A soft drink is made by dissolving CO_2 gas at 3.00 atm in a flavored solution a

Question

A soft drink is made by dissolving CO_2 gas at 3.00 atm in a flavored solution and sealing the solution in aluminum cans at 20.0 degree C. What amount (in moles) of CO_2 is contained in the.240.0 mL, can of the soft drink? At 20.00 degree C the Henry's Law constant for CO, is 2.3 x 10^-2 moL-atm. Ascorbic acid (vitamin c, c_6H_3O_6) is a water-soluble vitamin. A solution containing 80.5 g of ascorbic acid dissolved in 210.0 g of water has a density of 1.22 g/mL at 55 degree C. Calculate: the mass percentage; the mole fraction: the morality; the morality of ascorbic acid in this solution.

Explanation / Answer

1) According to Henry's law

Pressure =Concentration / Henry's law constant

So concentration = Pressure X Henry's law constant

Concentration = 3 X 2.3 X 10^-2 = 0.069 moles / L
0.069 moles are dissolved in 1L

so moles dissolved in 0.240 L = 0.0166 moles

2) a) Mass percentage = Mass of ascorbic acid / total mass = 80.5 / 210+ 80.5 = 0.28 = 28%

b)Mole fraction = Moles of ascorbic acid / Total moles

Moles of ascorbic acid = Mass / Mol wt = 80.5 / 176 = 0.457

Moles of water = 210 /18= 11.667

Total moles = 0.457 + 11.667 = 12.124

Mole fraction = 0.457 X 100/ 12.124 = 3.76%

c)Molality = Moles of solute / amount of solvent inKg = 0.457 / 0.210 = 2.17 molal

d) Molarity of ascorbic acid = Moles of solute / Volume of solution

Volume of solution = Mass of solution / Density of solution = 290.5 / 1.22 = 237.7 mL = 0.237L

Molarity = 0.457 / 0.237 = 1.93 Molar

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