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Types of complexometric titration
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Recommended: Types of complexometric titration
Complexometric titration is defined as a form of volumetric analysis in which the formation of a coloured complex is used to indicate the endpoint of the titration (1). Complexometric titrations rely on the formation of complexes between metal ions and compounds capable of donating electrons to form a stable, soluble complex (2). The complex is formed as a result of metal ions being titrated with a complexing agent or ligand. The principle of complexometric titrations is based on a simple ion being transformed into a complete ion and using a metal indicator to determine the endpoint (3), and the displacement of water from the solvation sphere of the metal ions by ligands (5). Different indicators are used in complexometric titrations as they have different pH ranges as well as detecting different metals in those ranges (1). Therefore complexometric titrations are useful in determining a mixture of different metals (1).
There are 4 types of complexometric titrations, namely direct titration, back titration, replacement titration and indirect titration (3). Direct titration is similar to an acid-base titration, whereby a standard chelon solution is added to the metal ion until the endpoint is detected (3). Although this method is the most convenient, it is limited by slow complexation reaction and interference due to the presence of other ions (3). In back titration an excess of standard EDTA solution is added to the metal solution to be analysed and the excess is back titrated to with a standard solution of a second metal ion (3). In replacement titration, the metal to be analysed displaces quantitatively from the complex (3). When the first 2 methods do not give a sharp endpoint, the metal may be determined by the displacement ...
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...rated against a known volume of EDTA
References
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Tandlich, R. (2014). Pharmaceutical Chemistry. Complexometric Titrations. Rhodes University. Grahamstown. South Africa. Slide 59-82
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For this solution, 5 mL of the solution with 2.5 mL of AMV was placed in the cuvette. The cuvette was placed inside of spectrophotometer and the amount of absorbance was recorded. This procedure that involves a solution with a known concentration was repeated for the concentrations:1.0x10-4 M,5.0x10-5 M,2.0x10-5M, and1.0x10-5M.A unknown solution absorbance was measured by putting 5 mL of unknown solution with 2.5 mL AMV in a cuvette. The cuvette was placed in the spectrophotometer and the amount of absorbance was recorded. The procedure that deals with the unknown solution was repeated 2 more times with the same solution and the same amount of solution and AMV.
Stability of a complex in solution is known to be the separation of two compound resulting in equilibrium state, theoretically it was observed that; there greater association, the higher the stability of the
Rang, H. P., Dale, M. M., Ritter, J. M., Flower, R. J., & Henderson, G. (2012). Pharmacology (7 ed.). London: Elsevier Inc.
Pharmaceutical journal: A weekly record of pharmacy and allied sciences. Third series, volume XXIV. Bloomsbury Square W.C.: 1894. 26 November 2011. http://books.google.com/books?
Ostrove, N. M. (2004). Statement of Nancy M. Ostrove, Ph.D., Deputy Director, Division of Drug.
Due to the nature of amino acids, a titration curve can be employed to identify
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Gusdinar T. COMPLEXOMETRIC TITRATION An application method of Inorganic Pharmaceutical Analysis [homepage on the internet] . No date. [cited 2014 Mar 20]. Available from: http://download.fa.itb.ac.id/filenya/Handout%20Kuliah/Inorganic%20Pharmaceutical%20Analysis%202008/English%20Version/05.%20COMPLEXOMETRIC%20TITRATION.pdf.
Titration is a technological process in which a solution, known as a titrant, is slowly and carefully added from a burrette into a fixed volume of another solution (known as the sample). In an acid-base titration an acid neutralizes a base or vice versa. This process is maintained untill the reaction between the titrant and the sample (acid and the base) is judged to be complete. The reaction is judged to be complete when the endpoint is reached. An endpoint in a titration analysis is referred to as the point at which no more titrant is added due to an observable colour change of an indicator. Indicators can be used to find an endpoint because they change colour when the pH of a solution changes and an endpoint in a titration is an empirical approximation of the equivalence point, which is the point of major pH change in the titration sample due to the fact that equal chemical amounts of reactants have been combined at that point. All indicators have a pH range, which is the range of pH values at which the colour of the indicator changes. Thus
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).