Estimation of Magnesium sulphate by Complexometric titration
Magnesium sulfate (MgSO4) can be estimated by complexometric titration using a chelating agent such as ethylenediaminetetraacetic acid (EDTA) as a titrant. The reaction between EDTA and magnesium ions forms a stable, water-soluble chelate complex, which serves as the basis for the titration.
The following steps are involved in the estimation of magnesium sulfate by complexometric titration:
- Preparation of the sample: A known quantity of the magnesium sulfate sample is dissolved in distilled water.
- Addition of the indicator: A few drops of the indicator, such as Eriochrome Black T, are added to the sample solution. The indicator forms a complex with magnesium ions, which changes color when all the magnesium ions have reacted with the EDTA.
- Titration: The EDTA solution is slowly added to the sample solution until the endpoint is reached. The endpoint is determined by observing the color change of the indicator from blue to red or pink. At the endpoint, all the magnesium ions in the sample have reacted with the EDTA.
- Calculation of results: The amount of EDTA solution added to the sample solution is used to calculate the amount of magnesium sulfate present in the sample, using the stoichiometry of the reaction.
It is important to standardize the EDTA solution against a standard solution of magnesium sulfate before use to ensure accurate results. Additionally, care should be taken to ensure that the sample solution is free from any interfering substances that may affect the accuracy of the titration.
Overall, complexometric titration using EDTA is a reliable and accurate method for the estimation of magnesium sulfate and is widely used in various industries, including pharmaceuticals and agriculture.
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