<p> Solution Questions Part 2</p><p>You must show all of your work on all calculations.</p><p>1. Describe how adding a solute to a solvent is able to raise the boiling point of the solution compared to the solvent’s boiling point.</p><p>2. What is the relationship between the moles of solute in a solution and the change in boiling point or change in freezing point of a solution?</p><p>3. A sugar solution, to be placed in a humming bird feeder, is prepared by adding 1.20 kg of sucrose, C12H22O11, to 800 g of water. a. What is the molality of this solution? b. Calculate the difference (change) in the freezing point of the solution compared to that of pure water? c. If the feeder is left out on a night where the temperature drops to -8.000C will the solution in the feeder freeze? Explain.</p><p>4. A car radiator is filled with a solution that contains 2500 grams of water mixed with 925.0 grams of ethylene glycol, the main ingredient in antifreeze. Ethylene glycol has the formula C2H4(OH)2. What will be the freezing point and boiling point of the antifreeze solution in the radiator?</p><p>5. List if the following solutions are acidic, basic, or neutral. Explain how you can tell. a. pH = 8.5 b. [H+] = 4.0 x 10-4 and [OH-] = 2.5 x 10-11 c. [H+] = 1.0 x 10-7 and [OH-] = 1.0 x 10-7</p><p>6. Calculate the pH of the following solutions. Remember pH = -log[H+] page 513 -514in your textbook a. Milk [H+] = 4.5 x 10-7 b. Ammonia household cleaner [H+] = 1.0 x 10-12</p><p>Bonus: If 65.0 grams of a solute is dissolved in 845 grams of water, and the freezing point of the resulting solution is -2.960C, what is the molecular mass of the solute? Hint: The units for molecular mass are grams/mole.</p>