1. Overview Prerequisite knowledge:
Students are able to define acids and bases in terms of the ions they produce in aqueous solution.
Students are able to describe the reactions of acids with metals, carbonates and bases.
Students are able to describe the reaction between hydrogen ions and hydroxide ions to form water as neutralization.
Students are able to differentiate between concentration and strength of acids and bases.
Specific Instructional Objectives (SIOs):
By the end of the lesson, students should be able to:
Describe what pH means and explain how the pH scale is used.
Describe the effects of acids and alkalis on Universal Indicator.
Describe how to test hydrogen ion concentration and relative acidity using Universal Indicator.

2. pH and Oxides

3. Overview of today’s lessonpH
pH Scale
Indicators
Universal Indicator
Other indicators
pH probe

4. Acids and Bases
How do you measure the strength or concentration of acids or bases?
pH Scale.

5. pH Scale Shows whether a solution is acidic, neutral or alkaline.
Very acidic
Neutral
Very alkaline
Shows whether a solution is acidic, neutral or alkaline.
pH < 7
pH = 7
pH > 7

6. Guess the pH of the following!5 3 13
3.4 8
Black Coffee
Orange Juice
Bleach
Coca Cola
Sea water

7. Just for fun Sulfuric acid is strong, but…
Fluoroantimonic acid (HSbHF5) is 2×1019 times stronger than sulfuric acid!

8. What exactly does pH mean?
pH is a measure of the concentration of H+ and OH- ions present in a solution.
pH = log10[H+]

9. High and low pH High concentration of hydrogen ions – low pH
High concentration of hydroxide ions – high pH
Hydrogen ion
Hydroxide ion

10. pH scale
One unit of change in pH represents a change of concentration of H+ ions or OH- by ten times!

11. Quickcheck! Hydrogen ion Hydroxide ion
Match the solutions to the correct pH values.
pH = 7
pH = 2
pH = 11

12. Determination of pH How do we determine the pH of a solution?
One way is by using an indicator.
A pH indicator is a chemical compound that changes colour in solutions of different pH.
Why is it called an indicator?

13. Universal Indicator
The Universal Indicator is one of the most useful indicators.
It gives different colours in solutions of different pH.

14. Universal Indicator
Demonstration

15. pH and strength of acids/alkalis
pH can be used to compare the strength of acids or alkalis of the same concentration.
For instance, from the demonstration, you can tell HCl is a stronger acid than ethanoic acid by the pH value.

16. Other kinds of indicators
Colour in acidic solution
pH range at which indicator changes colour
Colour in alkaline solution
methyl orange
red
3 – 5
yellow
screened methyl orange
violet
green
litmus
5 – 8
blue
bromothymol blue
6 – 8
phenolphthalein
colourless
8 – 10
pink

17. What exactly are indicators?
They themselves are weak acids or bases.
Indicators normally have two or more forms at different pH.
The colour of the different forms result in the colour of the solutions turning into different colours.
Why must indicator be added in small amounts?

18. What happened?
Indicators used in demonstration at the start of lesson are:
Phenolphthalein
Methyl Orange
In the second demonstration, when C (HCl with methyl orange, hence it is red) is mixed with B (excess NaOH), HCl is neutralized and since there is excess NaOH, the solution turns yellow in the presence of methyl orange.
What about the first demonstration?

19. Phenolphthalein in the news
Po Chai Pills incident
Phenolphthalein is possibly carcinogenic!
Po Chai Pills in capsule form
Po Chai Pills in pill form

20. Dove commercial

21. pH meter
In the laboratory, we usually use a pH probe attached to a data logger, or a pH meter.
Inserting the probe into the solution will give you the pH accurately.
Need to be calibrated.
Advantages
more reliable and accurate
portable
can be used in data logging to record changes in pH

22. By now you should know… What pH represents. How the pH scale is used.
What indicators are.
The effects of acids and alkalis on the Universal Indicator.

23. Just for fun
Jonathan got stung by a bee while walking towards the canteen at HCI. You are given two substances – Colgate and Vinegar. Which will you apply on Jonathan?

24. Homework The pH of our blood is about 7.4.
Find out what happens to our body system if the pH of blood drops too low, or rises too high.

25. pH and Soil Best pH for most plants is about 6 to 7.
Too much fertiliser can make the soil too acidic.
Why is it that Singapore soil is mostly acidic?

26. Control of Soil pH
If soil is too acidic, we can add quicklime (calcium oxide) or slaked lime (calcium hydroxide).
Different from lime juice!
If the soil is too basic, we can add ammonium phosphate or iron sulfate.
Take a look at this.
Orchids?

27. Oxides
What are oxides?
Oxides are compounds of oxygen and another element only.
Are these oxides?
CO2, CO, HNO3, H2O, CuSO4, CaO, NaOH.

28. Oxides
4 kinds of oxides.
Acidic, Basic, Neutral and Amphoteric.

29. Acidic Oxides
Acidic oxides are usually formed from oxides of non-metals.

30. Acidic Oxides sulfur dioxide + water → sulfurous acid
Most dissolve in water – forms acids in water.
For example, sulfur dioxide.
sulfur dioxide + water → sulfurous acid
SO2(g) + H2O(l) → H2SO3(aq)
(note: not sulfuric acid)
What do you think gives you sulfuric acid when dissolved in water?

31. Acidic Oxides carbon dioxide + water → carbonic acid
CO2(g) + H2O(l) → H2CO3(aq)
phosphorus pentoxide + water → phosphoric acid
P4O10(s)+ 6 H2O(l) → 4 H3PO4(aq)

32. Acidic Oxides Do NOT react with acids.
React with alkalis to form salt and water.
sulfur dioxide + sodium hydroxide → sodium sulfate (IV) or sodium sulfite + water
SO2(g) + 2NaOH(aq) → Na2SO3(aq) + H2O(l)
sulfur trioxide + sodium hydroxide →??
carbon dioxide + calcium hydroxide →?? (familiar?)

33. Some examples of Acidic Oxides
Formula
Physical state
Acid produced in water
Name
carbon dioxide
CO2
Gas
carbonic acid
H2CO3
sulfur trioxide
SO3
sulfuric acid
H2SO4
phosphorus(V) oxide
P4O10
Solid
phosphoric acid
H3PO4
silicon dioxide
SiO2 -
What kind of bonding exists here?
What is the structure of silicon dioxide?

34. Silicon dioxide
Some acidic oxides do not dissolve in water.
For example silicon(IV) oxide is a solid at room temperature and does not dissolve in water
It reacts with NaOH to form sodium silicate (a salt) and water.
silicon (IV) oxide + sodium hydroxide → sodium silicate + water
SiO2(s) + 2NaOH(aq) → Na2SiO3(aq) + H2O(l)

35. Acid Rain
Formed when acidic air pollutants (which are mostly acidic oxides) such as sulfur dioxide and nitrogen dioxide. Can go lower than 4! (As acidic as coke!)
SO2(g) + H2O(l) → H2SO3(aq)
Sulfurous acid can be oxidized to sulfuric acid (H2SO4) by oxygen.
4NO2(g) + 2H2O(l) + O2(g) → 4HNO3(aq)
Normally, unpolluted rain is slightly acidic (around 6) due to carbonic acid because of carbon dioxide.
CO2(g) + H2O(l) → H2CO3(aq)

36. Effects of acid rain Look at this video.
Acid rain reacts with metals and carbonates in marble and limestone, thus destroying buildings, monuments and bridges.
Kills fish and other aquatic life by lowering pH of water bodies to below 4.
Leaches important nutrients from soil and destroy plants.
Find out how these acidic pollutants are formed!

37. Uses of sulfur dioxide
Sulfur dioxide acts as a bleaching agent by removing oxygen from them.
It is a reducing agent.
When added to coloured wood pulp for making peper, sulfur dioxide is added to the wood pulp to remove oxygen from the dye, thus bleaching the pulp to white.

38. Uses of sulfur dioxide Sulfur dioxide is used as a food preservative.
It is poisonous to all organisms, especially bacteria.
Added in small amounts to prevent mould and bacteria growing.
Why must the addition of sulfur dioxide be strictly controlled in the food industry?

39. Basic Oxides Basic oxides are oxides of metals. Many are insoluble.
For those that can dissolve in water, they are called alkalis.
E.g. Sodium oxide (Na2O) and potassium oxide (K2O).

40. Basic Oxides Example – calcium oxide.
When CaO is added to water, calcium hydroxide is formed, which is sparingly soluble in water.
The reaction is as follows:
calcium oxide + water → calcium hydroxide
CaO(s) + H2O(l) → Ca(OH)2(aq)
Watch video.

41. Basic Oxides
Basic oxides react with acids to form salt and water only. (Are they bases?)
Example:
calcium oxide + nitric acid  calcium nitrate + water
CaO(s) + 2HNO3(aq)  Ca(NO3)2(aq) + H2O(l)
What reaction is this?

42. Flue Gas Desulfurization
Removing sulfur dioxide from waste gases when burning fossil fuels.
These waste gases are called flue gases and the process of removing sulfur dioxide from these gases is called desulfurization.
Watch this video.
Another way of desulfurization uses basic oxides like calcium oxide, or carbonates like calcium carbonate. Read about this in your textbook.

43. Rust
Rust is a complex mixture consisting of Fe2O3·nH2O, Fe(OH)3, Fe3O4 etc, formed in the presence of moisture and oxygen, and accelerated by the presence of electrolytes.
These are basic oxides/hydroxides.
How would you suggest removing rust?
Group activity: Imagine I have an iron nail. I want to store it in water for ten years without it rusting. What way can you suggest? Note: I am looking out for the cheapest and most efficient way.

44. Amphoteric Oxides Can behave as either acidic or basic oxide.
Example, zinc oxide, aluminium oxide and lead(II) oxide.
Metallic oxides that react with both acids and bases to form salts and water.
Tin and beryllium

45. Zinc Oxide It behaves as both a basic oxide and an acidic oxide.
hydrochloric acid + zinc oxide → zinc chloride + water
(acid basic oxide → salt water)
2HCl(aq) ZnO (s) → ZnCl2 (aq) H2O(l))
zinc oxide sodium hydroxide → sodium zincate + water
(acidic oxide + base → salt water)
ZnO (s) NaOH(aq) → Na2ZnO2(aq) H2O(l))
It behaves as both a basic oxide and an acidic oxide.

46. Aluminium oxide and lead(II) oxide
Sodium aluminate (NaAlO2) sodium plumbate(II) (Na2PbO2)

47. Neutral Oxides Mostly non-metallic oxides.
Do not show any acidic or basic properties.
They are mostly insoluble in water.
Examples: H2O, CO, NO.
What is dihydrogen monoxide?

48. Dihydrogen Monoxide hoax

49. Corresponding Hydroxides
NOTE: Corresponding hydroxides of the metal oxides will have the same characteristics as their oxides!
For example, sodium hydroxide will be basic (same as sodium oxide), zinc hydroxide will be amphoteric (same as zinc oxide) etc.

50. Classification of unknown oxide
Imagine you are a scientist working in ASTAR. You are now given a sample containing an oxide. How do you determine if it is basic, acidic, amphoteric or neutral?
Come up with a method to classify an unknown oxide, preferably using a flow chart.
Hint: Some reagents you can use are hydrochloric acid and sodium hydroxide.

51. Classification of unknown Oxide
Alkali
Is the oxide soluble in water?
Soluble
Amphoteric
oxide
Yes
Litmus test No
Yes
Acid
Soluble in alkali?
Insoluble
Basic or amphoteric oxide
Basic oxide
Soluble
Alkali
Does the oxide dissolve?
Acidic oxide
Unknown oxide No
Soluble in alkali?
Insoluble
Neutral oxide
Acidic or neutral oxide

52. Quickcheck!
When dilute hydrochloric acid was added to unknown oxide Z, it dissolved. When sodium hydroxide was added to Z, it did not dissolve. What kind of oxide is Z? Can you give an example of what Z can be?
When dilute hydrochloric acid was added to unknown oxide M, it did not dissolve. When sodium hydroxide was added to M, it did not dissolve as well. What kind of oxide is M?