Chemistry 'O' level syllabus: Acids, Bases & Salts Please download to access the animations that come with the slides. Some of the animations help to clear away hidden boxes. Slides include interactive learning elements!!! Contact me if you want more slides or to custom made for you at: Email: fazzydoo@gmail.com Facebook: Faiz Abdullah (look at picture) Twitter: @fazzydoo

1. ACIDS,
BASES &
SALTS
PREPARED BY: FAIZ ABDULLAH

2. ACIDS
Properties
Definition
Common
acids
Reactions
Weak Vs.
Strong

3. DEFINITION
A compound which produces hydrogen ions, H+, when
dissolved in water
Acid + H2O  H+

4. STRONG VS WEAK
ACIDS
Strong acids IONIZED COMPLETELY in water
Weak acids IONIZED PARTIALLY in water
HCl
water
H+
H+
H+Cl-
Cl-
Cl-
Strong Acid
Dissociate completely

5. WEAK ACIDS
water
CH3COOH
CH3COOH
CH3COOH
H+
H+
CH3COO-
CH3COO-
Weak acid does
Not dissociate
completely
Ada CH3COOH
Masih tetinggal

6. COMMON ACIDS
HCl
H2SO4
HNO3
CH3COOH
Sulfuric Acid
Nitric Acid
Ethanoic Acid
Hydrochloric Acid

7. PROPERTIES
Taste: Sour taste
Litmus paper: Blue Red

8. REACTIONS OF
DILUTE ACIDS
1. Some METALS to give SALT and HYDROGEN gas
Zn + 2HCL  ZnCl2 + H2
2. Bases to give SALT and WATER only
2NaOH + H2SO4 Na2SO4 + H2O
3. Carbonates and hydrogencarbonates (insoluble or
soluble) to give salt, water and CO2 gas
CaCO3 + 2HCl  CaCl2 + H2O + CO2

9. IONS THAT ARE
PRODUCED!
ACIDS BASES
H+
OH-

10. BASES
Properties
Definition
Common
bases
Reactions
Weak Vs.
Strong

11. DEFINITION
Substance which reacts with an acid to form salt
and water only
NEUTRALIZATION
ACIDS + BASE  SALT + WATER

12. REACTIONS
1) Reacts with acids to produce salt and water only
2) Ammonium salts to produce AMMONIA
NaOH + NH4Cl  NaCl + NH3 + H2O
AMMONIA

13. COMMON BASES
CaO
MgO
CuO
NaOH
NH3
Copper(II) Oxide
Calcium Oxide
Magnesium Oxide
Ammonia
Sodium Hydroxide

14. THEN, WHAT IS AN
ALKALI
Alkali are BASES THAT ARE SOLUBLE IN WATER
BASES
Soluble in water Insoluble in water
ALKALI

15. ALKALI
PROPERTIES
Slippery
Turns Litmus paper:
Red Blue
Produces OH-
when dissolved in
water

16. DISSOCIATION
EXAMPLES (REMEMBER)
Alkali when dissolved in water
NaOH OH- + Na+ NaOH
water
Na+
Na+
Na+
OH-
OH-
OH-

17. WHAT IF WE TRY TO
DISSOLVE AMMONIA
GAS?
NH3 + H2O  NH4
+ + OH-
Do not forget OH-

18. AGAIN, WHAT IS A WEAK
ALKALI?
Weak Alkali when dissolved in water
NH3 + H2O NH4
+ + OH- NH3
water
OH-
OH-
NH4
+
NH4
+
NH3

19. NEUTRALIZATION
In neutralization, the H+ from the ACID and the OH- from the Alkali react to
form water
H+ + OH-  H2O
Energy
Energy is being released:
EXOTHERMIC

20. OXIDES
ACIDIC OXIDES- OXIDES THAT ARE ACIDIC
BASIC OXIDES- OXIDES THAT ARE BASIC
AMPHOTERIC OXIDES- OXIDES THAT ARE ACIDIC AND BASIC

21. EXAMPLES OF OXIDES
BASIC ACIDIC
Na2O
CaO
Fe2O3
CO2
SO2
P4O10
Amphoteric
Al2O3
ZnO
H2O
CO, NO
Neutral

22. INDICATORS
Substances that change COLORS in acidic and alkaline solutions
Litmus indicator
Red
Blue
Acids
Bases
Phenolphthalein
Colorless
Red/Pink
Acids
Base
These are used in
TITRATION

23. PH SCALE
pH is a number to show how acidic or alkaline a solution is
0 14
Super
acidic
31 6 7 13108
Very
acidic
Becoming
Less acidic
Very
Little
acidity
neutral
Very
Less
alkaline
Getting
Less basic
Super
basic
Very
basic

24. EXAMPLES OF
NEUTRAL SOLUTION
• Pure Water
• NaCl solution
• Most soluble salts
• Ethanol solution
(not ethanoic acid)

25. APPLICATION: PH IN SOIL
Soil
Most plants
grow well almost
neutral
Plants grow poorly in
very high
Or very low pH
Soil can become
too acidic
because:
• Excessive use
of chemical
fertilizers
• Acid rain from
air pollution by
sulfur dioxide
and nitrogen
oxides
How to fix an acidic soil?

26. SALTS
A salt is obtained from an acid when the H+ is replaced by metal ion
or ammonium ion
H Cl
Acid
Na
Salt

27. SOLUBILITY OF SALTS:
MEMORIZE THIS PLEASE
Type of salts Soluble Insoluble
Carbonates (NH4)2CO3
Na2CO3
K2CO3
All the rest
Chlorides All the rest PbCl2
AgCl
Nitrates All -
Sulfates All the rest BaSO4
PbSO4
(CaSO4 is slightly soluble)

28. PRACTICE
Soluble Insoluble
K2SO4
Na2CO3
KNO3
Pb(NO3)2
BaSO4
CuSO4
BaCO3
AgCl

29. HOW DO WE PREPARE
SALTS???

30. CASE 1: I WANT TO MAKE
AN INSOLUBLE SALT,
PBCL2 (SOLID)
Step 1: think where PbCl2 comes from:
Pb
Cl2
Pb2+
Cl-
An aqueous solution (soluble)
Pb(NO3)3
An aqueous solution (soluble)
NaCl
Step: 2 Precipitation reaction
Pb(NO3)2(aq) + NaCl(aq)  NaNO3(aq) + PbCl2(s)Soluble SolubleSoluble Insoluble

31. ILLUSTRATION
water
Pb(NO3)2
solution
NaCl
solution
Pb2+
NO3
-
Na+
Cl-
Na+
Na+
NO3
-
NO3
-
NO3
-
PbCl2 solid

32. GETTING THE SALT
HOW?
We have solid in a liquid
Na+
Na+
NO3
-
NO3
-
NO3
-
PbCl2 solid
FILTRATION

33. THIS IS HOW YOU GET
PBCL2

34. CASE 2: SOLUBLE
SALTS
• 1. acid + excess metal/insoluble metal oxide/carbonate
• 2. acid+ alkali

35. HOW TO PREPARE
SALTS
START
Is the salt
soluble?
NO
YES React acid with
metal/alkali/metal
oxide/metal carbonate
Product soluble?
YESNO
Mix acid with excess metal/ metal
oxide/metal carbonate

36. WORK THIS OUT:
I WANT TO MAKE
COPPER SULFATE

37. IONIC EQUATION FAIZ,
DO IT ON THE BOARD