1. Chapter 13 PROPERTIES OF SOLUTIONS
Go Figure
Clicker Questions
Chapter 13 PROPERTIES OF SOLUTIONS
Lynn Mandeltort
Auburn University

3. What aspect of the kinetic theory of gases tells us that the gases will mix?
The gas molecules experience perfectly elastic collisions.
The gas molecules experience no intermolecular forces.
The gas molecules move constantly and randoml.y
The two types of molecules, Ar and O2 are attracted to each other.
Answer: c

4. What aspect of the kinetic theory of gases tells us that the gases will mix?
The gas molecules experience perfectly elastic collisions.
The gas molecules experience no intermolecular forces.
The gas molecules move constantly and randomly.
The two types of molecules, Ar and O2 are attracted to each other.
Answer: c

6. Why does the oxygen atom in H2O point toward Na+ in the ion–dipole interaction?
The electron-poor O atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
The electron-poor H atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
The electron-rich O atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
The electron-rich H atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
Answer: c

7. Why does the oxygen atom in H2O point toward Na+ in the ion–dipole interaction?
The electron-poor O atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
The electron-poor H atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
The electron-rich O atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
The electron-rich H atom in O—H bond dipole in H2O is attracted to Na+ ion by electrostatic attraction.
Answer: c

9. How does the orientation of H2O molecules around Na+ differ from that around Cl–?
The H atom of a water molecule points toward a Na+ ion, and the O atom of a water molecule points toward the Cl– ion.
The H atom of a water molecule points toward a Cl– ion, and the O atom of a water molecule points toward the Na+ ion.
Answer: b

10. How does the orientation of H2O molecules around Na+ differ from that around Cl–?
The H atom of a water molecule points toward a Na+ ion, and the O atom of a water molecule points toward the Cl– ion.
The H atom of a water molecule points toward a Cl– ion, and the O atom of a water molecule points toward the Na+ ion.
Answer: b

12. How does the magnitude of ΔHmix compare with the magnitude of ΔHsolute + ΔHsolvent for exothermic solution processes?
Larger
Almost the same
Smaller
Answer: a

13. How does the magnitude of ΔHmix compare with the magnitude of ΔHsolute + ΔHsolvent for exothermic solution processes?
Larger
Almost the same
Smaller
Answer: a

15. What is the molar mass of nickel chloride hexahydrate, NiCl2 · 6H2O(s)?
58.69 g/mol
g/mol
g/mol
g/mol
Answer: a

16. What is the molar mass of nickel chloride hexahydrate, NiCl2 · 6H2O(s)?
58.69 g/mol
g/mol
g/mol
g/mol
Answer: a

18. What is the evidence that the solution in the left photograph is supersaturated?
The solution is clear.
There would be no crystallization after adding a seed crystal without the solution being supersaturated.
Answer: b

19. What is the evidence that the solution in the left photograph is supersaturated?
The solution is clear.
There would be no crystallization after adding a seed crystal without the solution being supersaturated.
Answer: b

21. If the partial pressure of a gas over a solution is doubled, how has the concentration of gas in the solution changed after equilibrium is restored?
Concentration of gas in the solution does not change.
Concentration of gas in the solution decreases by a factor of one-half.
Concentration of gas in the solution increases by a factor of two.
Concentration of gas in the solution increases by a factor of four.
Answer: c

22. If the partial pressure of a gas over a solution is doubled, how has the concentration of gas in the solution changed after equilibrium is restored?
Concentration of gas in the solution does not change.
Concentration of gas in the solution decreases by a factor of one-half.
Concentration of gas in the solution increases by a factor of two.
Concentration of gas in the solution increases by a factor of four.
Answer: c

24. How do the slopes of the lines vary with the molecular weight of the gas? Explain the trend.
The slopes increase linearly as the molecular weights increase. Increasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
The slopes exponentially increase as the molecular weights increase. Increasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
The slopes increase linearly as the molecular weights decrease. Decreasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
The slopes exponentially decrease as the molecular weights decrease. Decreasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
Answer: a

25. How do the slopes of the lines vary with the molecular weight of the gas? Explain the trend.
The slopes increase linearly as the molecular weights increase. Increasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
The slopes exponentially increase as the molecular weights increase. Increasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
The slopes increase linearly as the molecular weights decrease. Decreasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
The slopes exponentially decrease as the molecular weights decrease. Decreasing molecular mass leads to greater polarizability of the gas molecules and greater intermolecular attractions between gas and water molecules.
Answer: a

27. How does the solubility of KCl at 80 °C compare with that of NaCl at the same temperature?
NaCl is more soluble.
KCl is more soluble.
NaCl and KCl have about the same solubility.
Answer: b

28. How does the solubility of KCl at 80 °C compare with that of NaCl at the same temperature?
NaCl is more soluble.
KCl is more soluble.
NaCl and KCl have about the same solubility.
Answer: b

30. Where would you expect N2 to fit on this graph?
Just below CH4 and above O2
Just below O2 and above CO
Just below CO and above He
Just below He
Answer: c

31. Where would you expect N2 to fit on this graph?
Just below CH4 and above O2
Just below O2 and above CO
Just below CO and above He
Just below He
Answer: c

33. If the pure water in the left arm of the U-tube is replaced by a solution more concentrated than the one in the right arm, what will happen?
Nothing
Water flows through the semipermeable membrane from the more dilute solution to the more concentrated solution, and the liquid level in the left arm rises.
Water flows through the semipermeable membrane from the more concentrated solution to the more dilute solution, and the liquid level in the right arm rises.
Answer: b

34. If the pure water in the left arm of the U-tube is replaced by a solution more concentrated than the one in the right arm, what will happen?
Nothing
Water flows through the semipermeable membrane from the more dilute solution to the more concentrated solution, and the liquid level in the left arm rises.
Water flows through the semipermeable membrane from the more concentrated solution to the more dilute solution, and the liquid level in the right arm rises.
Answer: b

36. If the fluid surrounding a patient’s red blood cells is depleted in electrolytes, is crenation or hemolysis more likely to occur?
Crenation, because fluid moves from the external fluids into the blood cells.
Crenation, because fluid moves from the blood cells to the external fluids.
Hemolysis, because fluid moves from the external fluids into the blood cells.
Hemolysis, because fluid moves from the blood cells into the external fluids.
Answer: c

37. If the fluid surrounding a patient’s red blood cells is depleted in electrolytes, is crenation or hemolysis more likely to occur?
Crenation, because fluid moves from the external fluids into the blood cells.
Crenation, because fluid moves from the blood cells to the external fluids.
Hemolysis, because fluid moves from the external fluids into the blood cells.
Hemolysis, because fluid moves from the blood cells into the external fluids.
Answer: c

39. What is the chemical composition of the groups that carry a negative charge?
Both groups contain –NH2–.
Both groups contain –COH–.
Both groups contain –CH3–.
Both groups contain –CO2–.
Answer: c

40. What is the chemical composition of the groups that carry a negative charge?
Both groups contain –NH2–.
Both groups contain –COH–.
Both groups contain –CH3–.
Both groups contain –CO2–.
Answer: c

42. Which kind of intermolecular force attracts the stearate ion to the oil drop?
Ion–dipole forces [hydrophilic end of stearate ion to polar oil drop]
Dipole–induced dipole forces [hydrophobic end of stearate ion to nonpolar oil drop]
Dipole–dipole forces [hydrophilic end of stearate ion to polar oil drop]
Dispersion forces [hydrophobic end of stearate ion to nonpolar oil drop]
Answer: d

43. Which kind of intermolecular force attracts the stearate ion to the oil drop?
Ion–dipole forces [hydrophilic end of stearate ion to polar oil drop]
Dipole–induced dipole forces [hydrophobic end of stearate ion to nonpolar oil drop]
Dipole–dipole forces [hydrophilic end of stearate ion to polar oil drop]
Dispersion forces [hydrophobic end of stearate ion to nonpolar oil drop]
Answer: d