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Estimation of Magnesium Sulfate by Complexometric Titration

Introduction:

  • In pharmaceutical analysis, the estimation of magnesium sulfate (MgSO₄) is done using complexometric titration with EDTA as the titrant.

  • This method relies on the formation of a stable complex between EDTA and magnesium ions (Mg²⁺).

Apparatus and reagents:

  1. Burette

  2. Erlenmeyer flask

  3. pH meter or pH indicator

  4. Magnesium sulfate solution (sample)

  5. Standard EDTA solution

  6. Buffer solution (pH ~10)

  7. Eriochrome Black T indicator (optional)

Procedure:

1) Preparation of Sample:

  • Weigh a sample of magnesium sulfate, dissolve it in distilled water, and transfer it to an Erlenmeyer flask.

2) Preparation of the Titrant (EDTA):

  • Use a standard EDTA solution (typically 0.01 M).

3) Buffering the Solution:

  • Add a buffer solution to the sample to maintain a pH of ~10.

4) Indicator (Eriochrome Black T):

  • If using Eriochrome Black T, add a few drops. The solution will turn pink due to the presence of magnesium ions.

5) Titration:

  • Titrate the magnesium sulfate solution with the EDTA solution from the burette.

  • As EDTA complexes with Mg²⁺, the solution's color (pink if using Eriochrome Black T) will remain until all magnesium ions are bound.

6) Endpoint Detection:

  • The endpoint is reached when the color changes, typically from pink to blue (if using Eriochrome Black T), or there is a noticeable color change.

7) Record Volume:

  • Note the volume of EDTA required to reach the endpoint.

Calculations of Magnesium Sulfate:

  • Amount of MgSO₄ (in grams):

  • Amount (in grams) of MgSO4 = (Volume of EDTA × Molarity of EDTA × Molar mass of MgSO4) / 2

% MgSO₄: % MgSO4 = (Volume of EDTA × Molarity of EDTA × Molecular weight of MgSO4 × 100) / (Volume of sample × Weight of sample)

  • The factor of 2 accounts for the reaction stoichiometry, as each Mg²⁺ ion reacts with one mole of EDTA.


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