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In a titration experiment, 25.0 cm³ of hydrochloric acid (HCl) is neutralized by 30.0 cm³ of sodium hydroxide (NaOH). Calculate the concentration of the hydrochloric acid solution if the concentration of sodium hydroxide is 0.1 mol/dm³.
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
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Topic
Acids and bases (A-level only)
Question
In a titration experiment, 25.0 cm³ of hydrochloric acid (HCl) is neutralized by 30.0 cm³ of sodium hydroxide (NaOH). Calculate the concentration of the hydrochloric acid solution if the concentration of sodium hydroxide is 0.1 mol/dm³.
Answer
The concentration of the hydrochloric acid solution is 0.12 mol/dm³. This answer is anchored to pH curves, titrations and indicators (A-level only).
Explanation
The concentration of the hydrochloric acid solution is 0.12 mol/dm³. is the best answer because it directly supports the AQA A-Level Chemistry objective to perform calculations using acid-base titration data. This reasoning is anchored to pH curves, titrations and indicators (A-level only) in Acids and bases (A-level only), and it separates titration 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
Misunderstanding Titration Calculations
Students often confuse the volumes of titrant and analyte when performing calculations using acid-base titration data.
To fix this, students should carefully identify which volume corresponds to the titrant (the solution of known concentration) and which corresponds to the analyte (the solution of unknown concentration) before performing any calculations.
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