Synopsis:
This experiment conducted used the Gravimetric Analysis method to determine the concentration of an unknown sulfate solution. The unknown sulfate solution was pipetted into a smaller beaker, acidified, heated, decanted through filtration, dried, cooled and weighed. What was found at the end of the result was Barium Sulfate precipitate which weighed 0.1783 grams. The concentration of the unknown sulfate solution was found to be 2.9385 g/L and its molarity was 0.0306M.
Objective:
To determine the amount of sulfate in an unknown concentrated solution by the Gravimetric Analysis method.
Theory:
Ba + SO42-→ BaSO4 (Precipitate)
Gravimetric analysis is a technique through which the amount of an analyte (sulfate being analysed) can be determined through the measurement of mass. The principle behind gravimetric
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Empty contents into crucible while the vacuum pump is working Further wash the precipitate with warm deionised water at vacuum pump for an additional 2 more times Discard the filtrate Dry crucible with Barium Sulfate precipitate in the oven at 150°C for 30 minutes. Cool crucible in a desiccator for 10 minutes. Weigh crucible once it has cooled down Weight the crucible and calculate the weight difference from before and now. The calculated weight difference is the weight of the Barium Sulfate precipitate.
Results and Calculations
Discussion
During the procedures, it is best to note the necessary precautions: Do not extract amount of solution from the source directly. Instead, extract a portion of it into a beaker and then take the precise solution out to prevent any contaminations in the source. Before using any of your equipment, it is best to condition them first to prevent any contamination that could affect the concentration of the 10% Barium Chloride and unknown concentration of sulfate solution
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11.) Subtract the mass of the evaporating dish from the mass of the evaporating dish and it's contents. Multiply that number by 10 to get the solubilty in grams per 100 cm3 of water.
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The formula for Epsom salts is MgSO4•7H2O. If 1.250 g of the compound is dissolved is water, calculate the number of milliliters of 0.200 M Ba(NO3)2 that would be required to precipitate all of the sulfate ions as barium sulfate. Make the same determination for 1.000 g of alum.
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The Effect of Salt Solution Concentration On The Mass Of Potatoes Introduction = == == == ==
borate) and 1.0 g. of sodium hydroxide in 20 mL of warm water. It may