Question

At 20°C, a 1.14 M aqueous solution of ammonium chloride has a density of 1.0168 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. At 20°C, a 1.14 M aqueous solution of ammonium chloride has a density of 1.0168 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. 6.00 m 1.19 m 1.14 m 0.892 m 0.0217 m

Answer 1

Answer:

The molality of ammonium chloride in the solution = 1.121 mol/kg

Explanation:

The Molality of a solution is defined as the number of moles of solute divided by the mass of the solvent in kg.

Molality = (Number of moles of solute)/(Mass of solvent in kg)

Using a basis of 1 L

Number of moles = (Concentration in mol/L) × (Volume in L)

Concentration in mol/L = 1.14 M

Volume in L = 1 L

Number of moles of solute = 1.14 × 1 = 1.14 moles

Mass of solvent = (Density of solution) × (Volume of solution)

Density of solution = 1.0168 g/mL = 1.0168 kg/L

Volume of solution = 1 L

Mass of solvent in kg = 1.0168 × 1 = 1.0168 kg

Molality = (Number of moles of solute)/(Mass of solvent in kg)

Molality = (1.14/1.0168) = 1.1211644375 mol/kg = 1.121 mol/kg

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