volumetric analysis. volumetric analysis involves the analysis of a solution of unknown...
TRANSCRIPT
Volumetric Analysis
• Volumetric analysis involves the analysis of a solution of unknown concentration with a standard solution.
• A pipette is used to transfer a known quantity of one of the solutions into a conical flask. This sample is called an aliquot
• The other solution is added to the burette. The amount of this solution that is needed to react with the aliquot is called the titre.
Volumetric Analysis (cont.)
• The point where the reactants are in exact mole ratio proportion is called the equivalence point.
• The point where we detect the change through an indicator or pH meter is called the end point.
• Titrations are repeated until three titrations are concordant, i.e. within 0.1ml of each other
Standard Solutions – Primary Standard
• A standard solution is a solution of precisely known concentration. For a solution to be used as a primary standard it must– be readily obtainable in a pure form– have a known formula– be easy to store without deteriorating or reacting
with the atmosphere– have a high molar mass to minimise the effect of
errors in weighing– be inexpensive.
Standard Solutions – Secondary standards
• If a primary standard solution can not be made a secondary standard solution is created by titrating it with a primary standard to find the exact concentration.
• Substances such as strong acids and strong bases are not suitable for primary standards as the concentrations prepared are not accurate and they can react with the atmosphere or containers
• Examples of recommended substances used to make secondary standards can be found in the table on the next slide
Back Titrations
• If an end point cannot be easily detected in a titration or the substance is toxic, volatile, a mixture of gases, in low concentration or insoluble in water a back titration is needed.
• A back titration involves first reacting the sample with an excess amount of a standard solution and titrating the product or excess with another suitable standard solution.
• Flow charts of back titrations can be found on the following slides
Acid-Base Titrations
• When completing an acid-base titration it is important to select an appropriate indicator to determine the end point.
• The pH of the equivalence point varies depending on the reactants that are used.
• The following slides show the pH curves of different acid and base reactions.
Choosing an appropriate indicator
• When selecting an indicator it is necessary to find one that changes colour in the range that has the sharp change in pH.
Redox Reactions
• Redox reactions occur when reactant loses reactions (oxidation) and another reactant gains electrons (reduction).
• These reactions occur spontaneously in solution and usually result in a change in colour, which can be used to find the end point.
Oxidation Number Rules Revision
• All free elements have an oxidation number of 0• Ionic compounds containing two ions have oxidation numbers
equal to their ions (related to their group number)• Oxygen is 2- except in peroxides (H2O2, BaO2) where it is 1-
• Hydrogen is 1+ except in metal hydrides (NaH, CaH2) where it is 1-
• The sum of oxidation numbers in a neutral compound is 0• The sum of oxidation numbers in a polyatomic ion is equal to
the charge on the ion.• The most electronegative element has the negative oxidation
number