All materials directly linked to this Web page, accompanying photos and videos are in the public domain and may be copied without restriction. Barium chloride solution is added in excess to precipitate barium sulfate, and the precipitate is digested in the hot solution. The precipitate is filtered through a paper filter which is then ignited and completely ashed. From the weight of the sample and weight of the precipitate, the percentage of sulfate in the sample is calculated.
Get Full Essay Get access to this section to get all help you need with your essay and educational issues. The amount of sulphate is determined quantitatively as barium sulphate, BaSO4, The gravimetric determination of sulphate gravimetric analysis.
For the experiment, a dilute solution of barium chloride was slowly added to a hot unknown sulphate solution slightly acidified with concentrated HCl. The precipitate is then filtered off by suction filtration, washed with water and dried in the oven at degree Celsius for about half an hour and cooled in the desiccator, and weighed as barium sulphate and the percentage of sulphate was calculated from the weight of barium sulphate.
The weight of barium sulphate was calculated to be 0.
There were also no hiccups during the experiment. Students can also be familiar to the ways to carry out Gravimetric Analysis through this experiment. Commonly, gravimetric analysis is being carried out by the following steps: Precipitation and filtration are the most commonly used methods to isolate the desired substances from a solution.
The reagents used in the reactions will form an insoluble compound with the desired constituents but not precipitate of other elements.
Firstly, exactly 25mL of given sulphate solution was used so that it would be a fair experiment in relation to how much sulphate will be obtained at the end of the experiment with regards to the amount of sulphate solution used. Secondly, concentrated HCL was added to water in the fume hood.
This is because water should not be added to concentrated acid as the heat of the solution will cause water to boil and the acid to splatter. Also, the process is done in the fume hood as concentrated HCL gives out vapour that is toxic and it should not be inhaled.
Thirdly, the beaker was covered with a watch glass while heat and the use of the watch glass is to let condensation occur to prevent the lost of solution through evaporation. After that, a few drops of barium chloride was added to see if everything has mixed together.
Next, the filtration of barium sulphate precipitate is done by the use of suction filtration. For this process, the use of a filter flask is that it can withstand pressure without imploding, and also helps speed up the process of filtration.
Also, the filter paper has to cover the entire base of the crucible so that now solvent will actually leak through when the suction starts up, resulting in the loss of solvent and also in severe cases, causing the flask to break due to pressure inside it.
Also, the use of a rubber policeman is to help dislodge any particles on the beaker into the crucible and the use of the rubber policeman instead of just a glass rod is that the surface area that the rubber policeman can cover is more and thus speeding up the dislodging of particles. For the drying and weighing of barium sulphate, the crucible with the barium sulphate precipitate was dried in the oven to let the remaining moisture be evaporated so that only the dried sample is left behind.
Cooling the precipitate in the desiccator is to prevent the capture of moisture in the outside air as the desiccator controls the level of humidity in it while the precipitate cools down. For the weighing of the crucible, it is done in a closed balance, so that it can measure a very accurate weight of the collected sulphate.
The solution was heated till boiling and vigorously stirred. The beaker was covered with a watch glass and digested for 20 minutes. A few drops of barium chloride was add to the clear supernatant liquid to test for complete precipitation. The clear supernatant solution was decanted by filtration into the pre-weighed crucible with filter paper.
The contents were emptied into the crucible while the vacuum pump was still at work.
The precipitate was further washed with warm deionised water at the vacuum pump two more times. The filtrate was discarded. The crucible was cooled in the desiccator for about 10 minutes. The crucible was weighed when it has cooled down. The weight of the barium sulphated was calculated.
Weight of crucible with precipitate Weight of crucible with a piece of filter paper Gravimetric Sulfate Determination by Ulrich de la Camp and Oliver Seely DISCUSSION.
A sample containing an alkali sulfate is dried, weighed and dissolved in dilute HCl. Barium chloride solution is added in excess to precipitate barium sulfate, and the precipitate is digested in the hot solution. The precipitate is filtered through a paper.
1 GRAVIMETRIC DETERMINATION OF SULFATE IN AN UNKNOWN SOLUTION AIM The main objective of this experiment is to determine the concentration of sulfate ion in an. The amount of sulphate is determined quantitatively as barium sulphate, BaSO4, by gravimetric analysis.
For the experiment, a dilute solution of barium chloride was slowly added to a hot unknown sulphate solution slightly acidified with concentrated HCl. The objective of this experiment is to determine the amount of sulphate by gravimetric analysis.
The amount of sulphate is determined quantitatively as barium sulphate, BaSO4, by gravimetric analysis. For the experiment, a dilute solution of barium chloride was slowly added to a hot unknown sulphate.
Feb 23, · attheheels.com The sulfate content of ammonia fertiliser can be determined gravimetrically by converting the sulfate in a weighed sample of fertiliser to barium sulfate. The precipitate obtained was weighed and a value of g was obtained, computations showed that the percent yield of Sulfate in the unknown was at % Sulfate.
Introduction: Gravimetric analysis is a method of quantitative determination of an analyte by based on the mass of a solid.5/5(7).