Complexometric Titration

Complex titration is defined as the form of volumetric analysis in which the formation of colored complexes is used to indicate the endpoint of the titration (1). Complex titration depends on the formation of a complex (2) between a metal ion and a compound capable of providing electrons to form a stable soluble complex. The metal ion is titrated with a complexing agent or a ligand to form a complex. The principle of the complexometric method is to convert from simple ions to complete ions, use of a metal indicator to determine the end point (3), and to the ligand (5) of water from solvated spheres of metal ions It is based on replacement.

The complexometric method depends on the complex formed between the analyte and the titrant. Typically, they require special complexing indicators to form weak complexes with analytes. The most common example is the use of a starch indicator to increase the sensitivity of iodometric titration. The dark blue complex of starch containing iodine and iodide is more prominent than iodine alone. Other complexing indicators are chromium black T for titrating calcium and magnesium ions and chelating agent EDTA for titrating metal ions in solution.

Different types of titration: acid based titration - neutralization between acid and base Redox titration - redox type complex titration - used to find some ion devices used in this experiment; funnel Hydrochloric acid sodium hydroxide Boss Head / Clamp Stand Conical Flask Burette White Tile Goggle Cylinder Phenolphthalein Funnel Boss Head / Clamp Burette Bracket Sodium Hydroxide Phenolphthalein White Tile Cylinder Hydrochloric Acid

Metal ion indicators (organic dyes that turn color when combined with metal ions) indicate the end of the EDTA complexation titration. However, for metal ion indicators suitable for EDTA titration, it should not bind strongly to metal ions such as EDTA. Therefore, murexide is suitable. About 6 g of nickel (II) hydrated hydrate was transferred to a weighing bottle, the contents were weighed and about 25 cm 3 of deionized water was added to a 100 cmφ beaker and the nickel was transferred to water. The bottle was weighed without leaving the bottle salt at all, then the mixture was stirred until the solid dissolved, and the resulting solution was transferred to a 100 cmφ standard flask.

This experiment was carried out to measure water hardness by titration with EDTA using the complexometric titration method. In some cases it is important to determine the hardness of the water to find the optimum water hardness. This was done using the concept of complex titration with an effective chelator EDTA. Sample mineral water was analyzed using standard EDTA as an index with EBT and calcium ions present in the solution were calculated to determine the hardness of the water sample. At the end of the experiment, the results indicate that mineral sample water contains large amounts of calcium and magnesium ions - meaning of hard water sample