Gravimetric Determination Of Sulphate In Fertiliser Lab Report
Gravimetric determination of sulphate in fertiliser
Question:
The proportion of sulphate present in a brand of commercial fertiliser under a range of temperatures.
Fertilisers provide plants with a number of sources necessary for them to grow, as follows, nitrogen, phosphorus, potassium and finally the one I will be concentrating on Sulfur. To cater for the varying plants, you wouldn’t require all these elements to the same extent as the necessities for each plant differ. The composition of different fertilisers is therefore of interest to farmers and other consumers who wish to ensure that the fertilisers they purchase represent good value and are suitable for particular applications, however for my case, I was asked by my grandfather whether …show more content…
The sulfate is precipitated as barium sulfate from a solution containing a known mass of fertiliser by adding from a solution containing a known mass of the fertiliser by adding an excess of barium chloride solution:
The proportion of sulfate ions and therefore of sulfate in the fertiliser is determined by collecting and weighing the precipitate that is formed during the above reaction at different temperatures specified bellow.
Independent variable:
In my experiment the IV will be the temperature of fertiliser prior to testing, I will be going in intervals of 10 starting at room temperature (24o) and ending at 74o, furthermore, I will accomplish by using a Bunsen burner to safely heat my fertiliser taking all precautions to avoid any harmful fumes to be released.
Dependent variable:
I will add Barium solution to my Sulfate solution which will give me Barium Sulfate solid, I will measure this solid by weighing it using a scale.
Control variable:
Factors I will keep constant are as follows the type of fertiliser, mass of fertiliser used, volume of water used and finally same equipment for …show more content…
Supplement 50 ml of distilled water and stir the liquefying liquid to increase in dissolve time and to get as much of the commercial fertiliser to disband.
4. Filter the mixture into a 600ml beaker, washing the residue several times using distilled water.
5. Add about 3 mL of 2 M hydrochloric acid to the filtrate and add more water so that the total volume is about 200ml. Boil the solution.
6.
7. Slowly add 15 mL of 0.5 M barium chloride solution drop by drop from a burette to the hot solution. A white precipitate of barium sulfate will form. Stir continuously throughout this process.
8. Boil the mixture for a further minute. Remove it form the heat and allow the precipitate to settle. Ensure that no sulfate ions remain in the solution by adding several drops of barium chloride solution. If more precipitate forms, add a further 3 mL of barium chloride solution and test again for unreacted sulfate ions.
9. Weigh a crucible fitted with filter paper.
10. Collect the precipitate in the crucible using gentle vacuum filtration. Use about 10 mL of warm distilled water to wash any precipitate remaining in the beaker into the
Question:
The proportion of sulphate present in a brand of commercial fertiliser under a range of temperatures.
Fertilisers provide plants with a number of sources necessary for them to grow, as follows, nitrogen, phosphorus, potassium and finally the one I will be concentrating on Sulfur. To cater for the varying plants, you wouldn’t require all these elements to the same extent as the necessities for each plant differ. The composition of different fertilisers is therefore of interest to farmers and other consumers who wish to ensure that the fertilisers they purchase represent good value and are suitable for particular applications, however for my case, I was asked by my grandfather whether …show more content…
The sulfate is precipitated as barium sulfate from a solution containing a known mass of fertiliser by adding from a solution containing a known mass of the fertiliser by adding an excess of barium chloride solution:
The proportion of sulfate ions and therefore of sulfate in the fertiliser is determined by collecting and weighing the precipitate that is formed during the above reaction at different temperatures specified bellow.
Independent variable:
In my experiment the IV will be the temperature of fertiliser prior to testing, I will be going in intervals of 10 starting at room temperature (24o) and ending at 74o, furthermore, I will accomplish by using a Bunsen burner to safely heat my fertiliser taking all precautions to avoid any harmful fumes to be released.
Dependent variable:
I will add Barium solution to my Sulfate solution which will give me Barium Sulfate solid, I will measure this solid by weighing it using a scale.
Control variable:
Factors I will keep constant are as follows the type of fertiliser, mass of fertiliser used, volume of water used and finally same equipment for …show more content…
Supplement 50 ml of distilled water and stir the liquefying liquid to increase in dissolve time and to get as much of the commercial fertiliser to disband.
4. Filter the mixture into a 600ml beaker, washing the residue several times using distilled water.
5. Add about 3 mL of 2 M hydrochloric acid to the filtrate and add more water so that the total volume is about 200ml. Boil the solution.
6.
7. Slowly add 15 mL of 0.5 M barium chloride solution drop by drop from a burette to the hot solution. A white precipitate of barium sulfate will form. Stir continuously throughout this process.
8. Boil the mixture for a further minute. Remove it form the heat and allow the precipitate to settle. Ensure that no sulfate ions remain in the solution by adding several drops of barium chloride solution. If more precipitate forms, add a further 3 mL of barium chloride solution and test again for unreacted sulfate ions.
9. Weigh a crucible fitted with filter paper.
10. Collect the precipitate in the crucible using gentle vacuum filtration. Use about 10 mL of warm distilled water to wash any precipitate remaining in the beaker into the