Taking into account the definition of molarity and molar mass, 330.425 grams of (NH₄)₂SO₄ are needed to make 500.0 mL of 5.0 M solution.
Molar concentration or molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.
The molarity of a solution is calculated by:
molarity= number of moles÷ volume
Molarity is expressed in units moles/L.
The molar mass of substance is a property defined as the amount of mass that a substance contains in one mole.
In this case, you know:
Replacing in the definition of molarity:
5 M= number of moles÷ 0.5 L
Solving:
5 M × 0.5 L= number of moles
2.5 moles= number of moles
Now, you know that the molar mass of (NH₄)₂SO₄ is 132.17 g/mol. So, you can apply the following rule of three: If by definition of molar mass 1 mole of the compound contains 132.17 g grams, 2.5 moles of the compound contains how much mass?
mass= (2.5 moles×132.17 grams)÷1 mole
mass= 330.425 grams
Finally, 330.425 grams of (NH₄)₂SO₄ are needed to make 500.0 mL of 5.0 M solution.
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