What mass of potassium sulfate is needed to prepare a 0.250 M potassium sulfate solution in a 500.0 mL volumetric flask? Express your answer to the correct number of significant figures.
Question
What mass of potassium sulfate is needed to prepare a 0.250 M potassium sulfate solution in a 500.0 mL volumetric flask? Express your answer to the correct number of significant figures.
Solution
To solve this problem, we need to use the formula for molarity which is:
Molarity (M) = moles of solute / liters of solution
We know the molarity (0.250 M) and the volume of the solution (500.0 mL or 0.500 L), and we need to find the mass of the potassium sulfate (K2SO4).
First, we need to find the number of moles of K2SO4. We can rearrange the molarity formula to find moles:
moles of solute = Molarity (M) * liters of solution moles of K2SO4 = 0.250 M * 0.500 L = 0.125 moles
Next, we need to convert moles of K2SO4 to grams. We do this by multiplying the number of moles by the molar mass of K2SO4. The molar mass of K2SO4 is approximately 174.26 g/mol.
mass of K2SO4 = moles of K2SO4 * molar mass of K2SO4 mass of K2SO4 = 0.125 moles * 174.26 g/mol = 21.78 g
So, you would need approximately 21.78 g of potassium sulfate to prepare a 0.250 M potassium sulfate solution in a 500.0 mL volumetric flask. This answer is rounded to the correct number of significant figures.
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