Solutions

Question 1

homogeneous mixtures composed of two or more substances that combine to form a single phase, usually the liquid phase; consists of a solvent and a solute

Answer 1

solutions

Question 2

is dissolved in a solvent

Answer 2

solute

Question 3

the component of the solution that remains the same after mixing

Answer 3

solvent

Question 4

process of solvent particles surrounding solute particles via electrostatic interactions

Answer 4

solvation/dissolution

Question 5

process of solvation/dissolution of an aqueous solution (solvent is water)

Answer 5

hydration

Question 6

the maximum amount of solute that can be dissolved in a given solvent at a given temperature; often expressed as molar ____ (the molarity of the solute at saturation)

Answer 6

solubility

Question 7

refers to a molecule in which a cation (metallic ions) is bonded to at least one electron pair donor (various neutral compounds and anions, referred to as ligands)

Answer 7

complex ions (coordination compounds)

Question 8

bonds between a Lewis acid and base that hold complex ions together

Answer 8

coordinate covalent bonds

Question 9

denotes the amount of solute dissolved in a solvent

Answer 9

concentration

Question 10

method of expressing concentration:

used for aqueous solutions and solid-in-solid solutions

Answer 10

percent composition by mass

Question 11

percent composition by mass

Answer 11

(mass of solute / mass of solution) x 100%

Question 12

method of expressing concentration:

used for calculating vapor pressure depression and partial pressures of gases in a system

Answer 12

mole fraction (𝜒)

Question 13

mole fraction (𝜒)

Answer 13

𝜒(A) = moles of A / total moles of all species

Question 14

method of expressing concentration:
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 14

molarity (M)

Question 15

molarity (M)

Answer 15

M = moles of solute / liters of solution

Question 16

method of expressing concentration:

used for boiling point elevation and freezing point depression

Answer 16

molality (m)

Question 17

molality (m)

Answer 17

m = moles of solute / kilograms of solvent

Question 18

method of expressing concentration:

the molarity of the species of interest and is used for acid-base and oxidation-reduction reactions

Answer 18

normality (N)

Question 19

normality (N)

Answer 19

N = number of equivalents / liters of solution

Question 20

dilution equation

Answer 20

M(1) V(1) = M(2) V(2)

Question 21

defined as equilibrium in the process of creating a solution, where the solute concentration is at its maximum value for the given temperature and pressure

Answer 21

saturation point

Question 22

the equilibrium constant for a dissociation reaction

Answer 22

solubility product constant (K(sp))

Question 23

solubility product constant (K(sp))

Answer 23

K(sp) = [A^n+]^m * [B^m-]^n

e.g. K(sp) = [Ag+] [Cl-]

Question 24

a calculated value that relates where the system is with respect to the equilibrium position (K(sp))

Answer 24

ion product (IP)

Question 25

ion product (IP)

Answer 25

IP = [A^n+]^m * [B^m-]^n

e.g. IP = [Ag+] [Cl-]

Question 26

comparison determines the level of saturation and behavior of the solution

Answer 26

comparison of K(sp) and IP

Question 27

comparison of K(sp) and IP:

indicates the solution is unsaturated, and if more solute is added, it will dissolve

Answer 27

IP < K(sp)

Question 28

comparison of K(sp) and IP:

indicates the solution is saturated (at equilibrium), and there will be no change in concentrations

Answer 28

IP = K(sp)

Question 29

comparison of K(sp) and IP:

indicates the solution is supersaturated, and a precipitate will form

Answer 29

IP > K(sp)

Question 30

the equilibrium constant for complex formation; value is usually much greater than K(sp)

Answer 30

formation/stability constant (K(f))

Question 31

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 31

common ion effect

Question 32

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

Answer 32

colligative properties

Question 33

accounts for vapor pressure depression caused by solutes in solution

Answer 33

Raoult’s law

Question 34

Raoult’s law

Answer 34

P(A) = 𝜒(A) P°(A)

where:
P(A) = vapor pressure of solvent A when solutes are present
𝜒(A) = mole fraction of solvent A in the solution
P°(A) = vapor pressure of solvent A in its pure state

Question 35

decreases the evaporation rate of a solvent without affecting its condensation rate, thus decreasing its vapor pressure

Answer 35

presence of other solutes

Question 36

shifts in the phase equilibria dependent on the molality (m) of the solution

Answer 36

freezing point depression and boiling point elevation

Question 37

freezing point depression

Answer 37

ΔT(f) = i K(f) m

where:
ΔT(f) = freezing point depression
i = van't Hoff factor
K(f) = proportionality constant characteristic of particular solvent
m = molality of solution

Question 38

boiling point elevation

Answer 38

ΔT(b) = i K(b) m

where:
ΔT(b) = boiling point elevation
i = van't Hoff factor
K(b) = proportionality constant characteristic of particular solvent
m = molality of solution

Question 39

corresponds to the number of particles into which a compound dissociates in solution

e.g. for NaCl i = 2 (1 for Na and 1 for Cl)

Answer 39

van’t Hoff factor

Question 40

refers to the “sucking” pressure generated by solutions in which water is drawn into a solution

Answer 40

osmotic pressure (π)

Question 41

osmotic pressure (π)

Answer 41

π = iMRT

where:
π = osmotic pressure