9 Solutions

Question 1

Molarity (M)

Answer 1

moles of solute / liters of solution

Question 2

Molality (m) =

Answer 2

moles of solute / kilograms of solvent

Question 3

Mole Fraction (X_s)

Answer 3

moles of substance S / total number of moles in solution

Question 4

van’t Hoff factor (i)

Answer 4

tells us how many ions one unit of a substance will dissociate into in solution.

Question 4

Boiling Point Elevation

{Delta}T =

Answer 4

iK_bm

i = ithe van’t Hoff factor; the number of particles into which the added solute dissociates

k_b = the boiling point elevation constant for the solvent

m = molality

Question 5

Freezing Point Depression

{Delta} T =

Answer 5

ik_fm

i = the van’t Hoff factor; the number of particles into which the added solute dissociates

k_{f =} the freezing point depression constant for the solvent

m = molality

Question 6

Vapor Pressure Lowering, Raoult’s Law

P =

Answer 6

XP°

P = vapor pressure of the solution

Pº = vapor pressure of the pure solvent

X = the mole fraction of the solvent

Question 7

Osmotic Pressure

{lambda} =

Answer 7

(nRT / V)i = MRTi

{lambda} = osmotic pressure (atm)

n = moles of solute

R =the gas constant 0.0821 (L•atm)/(mol•K)

T = absolute temperature (K)

V = volume of solution (L)

i = the van’t Hoff factor, the number of particles into which the added solute dissociates

M= molarity of the solution (M= m/V)

Question 8

Density of a Solution

D =

Answer 8

m / V

m = mass of the solution

V = volume of the solution

Question 9

Solubility Rules

Cations:

Alkali Metals: Li+, Na+, K+, Rb+, Cs+

All salts of the alkali metals are

Answer 9

soluble

Question 10

Solubility Rules

Cations:

Ammonium: NH₄⁺

All ammonium salts are

Answer 10

soluble

Question 11

Solubility Rules

Cations:

Alkaline Earths and Transition Metals

The solubility of these elements

Answer 11

varies depending on the identity of the anion.

Question 12

Solubility Rules

Anions:

Nitrate: NO₃^-

All nitrate salts are

Answer 12

soluble

Question 13

Solubility Rules
Anions:

Chlorate: ClO₃^-

All chlorate salts are

Answer 13

soluble

Question 14

Solubility Rules
Anions:

Perchlorate: ClO₄^-

All perchlorate salts are

Answer 14

soluble

Question 15

Solubility Rules
Anions:

Acetate: C₂H₃O₂^-

All acetate salts are

Answer 15

soluble

Question 16

Solubility Rules
Anions:

Chloride, Bromide, Iodide: Cl^-, Br^-. I^-

Salts containing Cl-, Br-. and I- are

Answer 16

soluble

EXCEPT for those containing Ag+, Pb2+, and Hg2²⁺

Question 17

Solubility Rules:

Anions:

Sulfate” SO₄^2-

Sulfate salts are

Answer 17

soluble

EXCEPT for those containing: Ag⁺, Pb2+, Hg22+, Ca2+, Sr2+, and Ba2+

Question 18

The lower the temperature and the higher the pressure the more soluble

Answer 18

gas will be

Question 19

Colligative Properties are properties of a solution that depends on the number of solute particles in the solution. For colligative properties the identity is not important.

Answer 19

Boiling point elevation

Freezing point depression

vapor pressure lowering

osmotic pressure

Question 20

Hydroxide: OH^-

Hydroxide salts are

Answer 20

insoluble.

Except for those containing alkali metals, which are soluble and those containing Ca²⁺, Sr2+, and Ba2+, which fall into a gray area of moderate solubility.

Question 21

Carbonate: CO₃^2-

Carbonate salts are

Answer 21

insoluble

Question 22

Phosphate: PO₄^3-

Phosphate salts are

Answer 22

insoluble

Question 23

Sulfite: SO₃^2-

Sulfite salts are

Answer 23

insoluble

Question 24

Chromate: CrO₄^2-

Chromate salts are

Answer 24

insoluble

Question 25

Sulfide: S^2-

Sulfide salts are

Answer 25

insoluble

Question 26

The greater the value of the solubility product for a salt, the

Answer 26

more soluble the salt.

Question 27

moles

Answer 27

(molarity)(volume)

volume = moles/ molarity