The document discusses acids and alkalis. It defines alkalis as bases with a pH over 7 and describes their characteristics as soluble in water, slippery feeling, and ability to cause chemical burns. Alkalis are formed from group 1 and 2 metals and are often hydroxides. Acids are defined as having a pH under 7, sour taste, and containing hydrogen and an oxide. Most acids are hydrogen compounds. When acids and alkalis are mixed, a neutralization reaction occurs where they cancel each other out, forming a salt and water. Carbonates react with acids in the same way, forming a salt, water, and releasing carbon dioxide.

1. Jacques Zeefenbergen © 2012

2. Remember:
What is pH of an ALKALI?
Alkalis have a pH value greater than 7
0 7 14
ALKALI
Jacques Zeefenbergen © 2012

3. Characteristics of ALKALI?
Alkalis is a base that is soluble in
water (can dissolve)
Strong alkali can cause chemical burns
Alkali feels slippery or like soap when
you touch it.
Jacques Zeefenbergen © 2012

4. FORMULA of an ALKALI?
Metals from group I and II
I – Alkali metals
II – Alkali earth metal
Most alkalis are hydroxide compounds
(I or II)OH (aq)
Jacques Zeefenbergen © 2012

5. Remember:
What is pH of an ACID?
Acids have a pH value less than 7
0 7 14
ACIDS
Jacques Zeefenbergen © 2012

6. Characteristics of ACID?
ACIDS can react with a base
Acids have a sour taste
Acids contain hydrogen and an oxide
Jacques Zeefenbergen © 2012

7. FORMULA of an ACID?
Metal oxide
H+ Non-metal oxide
Chloride gas
Most acids are hydrogen compounds
H(O-compound) (aq)
Jacques Zeefenbergen © 2012

8. What reaction will take place?
NEUTRALISATION
When ACID is added to ALKALI, they
will cancel one another out.
The reaction is called neutralisation,
because they neutralise one another.
Jacques Zeefenbergen © 2012

9. All neutralisation reactions follow the
same form:
Alkali + Acid  salt + water
(metal)OH + H(O compound) 
(metal)(O compound) + (H)(OH)
Jacques Zeefenbergen © 2012

10. Jacques Zeefenbergen © 2012

11. What is a CARBONATE?
(metal) + CO3 (s)
Examples:
CaCO3 (s)
MgCO3 (s)
CuCO3 (s)
Jacques Zeefenbergen © 2012

12. What is an ACID?
Hydrogen + (chloride OR sulphate OR
nitrate)
Examples:
HCl (aq) or (l)
H2SO4 (aq) or (l)
HNO3 (aq) or (l)
Jacques Zeefenbergen © 2012

13. ALL reactions between carbonates and
acid has the same form.
Carbonate + acid  salt + water +
carbon dioxide
Jacques Zeefenbergen © 2012

14. Steps:
1) Metal replaces “H” to form a salt
MgSO4 (s) + H
2) Carbonate decomposes
CO3  CO2 (g) + O
3) Extra “H” and “O” combines to form
water
2H + O  H2O(l)
Jacques Zeefenbergen © 2012

15. Calcium carbonate + hydrochloric
acid

Jacques Zeefenbergen © 2012

16. Magnesium carbonate + sulphuric
acid

Jacques Zeefenbergen © 2012

17. Copper carbonate + nitric acid

Jacques Zeefenbergen © 2012