Compound From Aluminum Metal
Preparation of an Ionic Compound from
Aluminum Metal
October 6, 2010
The purpose of this laboratory project was threefold, in that it presented three main objectives. The first objective was to prepare the ionic compound alum from aluminum powder. The alum was produced from the reduction-oxidation reaction of aluminum with potassium hydroxide and sulfuric acid in water. The second objective was to then analyze the alum product for water crystallization; that is, to determine the value of x in the following formula:
KAl(SO4)2(aq) xH20 After the formula of the product had been deduced, it was then possible to complete the third and final objective of the project, which was to calculate the theoretical yield, the actual yield, and then …show more content…
Bunsen burners heated two crucibles supported on clay triangles to red heat for no more than five minutes. After allowing the crucibles to cool, they were placed in a desiccator to cool to room temperature. The crucibles were weighed to 0.1 mg once they had reached room temperature. About .5 g of the air dried product was cautiously weighed into each crucible. The crucibles were once again placed on clay triangles and heated gently. After the product began to solidify, the Bunsen burners were adjusted so that maximum heat was provided to the crucibles for about five minutes. The crucibles were set aside to cool, and then placed in a desiccator to fully cool to room temperature. Once room temperature was reached, the crucibles were weighed to 0.1 mg. The mass of water of crystallization in the sample is represented by the loss in mass of the …show more content…
The actual yield was previously calculated from first weighing an empty crystallization dish, then weighing the air dried crystals with the dish one week later. The sum was subtracted by the weight of the crystallization dish to produce the mass of the crystals, or actual yield of the reaction: 4.91 g KAl(SO4)212H2O. To find the percent yield, the actual yield was divided by the theoretical yield, 17.55 g, and then multiplied by 100%. The discrepancy between the theoretical yield and the actual yield obtained, as seen by the percent yield, could have been caused due to the Bunsen burner not consistently heating the 2nd crucible containing the
Aluminum Metal
October 6, 2010
The purpose of this laboratory project was threefold, in that it presented three main objectives. The first objective was to prepare the ionic compound alum from aluminum powder. The alum was produced from the reduction-oxidation reaction of aluminum with potassium hydroxide and sulfuric acid in water. The second objective was to then analyze the alum product for water crystallization; that is, to determine the value of x in the following formula:
KAl(SO4)2(aq) xH20 After the formula of the product had been deduced, it was then possible to complete the third and final objective of the project, which was to calculate the theoretical yield, the actual yield, and then …show more content…
Bunsen burners heated two crucibles supported on clay triangles to red heat for no more than five minutes. After allowing the crucibles to cool, they were placed in a desiccator to cool to room temperature. The crucibles were weighed to 0.1 mg once they had reached room temperature. About .5 g of the air dried product was cautiously weighed into each crucible. The crucibles were once again placed on clay triangles and heated gently. After the product began to solidify, the Bunsen burners were adjusted so that maximum heat was provided to the crucibles for about five minutes. The crucibles were set aside to cool, and then placed in a desiccator to fully cool to room temperature. Once room temperature was reached, the crucibles were weighed to 0.1 mg. The mass of water of crystallization in the sample is represented by the loss in mass of the …show more content…
The actual yield was previously calculated from first weighing an empty crystallization dish, then weighing the air dried crystals with the dish one week later. The sum was subtracted by the weight of the crystallization dish to produce the mass of the crystals, or actual yield of the reaction: 4.91 g KAl(SO4)212H2O. To find the percent yield, the actual yield was divided by the theoretical yield, 17.55 g, and then multiplied by 100%. The discrepancy between the theoretical yield and the actual yield obtained, as seen by the percent yield, could have been caused due to the Bunsen burner not consistently heating the 2nd crucible containing the