Solutions and Solubility Curves

Multiple Choice

Which of the following refers to the substance that is being dissolved in a solution?

• solvent

• solute

• mixture

Multiple Choice

In sweet tea the solvent would be

• water

• tea

• sugar

• lemon

Multiple Choice

Which of the following is a solvent?

• Salt

• Water

• Sugar

• Oxygen

Multiple Choice

Electrolytes contain atoms from what type of bonds that help them conduct electricity?

• Ionic

• Covalent

• Metallic

• Polar

Multiple Choice

What type of bonds form partial charges allowing it to dissolve or like molecules?

• Non-polar covalent bonds

• Ionic bonds

• Polar covalent bonds

• Metallic bonds

Multiple Choice

What type of molecules consist of ions and can conduct electricity?

• Water

• Solutions

• Electrolytes

Multiple Choice

What property of water makes it an excellent solvent?

• Its solid state density

• Its molecular weight

• Its polarity

• Its boiling point

Multiple Choice

Which of the following is a reason why oil (a non-polar substance) does not mix with water?

• Oil molecules are too large to interact with water molecules

• Oil and water have the same density

• Oil molecules cannot bonds with water molecules due to intermolecular forces

• Oil is denser than water

Multiple Choice

What type of substance dissolves in water but does not form ions or conduct electricity?

• electrolyte

• nonelectrolyte

• saturated

• insoluble

Multiple Choice

The freezing point of a solution is ____ the freezing point of the pure solvent.

• the same as
• lower than
• higher than
• no relation to

Multiple Choice

The boiling point of a solution is ______ the boiling point of the pure solvent.

• higher than
• the same as
• lower than
• higher or lower than

Multiple Choice

Electrolytes have a greater effect on colligative properties than nonelectrolytes do because electrolytes

• are volatile

• have higher boiling points

• produce fewer moles of solute particles per mole of solvent

• produce more moles of solute particles per mole of solvent

Match

Match the following descriptions to the correct type of electrolyte:

• Weak electrolytes

• Non-electrolytes

• Strong electrolytes

• Insulators

Compounds whose aqueous solutions conduct electricity poorly due to partial dissociation of ions

Compounds whose aqueous solutions do not conduct electricity because they do not dissociate into ions

Compounds whose aqueous solutions conduct electricity effectively due to complete dissociation of ions

Materials that do not conduct electricity

• Compounds whose aqueous solutions conduct electricity poorly due to partial dissociation of ions

• Compounds whose aqueous solutions do not conduct electricity because they do not dissociate into ions

• Compounds whose aqueous solutions conduct electricity effectively due to complete dissociation of ions

• Materials that do not conduct electricity

Explanation Slide...

Compounds that can conduct electricity effectively due to complete dissociation of ions are called strong electrolytes.

Multiple Choice

What happens to NaCl when it is dissolved in water?

• A) It forms a precipitate

• B) It decomposes into gases

• C) It dissociates into Na+ and Cl- ions

• D) It reacts to form a new compound

Explanation Slide...

When NaCl is dissolved in water, it dissociates into Na+ and Cl- ions, which are surrounded by water molecules due to their charges.

Match

Match the following numbers of moles produced when dissolved in solution to their corresponding compounds.

• 2 moles

• 3 moles

• 4 moles

• 5 moles

NaCl dissolved in solution produces:

MgCl2 dissolved in solution produces:

Al2(SO4)3 dissolved in solution produces:

K2SO4 dissolved in solution produces:

• NaCl dissolved in solution produces:

• MgCl2 dissolved in solution produces:

• Al2(SO4)3 dissolved in solution produces:

• K2SO4 dissolved in solution produces:

Explanation Slide...

When MgCl2 is dissolved, it produces 3 moles of ions: 1 mole of Mg2+ ions and 2 moles of Cl- ions, totaling 3 moles of ions.

Multiple Choice

The exposed area of a solid; expressed as squared units of length

• Volume

• Surface Area

• Molarity

• Solubility

Multiple Choice

The stirring or mixing of a solution as to increase the particle movement of the solute particles in solution

• Agitation

• Settling

• Falling Out

• Crystallization

Multiple Choice

Most substances increase in solubility as temperature increases, why don't HCl, NH₃, and SO₂?

• They are insoluble in water

• They are all non-polar

• They are all polar

• They are all gases

Multiple Choice

If you halve the amount of water you dissolve a solute in (so 50 g instead of 100 g of water), what do you do to the amount of solute to find the saturation point?

• Halve it

• Leave it alone

• Double it

• Quadruple it

Multiple Choice

If you have 250 g of water, how many grams of NH₃ will dissolve in 40 ^oC water?

• 40 g

• 60 g

• 80 g

• 100 g

Multiple Choice

How many grams of KNO₃ will fall out of solution if 145 g are dissolved in 60^oC water?

• 40 g

• 35g

• 30 g

• 25 g

Multiple Choice

How many more grams of NaNO₃ do you need to 85 g of the solute in 70 ^oC of water?

• 135 g

• 50 g

• 85 g

• 25 g

Multiple Choice

Which substance is MOST soluble at 0^oC?

• KI

• NaNO₃

• NaCl

• Ce₂(SO₄)₃

Multiple Choice

How many grams of K₂Cr₂O₇, are soluble in 100 g of water at 95^oC?

• 83 grams

• 75 grams

• 40 grams

• 12 grams

Multiple Choice

At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K₂Cr₂O₇?

• 60^oC

• 30^oC

• 50^oC

• 83^oC

Multiple Choice

When 42 grams of potassium chloride, KCl, is dissolved in 100 grams of water at 50^oC, the solution can be correctly described as:

• supersaturated

• saturated

• unsaturated

Multiple Choice

When 20 grams of potassium chlorate, KClO3, is dissolved in 100 g of water at 80oC, the solution can be correctly describe as:

• supersaturated

• saturated

• unsaturated

Multiple Choice

What temperature does the solubility of NaCl match KNO₃?

• 50^oC

• 40^oC

• 35^oC

• 25^oC

Multiple Choice

Generally, for gases dissolving in liquids, how does an increase in temperature affect the solubility of the gas?

• decreases solubility
• increases solubility
• has no effect

Multiple Choice

Which of the following would result in being able to dissolve a greater amount of gas in a solution?

• Lower the temperature of the solution.

• Decrease the pressure of the solution.

• Stir the solution.

• Heat the solution.

Multiple Choice

You have some leftover soda after a party. Eventually, the soda will go flat. Which of the following options will slow the rate at which the CO_² gas escapes?

• Stir the soda.

• Store the soda bottle in the fridge.

• Store the soda in your hot car.

• Store the soda bottle in the room temperature cabinet.

Multiple Choice

Which solute is most likely a gas?

• NH₃

• NaNO₃

• KCl

• NaCl

Multiple Choice

Graph that shows the amount of solute that can be dissolved in 100 g of water at a certain temperature.

• Solubility curve
• Saturation curve
• Concentration curve
• Molarity curve