Question detail
During a titration, 25.0 mL of 0.100 M HCl is required to neutralise 30.0 mL of a 0.050 M NaOH solution. Which balanced equation correctly represents the reaction stoichiometry?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Amount of substance
Question
- A. HCl + NaOH → NaCl + H₂O
- B. 2HCl + NaOH → NaCl + H₂O
- C. HCl + 2NaOH → NaCl + H₂O
- D. HCl + NaOH → NaCl + 2H₂O
Answer
HCl + NaOH → NaCl + H₂O
Explanation
The correct option is HCl + NaOH → NaCl + H₂O. HCl + NaOH → NaCl + H₂O is the best answer because it directly supports the AQA A-Level Chemistry objective to link acid-base stoichiometry to balanced equations. This reasoning is anchored to Titration calculations in Amount of substance, and it separates acid-base from similar A-Level ideas rather than relying on a vague recall statement. Other options are weaker if they use the wrong evidence, calculation, mechanism, observation, unit, or conclusion for this subtopic.
Common mistake
Common Mistake in Titration Calculations
Students often forget to use the correct mole ratio from the balanced equation when calculating unknown concentrations in titration problems.
To fix this, first write the balanced equation for the acid-base reaction. Identify the mole ratio of the reactants involved. Then, use the formula: concentration (mol/dm³) = moles/volume (dm³). Substitute the known values, calculate the moles using the mole ratio, and finally determine the unknown concentration with the correct units.
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