- Page 1Introduction - ReviewReview: Introduction to titrations
- Page 2Procedure - ReviewReview: Introduction to titration procedure
- 8 marksPage 3QuestionQuestion: Completing sentences describing what a titration is and how a titration is carried out
- Page 4Measurement - ReviewReview: Highlight how precisely the burette must be read and introducing the concept of significant figures
- 1 marksPage 5QuestionsQuestions: Practice reading a burette and identifyin the number of significant figures
- 8 marksPage 6Significant figures
- Page 7Planning - ReviewReview: Two pages highlighting the importance of problem planning and how to go about this for stoichiometry problems
- Page 8More about planning stoichiometry problems - Review
- 16 marksPage 9ProblemCalculate the concentration of NaOH in a solution if 25.00 mL of the solution reacts completely with 28.92 mL 0.1000 mol L–1 HCl according to the equation given.
NaOH(aq) + HCl(aq) → NaCl(aq) + H2O
- 16 marksPage 10ProblemTitration of 25.00 mL of 0.0494 mol L–1 Na2CO3 with hydrochloric acid requires 21.22 mL to reach the endpoint. The reaction occurring in the flask during the titration is shown below. Calculate the concentration of the hydrochloric acid.
Na2CO3(aq) + 2HCl(aq) → 2NaCl(aq) + H2O + CO2(g)
- 19 marksPage 11Problem25.00 cm3 of commercial vinegar, which is an aqueous solution of acetic acid (ethanoic acid, CH3CO2H),is transferred by pipette to a volumetric flask and diluted to exactly 250.0 cm3.
25.00 cm3 of the diluted vinegar is titrated completely by 19.46 mL of 0.1220 mol L–1 NaOH. What is the mol L–1 concentration of the commercial vinegar?NaOH + CH3CO2H → CH3CO2Na + H2O