Chapter 12 Homework On a piece(s) of paper, write your name and the chapter number. For each slide, write the question number and the letter corresponding to your answer choice. On certain problems the required written work must be shown for full credit. * The homework assignment is worth a total of 13 pts. Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Question 1 Which of the following pairs of substances would be completely soluble in each other regardless of the proportions combined? A) nitrogen gas and gaseous ammonia B) sodium chloride and water C) gasoline and water D) all of the above Question 2 Which of the following would produce a 25% by mass solution of sodium chloride in water? (Show all calculation steps) A) 25 g of sodium chloride dissolved in 100 g of water. B) 50 g of sodium chloride dissolved in 200 g of water C) 25 g of sodium chloride dissolved in 75 g of water. D) both A and B. Question 3 The density of water is very close to 1.00 g/mL. If 3.00 moles of ethanol (molar mass 46 g/mol) is mixed with 1000. g of water, the solution will be… (Show all calculation steps) A) 3.00 molar (M) in ethanol. B) 3.00 molal (m) in ethanol. C) 3.00% by mass ethanol. D) all of the above. Question 4 Which of the following is true? (Rewrite the false statements into true statements.) A) The solubilities of solids in liquids always increase with temperature. B) The solubilities of gases in liquids always increase with temperature. C) The solubilities of solids in liquids rarely increase with temperature. D) None of the above. Question 5 The freezing point depression constant is… (Name an example chemical and provide its Kf) A) different for different solutes. B) different for different solvents. C) the same for all polar solvents. D) different for different temperatures. Question 6 How does a solution differ from a colloid? (In your own words, write a definition for a colloid) A) The solute particles are smaller in a solution than a colloid. B) A colloid will scatter visible light but a solution will not. C) Both A and B. D) None of the above. Question 7 A nonpolar liquid with a density of 0.870 g/mL is mixed in a beaker with water (density 1.00 g/mL). If the substances do not react chemically, then it is likely that… A) two phases will form, with the water phase on top. B) two phases will form, with the water phase on bottom. C) most (but not all) of the liquid will dissolve in the water. D) the nonpolar liquid will be miscible in the water. Question 8 A 135 g solution that has a mass percentage of salt equal to 21%. If the maximum amount of salt that will dissolve in 100 g of aqueous solution is 26 g, then the 21% solution is… (Calculate the grams of salt is dissolved in the solution) A) a saturated solution. B) an unsaturated solution. C) a supersaturated solution. D) none of the above. Question 9 Which compound should dissolve most in water? (include the structure plus the dipole of your answer) A) CO2 B) CS2 C) Br2 D) SO2 Question 10 How much water is present in 200. g of salt solution if the mass percent of salt is 26%? (Show all calculation steps) A) 26 g B) 52 g C) 74 g D) 148 g Question 11 What is the molarity of pure water? (Show all calculation steps) A) 1.00 M B) 55.6 M C) 100 % D) Cannot be determined without additional information. Question 12 What is the molality of a saturated salt solution? (maximum solubility of salt is 26% mass percentage) (Show all calculation steps) A) 6.0 m B) 260 m C) 4.44 m D) 26 m E) None of the above Question 13 Which NaOH solution is the most concentrated? Assume a liquid density of 1.00 g/mL in all cases. (Calculate the grams of NaOH for your answer) A) 10.0% NaOH by mass B) 10.0 M NaOH C) 10.0 m NaOH D) They all have the same concentration Question 14 How would you achieve a high concentration of CO2 in a soda bottle? A) Keep the bottle capped B) Keep the bottle refrigerated C) Keep the bottle upside down D) B and C E) A and B
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