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]

A 49.5 g sample of a substance which contains C, H, and O is burned in...

A 49.5 g sample of a substance which contains C, H, and O is burned in excess oxygen, producing 110.0 g of CO2 and 22.5 g of H2O. A mass spectrum confirms that the molar mass of the sample is 162.0 g/mol. a.) how many moles and grams of carbon were in the original sample? b.) How many moles and grams of hydrogen were in the original sample? c.) How many moles and grams of oxygen were in the original...

Question