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Answer :
Final answer:
The proper procedure is to weigh out 42.8 grams of KIO₃ and add 2.00 liters of H₂O (option D)
Explanation:
The proper procedure to prepare 2.00 liters of 0.100-molar KIO₃ involves weighing out 42.8 grams of KIO₃ and adding 2.00 liters of H₂O.
This is because the molarity of a solution is defined as the number of moles of solute divided by the volume of the solution in liters. To calculate the number of moles of KIO₃ needed, you can use the formula:
- moles of solute = molarity x volume of solution
- moles of KIO₃ = 0.100 mol/L x 2.00 L = 0.200 mol
Next, you need to calculate the mass of KIO₃ using its molecular weight:
- mass of KIO₃ = moles of KIO₃ x molecular weight of KIO₃
- mass of KIO₃ = 0.200 mol x 214 g/mol = 42.8 grams
Therefore, you should weigh out 42.8 grams of KIO₃ and add 2.00 liters of H₂O to prepare the desired solution.
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