2. During Amihan season, the crops in Benguet and other Northern Luzon provinces are prone to damage because of the colds temperature. Devise a plan to protect the crops from the very low temperature. 3. The Philippines is one of the countries most prone to natural hazards such as storms and earthquakes. When a natural calamity hits, it is often the lack of food and provisions that poses the greatest problem to the survivors. Using your knowledge about colligative properties, propose creative ways of preserving and storing.

2. During Amihan season, the crops in Benguet and other Northern Luzon provinces are prone to damage because of the colds temperature. Devise a plan to protect the crops from the very low temperature. 3. The Philippines is one of the countries most prone to natural hazards such as storms and earthquakes. When a natural calamity hits, it is often the lack of food and provisions that poses the greatest problem to the survivors. Using your knowledge about colligative properties, propose creative ways of preserving and storing.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 5ALQ: You have read that adding a solute to a solvent can both increase the boiling point and decrease the...

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Similar questions

Starch contains CC, CH, CO, and OH bonds. Hydrocarbons have only CC and CH bonds. Both starch and hydrocarbons can form colloidal dispersions in water. Which dispersion is classified as hydrophobic? Which is hydrophilic? Explain briefly.
Distinguish between dispersion methods and condensation methods for preparing colloidal systems.
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?
Define the terms in Raoults law. Figure 10-9 illustrates the net transfer of water molecules from pure water to an aqueous solution of a nonvolatile solute. Explain why eventually all of the water from the beaker of pure water will transfer to the aqueous solution. If the experiment illustrated in Fig. 10-9 was performed using a volatile solute, what would happen? How do you calculate the total vapor pressure when both the solute and solvent are volatile?
How do colloids differ from solutions with regard to dispersed particle size and homogeneity?
The specific gravity of a solution of KCl is greater than 1.00. The specific gravity of a solution of NH3 is less than 1.00. Is specific gravity a colligative property? Why, or why not?
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?