Experiments show that the solubility of alum in 25 mL of 1.4 M KOH plus 10 mL of

Question

Experiments show that the solubility of alum in 25 mL of 1.4 M KOH plus 10 mL of 9 M H_2 SO_4 is about 1.0 g at 1.0 degree C and 1.7 g at 6.0 degree C. Using your measured solution temperature, estimate the amount of alum left in your chilled solution. Alum left in solution: _________g Does the amount of alum left in solution account for most of the difference between the maximum grams of alum and your experimental grams of alum? Explain. Given the following unbalanced molecular equation: KAI (SO_4)_2 middot 12 H_2 O (aq) + BaCl2(s) rightarrow KCl(aq) + AICl_3 (aq) + BaSO_4(s) (a) Balance the reaction and calculate the amount of barium chloride needed to react with a 25 mL of a 0.10 M alum solution. (b) What is the percent yield of barium sulfate if 1.02 grams is isolated? A 10.0g sample to of alum is heated to drive off all of the water from the solid. Determine the mass of the dehydrated alum. Write the net ionic equation for formation of aluminum hydroxide in this experiment and explain the source of hydroxide.

Explanation / Answer

Dear Friend i am writing net ionic equation for the formation of aluminium hydroxide, but i need data before post-lab questions to answer the source of hydroxide. You have not provided that, but one way to get it is hydrolysis of AlCl3

AlCl3 (aq) + 3H2O (aq) --> Al(OH)3 (s) + 3HCl (aq)

Net ionic equation:      Al3+ (aq) + OH- (aq) --> Al(OH)3 (s)

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