1. Zinc iodide is dissolved in 2.5 L of water to make a solution. 1 L of this solution is then diluted to make 12.0 L of a 0.5 M solution. What mass of zinc was added to make the original solution?
2. Explain the steps you would follow to make 500 mL of a 0.3 M solution of sucrose (C12H22O11) in the lab.
Please, I'm so confused. If you could be as detailed and helpful as possible, that would be amazing. I'm so lost...
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Explanation:
12.0 L x 0.5 M = 6.0 moles zinc iodide in 1 L so 2.5 x 6.0 = 15 moles zinc iodide in
original solution. 55.38 g/mol Zn / 319.22 g/mol ZnI2 = 0.173485. Moles zinc =
0.173485 x 15 = 2.60. zinc mass = moles x std at wt = 2.60 mol x 55.38 g/mol
= 143.988 = 144 g.. That's mass of zinc; if it's mass of zinc iodide you require then
it's 144 x (319.22 / 55.38) = 830.040 = 830 g.
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