SPM Chemistry

5.4 Hydrogen Bonds

1 Exercise

5.4 Hydrogen Bonding

5.5 Dative Bonds

1 Exercise

5.5 Dative Bonds

5.6 Metallic Bonds

1 Exercise

5.6 Metallic Bonds

5.7 Ionic and Covalent Compounds

1 Lesson | 1 Exercise

5.7.1 Properties of Ionic and Covalent Compounds

5.7 Properties of Ionic Compounds and Covalent Compounds

06 Acids, Bases and Salts

6.1 The Role of Water in Acidic and Basic Properties

3 Lessons | 1 Exercise

6.1.2 Bases and Alkali

6.1.3 The Role of Water in Acidic and Basic Properties

6.1 The role of water in showing acidity and alkalinity

6.2 Meaning of pH and Determination of pH

1 Lesson | 1 Exercise

6.2.1 Meaning of pH and Determination of pH

6.3 Strength of Acids and Alkalis

1 Lesson | 1 Exercise

6.3.1 Strength of Acids and Alkalis

6.3 Acid and Alkali Strength

6.4 Chemical Properties of Acids and Alkalis

3 Lessons | 1 Exercise

6.4.1 Chemical Properties of Acids

6.4.2 Chemical Properties of Alkalis

6.4.3 Writing Ionic Equation of The Reaction of Acids and Alkalies

6.4 Chemical Properties of Acids and Alkalis

6.5 Concentration of Aqueous Solution

2 Lessons | 1 Exercise

6.5.1 Concentration of Aqueous Solution

6.5.2 Molarity and Number of Moles

6.5 Concentration of Aqueous Solutions

6.6 Standard Solution

2 Lessons | 1 Exercise

6.6.1 Standard Solution

6.6 Standard Solutions

6.7 Neutralisation

2 Lessons | 1 Exercise

6.7.1 Neutralisation

6.7.2 Acid-Base Titration

6.7 Neutralization

6.8 Salts, Crystals and Their Uses in Daily Life

1 Lesson | 1 Exercise

6.8.1 Introduction to Salts

6.8 Salt, Crystals and Uses in Daily Life

6.9 Preparation of Salts

4 Lessons | 1 Exercise

6.9.1 Solubility of Salts, Oxide and Hydroxide

6.9.2 Preparing Salts

6.9.3 Preparing Soluble Salts

6.9.4 Preparing Insoluble Salts

6.9 Preparation of Salts

6.10 Action of Heat on Salts

2 Lessons | 1 Exercise

6.10.1 Identifying Gases

6.10.2 Effect of Heat on Salts

6.10 Action of Heat on Salt

6.11 Qualitative Analysis

3 Lessons | 1 Exercise

6.11.1 Colour of Salts

6.11.2 Identifying Anions

6.11.3 Identifying Cations

6.11 Qualitative Analysis

07 Rate of Reaction

7.1 Determining The Rate of Reaction

2 Lessons | 1 Exercise

7.1.1 Determining the Rate of Reaction

7.1.2 Analysing Rate of Reaction from Graph

7.1 Determining the Rate of Reaction

7.2 Factors Affecting the Rate of Reaction

1 Lesson | 1 Exercise

7.2.1 Factors Affecting the Rate of Reaction

7.2 Factors Affecting Reaction Rates

7.3 Applications of Factors that Affect the Rate of Reaction

1 Lesson | 1 Exercise

7.3.1 Applications of Factors that Affect the Rate of Reaction

7.3 Applications of Factors Affecting Reaction Rates in Life

7.4 The Collision Theory

1 Lesson | 1 Exercise

7.4.1 The Collision Theory

7.4 Collision Theory

08 Manufactured Substances in Industry

8.1 Alloys and Their Importance

1 Lesson | 1 Exercise

8.1.1 Alloys and Their Importance

8.1 Alloys and Their Importance

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6.3 Acid and Alkali Strength

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SPM Chemistry 6.3 Strength of Acids and Alkalis 6.3 Acid and Alkali Strength

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Question 1 of 8

1. Question
1 point(s)
What is the main factor that determines whether an acid is categorized as a strong acid or a weak acid?
- The volume of water used to dissolve the acid.
- The ability of the acid to react with all types of metals.
- The color of an acid solution when tested with a universal indicator.
- The degree of ionization of the acid molecule in water.
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Question 2 of 8

2. Question
1 point(s)
Which of the following is the main characteristic of ethanoic acid (CH₃COOH) as a weak acid?
- It has a pH value between 1 and 2 at the same concentration as a strong acid.
- It produces a high concentration of H⁺ ions.
- Its ionization equation uses a double-headed arrow (⇌).
- It ionizes completely in water.
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Question 3 of 8

3. Question
1 point(s)
Why is sodium hydroxide (NaOH) considered a strong alkali?
- Because it can only dissolve a small amount of other chemicals.
- Because it ionizes completely in water to produce a high concentration of OH⁻ ions.
- Because it has a low pH value (around pH 8).
- Because it reacts slowly with acids.
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Question 4 of 8

4. Question
1 point(s)
Which of the following acids would exhibit the lowest pH value if they all had the same molarity?
- Carbonic acid (H₂CO₃)
- Ethanoic acid (CH₃COOH)
- Aqueous ammonia (NH₃)
- Hydrochloric acid (HCl)
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Question 5 of 8

5. Question
1 point(s)
Given two solutions, P and Q, with the same concentration. The bulb glows brightly in solution P, while the bulb glows dimly in solution Q. What conclusion can be drawn?
- Both solutions are organic substances.
- Solution P is a weak acid or alkali.
- Solution P contains a higher concentration of free ions than solution Q.
- Solution Q has a high degree of ionization.
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Question 6 of 8

6. Question
1 point(s)
When sulfuric acid (H₂SO₄) reacts with magnesium metal, gas is released more vigorously. Why is this the case compared to the reaction with ethanoic acid?
- Magnesium metal only reacts with mineral acids.
- Sulfuric acid is a non-ionizing substance.
- Sulfuric acid has a higher concentration of H⁺ ions.
- Ethanoic acid has a greater degree of ionization.
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Question 7 of 8

7. Question
1 point(s)
Which of the following substances will produce an ionization equation using a single arrow (→) in water?
- Ammonia (NH₃)
- Magnesium hydroxide (Mg(OH)₂)
- Carbonic acid (H₂CO₃)
- Potassium hydroxide (KOH)
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Question 8 of 8

8. Question
1 point(s)
What is meant by the degree of ionization?
- The pH value measured using a digital pH meter.
- The number of atoms in one molecule of an acid or alkali.
- The percentage or fraction of molecules that dissociate into ions in water.
- The total volume of gas produced in a chemical reaction.
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