An aqueous KNO3 solution is made using 83.8 g of KNO3diluted to a total solution volume of 2.08 L. (Assume a density of 1.05 g/mL for the solution.)
Part A
Calculate the molarity of the solution.
Express the molarity to three significant figures.
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Part B
Calculate the molality of the solution.
Express the molality to three significant figures.
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Part C
Calculate the mass percent of the solution.
Express the mass percent to three significant figures.
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Part A
Molar mass of KNO3 = 101.1032 g/mol
Mass of KNO3 dissolved in solution= 83.8g
No. of moles of KNO3 dissolved in solution = (83.8g)/ (101.1032 g/mol)
=0.8289 moles
[ using no. of moles= given mass/ molar mass]
Volume of KNO3 solution=2.08 litres
Molarity of solution= No. of moles of solute/ volume of solution in litres
Molarity of KNO3 solution= No. of moles of KNO3 / volume of solution in litres
Molarity of KNO3 solution= 0.8289 moles/2.08 litres
=0.398 moles/litre
= 0.398 M
Part B
Molality of solution= No. of moles of solute/ mass of solvent in kg
Density of solution=1.05g/ml
Volume of solution=2.08 L=2080 ml [using 1 litre= 1000 ml]
Mass of solution= 2080 ml x 1.05g/ml [ using mass = volume x density]
= 2,184 g
Mass of KNO3= 83.8 g
Therefore mass of solvent = 2184 g- 83.8 g
= 2100.2 g
= 2.1002 kg
No. of moles of KNO3= 0.8289 moles
Molality of KNO3 solution= No. of moles of KNO3/ mass of solvent in kg
=0.8289 moles/2.1002 kg
= 0.395 moles/kg
=0.395 m
Part C
Mass percent of solution = (Mass of solute/ mass of solution ) x100
Mass of KNO3= 83.8 g
Mass of solution=2,184 g
Therefore, Mass percent of solution = (83.8 g/2,184 g)x 100 %
=3.93%
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