tester NOT REAL NOTES
tester NOT REAL NOTES econ 101
SUNY Broome Community College
Popular in Economics
This 6 page Class Notes was uploaded by Nosa Akol on Monday October 3, 2016. The Class Notes belongs to econ 101 at SUNY Broome Community College taught by in Fall 2016. Since its upload, it has received 2 views. For similar materials see in Economics at SUNY Broome Community College.
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Date Created: 10/03/16
AP Chemistry Ch. 13 Practice test 1) The process of solute particles being surrounded by solvent particles is known as __________. A) salutation B) agglomeration C) solvation D) agglutination E) dehydration Answer: C Sec. 13.1 2) The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L The solubility of oxygen in water at 3.0 atm and 25 °C is __________ g/L. A) 0.041 B) 0.014 C) 0.31 D) 0.12 E) 3.0 Answer: D Sec. 13.3 3) The solubility of nitrogen gas in water at 25 °C and a nitrogen pressure of 1.0 atm is 6.9 10 M4 The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm is __________ M. A) 5.5 × 10 4 B) 8.6 10 4 C) 1.2 103 D) 3.7 10 E) 0.80 Answer: A Sec. 13.3 4) On a clear day at sea level, with a temperature of 25 °C, the partial pressure of 2 in air is 0.78 atm and the concentration of nitrogen in water is 5.3 × 4 . When the partial pressure of N is __________ atm, the concentration in water is 1.1 × 3 . 10 M 2 10 M A) 0.63 atm B) 0.78 atm C) 1.0 atm D) 2.1 atm E) 1.6 atm Answer: E Sec. 13.3 5) A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and a small amount of precipitate is observed. This solution is __________. A) hydrated B) placated C) saturated D) unsaturated E) supersaturated Answer: C Sec. 13.3 6) The solubility of MnSO 4onohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO 4 monohydrate is best described as a(n) __________ solution. The formula weight of MnSO monohydrate is 168.97 g/mol. 4 A) hydrated B) solvated C) saturated D) unsaturated E) supersaturated Answer: E Sec. 13.3 7) The concentration of urea in a solution prepared by dissolving 16 g of urea in 39 g of H O is __________% by mass. The molar mass of 2 urea is 60.0 g/mol. A) 29 B) 41 C) 0.29 D) 0.41 E) 0.48 Answer: A Sec. 13.4 8) The concentration of nitrate ion in a solution that contains 0.900 M aluminum nitrate is __________ M. A) 0.900 B) 0.450 C) 0.300 D) 2.70 E) 1.80 Answer: D Sec. 13.4 9) The concentration of KBr in a solution prepared by dissolving 2.21 g of KBr in 897 g of water is __________ molal. A) 2.46 B) 0.0167 C) 0.0207 D) 2.0710 5 E) 0.0186 Answer: C Sec. 13.4 10) The concentration (M) of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C 2 O6 is __________ M. The density of the solution is 0.79 g/mL. A) 21 B) 0.93 C) 0.58 D) 6.0 × 4 E) 1.72 Answer: C Sec. 13.4 10 11) The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H 2 is __________. A) 0.58 B) 0.37 C) 0.13 D) 0.11 E) 9.1 Answer: D Sec. 13.4 12) The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H O is __________ molal. 2 A) 96 B) 6.9 C) 0.68 D) 6.3 E) 0.11 Answer: B Sec. 13.4 13) What is the molarity of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL? A) 143 B) 2.45 C) 2.56 D) 2.23 E) 1.410× 2 Answer: B Sec. 13.4 14) The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult's Law predicts that a solution prepared by dissolving 10.0 mmol naphthalene (nonvolatile) in 90.0 mmol ethanol will have a vapor pressure of __________ atm. A) 0.498 B) 0.413 C) 0.790 D) 0.367 E) 0.0918 Answer: B Sec. 13.5 15) The vapor pressure of pure water at 25 °C is 23.8 torr. What is the vapor pressure (torr) of water above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol) in 95.0 g of water? A) 24.3 B) 23.4 C) 0.451 D) 0.443 E) 23.8 Answer: B Sec. 13.5 16) The freezing point of ethanol (C 2 O5) is 114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C) of a solution prepared by dissolving 50.0 g of glycerin (C H O a nonelectrolyte) in 3 8 3 200 g of ethanol? A) 115 B) 5.42 C) 132.3 D) 120.0 E) 114.6 Answer: D Sec. 13.5 17) What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO )3 2 (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m. A) 3.34 B) 1.11 C) 3.34 D) 1.11 E) 0.00 Answer: A Sec. 13.5 18) A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of 3.33 °C. Given K f = 1.86°C/m for water, the molar mass of the unknown liquid is ________ g/mol. A) 69.0 B) 333 C) 619 D) 161 E) 62.1 Answer: E Sec. 13.5 19) Determine the fraction of ionization of HX if a solution prepared by dissolving 0.020 mol of HX in 115 g of water freezes at 0.47 °C. The molal freezingpointdepression constant of water is 1.86 °C/m. A) 0.044 B) 0.30 C) 0.45 D) 1.45 E) 0.348 Answer: C Sec. 13.5 20) The dissolution of gases in water is virtually always exothermic because __________. A) one of the two endothermic steps (separation of solute particles) in the solutionformation process is unnecessary B) the exothermic step in the solutionformation process is unnecessary C) gases react exothermically with water D) neither of the two endothermic steps in the solutionformation process is necessary E) all three steps in the solutionformation process are exothermic Answer: A Sec. 13.1 21) Formation of solutions where the process is endothermic can be spontaneous provided that __________. A) they are accompanied by another process that is exothermic B) they are accompanied by an increase in order C) they are accompanied by an increase in disorder D) the solvent is a gas and the solute is a solid E) the solvent is water and the solute is a gas Answer: C Sec. 13.1 22) The phrase "like dissolves like" refers to the fact that __________. A) gases can only dissolve other gases B) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes C) solvents can only dissolve solutes of similar molar mass D) condensed phases can only dissolve other condensed phases E) polar solvents dissolve nonpolar solutes and vice versa Answer: B Sec. 13.1 23) Ammonium nitrate (NH NO 4 dis3olves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. The solution process is spontaneous because __________. A) the vapor pressure of the water decreases upon addition of the solute B) osmotic properties predict this behavior C) of the decrease in enthalpy upon addition of the solute D) of the increase in enthalpy upon dissolution of this strong electrolyte E) of the increase in disorder upon dissolution of this strong electrolyte Answer: E Diff: 2 Page Ref: Sec. 13.1 24) In a saturated solution of a salt in water, __________. A) the rate of crystallization > the rate of dissolution B) the rate of dissolution > the rate of crystallization C) seed crystal addition may cause massive crystallization D) the rate of crystallization = the rate of dissolution E) addition of more water causes massive crystallization Answer: D Sec. 13.2 25) Which one of the following substances would be the most soluble in CCl ? 4 A) CH 3H OH2 B) 2 C) 3 D) 10 22 E) NaCl Answer: D Sec. 13.3 26) Which one of the following substances is more likely to dissolve in CCl 4? A) CBr 4 B) HBr C) HCl D) C3 OH 2 E) NaCl Answer: A Sec. 13.3 27) Which one of the following is most soluble in water? A) CH 3H B) C3 CH 2H 2 C) H C3 OH 2 D) H 3H CH2CH O2 2 E) C3 CH 2H C2 OH 2 2 Answer: A Sec. 13.3 28) Which one of the following concentration units varies with temperature? A) molarity B) mass percent C) mole fraction D) molality E) all of the above Answer: A Sec. 13.4 29) A 1.35 m aqueous solution of compound X had a boiling point of 101.4°C. Which one of the following could be compound X? The boiling point elevation constant for water is 0.52°C/m. A) CH 3H OH2 B) 6 O12 6 C) a 3O 4 D) KCl E) Cl 2 Answer: D Sec. 13.5 30) Colligative properties of solutions include all of the following except __________. A) depression of vapor pressure upon addition of a solute to a solvent B) elevation of the boiling point of a solution upon addition of a solute to a solvent C) depression of the freezing point of a solution upon addition of a solute to a solvent D) an increase in the osmotic pressure of a solution upon the addition of more solute E) the increase of reaction rates with increase in temperature Answer: E Sec. 13.5 13 Solutions 6. A 1.25 M Cu(NO ) 3 2lar mass = 187.56 g/mol) P R A C T I C E T E S T solution has a density of 1.19 g/cm . What is the weight percent Cu(NO ) 3 2 the solution? 1. What is the molality of 7.80% by weight glucose a) 1.88% d) 14.3% (C6H 12 6olar mass = 180.16 g/mol) solution? b) 2.36% e) 19.9% a) 0.470 m d) 0.0454 m c) 10.5% b) 0.845 m e) 0.0844 m c) 0.0432 m 7. Hydrobromic acid (molar mass = 80.9 g/mol) is commercially available in a 34.0 mass percent solution 2. The mol fraction of NH C4 in a solution is 0.0311. which has a density of 1.31 g/cm . What is the What is its molality? molarity of the commercially available hydrobromic (The molar mass of water is 18.016 g/mol.) acid? a) 1.78 m d) 0.562 m a) 2.75 M d) 9.35 M b) 1.66 m e) 0.0983 m b) 4.45 M e) 10.2 M c) 0.969 m c) 5.50 M 3. What is the mol fraction Na SO in a solution which is 2 4 8. The maximum contamination level of arsenic ion in a 11.5% by weight Na S2 (4olar mass Na SO 2= 4 water system is 0.050 parts per million. If the arsenic 142.06 g/mol and H O2= 18.016 g/mol)? is present as AsCl3, how many grams of arsenic a) 0.0810 d) 0.0173 chloride could be present in a system that contains 8.2 5 b) 0.0914 e) 0.0162 x 10 Liters? c) 0.0745 a) 0.55 g d) 62 g b) 7.3 g e) 98 g 4. What is the mol fraction NaNO 3n a solution which is c) 41 g 2.15 m? a) 0.0180 d) 0.09387 9. A student prepared a solution containing 0.30 mol b) 0.0268 e) 0.0785 solute and 1.00 mole solvent. The mole fraction of c) 0.0373 solvent is a) 1.30 d) 0.30 5. A 1.34 M NiCl 2molar mass = 129.6 g/mol) solution b) 1.00 e) 0.23 has a density of 1.12 g/cm . What is the weight c) 0.77 percent NiCl 2of the solution? a) 1.73% d) 25.4% b) 8.64% e) 29.8% c) 15.5% 10. Which measure of concentration is most appropriate 15. What is the primary energetic factor in the lack of for the calculation of the vapor pressure of a solution? miscibility between CCl (l4 and water? a) mol fraction d) weight % a) the strength of intermolecular forces between CCl 4 b) molarity e) ppm molecules c) molality b) the strength of intermolecular forces between H O 2 molecules 11. A chemist knows the empirical formula of a new c) the charge on the C atom in CCl 4 compound but not the molecular formula. What must d) the difference between the molecular weights of be determined experimentally so that the molecular the molecules formula can be determined? e) the electronegativity difference between carbon a) density d) melting point and chlorine b) viscosity e) molar mass c) % composition 16. Which of the following would have a boiling point closes to that of 1 m NaCl? 12. A volumetric flask is necessary for the preparation of a) 1 m sucrose (C H 12)22 11 which one of the following concentration b) pure H O 2 d) 0.5 m CH OH3 measurements? c) 1 m MgCl 2 e) 1 m NH NO4 3 a) molality d) molarity b) X e) ppm 17. Which of the following would have the highest c) mass % freezing point? a) 1 m glucose (C H 6 )12 6 13. If the pressure of a gas over a liquid increases, the b) 1 m MgCl 2 d) 1 m (NH ) 4 2 4 amount of gas dissolved in the liquid will c) 1 m NaNO 3 e) pure H O2 a) increase b) decrease 18. You need a solution that is 0.15 m in ions. How many c) remain the same grams of MgCl (molar mass = 95.2 g/mol) must you 2 d) have a higher vapor pressure dissolve in 400. g of water? (Assume total dissociation e) depends on the polarity of the gas of the ionic salt.) a) 0.060 g d) 7.6 g 14. Which of the following solutions would have the b) 1.9 g e) 17 g lowest vapor pressure? c) 5.7 g a) 1 m glucose (C H 6 )12 6 b) 1 m MgCl d) 1 m NaBr 2 c) 1 m NaNO 3 e) pure H O2 19. A solution is prepared by dissolving 0.500 g of non 22. Concentrated salt solutions have boiling points lower dissociating solute in 12.0 g of cyclohexane. The than those calculated using the equation, freezing point depression of the solution is 8.94C. Tb = Kb ∙ m.∙ i Which of the following is a reasonable The K fpor cyclohexane is 20.0C/m. Calculate the explanation of this observation? molar mass of the solute. a) Positive ions repel each other more at high a) 93.2 g/mol d) 182 g/mol concentration. b) 112 g/mol e) 205 g/mol b) Ions of opposite charge will tend to stay paired c) 128 g/mol instead of breaking up. c) The water molecules will have a greater attraction 20. What is the freezing point of a solution containing for each other. 4.134 grams naphthalene (molar mass = 128.2) d) Concentrated solutions really have small particles dissolved in 30.0 grams paradichlorobenzene? The of nondissolved salt, thus lowering the molality. freezing point of pure paradichlorobenzene is 53.0C e) The difference between the crystal lattice energy and the freezing point depressing constafp K is and the heat of hydration must be taken into 7.10C/m. consideration. a) 52.0C d) 17.6C b) 48.7C e) 7.63C c) 45.4C Answers: 21. What is the molar mass of a compound if 4.28 grams is 1. A 11. E dissolved in 25.0 grams of chloroform solvent to form 2. A 12. D a solution which has a boiling point elevation of 3. E 13. A 2.30C. The boiling point constant of chlorofobp K 4. C 14. B is +3.63C/m. 5. C 15. B a) 34.5 g/mol d) 168 g/mol b) 67.5 g/mol e) 270 g/mol 6. E 16. E c) 135 g/mol 7. C 17. E 8. E 18. B 9. C 19. A 10. A 20. C 21. E 22. B
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