Unit 8 – Solutions Review Game

Unit 8 – Solutions Review Game

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Question 1

• Describes two or more liquids that can dissolve into each other in various proportions.

Answer: Miscible

Question 2

• A student is trying to determine if a liquid is a colloid, solution or suspension. The student cannot see through the mixture and the particles are not settling out. The liquid should be classified as a _______________________.

Answer: Colloid

Question 3

• How can the solubility of a gas be increased?

Answer: Increase pressure, decrease temp, decrease agitation

Question 4

• A compound that concentrates at the boundary surface between two immiscible phases (solid-liquid, liquid-liquid, or liquid-gas).

Answer: Surfactant

Question 5

• What does not experience the Tyndall effect?

Answer: Solutions or homogeneous mixtures

Question 6

• The law that relates partial pressure of a gas to its solubility is ____________________.

Answer: Henry’s Law

Question 7

• How do we change mg into grams?

Answer: divide by 1000

Question 8

• Carbon dioxide in water is an example of which solute-solvent combination?

Answer: Gas-liquid

Question 9

• This can be used to separate a solid from a liquid using heat.

Answer: Evaporation

Question 10

• Describes two or more liquids that do not mix with each other.

Answer: Immiscible

Question 11

• Silver and gold is an example of which solute-solvent combination?

Answer: solid-solid

Question 12

• What is symbolized by a capital M?

Answer: Molarity

Question 13

• This process can be used to separate two liquids that have different boiling points.

Answer: Distillation

Question 14

• A sample of 1500.0 g of drinking water is found to contain 42 mg Pb. What is this concentration in parts per million?

Answer: 28 ppm

Question 15

• The ability of one substance to dissolve in another at a given temperature and pressure.

Answer: Solubility

Question 16

• Name two ways that concentration is expressed.

Answer: Molarity, Molality, and parts per million

Question 17

• You need to make 200 mL of 0.25 M HCl. How much 6.0 M HCl would you need?

Answer: 8.33 mL (use M1V1=M2V2)

Question 18

• This can be used to separate liquids that have different densities.

Answer: Centrifuge

Question 19

• The amount of a particular substance in a given quantity of a mixture, solution, or ore.

Answer: Concentration

Question 20

• To determine the melting point elevation, the concentration of the solution should be in:

Answer: Molality

Question 21

Which of the following has the least impact on solubility?

a. Density

b. Temperature

c. Agitation

d. Surface Area

Answer: A

Question 22

The compound that will most likely dissolve in water

a. is nonpolar

b. is not a dipole.

c. contains hydrogen sulfide.

d. has a positive and negative region.

Answer: D

Question 23

• A property that is determined by the number of particles present in a system but that is independent of the properties of the particles themselves.

Answer: Colligative Property

Question 24Which of the following is an example of using the

concept of boiling point elevation?

a. Adding table salt in water to cook pasta

b. Adding rock salt on icy roads

c. Adding valve oil to a brass instrument during a Christmas parade to keep the valves from locking up.

d. Adding ethylene glycol (antifreeze) to a car engine during the winter.

Answer: a

Question 25

• A homogeneous mixture of two or more substances uniformly dispensed throughout a single phase.

Answer: Solution

Question 26• Describe a condition that has an effect on

solubility.

Answer: Temperature – increases solubility of solids and liquids, decreases solubility of gases,Agitation – increases solubility of liquids and solidsSurface area – the smaller the surface area, the greater impact on solubilityPolarity – has to be the same polarity to be soluble

Question 27

• How is molality calculated?

Answer: moles divided by kilograms

Question 28

• What does a small italicized m mean?

Answer: molality

Question 29

• In a solution, the substance that is dissolved.

Answer: Solute

Question 30

• The random movement of microscopic particles suspended in a fluid is known as:

Answer: Brownian Motion

Question 31

Which of the following would have the greatest impact on the freezing point of water?

a. glucose (C6H12O6)

b. strontium sulfide (SrS)

c. lithium bromide (LiBr2)

d. sodium chloride (NaCl)

Answer: C

Question 32

• A water-soluble cleaner that can emulsify dirt and oil.

Answer: Detergent

Question 33

Molecules that have both polar and nonpolar regions

a. are unstable.

b. could act as emulsifying agents.

c. are likely to be flammable.

d. will not dissolve in any solvent.

Answer: b

Question 34

• A special word that relates to separating a solid from a liquid by pouring.

Answer: Decanting

Question 35

• A solution contains 76.0 g of NaCl and has a volume of 550 mL. Find the molarity of the solution.

Answer: 2.36 M

Question 36

• In a solution, the substance that dissolves the other substance.

Answer: Solvent

Question 37

• 607 g of NaCl is dissolved into 400 g of water. What is this concentration in the molality?

Answer: 25.9 m

Question 38

• What is the formula to calculate the parts per million of a solution?

Answer: m = gsolute /gsolvent x 1000000Orm = masssolute /masssolvent x 1000000

Question 39

• What is the formula used to calculate the change in freezing point.

Answer: Tf = kfmN

Question 40• What chemical

has the most change in solubility as the temperature is changed from 0C to 100 C

Answer: NaC2H3O2 or sodium acetate

Question 41

• Legally, the concentration of methyl mercury needs to be less than 1.0 ppm in fish meat to be sold or eaten. What is the maximum amount in milligrams of methyl mercury allowed in a fish that weighs 2.25 kg?

Answer: 2.25 mg

1.0 = x/2250 x 1000000

x = 0.00225 g x 1000 = 2.25 mg

Question 42

• 3.60 kg of water contains 1.52 moles of calcium hydroxide (Ca(OH)2). What is the approximate molality of the solution?

Answer: 0.422 m

m = mol/kg = 1.52/3.60

Question 43

• How many grams of NaOH are required to prepare 1200 mL of a 0.50 M solution?

Answer: 24 g

0.50 = x/1.200 (M=mol/L)

x = 0.6 mol x 40g/1mol = 24 g

Question 44

• Identify whether the following scenario describes a saturated, unsaturated or supersaturated solution.

• A single grain of solute is added to the solution, it sinks to the bottom of the container, and nothing else happens.

Answer: Saturated

Question 45

• At 90C, 30 g of Li2SO4 is dissolved in 100 g of water. Is this solution saturated, unsaturated, or supersaturated?

Answer: Unsaturated, because at 90C, water can hold 31 g of Li2SO4

Question 46

• Which of the pictures on the right is a homogenous mixture?

Answer: A

Question 47

• Calculate the boiling point of a solution of 520 g of the ionic compound magnesium chloride, MgCl2, dissolved in 900 g of water. (kb of water is 0.51ºC/m and the normal boiling point of water is 100ºC)

Answer: 520g x 1mol/95.3g = 5.45 mol

Tb = KbmN = (0.51)(5.45/.900)(3) = 9.265ºC

100 + (9.265) = 109.3ºC

Question 48

• At 10 °C, how much CsCl can be dissolved in 300 g of water?

Answer: about 513 g

171 x 3