A 1.159 g sample contains only vitamin C (C6H8O6) and sucralose (C12H19Cl3O8). When the sample is...

A 1.159 g sample contains only vitamin C (C6H8O6) and sucralose (C12H19Cl3O8). When the sample is dissolved in water to a total volume of 34.0 mL, the osmotic pressure of the solution is 4.06 atm at 297 K. What is the mass percent of vitamin C and sucralose in the sample?

Comments: No Ionization of Vitamin C

Expert Solution

mass percentage of vitamin c is 75.06%

queen_honey_blossom answered 1 year ago

A 1.198 g sample contains only vitamin C (C6H8O6) and sucralose (C12H19Cl3O8). When the sample is...

A 1.198 g sample contains only vitamin C (C6H8O6) and sucralose (C12H19Cl3O8). When the sample is dissolved in water to a total volume of 25.3 mL, the osmotic pressure of the solution is 5.62 atm at 303 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: % sucralose: %

1. A 1.189 g sample contains only vitamin C (C6H8O6) and sucralose (C12H19Cl3O8). When the sample...

1. A 1.189 g sample contains only vitamin C (C6H8O6) and sucralose (C12H19Cl3O8). When the sample is dissolved in water to a total volume of 39.0 mL, the osmotic pressure of the solution is 3.57 atm at 297 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: % sucralose: % 2. A chemist combined chloroform (CHCl3) and acetone (C3H6O) to create a solution where the mole fraction of chloroform, χchloroform,χchloroform, is 0.187 The...

Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin. A solution containing 81.0 g of ascorbic...

Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin. A solution containing 81.0 g of ascorbic acid dissolved in 220 g of water has a density of 1.22 g/mL at 55 ∘C. Calculate the mass percentage. Calculate the mole fraction. Calculate the molality. Calculate the molarity of ascorbic acid in this solution.

A sample that contains only BaCO3 and MnCO3 weighs 0.8192 g. When it is dissolved in...

A sample that contains only BaCO3 and MnCO3 weighs 0.8192 g. When it is dissolved in excess acid, 0.2420 g of carbon dioxide is liberated. What percentage of BaCO3 did the sample contain? Assume all the carbon originally present is converted to carbon dioxide.

Combustion of 0.2000 g sample of Vitamin C yields 0.2998 g CO2 and 0.0819 g H2O.

Combustion of 0.2000 g sample of Vitamin C yields 0.2998 g CO2 and 0.0819 g H2O. What is the mass percent of each element? What is the empirical formula for Vitamin C?

A 0.1219 g sample of a Vitamin C (ascorbic acid) tablet was dissolved in acid. A...

A 0.1219 g sample of a Vitamin C (ascorbic acid) tablet was dissolved in acid. A 25.00 mL aliquot of 0.01739 M KIO3 was added along with excess KI. The resulting solution was titrated with 0.07211 M thiosulfate, requiring 21.44 mL to reach the endpoint. Compute the weight percent of ascorbic acid (FW = 176.12) in the tablet.

a 0.580 g sample of a compound containing only carbon and hydrogen contains .480 g of...

a 0.580 g sample of a compound containing only carbon and hydrogen contains .480 g of carbon and .100g of hydrogen. At STP 33.6mL of the gas has a mass of .087g. What is the molecular formula for the compound? The answer should be C4H10. Please explain with steps. Thank you.

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water...

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water and an excess of is added, producing a precipitate of . The precipitate is filtered, dried, and weighed. The mass of the precipitate is 1.06 g. What is the mass percent of in the sample? %

An unknown compound contains only C , H , and O . Combustion of 6.50 g...

An unknown compound contains only C , H , and O . Combustion of 6.50 g of this compound produced 15.9 g CO2 and 6.50 g H2O . What is the empirical formula of the unknown compound? Insert subscripts as needed. empirical formula:[CHO]

An unknown compound contains only C, H, and O. Combustion of 3.50 g of this compound...

An unknown compound contains only C, H, and O. Combustion of 3.50 g of this compound produced 7.96 g of CO2 and 3.26 g of H2O.What is the empirical formula of the unknown compound?

Question