Chemistry Chapter 9: Solutions (4 Stars)

Question 1

______ are homogenous mixtures composed of two or more substances.

Answer 1

Solutions

Question 2

Solutions combine to form a single phase, generally the _____ phase.

Answer 2

liquid

Question 3

Solvent particles surround solute particles via ______ interactions in a process called solvation or dissolution.

Answer 3

electrostatic

Question 4

Aqueous solutions are most important for the MCAT; solvation in water can also be called ______

Answer 4

hydration.

Question 5

Most dissolutions are ______, although the dissolution of gas into liquid is ______

Answer 5

endothermic

exothermic.

Question 6

_______ is the maximum amount of a solute that can be dissolved in a given solvent at a given temperature; it is often expressed as molar solubility—the molarity of the solute at saturation.

Answer 6

Solubility

Question 7

Complex ions or coordination compounds are composed of metallic ions bonded to various neutral compounds and anions, referred to as _______

Answer 7

ligands.

Question 8

Formation of complex ions increases the _____ of otherwise insoluble ions (the opposite of the common ion effect).

Answer 8

solubility

Question 9

The process of forming a complex ion involves electron pair donors and electron pair acceptors such as those seen in __________ bonding.

Answer 9

coordinate covalent

Question 10

Percent composition by mass (mass of solute per mass of solution times 100%) is used for ______ solutions and solid-in-solid solutions.

Answer 10

aqueous

Question 11

The mole fraction (moles of solute per total moles) is used for calculating vapor pressure depression and _______ of gases in a system.

Answer 11

partial pressures

Question 12

______ (moles of solute per liters of solution) is the most common unit for concentration and is used for rate laws, the law of mass action, osmotic pressure, pH and pOH, and the Nernst equation.

Answer 12

Molarity

Question 13

_____ (moles of solute per kilograms of solvent) is used for boiling point elevation and freezing point depression.

Answer 13

Molality

Question 14

_______ (number of equivalents per liters of solution) is the molarity of the species of interest and is used for acid–base and oxidation–reduction reactions.

Answer 14

Normality

Question 15

______ solutions are in equilibrium at that particular temperature.

Answer 15

Saturated

Question 16

The solubility product constant (Ksp) is simply the equilibrium constant for a _____ reaction.

Answer 16

dissociation

Question 17

Comparison of the ion product (IP) to ____ determines the level of saturation and behavior of the solution:

Answer 17

Ksp

Question 18

IP < Ksp: the solution is unsaturated, and if more solute is added, it will ______

Answer 18

dissolve

Question 19

IP = Ksp: the solution is saturated (at equilibrium), and there will be ____ change in concentrations

Answer 19

no

Question 20

IP > Ksp: the solution is supersaturated, and a _____ will form

Answer 20

precipitate

Question 21

Formation of a complex ion in solution greatly ______ solubility.

Answer 21

increases

Question 22

The formation or stability constant (Kf ) is the equilibrium constant for complex formation. Its value is usually much _____ than Ksp.

Answer 22

greater

Question 23

The formation of a complex _____ the solubility of other salts containing the same ions because it uses up the products of those dissolution reactions, shifting the equilibrium to the right (the opposite of the common ion effect).

Answer 23

increases

Question 24

The _______ effect decreases the solubility of a compound in a solution that already contains one of the ions in the compound. The presence of that ion in solution shifts the dissolution reaction to the left, decreasing its dissociation.

Answer 24

common ion

Question 25

______ properties are physical properties of solutions that depend on the concentration of dissolved particles but not on their chemical identity.

Answer 25

Colligative

Question 26

_____ pressure depression follows Raoult’s law.

Answer 26

Vapor

Question 27

The presence of other solutes ______ the evaporation rate of a solvent without affecting its condensation rate, thus decreasing its vapor pressure.

Answer 27

decreases

Question 28

____ pressure depression also explains boiling point elevation—as the vapor pressure decreases, the temperature (energy) required to boil the liquid must be raised.

Answer 28

Vapor

Question 29

Freezing point depression and boiling point elevation are ____ in the phase equilibria dependent on the molality of the solution.

Answer 29

shifts

Question 30

_____ pressure is primarily dependent on the molarity of the solution.

Answer 30

Osmotic

Question 31

For _____ that dissociate, the van ’t Hoff factor (i) is used in freezing point depression, boiling point elevation, and osmotic pressure calculations.

Answer 31

solutes