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1. Calculate the moles of anhydrous (dry) KAI(SO4)2 that were present in the sample. Show all work including units. B IU T₂ moles= mass of substance in (g) / molar mass of the substance (g/mol) molar mass of KAI(SO4)2 39g/mol+ 27g/mol+ 2*(32g/mol + (4*16 g/mol)) = 39+27+2*(32+64) = 258g/mol mass of dry sal = 1.1g moles of dry KAI(SO4)₂ = 1.1(g) / 258 (g/mol) = 0.0043 mol Question 2 2. Calculate the ratio of moles of H₂O to moles of anhydrous KAI(SO4)2. Show all work including units. 37 Word(s)
Question 2 2. Calculate the ratio of moles of H₂O to moles of anhydrous KAI(SO4)2. Show all work including units. Note: Report the ratio to the closest whole number. BIU T² BIU T₂ Question 3 3. Write the empirical formula for the hydrated KAI(SO4)2, based on your experimental results and answer to Question 2. Show all work including units. Hint: if the ratio of moles of H₂O to moles of anhydrous KAI(SO4)2 was 4, then the empirical formula would be: KAI(SO4)2 4H₂O. 0 Word(s) T² 0 Word(s) T₂
Question 4 4. Describe any visual differences between the hydrated sample and the dried, anhydrous form. E T² T₂ в / Question 5 U O Word(s) 5. How would the following errors affect the empirical formula for the compound? That is, will these errors cause the calculated number of moles of water in the hydrate to be artificially high or low? a. The student ran out of time and did not do the second heating. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will ht efinal answer be artificially high or low? b. The student recorded the mass of the cup + sample incorrectly and started with 2.20 g of hydrated compound but used 2.00 g in the calculations. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know? BIU EE T² T₂ O Word(s)