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# 20 quest collig review

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### 20 quest collig review

1. 1. Twenty Questions AP Chemistry Colligative Property Review Chapter 11
2. 2. Twenty Questions 20 19 18 17 16 15 14 13 12 11 10 9 8 7 6 5 4 3 2 1
3. 3. <ul><li>A solution is prepared by dissolving 85.0 grams of ammonia (NH 3 ) in sufficient water to produce 1.00 liter of solution. This solution has a density of 0.960 g/ml. What is the percent ammonia by weight in this solution? A) 8.50%; B) 8.85%; C) 9.71%; D) 7.83%; E) 9.29% </li></ul><ul><li>8.85% </li></ul>
4. 4. 2. A solution is prepared by dissolving 85.0 grams of ammonia (NH 3 ) in sufficient water to produce 1.00 liter of solution. This solution has a density of 0.960 g/ml. What is the mole fraction of ammonia in the solution? A) 0.093; B) 0.103; C) 0.086; D) 0.096; E) 0.089 <ul><li>A </li></ul>
5. 5. 3. A solution is prepared by dissolving 85.0 grams of ammonia (NH 3 ) in sufficient water to produce 1.00 liter of solution. This solution has a density of 0.960 g/ml. The molality of ammonia in the solution is: A) 5.21; B) 5.00; C) 5.71; D) 4.61; E) 4.78 <ul><li>A) 5.71; </li></ul>
6. 6. 4. A solution is prepared by dissolving 85.0 grams of ammonia (NH 3 ) in sufficient water to produce 1.00 liter of solution. This solution has a density of 0.960 g/ml.What is the molarity of ammonia in the solution? A) 5.21; B) 5.00; C) 5.71; D) 4.61; E) 4.78 <ul><li>B) 5.00; . </li></ul>
7. 7. <ul><li>Which of the following is a weak electrolyte in aqueous solution? A) ethyl alcohol; B) H 2 SO 4 ; C) HCl; D) NaCl; E) HC 2 H 3 O 2 </li></ul><ul><li>E) HC 2 H 3 O 2 . </li></ul>
8. 8. 6. Dissolving a solute such as NaCl in a solvent at 25 o C results in: A) an increase in the kinetic energy of the solvent molecules; B) a decrease in the kinetic energy of the solvent molecules; C) a decrease in the boiling point of the liquid; D) an increase in the melting point of the liquid; E) a decrease in the vapor pressure over the solution. <ul><li>E) a decrease in the vapor pressure over the solution. </li></ul>
9. 9. 7. Which of the following solutions would have the lowest freezing point? A) 0.1 m Ca(NO 3 ) 2 ; B) 0.1 m KNO 3 ; C) 0.2 m sucrose (sugar); D) 0.1 m HCl; E) 0.1 m sucrose (sugar). . <ul><li>A) 0.1 m Ca(NO 3 ) 2 ; </li></ul>
10. 10. 8 . Which of the following nonelectrolytes would produce the solution having the lowest freezing point if 10.0 grams of the respective compounds were dissolved in 1000 grams of water? A) alcohol, C 2 H 6 O; B) glycerin, C 3 H 8 O 3 ; C) glucose, C 6 H 12 O 6 ; D) methanol, CH 4 O; E) all produce the same effect. <ul><li>D) methanol, CH 4 O; </li></ul>
11. 11. 9. A solution made from water and a nondissociating solute contains 10.0 grams of solute X and 800 grams of water. The freezing point of the solution is -0.31 o C. What is the molecular weight of X? ( k f for water = 1.86 o C/ m ) A) 40; B) 50; C) 80; D) 75; E) 60 . <ul><li>D) 75 </li></ul>
12. 12. 10. The following experimental data were obtained for pure solvent S and solutions of solute X (MW = 100.) in this solvent. Solute X neither associates nor dissociates in solvent S. Experiment Grams S Grams X Freezing point, o C I. 100.0 0.000 16.605 II. 100.0 1.000 16.200 III. 100.0 1.750 15.907 IV. 100.0 2.200 15.710 V. 100.0 4.200 14.960 11. What is the molality of X for the solution of Experiment V? A) 0.0420 m ; B) 0.420 m ; C) 4.20 m ; D) 0.0403 m ; E) 0.104 m <ul><li>B) 0.420 m ; . </li></ul>
13. 13. 11. The following experimental data were obtained for pure solvent S and solutions of solute X (MW = 100.) in this solvent. Solute X neither associates nor dissociates in solvent S. Experiment Grams S Grams X Freezing point, o C I. 100.0 0.000 16.605 II. 100.0 1.000 16.200 III. 100.0 1.750 15.907 IV. 100.0 2.200 15.710 V. 100.0 4.200 14.960 For Solutions II - V, one would need to know the (__  __) in order to determine the mole fraction of X; one would need to know (__  __) in order to calculate the molarity of X.  A)MW of X; density of S B) MW of S; density of X C)MW of S; density of S D) MW of X; density of the solution E) MW of S; density of the solution <ul><li>E) MW of S; density of the solution </li></ul>
14. 14. 12. The following experimental data were obtained for pure solvent S and solutions of solute X (MW = 100.) in this solvent. Solute X neither associates nor dissociates in solvent S. Experiment Grams S Grams X Freezing point, o C I. 100.0 0.000 16.605 II. 100.0 1.000 16.200 III. 100.0 1.750 15.907 IV. 100.0 2.200 15.710 V. 100.0 4.200 14.960 From these data, what is the molal freezing point depression constant, K f , characteristic of solvent S? A) 1.86 o C/ m ; B) 2.98 o C/ m ; C) 3.73 o C/ m ; D) 4.01 o C/ m ; E) 5.12 o C/ m . <ul><li>D) 4.01 o C/ m ; . </li></ul>
15. 15. 13. Barium phosphate is insoluble in water. If equal volumes of 0.50 M Ba(ClO 4 ) 2 and 0.20 M K 3 PO 4 are mixed, what is the concentration of Ba 2+ ions in the resulting solution? A) 0.20 M; B) 0.00 M; C) 0.37 M; D) 0.10 M; E) 0.25 M . <ul><li>E) 0.1 </li></ul>
16. 16. 14. Assuming that the volumes are additive, how much water would need to be added to 30.0 ml of a 12.0 M HCl solution in order to prepare a 2.0 M HCl solution? A) 180 ml; B) 150 ml; C) 120 ml; D) 90 ml; E) 60 ml <ul><li>A) 150 ml; . </li></ul>
17. 17. 15. If 28.6 grams of &quot;washing soda&quot;, Na 2 CO 3 . 10 H2O (FW = 286) is dissolved in 130. grams of water, what is the molality of Na 2 CO 3 in the resulting solution? A) 0.676; B) 0.220; C) 0.893; D) 0.459; E) 0.769 . <ul><li>E) 0.769 . </li></ul>
18. 18. 16. If the dissolution of an ionic solid in water is endothermic, then it can be concluded that: A) the solubility of the solid will decrease with increasing temperature; B) the solubility of the solid will increase with increasing temperature; C) the solution process releases heat; D) the solubility of the solid is independent of temperature; E) the hydration energy exceeds the lattice energy . <ul><li>B) the solubility of the solid will increase with increasing temperature; </li></ul>
19. 19. 17. What is the osmotic pressure (in atm.) at 0.0 o C of a solution containing 1.00 gram per liter of sucrose, C 12 H 22 O 11 ? A) 0.066; B) 0.11; C) 0.24; D) 0.29; E) 0.48 . <ul><li>A) 0.066; . </li></ul>
20. 20. 18. Pure cyclohexane (C 6 H 12 , FW = 84.16) freezes at 6.55 o C and has a molal freezing point depression constant, K f , of 20.0 o C/molal. A solution of a molecular unknown X, made by dissolving 5.00 grams of X in 100.0 grams of cyclohexane, has a freezing point of 3.00 o C. What is the molecular weight of X? A) 8.88; B) 153; C) 282; D) 333; E) 747 . <ul><li>C) 282; . </li></ul>
21. 21. 19. What is the van't Hoff factor, i , of a 0.220-molal aqueous solution of a nonvolatile, weak electrolyte if the freezing point is -0.63 o C? A) 1.22; B) 2.05; C) 1.78; D) 3.04; E) 1.54 . <ul><li>E) 1.54 . </li></ul>
22. 22. 20. Which substance would raise the boiling point of water the LEAST? a) HClO 4 b) Mg(NO 3 ) 3 c) CaCl 2 d) LiOH e) HC 2 H 3 O 2 . <ul><li>e) HC 2 H 3 O 2 . </li></ul>