5. Calculate the molal concentration of a solution that contains 18 g of sodium hydroxide in 100 ml of water. (molar mass of NaOH is 40 g/mol) 6. Determine the molar concentration of a solution that contains 25 g of potassium hydroxide in 250 ml of solution. (molar mass of KOH is 56 g/mol) 7. Calculate the molality of a solution containing 10.8 g of ethylene glycol in 360 g of water. (molar mass of ethylene glycol is 62.07 g/mol) 8. What is the freezing and boiling point of a solution that contains 5 g of glycerol and 20 ml of water? (molar mass of glycerol is 92.09 g/mol)

5. Calculate the molal concentration of a solution that contains 18 g of sodium hydroxide in 100 ml of water. (molar mass of NaOH is 40 g/mol) 6. Determine the molar concentration of a solution that contains 25 g of potassium hydroxide in 250 ml of solution. (molar mass of KOH is 56 g/mol) 7. Calculate the molality of a solution containing 10.8 g of ethylene glycol in 360 g of water. (molar mass of ethylene glycol is 62.07 g/mol) 8. What is the freezing and boiling point of a solution that contains 5 g of glycerol and 20 ml of water? (molar mass of glycerol is 92.09 g/mol)

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter1: Matter, Measurements, And Calculations

Section: Chapter Questions

Problem 1.126E

See similar textbooks

Similar questions

A 12-oz (355-mL) Pepsi contains 38.9 mg caffeine (molar mass = 194.2 g/mol). Assume that the Pepsi, mainly water, has a density of 1.01 g/mL. For such a Pepsi, calculate: (a) its caffeine concentration in ppm; (b) its molarity of caffeine; and (c) the molality of caffeine.
Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?