Final answer:
To determine the mass of KBr solute required to make 416.6 ml of a 0.152 m solution, convert the volume to liters, use the molarity to find moles, and then convert moles to grams using the molar mass of KBr.
Step-by-step explanation:
The question 'What mass of solute is required to produce 416.6 ml of a 0.152 m solution of KBr?' requires the application of molarity concepts in chemistry. To find the mass of the solute KBr needed, we use the formula:
Mass of solute (g) = Molarity (M) × Volume of solution (L) × Molar mass of solute (g/mol)
First, convert the volume from mL to L:
416.6 mL = 0.4166 L
Then, identify the molarity as 0.152 M and the molar mass of KBr (potassium bromide) as 119 g/mol. With these values, we calculate the moles of KBr:
Moles of KBr = 0.152 M × 0.4166 L
Finally, we convert moles to mass using the molar mass of KBr:
Mass of KBr = Moles of KBr × Molar mass of KBr
Through this process, we can determine the mass of solute required for the solution.