how many grams of kno3 should be used to prepare
2.00 l of a 0.500m solution
101g
To determine the number of grams of KNO3 needed to prepare a 0.500 M solution in 2.00 L, you need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
Rearranging the formula, we have:
moles of solute = Molarity (M) x volume of solution in liters
First, calculate the moles of solute needed:
moles of solute = 0.500 M x 2.00 L = 1.00 moles
Now, we need to convert moles of solute to grams using the molar mass of KNO3:
Molar mass of KNO3 = atomic mass of K (39.10 g/mol) + atomic mass of N (14.01 g/mol) + 3 x atomic mass of O (16.00 g/mol) = 39.10 g/mol + 14.01 g/mol + 3 x 16.00 g/mol = 101.11 g/mol
Finally, we can calculate the grams of KNO3 needed:
grams of KNO3 = moles of solute x molar mass of KNO3 = 1.00 moles x 101.11 g/mol = 101.11 grams
Therefore, you will need 101.11 grams of KNO3 to prepare a 2.00 L solution with a concentration of 0.500 M.