What mass of K2SO4 is required to make a 600.0 mL solution with a concentration of 0.50 M?

To determine the mass of K₂SO₄ required to create a 600.0 mL solution with a concentration of 0.50 M, we begin by using the relationship between molarity, volume, and number of moles.

Molarity (M) is defined as the number of moles of solute per liter of solution. The formula to calculate the number of moles from molarity and volume is:

[ \text{Moles of solute} = \text{Molarity} \times \text{Volume in liters} ]

First, we convert the volume from milliliters to liters:

600.0 mL = 0.600 L

Next, we can substitute the values into the formula:

[ \text{Moles of K₂SO₄} = 0.50 , \text{M} \times 0.600 , \text{L} = 0.30 , \text{moles} ]

Now, we need to find the mass of K₂SO₄ in grams. To do this, we use the molar mass of K₂SO₄. The molar mass can be calculated by adding