Using these equations. What would my theoretical yield be of aluminum potassium
ID: 538202 • Letter: U
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Using these equations. What would my theoretical yield be of aluminum potassium sulfate dodecohydrate If I put 1.00g aluminum foil in? tassium sulfate dodecahydrate, including as stop the bleeding of a minor cht), sizing agent in the papermaking industry, an e in many grocery ith alum prevents ink that is applied to the paper from spreading out or bleeding aluminum ions. These aluminum ions attract the hydroxide (OH-) part of the water molecin g an acidic medium. This acid will break down the paper over time. Papers used for archivin alum as a sizing agent and are labeled as "acid-free." a na stores. Alum is commonly used in the papermaking process to m prevents ink that is applied to the paper from spreading out or bleeding. Alum also t to fill in the ced in industry by chemical synthesis. A synthesis reaction occurs when two or more su bs mplex new substance. In industry, the goal is to optimize chemical processes to give the hi of resources (cost). ry synthesis of alum, aluminum foil is the source of aluminum, potassium hydroxide is th the sulfate source. The process has two main steps-dissolving aluminum metal and the alum. Aluminum is dissolved into solution so the ions are more inum to form AI(OH),complex ions and hydrogen gas (see Equation 1) readily available to react. P --> 2Al(s) + 2OH-(aq) + .) 2Al(s) + 20Haq) + 6H20(1)-2A1(OH),-(aq) + 3H2(g) he complex ion [AI(OH)breaks down. Sulfuric acid is a strong acid and a good source een dissolved, the basic mixture will be acidified with sulfuric acid, H2SO Initially, a itate out of solution as a white solid. See Equation 2. Al(OH),Taq) + H2SO4(aq) Al(OH)3(s) + HS04-(aq) + H2O(l) Al(OH),(S) will dissolve in solution however as excess acid is added. See Equation3 Al(OH)3(s) + 3Hor(aq) A13+(aq) + 6H20(1) heated to dissolve any remaining solid and the solution is then cooled to allow crystals this synthesis is shown in Equation 4 Al3+(aq) + K+(aq) + 2SO42(aq) + 12H2O(1) KAI(SO4)212H20(s rview nt, a quantitative synthesis react reated working with aluminum foil, potassium hydroxide, sulfuric acid, water, and usi zation, and filtering. The percent yield of alum will be determined. CEM-FAX". . makes science teaching easier.Explanation / Answer
From the given reaction it is clear that one mole Al3+ produce one-mole aluminum potassium sulfate dodecahydrate.
atomic mass of Al is 27 g/mole
1 g Al contains 1/27 =0.037 moles and this will yield 0.037 moles aluminum potassium sulfate dodecahydrate.
molar mass of aluminum potassium sulfate dodecahydrate is 474.3884 g/mole
thus expected theoretical yield = 474.3884 x 0.037 = 17.55 g
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