REVIEW



REVIEWChapter 14Differentiate between colloids, solutions, and suspensionsDefine solvent and solute and be able to identify them in a solution.Describe the process of solvation, dissociation, and dissolving. Be sure to study polarity of compounds to be able to predict solubility.Differentiate between saturated, unsaturated, and supersaturated.State and discuss the factors affecting the rate of solubility. State and discuss the factors that affect solubility.Be able to read a solubility curve graph.Relate the enthalpy of solution to endothermic and exothermic dissolving processes.Differentiate between molarity and molality.Solve problems involving molarity, molality, mole fraction mass percent, and making solutions.Describe the three colligative properties of solutions (vapor pressure reduction, freezing point depression, and boiling point elevation).Relate the colligative properties to everyday situations.Calculate the freezing point, boiling point and molar mass using changes in temperature and molality.REVIEW QUESTIONSWrite T for true or F for false. If the statement is false, replace the underlined word or phrase with one that will make the statement true, and write your correction on the blank provided.________________________1. Most solutions consist of a gas dissolved in a liquid.________________________2. Molality is the most common concentration unit in chemistry.________________________3. Water is the most common solvent.________________________4. The solubility of a substance can be changed by altering the temperature.________________________5. In terms of physical states of matter, there are three possible combination of solvent-solute pairs.________________________6. The differing solubilities of substances can be used to separate them from mixtures. ________________________7. Solvation does not occur in the case of a polar solvent and a nonpolar solute.________________________8. The solution process is usually exothermic.________________________9. Vapor pressure, freezing point, and boiling point are chemical properties of a solution.________________________10. Colligative properties depend on the kind of particles present in a solution.________________________11. If fewer solvent particles can evaporate from a solution, the vapor pressure of the solvent is lowered.________________________12. For a solution having a specific concentration, the amount that the vapor pressure of the solvent is lowered depends on the characteristics of the solute.________________________13. Glucose, sucrose, and other molecular compounds with high melting points are considered to be volatile solutes.________________________14. The amount of vapor pressure of a solvent is lowered is equal to the difference between the vapor pressure of the pure solvent and the vapor pressure of the solution.________________________15. In an ideal solution, all possible attractions among particles of solute and solvent are the same. How is supersaturation possible?What are three things that you could do to speed up the rate of a solution?What is the difference between molarity and molality?In terms of polarity, which solvent-solute combinations are most likely to form solutions? Why?Why is the vapor pressure reduced in a solution as compared to the pure solvent?Describe freezing point depression in terms of the freezing points of pure solvent and a solution made from that solvent.Why is the addition of antifreeze to the water in a car radiator just as important in hot climates as in cold climates?PROBLEM SETShow all work, units, and correct significant digits.64.2 g of KCl is added to 0.250 L of distilled water. Assuming the volume of the solution is the same as the water, calculate the molarity of the solution. (The molecular mass of KCl is 74.55 g/mol)630.0 g of nitric acid, HNO3, are added to 6.500 Kg of water. Calculate the molality of this solution. (The molecular mass of HNO3 is 63.02 g/mol)3. How many liters of water must be added to 5.50 moles of sugar to make a 2.00M solution?4. Calculate the mole fraction for each component in 22.5 g CH3CH2OH in a 1.00 x 102 g H2O solution.Calculate the mass percent for each component in problem number 4.Prepare 750.0 mL of a 6.0M solution from the 18.0M stock solution of H2SO4.Calculate the freezing point if 46.0 g glycerol, C3H5(OH) 3, are dissolved in 0.500 kg water. (The molecular mass of C3H5(OH)3 is 92.11 g/mol and the Kfp of water is 1.853°C/m)A 0.171 g sample of an unknown organic compound is dissolved in ether. The solution has a total mass of 2.470 g. The boiling point of the solution is found to be 36.43C. What is the molar (molecular) mass of the organic compound? (The Kbp of ether is 2.02C/m and the boiling point of ether is 34.6C.) ................
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