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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.

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Presentation on theme: "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."— Presentation transcript:

1 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.

2 pH and Oxides

3 Overview of today’s lesson 1. pH 2. pH Scale 3. 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 Very acidic Very alkalineNeutral Shows whether a solution is acidic, neutral or alkaline. pH < 7 pH = 7 pH > 7

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

7 Just for fun Sulfuric acid is strong, but… Fluoroantimonic acid (HSbHF 5 ) is 2×10 19 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 = log 10 [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 = 2pH = 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

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 IndicatorColour in acidic solution pH range at which indicator changes colour Colour in alkaline solution methyl orangered3 – 5yellow screened methyl orange violet3 – 5green litmusred5 – 8blue bromothymol blueyellow6 – 8blue phenolphthaleincolourless8 – 10pink

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 o more reliable and accurate o portable o 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.this. Orchids?

27 Oxides What are oxides? Oxides are compounds of oxygen and another element only. Are these oxides? CO 2, CO, HNO 3, H 2 O, CuSO 4, 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 Most dissolve in water – forms acids in water. For example, sulfur dioxide. sulfur dioxide + water → sulfurous acid SO 2(g) + H 2 O (l) → H 2 SO 3(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 CO 2(g) + H 2 O (l) → H 2 CO 3(aq) phosphorus pentoxide + water → phosphoric acid P 4 O 10(s) + 6 H 2 O (l) → 4 H 3 PO 4(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 SO 2(g) + 2NaOH (aq) → Na 2 SO 3(aq) + H 2 O (l) sulfur trioxide + sodium hydroxide → ?? carbon dioxide + calcium hydroxide → ?? (familiar?)

33 Some examples of Acidic Oxides Acidic OxideFormulaPhysical state Acid produced in water NameFormula carbon dioxideCO 2 Gascarbonic acidH 2 CO 3 sulfur trioxideSO 3 Gassulfuric acidH 2 SO 4 phosphorus(V) oxideP 4 O 10 Solidphosphoric acidH 3 PO 4 silicon dioxideSiO 2 Solid-- 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 SiO 2(s) + 2NaOH (aq) → Na 2 SiO 3(aq) + H 2 O (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!) SO 2(g) + H 2 O (l) → H 2 SO 3(aq) Sulfurous acid can be oxidized to sulfuric acid (H 2 SO 4 ) by oxygen. 4NO 2(g) + 2H 2 O (l) + O 2(g) → 4HNO 3(aq) Normally, unpolluted rain is slightly acidic (around 6) due to carbonic acid because of carbon dioxide. CO 2(g) + H 2 O (l) → H 2 CO 3(aq)

36 Effects of acid rain Look at this 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 (Na 2 O) and potassium oxide (K 2 O).

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) + H 2 O (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) + 2HNO 3 (aq)  Ca(NO 3 ) 2 (aq) + H 2 O(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 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 Fe 2 O 3 ·nH 2 O, Fe(OH) 3, Fe 3 O 4 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 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

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

46 Aluminium oxide and lead(II) oxide

47 Neutral Oxides Mostly non-metallic oxides. Do not show any acidic or basic properties. They are mostly insoluble in water. Examples: H 2 O, 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 Acid Does the oxide dissolve? Unknown oxide Yes No Basic or amphoteric oxide Acidic or neutral oxide 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

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?

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