University of Kentucky Clicker Questions Chapter 12 Solutions Allison Soult University of Kentucky

Which of the following pairs is likely to form a homogeneous mixture? LiI and Hg C6H14 and Br2 CH3OH and C6H6 CCl4 and H2O All pairs above are miscible. Answer: b

Which of the following pairs is likely to form a homogeneous mixture? LiI and Hg C6H14 and Br2 CH3OH and C6H6 CCl4 and H2O All pairs above are miscible. Answer: b

Why is chloroform, CHCl3, more soluble in water than is carbon tetrachloride, CCl4? CCl4 is nonpolar and has stronger solute–solute interactions. CHCl3 is polar and has stronger solute–solute interactions. CHCl3 is polar and has stronger solute–solvent interactions. CCl4 is nonpolar and has an exothermic ΔHsolute. Answer: c

Why is chloroform, CHCl3, more soluble in water than is carbon tetrachloride, CCl4? CCl4 is nonpolar and has stronger solute–solute interactions. CHCl3 is polar and has stronger solute–solute interactions. CHCl3 is polar and has stronger solute–solvent interactions. CCl4 is nonpolar and has an exothermic ΔHsolute. Answer: c

Which of the following statements is NOT true? All soluble ionic compounds become more soluble with increasing temperature. Additional solvent cannot dissolve in a saturated solution. Some ionic compounds become less soluble with increasing temperature. Supersaturated solutions are very stable. Answer: d

Which of the following statements is NOT true? All soluble ionic compounds become more soluble with increasing temperature. Additional solvent cannot dissolve in a saturated solution. Some ionic compounds become less soluble with increasing temperature. Supersaturated solutions are very stable. Answer: d

A pressure of 3. 5 atm in CO2 is required to maintain a 0 A pressure of 3.5 atm in CO2 is required to maintain a 0.12 M CO2 concentration in soda. Calculate the Henry’s Law constant for CO2. 29.2 0.42 2.9 × 101 3.4 × 10–2 4.2 Answer: d

A pressure of 3. 5 atm in CO2 is required to maintain a 0 A pressure of 3.5 atm in CO2 is required to maintain a 0.12 M CO2 concentration in soda. Calculate the Henry’s Law constant for CO2. 29.2 0.42 2.9 × 101 3.4 × 10–2 4.2 Answer: d

On a clear day at sea level, the partial pressure of N2 in air is 0 On a clear day at sea level, the partial pressure of N2 in air is 0.78 atm at 25°C. Under these conditions, the concentration of N2 in water is 5.3 × 10–4 M. What is the partial pressure of N2 when the concentration in water is 1.1 × 10–3 M? 0.63 atm 0.78 atm 1.0 atm 2.1 atm 1.6 atm Answer: e

On a clear day at sea level, the partial pressure of N2 in air is 0 On a clear day at sea level, the partial pressure of N2 in air is 0.78 atm at 25°C. Under these conditions, the concentration of N2 in water is 5.3 × 10–4 M. What is the partial pressure of N2 when the concentration in water is 1.1 × 10–3 M? 0.63 atm 0.78 atm 1.0 atm 2.1 atm 1.6 atm Answer: e

Which of the following solutions has its solubility most strongly dependent on pressure? 0.05 m NaCl 0.05 m C6H12O6 0.02 m Al(NO3)3 0.005 m CO2 0.02 m NH4Cl Answer: d

Which of the following solutions has its solubility most strongly dependent on pressure? 0.05 m NaCl 0.05 m C6H12O6 0.02 m Al(NO3)3 0.005 m CO2 0.02 m NH4Cl Answer: d

Some KCl precipitates out of solution. A room-temperature solution is saturated in both KCl and CO2. When the solution is heated to near boiling, which of the following is most likely to occur? Some KCl precipitates out of solution. Some CO2 bubbles out of solution. Some CO2 bubbles out of solution and some KCl precipitates. Nothing is likely to happen. Answer: b

Some KCl precipitates out of solution. A room-temperature solution is saturated in both KCl and CO2. When the solution is heated to near boiling, which of the following is most likely to occur? Some KCl precipitates out of solution. Some CO2 bubbles out of solution. Some CO2 bubbles out of solution and some KCl precipitates. Nothing is likely to happen. Answer: b

not possible to calculate A solution of ammonia is made by dissolving 35 g of NH3 in 90.0 g of H2O. The density of the solution is 0.898 g/mL. What is the molarity of NH3? 53 M 0.39 M 23 M 15 M not possible to calculate Answer: d

not possible to calculate A solution of ammonia is made by dissolving 35 g of NH3 in 90.0 g of H2O. The density of the solution is 0.898 g/mL. What is the molarity of NH3? 53 M 0.39 M 23 M 15 M not possible to calculate Answer: d

What is the molality a 4. 0 M NaOH solution What is the molality a 4.0 M NaOH solution? The density of the solution is 1.04 g/mL. 0.15 m 4.5 m 0.18 m 4.0 m 3.8 m Answer: b

What is the molality a 4. 0 M NaOH solution What is the molality a 4.0 M NaOH solution? The density of the solution is 1.04 g/mL. 0.15 m 4.5 m 0.18 m 4.0 m 3.8 m Answer: b

What is the mass percent of a solution prepared from 15 g of NaCl in 45 g of H2O? 33% 25% 50% 15% Answer: b

What is the mass percent of a solution prepared from 15 g of NaCl in 45 g of H2O? 33% 25% 50% 15% Answer: b

The glucose solution has the higher vapor pressure. Consider two solutions: (1) 10 g of glucose (C6H12O6) in 1 L of water and (2) 10 g of sucrose (C12H22O11) in 1 L of water. Which of the following is true? The glucose solution has the higher vapor pressure. The sucrose solution has the higher vapor pressure. Both solutions have the same vapor pressure. There is not enough information to compare vapor pressures. Answer: b

The glucose solution has the higher vapor pressure. Consider two solutions: (1) 10 g of glucose (C6H12O6) in 1 L of water and (2) 10 g of sucrose (C12H22O11) in 1 L of water. Which of the following is true? The glucose solution has the higher vapor pressure. The sucrose solution has the higher vapor pressure. Both solutions have the same vapor pressure. There is not enough information to compare vapor pressures. Answer: b

Lauryl alcohol, a component of coconut oil, is used to make detergents Lauryl alcohol, a component of coconut oil, is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1°C. What is the molar mass of lauryl alcohol? Kf (benzene) = 5.12°C/m; Tf (benzene) = 5.50°C. 270 g/mol 13.7 g/mol 62.4 g/mol 46.5 g/mol 183 g/mol Answer: e

Lauryl alcohol, a component of coconut oil, is used to make detergents Lauryl alcohol, a component of coconut oil, is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1°C. What is the molar mass of lauryl alcohol? Kf (benzene) = 5.12°C/m; Tf (benzene) = 5.50°C. 270 g/mol 13.7 g/mol 62.4 g/mol 46.5 g/mol 183 g/mol Answer: e

Which of the following solutions will have the largest osmotic pressure? 0.50 m C6H12O6 b) 0.50 m NaCl 0.50 m K2SO4 d) 0.50 m FeCl3 Answer: d

Which of the following solutions will have the largest osmotic pressure? 0.50 m C6H12O6 b) 0.50 m NaCl 0.50 m K2SO4 d) 0.50 m FeCl3 Answer: d

What is the ideal van’t Hoff factor for Mg(NO2)2? 3 4 6 7 Answer: b

What is the ideal van’t Hoff factor for Mg(NO2)2? 3 4 6 7 Answer: b

Which of the following has the highest boiling point? 0.05 m NaCl 0.05 m C6H12O6 0.02 m Al(NO3)3 0.005 m CO2 0.02 m NH4Cl Answer: a

Which of the following has the highest boiling point? 0.05 m NaCl 0.05 m C6H12O6 0.02 m Al(NO3)3 0.005 m CO2 0.02 m NH4Cl Answer: a

What concentration of NaCl (i = 1 What concentration of NaCl (i = 1.9) will have the same boiling point as a 0.50 m glucose solution? 0.95 m 1.9 m 0.26 m 0.50 m 3.8 m Answer: c

What concentration of NaCl (i = 1 What concentration of NaCl (i = 1.9) will have the same boiling point as a 0.50 m glucose solution? 0.95 m 1.9 m 0.26 m 0.50 m 3.8 m Answer: c