Deck 13: Solutions

Question 1

The process of surrounding each solute particle with particles of solvent is called _____.

Answer 1

solvation

Question 2

The interactions that determine the solubility of a substance in a liquid depend on the physical state of the solute.

Answer 2

False

Question 3

Which of the following substances are completely miscible?

A) Water and oil
B) Ethanol and water
C) Oil and milk
D) Gasoline and water
E) Water and acetic acid

Answer 3

Ethanol and water

Question 4

The process of surrounding solute particles with water molecules is called _____.

A) crystallization
B) osmosis
C) dialysis
D) hydration
E) precipitation

Question 5

A saturated solution is formed when the maximum possible amount of a solute has dissolved in a given amount of a specified solvent.

Question 6

Which of the following compounds will be most soluble in water?

A) Naphthalene
B) Silver chloride
C) Ethylene glycol
D) Lithium chloride
E) Benzoic acid

Question 7

The degree of disorder in a thermodynamic system is referred to as its _____.

A) enthalpy
B) molarity
C) molality
D) free energy
E) entropy

Question 8

Which of the following processes involves a chemical transformation?

A) A sugar cube dissolving in a cup of hot tea
B) Adding iodine crystals to CCl₄
C) Mixing an aqueous solution of NaOH with an aqueous solution of HCl
D) Metallic gold dissolving in a small quantity of liquid mercury.
E) Sodium metal dissolving in liquid ammonia

Question 9

_____ is a thermodynamic property of a substance that is proportional to its degree of disorder.

Question 10

The substances that are capable of forming a single homogenous phase, regardless of the proportions with which they are mixed are said to be _____.

Question 11

The physical state of the solute determines the state of the solution.

Question 12

Which of the following processes is a simple dissolution?

A) Adding iodine crystals to CCl₄
B) Mixing an aqueous solution of NaOH with an aqueous solution of HCl
C) Bubbling HCl gas through water
D) SO₃ gas dissolving in water to produce sulfuric acid.
E) Adding sodium metal to ethanol to produce sodium ethoxide and hydrogen gas

Question 13

A change in enthalpy always favors solution formation.

Question 14

The solvation process is a unidirectional process.

Question 15

The dissolution of a solute in a solvent to form a solution involves a chemical transformation.

Question 16

Which of the following is a heterogeneous mixture?

A) Liquid decongestant
B) Vinegar
C) Fog
D) Gasoline
E) Aqueous ammonia

Question 17

The solubility of most solids increases with increasing temperature.

Question 18

How does the nature of a solute and a solvent determine whether the solvation process is exothermic or endothermic?

Question 19

How does the entropy of a system affect the solution formation?

Question 20

If the enthalpy of solution for a combination of solute and solvent is large and positive, then they do not form a solution readily.

Question 21

The substance that has an electrostatic attraction to water is classified as _____.

Question 22

The 'unit parts per million (ppm)' refers to grams of solute per kilogram of solvent.

Question 23

Why are nonpolar gases less soluble in polar solvents than nonpolar solvents?

Question 24

The ratio of total mass of the solute to the total mass of the solution is referred to as the _____.

A) mole fraction
B) molarity
C) molarity.
D) mass percentage
E) molar mass

Question 25

A solid sample of a substance that can be added to a supercooled liquid or supersaturated solution to help induce crystallization is called a(n) _____.

A) cryptand
B) seed crystal
C) amalgam
D) liquid crystal
E) crown ether

Question 26

The units parts per million (ppm) and parts per billion (ppb) are used to describe concentrations of highly dilute solutions.

Question 27

The molarity of a solution with 16.5 g of glucose in a 200.0 ml solution is _____ M. (Molar mass of glucose = 180.16 g/mol)

A) 0.092
B) 0.458
C) 9.158
D) 4.579
E) 0.018

Question 28

_____ is a measure of the amount of a solid substance that remains dissolved in a given amount of a specific liquid at a specified temperature and pressure.

Question 29

_____ are cyclic polyethers that have a central cavity large enough to be occupied by a metal ion coordinated to the ring of oxygen atoms.

A) Crown ethers
B) Amalgams
C) Seed crystals
D) Cryptands
E) Aerosols

Question 30

Which of the following substances is hydrophilic?

A) Naphthalene
B) Vitamin A
C) Glucose
D) Octane
E) Oleic acid

Question 31

_____ which are usually solids, are solutions of metals in liquid mercury.

Question 32

_____ is defined as the number of moles of solute present in exactly 1 kg of solvent.

A) Molarity
B) Mass percentage
C) Molality
D) Mole fraction
E) Enthalpy

Question 33

Which of the following substances is hydrophobic?

A) Vitamin C
B) Naphthalene
C) Glucose
D) Arginine
E) Pantothenic acid

Question 34

A hydrophobic substance contains _____ bonds that do not interact favourably with water.

Question 35

A solution with maximum possible amount of a solute under a given set of conditions is called a(n) _____.

A) supercritical fluid
B) saturated solution
C) crystalline solution
D) electrolyte
E) supercooled solution

Question 36

Explain with an example, the consequences of the difference between hydrophilic and hydrophobic substances in biological systems.

Question 37

Molarity is the number of moles of solute divided by the volume of the solution.

Question 38

A(n) _____ constant is a constant that expresses the ability of a bulk substance to decrease the electrostatic forces between two charged particles.

A) rate
B) dielectric
C) Planck's
D) equilibrium
E) proportionality

Question 39

The molality of a solution is temperature dependent.

Question 40

A _____ is an unstable solution with more dissolved solute than it would normally contain under the given set of conditions.

A) saturated solution
B) supercritical fluid
C) supersaturated solution
D) supercooled liquid
E) unsaturated solution

Question 41

The quantity of solute that is dissolved in a particular quantity of solvent or solution is referred to as its _____.

Question 42

The molality of a solution that contains 36.6 g of NaCl in 200.0 g of water is _____ m. (Molar mass of NaCl = 58.44 g/mol)

A) 3.66
B) 3.13
C) 31.3
D) 36.6
E) 0.36

Question 43

What is the drawback of using molarity to express concentrations of reactions in solution or for titrations?

Question 44

The unit primarily used to express the concentration of a solution in the health sciences is _____.

Question 45

What is the role of haemoglobin in increasing the O₂ concentration in the blood serum of humans?

Question 46

In the equation, C = kP, k represents _____.

A) concentration of dissolved gas at equilibrium
B) concentration of the solvent
C) partial pressure of the gas
D) Henry's law constant
E) Dalton's constant

Question 47

A 100.0 mL solution of ethanol that has density of 0.789 g/mL, contains 15.6 mL of iodine. The concentration of the aqueous solution is _____ ppm. (Density of iodine = 4.94 g/mL)

A) 9.77 × 10⁵
B) 9.8 × 10⁷
C) 0.98 × 10⁹
D) 9.77 × 10⁶
E) 0.97 × 10³

Question 48

_____ of a solution is described in terms of mol/L.

Question 49

_____ is a process of separation of compounds based on their relative solubilities in a given solvent.

Question 50

The solubility of a gas depends on both temperature and pressure.

Question 51

The Henry's law constant for helium in water at 20.0˚C and 0.25 atm is 3.9 × 10^-4 M/atm. The solubility of helium in water at 20.0˚C at an atmospheric pressure of 0.25 atm is _____ M.

A) 0.97 × 10^-3
B) 9.8 × 10^-5
C) 9.6 × 10^-4
D) 0.98 × 10^-5
E) 0.39 × 10^-4

Question 52

The relationship between the pressure and the solubility of a gas is quantitatively described by _____ law.

A) Raoult's
B) Henry's
C) Dalton's
D) Hess'
E) Boyle's

Question 53

Gases that react with water do not obey Henry's law.

Question 54

The mole fraction of benzene in a 100.0g solution containing 30.0g of benzene and 70.0g of water is _____. (molar mass of benzene = 78.11 g/mol and molar mass of water = 18.02 g/mol)

A) 0.3889
B) 3.889
C) 0.0900
D) 0.1090
E) 1.630

Question 55

The Henry's law constant for nitrogen in seawater at 25˚C is 7.1 × 10^-4 M/atm and the mole fraction of N₂ in the atmosphere is 0.78. The solubility of N₂ in seawater at 25˚C at an atmospheric pressure of 1.00 atm is _____ M.

A) 7.1 × 10^-4
B) 0.53 × 10^-4
C) 0.71 × 10^-4
D) 5.5 × 10^-4
E) 71 × 10^-4

Question 56

The mass percentage of toluene in a solution containing 100.0 mL of toluene and 200.0 mL of benzene is _____%. (Density of toluene = 0.865 g/mL and density of benzene = 0.875 g/mL)

A) 10.0
B) 25.0
C) 33.1
D) 49.4
E) 86.5

Question 57

A 200.0 mL aqueous solution contains 58.8 mL of H₂SO₄. The concentration of the aqueous solution is _____ ppb. (Density of solution = 0.998 g/mL; density of H₂SO₄ = 1.84 g/mL)

A) 0.542 × 10⁶
B) 0.530 × 10⁷
C) 5.42 × 10⁸
D) 58.8 × 10⁶
E) 5.42 × 10⁹

Question 58

The solubility of gases in liquids increases with increasing temperature.

Question 59

Fractional crystallization separates components of a mixture based on their solubilities.

Question 60

What are the requirements for fractional crystallization to be an effective technique for separation of compounds?

Question 61

Adding a nonvolatile solute to a volatile solvent increases the vapor pressure of the solvent.

Question 62

The concentration of a solute is typically expressed as molality rather than molarity.

Question 63

The net flow of solvent through a semipermeable membrane is called _____.

Question 64

Which of the following systems will have a vapor pressure approximately equal to that predicted by the Raoult's law?

A) Ethylene glycol and chloroform
B) Acetic acid and n-propanol
C) Benzene and n-hexane
D) Cyclohexane and ethanol
E) Methanol and acetone

Question 65

The properties of a solution that depend primarily on the number of solute particles rather than the kind of solute particles are called _____.

Question 66

The units of Henry's law constant are _____.

Question 67

A solution that exhibits a negative deviation from Raoult's law will:

A) have weaker solute-solvent interactions compared to both solute-solute interactions and solvent-solvent interactions.
B) have weaker solute-solvent interactions compared to only solute-solute interactions.
C) have a higher vapor pressure than expected for an ideal solution.
D) have stronger solute-solvent interactions compared to both solute-solute interactions and solvent-solvent interactions.
E) have solute-solute interactions that are identical to the solute-solvent interactions.

Question 68

A process that uses a semipermeable membrane with pores large enough to allow small solute and solvent molecules to pass through but not large solute molecules is called _____.

Question 69

The van't Hoff factor increases with increase in solute concentration.

Question 70

_____ law is an equation that quantifies the relationship between the solution composition and vapor pressure of the solution.

A) Henry's
B) Dalton's
C) Hess'
D) Raoult's
E) Boyle's

Question 71

The osmotic pressure of a solution that contains 6.0 g of NaCl per 100.0 g of solution that has a density of 1.02 g/mL at a temperature of 25˚C is _____ atm. (Given R = 0.0821 L.atm/mol.K)

A) 32
B) 51
C) 45
D) 25
E) 5

Question 72

A solution that obeys Raoult's law is called a(n) _____.

Question 73

The boiling point of an aqueous solution that contains 40.0 g of NaCl in 100.0g of water is _____˚C. (Given; K_b for water = 0.51˚C/m)

A) 103
B) 107
C) 100
D) 93
E) 95

Question 74

Aqueous solutions have a higher boiling point than pure water.

Question 75

Solutions with the same molarity contain the same concentration of solute particles.

Question 76

The decrease in vapor pressure of an aqueous solution that contains 45.0% ethylene glycol (C₂H₄(OH)₂) by mass is _____ mmHg. (Given; vapor pressure of pure water at 100.0˚C is 760.0 mmHg)

A) 656
B) 569
C) 614
D) 164
E) 416

Question 77

The freezing point of an aqueous solution that contains 25.0 g of CaCl2 in 100.0 g of water is _____˚C. (Given; K_f for water = 1.86˚C/m)

A) -13.8˚C
B) 4˚C
C) -12.6˚C
D) -4˚C
E) 12.5˚C

Question 78

Which of the following systems will exhibit a negative deviation from Raoult's law?

A) Ethylene glycol and chloroform
B) n-hexane and 2,2,4-trimethylpentane
C) Benzene and n-hexane
D) Cyclohexane and ethanol
E) Methanol and acetone

Question 79

Define the van't Hoff factor of a solution.

Question 80

The solubility of gases _____ as the partial pressure of the gas above a solution increases.