What mass of KNO3 in grams would be required to prepare 0.6 liters of a 1.8 M KNO3 solution?

mass= molarity*volumesolution*formulamassKNO3

To determine the mass of KNO3 required to prepare a certain volume and concentration of solution, we can use the formula:

Mass (in grams) = Volume (in liters) × Concentration (in Molarity) × Molar mass of KNO3

First, let's calculate the molar mass of KNO3:
- The molar mass of K is approximately 39.10 g/mol.
- The molar mass of N is approximately 14.01 g/mol.
- The molar mass of O is approximately 16.00 g/mol (there are 3 oxygens in KNO3, so we multiply it by 3).

Molar mass of KNO3 = (39.10 g/mol) + (14.01 g/mol) + (16.00 g/mol × 3) = 101.10 g/mol

Now we can plug in the given values into the formula and calculate the mass of KNO3:
Mass = 0.6 L × 1.8 M × 101.10 g/mol

Mass = 0.6 × 1.8 × 101.10 g

Mass ≈ 109.01 grams

Therefore, approximately 109.01 grams of KNO3 would be required to prepare 0.6 liters of a 1.8 M KNO3 solution.