The boiling point of water, H₂O is 100.00 °C at 1 atmosphere and its Kop value is 0.512 °C/m. A nonvolatile, nonelectrolyte that dissolves in water is sucrose. How many grams of sucrose, C12H22O11 (342.3 g/mol), must be dissolved in 208.0 grams of water to raise the boiling point by 0.350 °C? g sucrose.

The normal freezing point of water, H₂O is 0.00 °C and its Kip value is 1.86 °C/m. Assuming complete dissociation of the electrolyte, if 13.87 grams of barium chloride (BaCl2, 208.2 g/mol) are dissolved in 260.7 grams of water what is the freezing point of the solution? °C

You are analyzing 100 g of a solution that contains 12.5 g of the ionic compound KBr (MM = 119.0 g/mol) in water.  Here is some useful information:  KFP of water is 1.86 °C/m; KBP for water is 0.512 °C/m.  The density of the solution is 1.094 g/mL. Calculate the boiling point of this solution (bp of water is 100.0°C).   Calculate the osmotic pressure (in atm) of this solution at 25°C.

A 83.5 g sample of a nonelectrolyte is dissolved in 206.1 g of water. The solution is determined to have a boiling point of 102.3 °C. What is the molar mass of the compound? (Kb for water is 0.510 °C/m).

[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

When 105.g of glycine C2H5NO2 are dissolved in 1200.g of a certain mystery liquid X, the freezing point of the solution is 4.6°C lower than the freezing point of pure X. On the other hand, when 105.g of iron(III) chloride are dissolved in the same mass of X, the freezing point of the solution is 7.5°C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits.      i=

1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)   2-What is the rate law expression for the reaction A + B → C, based on the following data

What is the freezing point (in K) of a solution made by dissolving 19.543g of CCl4 in 130.0 g of benzene? Pure benzene has a freezing point of 5.5°C and a Kf = 5.12 °C/m.

Calculate the vapor pressure above a solution prepared by dissolving 2.00 g of aspirin (C9H8O4) in 50.0 g of methanol (CH3OH) at 21.2 °C. Pure methanol has a vapor pressure of 101 torr at 21.2 °C.

11. Calculate the molality of a solution containing 398 g glucose (C,H12O6) dissolved in 2.00 L of water (density 0.997 g/mL). 12. An ethylene glycol solution contains 27.8 g of ethylene glycol (C;H,O2) in 79.2 mL of water (density 0.997 g/mL). Calculate the freezing point and boiling point of the solution.