AP Chemistry : Solutions and States of Matter
Study concepts, example questions & explanations for AP Chemistry
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Example Questions
Example Question #11 : Other Solution Concepts
A solution was prepared by diluting 10mL of a 0.500M salt solution to 20mL. What would be the final concentration of this solution?
Use the dilution formula:
Rearranging this equation gives:
Plugging in the values gives:
Therefore, after diluting the solution to 20mL, the solution concentration would be lowered from 0.50M to 0.25M.
Example Question #51 : Solutions
Which of the following is a weak electrolyte?
Solutes that dissociate completely in a solution are called strong electrolytes. Weak electrolytes stay paired to some extent in solutions. As a result, strong electrolytes include ionic compounds and strong acid and bases.
Example Question #11 : Other Solution Concepts
Which of the following definitions is false?
The van't Hoff factor, i, is the number of ions that a compound produces in a solution.
Ion-product constant of water, 
Molality is the number of moles of solute in a solution divided by the number of kilogram of solvent.
Solubility product, 
Solubility product,
Solubility product,
Example Question #11 : Gases
Under which conditions would you expect Ar to deviate the most from ideal behavior?
300K and 5 atm
Ar always behaves ideally
300K and 10 atm
200 K and 10 atm
200 K and 1 atm
200 K and 10 atm
The ideal gas law assumes the gas particles are non-interacting and small relative to the size of their container. At 200K (lowest temperature in the list, and the highest pressure). This gives Ar the most time to interact due to molecular speeds and the high pressure implies the molecular size is not insignificant relative to the container.
Example Question #2 : Deviations From Ideal Gas Law
Would you expect a polar or non polar gas to deviate most from ideal gas behavior?
Polar gases because of hydrogen bonding
Polar gases, because of high dipole-dipole interactions
Non polar gases, because of high dispersion interactions
Non polar gases because of reduced overall intermolecular forces
Both polar and non polar gases behave ideally
Polar gases, because of high dipole-dipole interactions
Polar gases would have increased interactions due to their dipoles that would lead to deviations from ideal gas behavior.
Example Question #102 : Solutions And States Of Matter
Which of the following would behave most like an ideal gas?
All are ideal gases because they are non-polar
Example Question #3 : Deviations From Ideal Gas Law
Why do gases deviate from ideal behavior as the temperature is decreased?
As the temperature is decreased the molecules have less kinetic energy and can’t break the intermolecular interactions between them.
As the temperatures is decreased the molecules become frozen in place.
As the temperature is decreased the molecules have less kinetic energy and can’t maintain the intermolecular forces necessary for ideal gas behavior.
As the temperature is decreased the molecules have more kinetic energy and break the intermolecular interactions keeping them together.
None of the above.
As the temperature is decreased the molecules have less kinetic energy and can’t break the intermolecular interactions between them.
The ideal gas law assumes the gas particles are non-interacting and small relative to the size of their container. As the temperature is decreased the gas molecules are moving slower and allow for a greater degree of interaction.
Example Question #1 : Deviations From Ideal Gas Law
When does a gas behave most like an ideal gas?
At high temperatures, high volume, low intermolecular interactions
At low temperatures, high volume, and low intermolecular interactions
At low volumes, high temperatures, and high intermolecular interactions
At high temperature, high volumes, and high intermolecular interactions
At low temperatures, low volume, low intermolecular interactions
At high temperatures, high volume, low intermolecular interactions
The ideal gas law assumes the gas particles are non-interacting and small relative to the size of their container. At high temperatures the gas molecules are moving fast enough to shorten the time scale for any interactions. At high volumes, the molecular size becomes small relative to the size of the container, and the low interactions mean the molecules act more independently.
Example Question #61 : Solutions
Which of these solutions can be separated via chromatography?
Soil and water
A homogeneous solution of organic solvents
B and C
None of the above
Ethanol and water
B and C
Chromatography is the physical separation of components of a mixture. Answers b and c can be separated by chromatography due to their homogeneous nature. The soil and water example would be separated by filtration.
Example Question #62 : Solutions
Which of the following would most likely form a homogeneous solution?
All would form homogeneous solutions
A and B
Water and benzene (C6H6)
NH4Cl and water
NaNO3 and octanol (C8H18O)
NH4Cl and water
Like dissolves like. The NH4Cl and water mixture involves an ionic solid and a polar solvent. Examples a and b involve mixing polar/non-polar solvents and ionic and non-polar solvents.
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