A) Calculate the theoretical yield (in g) of alum from 1.00g of aluminumB) 1.00g of aluminum metal is dissolved in 40mL of KOH solutionhow many grams of aluminum would be present in a 10mL sample of this solution
Question A: According to the Wikipedia, the specific compound is the hydrated potassium aluminium sulfate (potassium alum) with the formula KAl(SO4)2·12H2OTo find the theoretical yield (in g) of alumwe need to find the percent composition by mass of aluminum in alum using its chemical formula% Al [(Al)(100%)] / [KAl(SO4)2·12H2O] % Al [(26.9815)(100%)] / [462.29078] % Al 5.836478% To calculate the mass of alum that could be made from 1.00 g of aluminum, we can use a simple proportion: (1.00 g ) : (5.836478 % ) (X) : (100%) X 17.13362 g or 17.1 g rounded to three significant figures Answer: The theoretical yield of alum that can be made from 1.00 g of aluminum is about 17.1 gramsQuestion B: Since 10 mL is one quarter of 40 mL, then the amount of aluminum dissolved in 10 mL of the solution will be one quarter of the amount dissolved in 40 mL of the solutionAnswer: If 1.00 g of aluminum is dissolved in 40 mL of KOH solution, then 0.25 g of aluminum would be present in a 10 mL sample of this solution.
