Solutions Test Review

Solutions Test Review

Multiple Choice

The _____is the part that gets dissolved.

• solute

• solvent

• solution

• Sacajawea

Multiple Choice

The amount of solute that can be dissolved in a specific amount of solvent at a given temperature is its

• concentration.

• density.

• dilution.

• solubility.

Multiple Choice

A solution that contains all of the solute it can hold at a given temperature is

• diluted.

• saturated.

• supersaturated.

• unsaturated.

Multiple Choice

Which would NOT increase the rate at which a sugar cube dissolves?

• Reducing the amount of solvent

• Crushing the sugar cube

• Stirring the solution

• Heating the solvent

Multiple Choice

The reason why water is able to dissolve many ionic compounds, such as table salt (NaCl), is because

• water is polar covalent and the partially positive hydrogens pull the cationios out of the salt crystal
• water is polar covalent and the partially negative oxygens pull the cations out of the crystal
• water is polar covalent and the partially negative oxygens pull the anions out of the crystal
• water is an ionic compound and the negative ion of oxygen pulls out the positive ion of sodium

Multiple Choice

What does "like dissolves like" mean?

• polar solvents dissolve in polar solutes

• polar solutes dissolve in polar solvents

• non-polar solvents dissolve in polar solutes

• non-polar solutes dissolve in polar solvents

Multiple Choice

____________ is the process whereby particles of a solvent completely surround the particles of a solute, disperse them throughout the solvent particles, and hold them in solution.

• solvation

• immisciblation

• dissolution

• saturation

Multiple Choice

Since "like dissolves like", water and oil will not mix because

• both of them are polar

• both of them are nonpolar

• oil is polar and water is nonpolar

• oil is nonpolar and water is polar

Multiple Choice

Three 10 g samples of sugar are represented below.

Sample A dissolves in water more slowly than sample B.

Sample B dissolves more slowly than sample C.

Which of the following best explains why sample A dissolves more slowly than the other two?

• It has the most volume.

• It has the smallest surface area.

• It has the largest number of sugar molecules.

• It has the fewest bonds between sugar modules.

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

Which of the following would increase the rate of dissolution of a solid?

• Cool the solution.

• Decrease the surface area of the solute.

• Increase the polarity of the solution.

• Break the solute into smaller particles.

Multiple Choice

Which of the following statements is true?

• An increase in temperature decreases the solubility of most solids, but increases the solubility of gases.

• An increase in temperature increases the solubility of most solids and gases.

• An increase in temperature decreases the solubility of most solids and gases.

• An increase in temperature increases the solubility of most solids, but decreases the solubility of gases.

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 CO2 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

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

• supersaturated
• saturated
• unsaturated

Multiple Choice

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

• supersaturated
• unsaturated
• saturated

Multiple Choice

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

• supersaturated
• saturated
• unsaturated

Multiple Choice

Which solute does not increase in solubility as temperature rises?

• NH₃
• NaNO₃
• KNO₃
• NaCl

Multiple Choice

Which solute is the most soluble at 10 ⁰C?

• KI
• KClO₃
• NH₄Cl
• NH₃

Multiple Choice

A technican prepared a solution by heating 100 mL of distilled water while adding KCl crystals until no more KCl would dissolve. She then capped the clear solution and set it aside on the lab counter. After several hours she noticed the solution had become cloudly and some solid had settled to the bottom of the flask. Which statement best describes what happened?

• As the solution cooled, evaporation of water increased the KCl concentration beyond its solubility.

• Water molecules, trapped with the KCl crystals, were released after heating.

• At lower temperatures the solubility of KCl decreased and recrystallization occurred.

• At increased temperatures the solubility of KCl increased and remained too high after cooling.

Multiple Choice

How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?

• 1074 mol
• 0.069 mol
• 1.07 mol
• 62.7 mol

Multiple Choice

What is the percent by mass of a solution containing 56.5 g of salt in 500 g of water?

• 11.3 %

• 5.56%

• 8.85%

• 10.2 %

Multiple Choice

What is the percent concentration of sugar in pink lemonade if 28 g of sugar is added to 209 g of water?

• 14.7 %

• 5.14 %

• 13.4 %

• 8.47 %

• 11.8 %

Multiple Choice

What mass of water should be added to 22.0 g of KCl to make 5.50% by mass solution?

• 400 g

• 40 g

• 0.25 g

• 25 g

Multiple Choice

What is the percent by mass of a sugar solution where 10 grams of sugar is added to 100 grams of water?

• .10%

• 0.091%

• 9.1%

Multiple Choice

How many grams of AgNO₃ (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 

• .03g
• 0.5g
• 5.3g
• 84.9g

Multiple Choice

Find the molarity of 186.55 g of sucrose, C₁₂H₂₂O₁₁ (MM = 342) in 250 mL of water.

• 2.18 M
• 0.746 M
• 1.18 M
• 0.545 M

Multiple Choice

How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?

• 0.625 g NaCl
• 625 g NaCl
• 36.5 g NaCl
• 0.04 mol NaCl

Multiple Choice

Rank the following solutes from least to greatest effect on freezing point:

KI, CH₃OH, Li₃PO₄, CaCl₂

• KI, CH₃OH, Li₃PO₄, CaCl₂

• Li₃PO₄, CaCl₂, KI, CH₃OH

• Li₃PO₄, CH₃OH, CaCl₂, KI

• CH₃OH, KI, CaCl₂, Li₃PO₄

Multiple Choice

Which type of solute affects colligative properties like freezing point and boiling point the LEAST?

• ionic because they dissociate into at least 2 solute particles

• ionic because they are non-dissociative and always pull into one molecule at a time

• covalent because they dissociate into at least 2 solute particles

• covalent because they are non-dissociative and always pull into one molecule at a time

Multiple Choice

Which of the following statements is TRUE?

• Ionic solutes affect colligative properties more than covalently bonded solutes because they produce more moles of solute in solution.

• Ionic solutes affect colligative properties less than covalently bonded solutes because they produce less moles of solute in solution.

• Covalent solutes affect colligative properties more than ionically bonded solutes because they produce more moles of solute in solution.

• Covalent solutes affect colligative properties less than ionically bonded solutes because they produce more moles of solute in solution.

Multiple Choice

Which salt below has the largest effect on freezing point?

• C₂H₄O₂

• H₂S

• LiBr

• CaF₂

Multiple Choice

125.0 mL of 2.00 M calcium hydroxide solution is diluted to a concentration of 1.50 M. How many mL of water was added to the original volume?

• 167 mL

• 42.0 mL

• 93.8 mL

• 0.0240 mL

Multiple Choice

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO₃ to a volume of 250.0 mL?

• 15.9 M

• 0.636 M

• 0.642 M

• 1.59 M

Multiple Choice

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

• 0.067 mL

• 60.0 mL

• 100 mL

• 125 mL

Multiple Choice

A dilution is when

• solute is added to the volume of solution

• water is added to the volume of solution

• solute is removed from the volume of solution

• water is removed from the volume of solution