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Course: IAL Edexcel Linear (Chemistry)
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Curriculum

IAL Edexcel Linear (Chemistry)

Unit 1. Structure, Bonding and Introduction to Organic Chemistry

0/52 Dr Dabour Hub Science Diagram and Course Material

Unit 2. Energetics, Group Chemistry, Halogenoalkanes and Alcohols

0/68 Dr Dabour Hub Science Diagram and Course Material

Unit 3. Practical Skills in Chemistry I

0/13 Dr Dabour Hub Science Diagram and Course Material

Unit 4. Rates, Equilibria and Further Organic Chemistry

0/71 Dr Dabour Hub Science Diagram and Course Material

Unit 5. Transition Metals and Organic Nitrogen Chemistry

0/57 Dr Dabour Hub Science Diagram and Course Material

Unit 6. Practical Skills in Chemistry II

0/17 Dr Dabour Hub Science Diagram and Course Material
Quiz

4.4 Acid-base Equilibria – Check yourself

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Acid-base Equilibria IAL Modular Chemistry check yourself quiz: free practice for IAL Edexcel Modular (chemistry). Work through this Acid-base Equilibria IAL Modular Chemistry check yourself quiz and get instant feedback on every answer. If you get stuck, review the 4.4 Acid-base Equilibria — Notes — IAL Chemistry Notes lesson. More practice: IAL Edexcel Modular (chemistry) — all units. Syllabus: Pearson Edexcel International A Levels.

  • Questions count: 10
  • Passing grade: B+
  • Time limit: 10 minutes
Start Quiz
1.
In NH3 + H2O ⇒ NH4+ + OH-, water acts as:
A base
An acid
A buffer
An indicator
2.
pH of 0.010 mol dm-3 HCl is:
1.0
2.0
12.0
0.01
3.
What is the pH of pure water at 50 °C where Kw = 5.5 × 10-14?
7.00
7.26
6.63
14.0
4.
At half-equivalence in a weak acid/strong base titration:
pH = 7
pH = pKa
pH = 14 - pKa
[HA] = 0
5.
Which mixture forms a buffer?
HCl and NaCl
NaOH and NaCl
CH3COOH and CH3COONa
HNO3 and KNO3
6.
Acid A has pKa 3.2, acid B 4.8. Which is true?
B is stronger
Both equally strong
A has smaller Ka
A is stronger
7.
Which statement best describes Strong acid?
The point where half the weak acid has been neutralised; here pH = pKa.
A proton (H+) donor.
An acid that dissociates completely in aqueous solution.
The acid dissociation constant: Ka = [H+][A-]/[HA].
8.
Which statement best describes Kw?
The ionic product of water: Kw = [H+][OH-] = 1.00 × 10-14 mol2 dm-6 at 298 K.
Two species differing by one proton, e.g. CH3COOH / CH3COO-.
An acid that dissociates completely in aqueous solution.
A solution that minimises pH change when small amounts of acid or alkali are added.
9.
Which statement best describes Brønsted-Lowry base?
Two species differing by one proton, e.g. CH3COOH / CH3COO-.
A proton (H+) donor.
The acid dissociation constant: Ka = [H+][A-]/[HA].
A proton (H+) acceptor.
10.
Which statement best describes Brønsted-Lowry acid?
The ionic product of water: Kw = [H+][OH-] = 1.00 × 10-14 mol2 dm-6 at 298 K.
A solution that minimises pH change when small amounts of acid or alkali are added.
An acid that only partially dissociates in aqueous solution.
A proton (H+) donor.
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Part of Unit 4. Rates, Equilibria and Further Organic Chemistry — see every lesson and quiz in this unit.
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