Question

What is the molarity of a 2.351 m ammonium nitrate solution? (d = 1.104 g/mL)

Answer 1

1)Assume you have 1 kg of solvent (water)

2) 2.351 m means 2.351 moles /kg solvent (water). or

mass in grams = moles * molar mass ammonium nitrate = 2.351 moles * 80.052 = 188.20 g/ Kg of solvent

3). Calculate the total grams of the solution.

1000 grams solvent (water) + 188.20 grams ammonium nitrate = 1188.20 grams solution

4) Calculate the volume (Liters) of solution.d = 1.104 g/ml

d= m/V

Volme of solution = mass of solution /density= 1188.20 /1.104 = 1076.27 ml = 1.076 L

5). Calculate the molarity.

2.351moles solute / 1.076 L = 2.18M (answer)