overview prerequisite knowledge: 1. students are able to define acids and bases in terms of the ions...
TRANSCRIPT
Overview
Prerequisite knowledge:1. Students are able to define acids and bases in terms of the ions they
produce in aqueous solution.2. Students are able to describe the reactions of acids with metals,
carbonates and bases.3. Students are able to describe the reaction between hydrogen ions and
hydroxide ions to form water as neutralization.4. Students are able to differentiate between concentration and strength of
acids and bases.
Specific Instructional Objectives (SIOs):1. By the end of the lesson, students should be able to:2. Describe what pH means and explain how the pH scale is used. 3. Describe the effects of acids and alkalis on Universal Indicator.4. Describe how to test hydrogen ion concentration and relative acidity
using Universal Indicator.
pH and Oxides
Overview of today’s lesson
1. pH2. pH Scale3. Indicators
Universal Indicator Other indicators pH probe
Acids and Bases
How do you measure the strength or concentration of acids or bases?
pH Scale.
pH Scale
Very acidic Very alkaline
Neutral
Shows whether a solution is acidic, neutral or alkaline.
pH < 7pH = 7pH > 7
Guess the pH of the following!
Black CoffeeOrange JuiceBleachCoca ColaSea water
53
133.48
What exactly does pH mean?
pH is a measure of the concentration of H+
and OH- ions present in a solution.pH = log10[H+]
High and low pH
High concentration of hydrogen ions – low pHHigh concentration of hydroxide ions – high
pH
Hydrogen ion
Hydroxide ion
pH scale
One unit of change in pH represents a change of concentration of H+ ions or OH- by ten times!
Quickcheck!
Hydrogen ion
Hydroxide ion
Match the solutions to the correct pH values.
pH = 7 pH = 2 pH = 11
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?
Universal Indicator
The Universal Indicator is one of the most useful indicators.
It gives different colours in solutions of different pH.
Universal Indicator
Demonstration
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.
Other kinds of indicators
Indicator 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 3 – 5 green
litmus red 5 – 8 blue
bromothymol blue
yellow 6 – 8 blue
phenolphthalein colourless 8 – 10 pink
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?
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?
Phenolphthalein in the news
Po Chai Pills incidentPhenolphthalein is possibly carcinogenic!
Po Chai Pills in capsule form
Po Chai Pills in pill form
Dove commercial
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.Advantageso more reliable and accurateo portableo can be used in data logging to record
changes in pH
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.
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?
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.
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?
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?
http://www.uvm.edu/pss/ppp/pubs/oh34.htm
Oxides
What are oxides?Oxides are compounds of oxygen and another
element only. Are these oxides?CO2, CO, HNO3, H2O, CuSO4, CaO, NaOH.
Oxides
4 kinds of oxides.Acidic, Basic, Neutral and Amphoteric.
Acidic Oxides
Acidic oxides are usually formed from oxides of non-metals.
Acidic Oxides
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?
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)
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 + waterSO2(g) + 2NaOH(aq) → Na2SO3(aq) + H2O(l)
sulfur trioxide + sodium hydroxide →??carbon dioxide + calcium hydroxide →??
(familiar?)
Some examples of Acidic Oxides
Acidic Oxide Formula
Physical state
Acid produced in water
Name Formula
carbon dioxide CO2 Gas carbonic acid H2CO3
sulfur trioxide SO3 Gas sulfuric acid H2SO4
phosphorus(V) oxide P4O10 Solid phosphoric acid
H3PO4
silicon dioxide SiO2 Solid - -
What kind of bonding exists here?What is the structure of silicon dioxide?
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)
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)
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!
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.
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?
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).
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 hydroxideCaO(s) + H2O(l) → Ca(OH)2(aq)
Watch video.
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?
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.
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.
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.
Amphoteric Oxides
Zinc 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) + 2NaOH(aq) → Na2ZnO2(aq) + H2O(l))
It behaves as both a basic oxide and an acidic oxide.
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?
Dihydrogen Monoxide hoax
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.
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.
Classification of unknown Oxide
Acid
Does the oxide dissolve?
Unknown oxide
Yes
No
Basic or amphoteric oxide
Acidic or neutral oxide
Alkali
Alkali
Soluble in alkali?
Soluble
Insoluble
Amphoteric oxide
Basic oxide
Soluble in alkali?
Soluble
Insoluble
Acidic oxide
Neutral oxide
Is the oxide soluble in water?Yes
Litmus test
No
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?