Calculate the freezing point for a solution containing 55 grams of sucrose, C12H22O11, dissolved in 80.0grams of water.

The boiling point of chloroform, CHCl3, is 61.700 °C at 1 atmosphere. Kb(chloroform) = 3.67 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.11 grams of the compound were dissolved in 204.7 grams of chloroform, the solution began to boil at 62.577 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound ? _____g/mol

A solution prepared by dissolving 6.95 X 10^3 g of protein in 0.0300 L of water has an osmotic pressure of 0.195 torr at 25 C. Assuming the protein is a non electrolyte, determine the molar mass of the gene fragment.

Calculate the molality of a sugar in a sampleofnormal spinal fluid.The concentration of this sugar, C6H12O6, is around 76 μg per 100 mg of fluid.

Calculate the osmotic pressure of a solution containing 19.25 mg of hemoglobin in 16.1 mL of solution at 18 °C.The molar mass of hemoglobin is 6.5 x 104 g/mol. Express your answer in atmospheres. Hνα ΑΣφ II = 0.342 atm %|

A 365 µM solution of a dye molecule, Rhodamine 6G, dissolved in methanol is allowed to sit open to the air such that the volume of the solution is reduced to 43% of its original volume due to evaporation of methanol. Assuming that no dye molecules are lost during the evaporation process, what is the concentration of the dye in the remaining ethanol after evaporation?

[References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. K₁ (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.95 grams of the compound were dissolved in 293.3 grams of ethanol, the solution began to boll at 78.570 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer Retry Entire Group 9 more group attempts remaining Show Hint Congage Learning Cengage Technical Support Previous Next Save and Exit

What is the osmotic pressure of a 4.5 FL OZ solution containing 30.6 g of fructose (C6H12O6) at 40 °F.  Osmotic pressure is 29.2 atm. Explain why.

Please provide detailed solution and give the explanation of the concept   Calculate the osmotic pressure of a solution containing 19.25 mg of hemoglobin in 14.7 mL of solution at 35 °C. The molar mass of hemoglobin is 6.5 x 10^4 g/mol. Express your answer in atmospheres.

3) Camphor (CoH160) melts at 179.8 °C, and it has a particularly large freezing point depression constant of 40.0 "C/m. When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.10 g of liquid camphor, the freezing point of the mixture is found to be 176.7 C. What is the molar mass of the organic substance?