QCAA Chemistry Revision Quiz
Test your knowledge on QCAA Chemistry concepts including acids, bases, pH, equilibrium, and indicators.
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Quiz Questions & Answers
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Question 1: Which statement best describes a weak acid according to the provided material?
It has a low concentration of acid particles.
It undergoes complete dissociation into ions in water.
It has a very large Ka value (Ka >> 1).
It is only partially ionised, with mostly unionised acid molecules.
Question 2: Which of the following substances is identified as a weak base in the provided material?
Ammonia
Potassium hydroxide
Barium hydroxide
Sodium hydroxide
Question 3: What does a large equilibrium constant (Kc > 1) for a reaction indicate?
The rate of the forward reaction is slower than the reverse reaction.
The system is not in equilibrium.
The equilibrium position is to the left, favouring reactants.
The equilibrium position is to the right, favouring products.
Question 4: According to the Brønsted-Lowry model, what is a conjugate acid?
A substance that donates a hydrogen ion.
A substance that remains after donating a hydrogen ion.
A substance that accepts a hydrogen ion.
A substance that has accepted a hydrogen ion.
Question 5: What is the primary function of a buffer solution?
To increase the electrical conductivity of a solution.
To shift the equilibrium position entirely to the product side.
To completely neutralize any added acid or base.
To resist changes in pH when small amounts of acid or base are added.
Question 6: If the pH of a solution is 2.8, what is the hydrogen ion concentration [H+]?
10^-2.8 M
-log(2.8) M
2.8 x 10^-14 M
14 - 2.8 M
Question 7: What is the relationship between Ka and the strength of an acid?
Strong acids have very large Ka values (Ka >> 1).
Ka is inversely proportional to the acid's strength.
Weak acids have very large Ka values (Ka >> 1).
Strong acids have very small Ka values (Ka << 1).
Question 8: An acid-base indicator changes color when its pH is approximately equal to what value?
Its pKb value.
Its pKa value.
The pH of a neutral solution (7.0).
The equivalence point of the titration.