Describe how to prepare each solution from the dry solute and the solvent. a. 1.00×10² mL of 0.500 M KCl b. 1.00×10² g of 0.500 m KCl c. 1.00×10² g of 5.0% KCl solution by mass

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1. Step 1: For part (a), calculate the moles of KCl needed using the formula: \( \text{Moles of KCl} = \text{Molarity} \times \text{Volume in Liters} \). Convert 100 mL to liters by dividing by 1000.
2. Step 2: Convert the moles of KCl to grams using the molar mass of KCl. The molar mass of KCl is approximately 74.55 g/mol.
3. Step 3: Weigh the calculated mass of KCl using a balance.
4. Step 4: Dissolve the weighed KCl in a volume of water less than 100 mL, then transfer the solution to a 100 mL volumetric flask.
5. Step 5: Add more water to the volumetric flask until the bottom of the meniscus is at the 100 mL mark, ensuring the solution is well mixed.