Question detail
In a titration, 30.0 cm³ of a 0.2 mol/dm³ solution of sulfuric acid (H₂SO₄) is neutralized by a sodium hydroxide (NaOH) solution. Calculate the volume of NaOH solution required to neutralize the acid if the concentration of NaOH is 0.1 mol/dm³.
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
Type
exam_style
Style
Topic
Using concentrations of solutions in mol/dm3 (chemistry only) (HT only)
Question
In a titration, 30.0 cm³ of a 0.2 mol/dm³ solution of sulfuric acid (H₂SO₄) is neutralized by a sodium hydroxide (NaOH) solution. Calculate the volume of NaOH solution required to neutralize the acid if the concentration of NaOH is 0.1 mol/dm³.
Answer
60.0 cm³
Explanation
This question assesses the understanding of titration calculations and the stoichiometry involved in neutralization reactions. It requires the application of the relationship between moles, concentration, and volume to find the required volume of NaOH.
Common mistake
Misunderstanding Titration Calculations
Students often confuse the volumes of acid and alkali used in titrations, leading to incorrect concentration calculations.
Always ensure to use the correct volume for each solution in the titration and double-check the balanced equation to find the correct mole ratio.
Related flashcards
Flashcard 1 of 5
Related practice questions
Question 1 of 5
Choose an answer, get feedback, then move sideways through the set.