Page 1 of 5 Chapter 11 Learning Objectives 1 Define the terms solute solvent solution and aqueous solution 2 Define and differentiate nonelectrolytes weak electrolytes and strong electrolytes Note you are not responsible for content on electrolytes 1 HCl KOH LiCl and KI are ALL classified as A nonelectrolytes B weak electrolytes C strong electrolytes D acids 2 Which of the following is a strong electrolyte B NH4NO3 C H2O A CH4 D CH3OH E CCl4 3 Which of the following is a nonelectrolyte when dissolving in water A HCl B NaNO3 C CH3CH2OH D CuCl2 E NaOH 4 Three different substances A2X A2Y and A2Z were dissolved in water with the following results Water molecules are omitted for clarity Which of the substances is the strongest electrolyte and which is the weakest A2Y A2X A2Z A A2Y is the strongest electrolyte and A2Z is the weakest electrolyte B A2Z is the strongest electrolyte and A2Y is the weakest electrolyte C A2X is the strongest electrolyte and A2Y is the weakest electrolyte D A2Y is the strongest electrolyte and A2X is the weakest electrolyte 3 Define solubility and differentiate unsaturated saturated and supersaturated solutions 5 A solution containing more than the equilibrium amount is called A an unsaturated solution B a dilute solution C a supersaturated solution D a concentrated solution E a saturated solution 6 Which statement is correct A A saturated solution involves a dynamic equilibrium between dissolving and recrystallization B A saturated solution always contains a high concentration of solute C The solubility of solids always decreases with increasing temperature D The solubility of a gas usually increases with increasing temperature Page 2 of 5 7 A saturated solution was made by dissolving a solid into a liquid Which of the following is NOT TRUE in a dynamic equilibrium describing the saturated solution A Concentration of dissolved solute remains constant B Rate of dissolving is double the rate of crystallization C Solid dissolves into solution D Solid crystallizes from solution E Quantity of undissolved solute remains constant 8 Determine whether the following solutions are unsaturated saturated or supersaturated Right figure a 25 g of KNO3 per 100 0 g of water at 25 C Below the solubility curve unsaturated b 45 g of KNO3 per 100 0 g of water at 25 C Above the solubility curve supersaturated c 20 g of KNO3 per 50 0 g of water at 25 C 20 g solute in 50 g H2O is equivalent to 40 g solute in 100 g H2O Then you can use the graph Above the solubility curve supersaturated 9 45 g of KNO3 per 100 0 g of water is cooled from 40 C to 0 C What happens during cooling top figure There is 45 g KNO3 per 100 g H2O Solubility at 40 C is 63 g per 100 g H2O and solubility at 0 C is 14 g per 100 g H2O So 31 g of KNO3 will precipitate out of the solution 4 Describe the effect of temperature and pressure on solubility 10 Which of the following statements is generally TRUE A The solubility of a solid is not dependent on either temperature or pressure B The solubility of a solid is highly dependent on pressure C The solubility of a solid is highly dependent on both pressure and temperature D The solubility of a solid is highly dependent on temperature E None of the above 11 Which of the following does not affect the solubility of a covalent solute in a given solvent A polarity of the solvent B polarity of the solute C rate of stirring D temperature of the solvent and solute Page 3 of 5 5 Define solve for and convert between Molarity molality and mole fraction 12 Commercial nitric acid is 16 0 M HNO3 aq and has a density of 1 42 g mL What is the mole fraction of HNO3 in this solution The molar mass of nitric acid is 63 018 g mol A 0 412 B 0 169 C 0 699 D 0 704 13 What is the molarity of a saturated solution of potassium sulfate K2SO4 if the solubility is 13 g per 100 g H2O at 25 C The density of the solution is 1 1 g mL The molar mass of potassium sulfate is 174 27 g mol A 1 1 M B 0 14 M C 0 82 M D 0 73 M E 0 96 M 14 A solution is prepared by dissolving 17 75 g sulfuric acid H2SO4 in enough water to make 100 0 mL of solution If the density of the solution is 1 1094 g mL what is the molality Molar mass of sulfuric acid is 98 086 g mol A 1 810 m H2SO4 B 0 1810 m H2SO4 C 0 1775 m H2SO4 D 1 943 m H2SO4 15 A solution is prepared by dissolving 38 6 g sucrose C12H22O11 in 495 g of water Determine the mole fraction of sucrose A 4 09 10 3 B 7 80 10 2 C 1 28 10 3 D 7 23 10 2 E 2 45 10 3 16 A solution is 0 0480 m LiF What is the molarity of the solution if the density is 1 10 g mL A 0 0441 M B 0 0480 M C 0 0436 M D 0 0528 M E 0 0417 M 17 At 20 C a 2 32 M aqueous solution of ammonium chloride has a density of 1 0344 g mL What is the molality of ammonium chloride in the solution The molar mass of NH4Cl is 53 50 g mol A 2 55 m B 0 0449 m C 2 32 m D 0 446 m E 12 00 m 18 Calculate the molality of a solution that is prepared by mixing 25 5 mL of CH3OH d 0 792 g mL and 387 mL of CH3CH2CH2OH d 0 811 g mL A 0 630 m B 0 812 m C 1 57 m D 2 01 m E 4 98 m 6 Define and provide examples of colligative properties 19 Identify the colligative property A vapor pressure lowering B freezing point depression C boiling point elevation D osmotic pressure Page 4 of 5 E all of the above 20 Which statement is NOT true regarding colligative properties A Raoult s Law describes the vapor pressure above a solution B Since the vapor pressure of the solvent is lowered by a nonvolatile solute the boiling point of the solution is higher C The magnitude depends on the concentration of solute D The magnitude depends on the identity of the solute E The magnitude depends on whether the solute is an electrolyte or not 7 For the colligative property relationships be able to conceptually describe and mathematically solve for a missing value a Raoult s Law to determine the vapor pressure of a solution for either a nonvolatile or volatile solute 21 Determine the vapor pressure of a solution at 25 C that contains 76 6 g of glucose C6H12O6 in 250 0 mL of water The vapor pressure of pure water …