A 1.10 g sample of an unknown compound reduces the freezing point of 75.22 g benzene from 5.53 to 4.92 ºC. What is the molar mass of the compound? The freezing point of a 0.010 m aqueous solution of a nonvolatile solute is -0.072 ºC. What would you expect the normal boiling point of this same solution to be? Predict the approximate boiling points of 0.10 m solutions of the following solutes dissolved in water (Kb (H2O) = 0.512 ∞C/m):Al(NO3)3 (aluminum nitrate) CH2O (formaldehyde) RbI (rubidium iodide) C6H6 (benzene) Calculate the van’t Hoff factor, i, for the following weak electrolyte solution: 0.050 m HCHO2, which begins to freeze at -0.0986 ∞C. Calculate the vapor pressure at 25 ∞C of a solution containing 255 g of the nonvolatile solute, glucose, C6H12O6, in 1.50 kg of H2O. The vapor pressure of water at 25 ∞C is 23.8 mmHg. Calculate the vapor pressure at 20 ºC of a saturated solution of the nonvolatile solute, urea, CO(NH2)2, in methanol, CH3OH. The solubility is 17 g urea/100 mL methanol. The density of methanol is 0.792 g/mL, and its vapor pressure at 20 ºC is 95.7 mmHg. Some fish live in saltwater environments and some in freshwater, but in either environment they need water to survive. Saltwater fish drink water, but freshwater fish do not. Explain this difference between the two types of fish. Use the concentration of an isotonic saline solution, 0.92% NaCl (mass/volume), to determine the osmotic pressure of blood at body temperature, 37.0 ºC. (Hint: Assume that NaCl is completely dissociated in aqueous solutions.) The molecular mass of hemoglobin is 6.86 x 104 g/mol. What mass of hemoglobin must be present per 100.0 mL of a solution to exert an osmotic pressure of 7.25 mmHg at 25 ºC?

Given: Mass of substance (solute) = 1.10 g mass of benzene (here solvent) = 75.22 g Initial…

Answered: A 1.10 g sample of an unknown compound…

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.95QE

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Question

A 1.10 g sample of an unknown compound reduces the freezing point of 75.22 g benzene from 5.53 to 4.92 ºC. What is the molar mass of the compound?

The freezing point of a 0.010 m aqueous solution of a nonvolatile solute is -0.072 ºC. What would you expect the normal boiling point of this same solution to be?

Predict the approximate boiling points of 0.10 m solutions of the following solutes dissolved in water (K_b(H₂O) = 0.512 ∞C/m):

Calculate the van’t Hoff factor, i, for the following weak electrolyte solution: 0.050 m HCHO₂, which begins to freeze at -0.0986 ∞C.

Calculate the vapor pressure at 25 ∞C of a solution containing 255 g of the nonvolatile solute, glucose, C₆H₁₂O₆, in 1.50 kg of H₂O. The vapor pressure of water at 25 ∞C is 23.8 mmHg.

Calculate the vapor pressure at 20 ºC of a saturated solution of the nonvolatile solute, urea, CO(NH₂)₂, in methanol, CH₃OH. The solubility is 17 g urea/100 mL methanol. The density of methanol is 0.792 g/mL, and its vapor pressure at 20 ºC is 95.7 mmHg.

Some fish live in saltwater environments and some in freshwater, but in either environment they need water to survive. Saltwater fish drink water, but freshwater fish do not. Explain this difference between the two types of fish.

Use the concentration of an isotonic saline solution, 0.92% NaCl (mass/volume), to determine the osmotic pressure of blood at body temperature, 37.0 ºC. (Hint: Assume that NaCl is completely dissociated in aqueous solutions.)

The molecular mass of hemoglobin is 6.86 x 10⁴ g/mol. What mass of hemoglobin must be present per 100.0 mL of a solution to exert an osmotic pressure of 7.25 mmHg at 25 ºC?

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