties
Acids have a sour taste
Acids dissolve in water to form solutions wich
conduce electricity.
Acids turn blue litmus paper red
pH value < 7

5. Chemical properties
1 Acids react with reactive metals to
form hydrogen and salt
 METAL + ACID  SALT + HYDROGEN
Reactive metals give out electrons easily to form
positive ions
Example: Magnesium ribbon with dilute sulphuric acid
 Mg(s) + (H2SO4) (aq)  MgSO4 (aq) + H2 (g)

6. Chemical properties
To test for hydrogen, place a lighted splint at the test
tube and a “pop sound” will be heard.
Some acids and metal reactions which do not give
hydrogen:
Unreactive metals ( copper and silver)
Concentrated nitric acid react with metals but it does
not give hydrogen (gives nitrogen dioxide)
Lead does not react as a coating is formed once lead is
placed inside the acid

7. Chemical properties
2. Acids react with carbonates to form a
salt, carbon dioxide and water.
 ACID + CARBONATE  SALT + CARBON DIOXIDE +
WATER
 Example:
 Sodium carbonate + Dilute hydrochloric acid  Sodium
Choride + Water + carbon dioxide
Bubble the gas through limewater to test for carbon
dioxide

8. Chemical properties
3. Acids react with metal oxides and
hydroxides (insoluble bases) to form salt
and water.
 METAL OXIDE + ACID  SALT + WATER
 HYDROXIDE + ACID  SALT + WATER

9. The role of Water in Acidity
Acids only react when placed on water. This is
because water can break apart the acid into hydrogen
ions and salt.
Therefore, and acid dissociate in water to produce
hydrogen ions wich are responsible for the cidic
properties.
Acids only shor they properties when dissolved in
water

10. The role of Water in Acidity
The hydrogen ions produced are not hydrogen gas.
They react with metals like magnessium to produce
hydrogen gas and magnessium ions
A few drops of water are enough to allow an acid to
dissociate

11. Uses of Acids
Sulphuric acid:
 Detergents
 Car batteries
Ethanoic acid:
 Vinegar to preserve food
 Adhesives (glue)
Hidrochloric Acid:
 Cleaning metals
 Leather processing

13. Base
A base is any metal oxide or hydroxide
A base is a substance that reacts with an acid to give
salt and water only
 ACID + BASE  SALT + WATER
 Similar to:
 ACID + METAL OXIDE / HYDROXIDE  SALT + WATER
Ionic equation for this is always standard:

OH- + H+  H2O (l)

14. Some common bases
Sodium Oxide
Zinc Oxide
Copper (II) Oxide
Magnessium Hydroxide
Aluminum Hydroxide

15. The
Family of
Bases

16. Alkalis
DEFINITION: An alkali is a base that is soluble in
water.
Some examples include:
Sodium Hydroxide
Potassium Hydroxide
Calcium Hydroxide
Barium Hydroxide
Aqueous Ammonia

17. Properties of Alkalis
Alkalis have a bitter taste and soapy feel.
Alkalis turn red litmus paper blue.
pH value > 7.

18. Chemical Properties of Alkalis
All alkalis produce hydroxide ions when dissolved
in water.
Example:
Sodium Hydroxide + Water  Sodium Ion +
Hydroxide ion

19. Chemical Properties of Alkalis
All alkalis react with acids to form salt and water only.
This is also known as neutralisation.
The salt depends on the acid used.
 Sulphuric Acid  Sulphide
 Hydrochloric Acid  Chloride
The ionic equation for this is standardized.
 H+ (aq) + OH- (aq)  H2O (l).

20. Chemical Properties of Alkalis
Alkalis heated with ammonium salts gives off
ammonia gas.
General Equation:
 Alkali + Ammonium Salt  Ammonia + Water + Salt.
Ammonia has a strong smell and turn red litmus
paper blue.
Example:
 Calcium hydroxide + Ammonium chloride  Calcium
Chloride + Water + Ammonia.

21. Chemical Properties of Alkalis
Alkalis can react with the solution of 1 metal salt to give
metal hydroxide and another metal salt.
General Equation:
 Alkali + Salt (of metal A)  Metal Hydroxide + Salt (of metal B)
Example:
 Sodium Hydroxide + Iron (II) Sulphate  Iron (II) Hydroxide +
Sodium Sulphate.

22. Uses of Alkalis
Ammonia Solution:
Window cleaning solutions
Calcium Oxide:
To make iron, concrete, cement
Magnesium Hydroxide:
Toothpaste to neutralise acid o teeth
In antacids to relieve indigestion.
Sodium Hydroxide:
In making soaps and detergents.

23. •Concentration tells us how much of aConcentration tells us how much of a
substance is dissolved insubstance is dissolved in 11 dmdm33
of a solution.of a solution.
•It can be changed by either adding moreIt can be changed by either adding more
solute or more solventsolute or more solvent

24. •Strength refers to how easily an acid orStrength refers to how easily an acid or
alkalialkali dissociatesdissociates when dissolved in water.when dissolved in water.
•A strong acid like hydrochloric acidA strong acid like hydrochloric acid
dissociates easily in water (almost 100% ofdissociates easily in water (almost 100% of
the acid dissociates)the acid dissociates)
•A weak acid like ethanoic acid does notA weak acid like ethanoic acid does not
fully dissociate when dissolved in water.fully dissociate when dissolved in water.

25. • The strength of an acid cannot be changed.The strength of an acid cannot be changed.
• No matter how concentrated ethanoic acidNo matter how concentrated ethanoic acid
is, it is still a weak acid.is, it is still a weak acid.
• The strength of an acid of an alkali can beThe strength of an acid of an alkali can be
shown using the pH scale.shown using the pH scale.