Acid–base titration lab

Learning objectives

• describe the meanings of the terms acid and alkali in terms of the ions they produce in aqueous solution and their effects on Universal Indicator
• describe neutrality and relative acidity and alkalinity, in terms of — colour in Universal Indicator, and
• describe neutrality and relative acidity and alkalinity, in terms of — the pH scale (calculation of pH from hydrogen ion concentration is not required)
• describe the reaction between hydrogen ions and hydroxide ions to produce water, H+ + OH– → H2O, as neutralisation
• name appropriate apparatus for the measurement of time, temperature, mass and volume; including burettes, pipettes, measuring cylinders and gas syringes
• use techniques, apparatus and materials;
• make and record observations, measurements and estimates;
• apply the concept of solution concentration (in mol/dm3 or g/dm3) to process the results of volumetric experiments (e.g. titration) and to solve simple problems. (appropriate guidance will be provided where unfamiliar reactions such as redox are involved. Calculations on % yield and % purity are not required.)
• apply the concept of solution concentration (in mol/dm3 or g/dm3) to process the results of volumetric experiments (e.g. titration) and to solve simple problems (appropriate guidance will be provided where unfamiliar reactions are involved)
• explain qualitatively the differences in behaviour between strong and weak acids and bases in terms of the extent of dissociation
• explain the choice of suitable indicators for acid-base titrations, given appropriate data, in terms of the strengths of the acids and bases
• — explain how buffer solutions control pH
• Ka, Kb, Kw, pKa, pKb
• Titration Curves and Indicators
• Buffer Solutions