A sucrose solution is prepared to a final concentration of 0.250 M. Convert this value into terms of g/L, molality, and mass %. (Use the following values: molecular weight MWsucrose = 342.296 g/mol; density rhosol′n = 1.02 g/mL; and mass of water, mwat = 934.4 g). Note that the mass of solute is included in the density of the solution.

Question

Jamar Wiggins

Chemistry

15 March, 12:12

A sucrose solution is prepared to a final concentration of 0.250 M. Convert this value into terms of g/L, molality, and mass %. (Use the following values: molecular weight MWsucrose = 342.296 g/mol; density rhosol′n = 1.02 g/mL; and mass of water, mwat = 934.4 g). Note that the mass of solute is included in the density of the solution.

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Answers (1)

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Myah Choi · Answer 1

A. 85.6 g

= 0.0856 kg.

B. 0.00027 mol/g

= 0.27 mol/kg.

C. 8.39 %

Explanation:

Given:

Molar concentration = 0.25 M

Molar weight of sucrose = 342.296 g/mol

Density of solution = 1.02 g/mL

Mass of water = 934.4 g.

Density in g/l = 1.020 g/ml * 1000ml/1 l

= 1020 g/l

Mass of solution in 1 l of solution = 1020 g

Mass of solution = mass of solvent + mass of solute

Mass of sucrose = 1020 - 934.4

= 85.6 g of sucrose in 1 l of solution.

A.

Density of sucrose = mass/volume

= molar mass/molar concentration

= 342.296 * 0.25

= 85.6 g/l

Number of moles = mass/molar mass

= 85.6/342.296

= 0.25 mol

B.

Molality = number of moles of solute/mass of solvent

= 0.25/934.4

= 0.00027 mol/g

C.

% mass of sucrose = mass of sucrose/total mass of solution * 100

= 85.6/1020 * 100

= 8.39 %