Learn about the preparation and standardization of 0.05 m magnesium sulphate solution through a laboratory experiment or practical.
Aim:
To prepare and standardize 0.05 m magnesium sulphate solution using standard 0.1M EDTA (volumetric solution).
Requirements:
Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, and wash bottle, etc.
Chemicals: Magnesium sulfate (MgSO4), disodium edetate (EDTA), ammonia-ammonium chloride solution, and mordant back II, etc.
Preparation of 0.05 M magnesium sulphate solution:
Take properly weighed 12.50 gm of magnesium sulfate and add in 500 ml of distilled water, Once it has completely dissolved, make up the volume to 1000 ml with water.
Titration procedure:
- All glassware should be cleaned and dried according to standard laboratory procedures.
- Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
- Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
- Remove air bubbles from the burette and adjust the reading to zero.
- Take 30.00 ml of a prepared 0.05 m magnesium sulphate solution and pour it into a conical flask.
- Then add 20.00 ml of distilled water and 10.00 ml of ammonia-ammonium chloride solution and shake well.
- Add 50 mg mordant back II as an indicator.
- Titrate it with 0.1 M disodium edetate solution with constant stirring until the endpoint.
- The actual endpoint is indicated by the appearance of a violet color to blue.
- To get accurate results, repeat the titration three times.
- Properly record the readings of the burette.
- Take their mean and calculate the molarity of the magnesium sulphate solution.
Observation table:
Sr. No. | Content in conical flask | Burette reading | Volume of titrant used (ml) | |
Initial | Final | |||
1 | | | | |
2 | | | | |
3 | | | | |
| Mean: | |||
Calculations:
1 ml of 0.1 M EDTA is equivalent to 0.02465 g of magnesium sulphate.
M = Molarity of EDTA x reading of the burette / 25
Result:
The strength of the prepared magnesium sulphate solution was found to be_____M.
Frequently Asked Questions (FAQ):
What is the molecular mass of MgSO4?
Magnesium sulphate, often known as magnesium sulphate, is a salt with the formula MgSO4 with a molecular weight of 120.366 g/mol.
Which indicator is used in the assay of magnesium sulphate?
Titration with 0.1 M MgSO4 solution is performed in the presence of an eriochrome black T solution as an indicator.
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