Chapter 11 Solutions

Question 1

Colligative Properties:

Answer 1

Properties that do not depend on the identity of the solute only on the number of solute particles.

Question 2

Percent by mass

Answer 2

grams of solute/grams of solution x 100

Question 3

Percent by volume

Answer 3

Volume of solute/ volume of solution x100

Question 4

Mass/volume percent

Answer 4

Grams of solute/volume of solution x 100

Question 5

Ppm

Answer 5

Grams of solute/grams of solution x 10^6

Question 6

Ppb

Answer 6

Grams of solute/grams of solution x 10^9

Question 7

Molarity

Answer 7

Moles of solute/liters of solution

Question 8

Molality

Answer 8

Moles of solute/ kg of solvent

Question 9

Boiling Point Elevation

Answer 9

Tb= Kb(m)

Question 10

Freezing point depression

Answer 10

Tf= kf(m)

Question 11

Solution

Answer 11

Homogeneous nixture with uniform composition throughout

Question 12

Solute

Answer 12

Substance being dissolved

Question 13

Solvent

Answer 13

Substance doing dissolving

Question 14

CP
Osmotic Pressure (osmosis, semipermeable membrane)

Answer 14

Osmotic pressure is the pressure exerted on a solution to prevent osmosis -solvent particles diffuse through a semipermeable membrane-

Question 15

Vapor Pressure Lowering

Answer 15

When it equals the atmospheric pressure system is at equilibrium.
Greater vapor pressure=more surface particles escaping.
Lower vapor pressure=more condensation
Volatile solutions are easily turned into gas

Question 16

Strong Electrolytes and boiling point.. Number of particles

Answer 16

Dissociate into ions when dissolved in water more particles stronger electrolyte
More dissociated ions higher boiling point

Question 17

Electrolytes vs nonelectrolytes

Answer 17

Strong: dissociate into ions
Weak: dissociate partially into ions
Non: do not dissociate into ions

Question 18

Miscible

Answer 18

Solute and solvent that can be mixed in any proportion still giving a homogeneous mixture

Question 19

When ionic compounds dissolve in water…

Answer 19

Ionic bonds in solute break
Hydrogen bonds between water molecules break
Ion-dipole forces form between ions and water molecules

Question 20

Entropy

Answer 20

Tendency of matter to become disordered and more random

Question 21

Factors that affect solubility

Structure

Answer 21

Like dissolves like

Solvents dissolve similar solutes

Question 22

Factors that affect solubility

Temperature

Answer 22

Water: Solubility increases as temp increases
Gas: less soluble in higher temperatures (higher k.energy)

Question 23

Factors that affect solubility

Pressure

Answer 23

Gases only

More pressure more solubility

Question 24

Unsaturated vs saturated vs supersaturated

Answer 24

Less than max amount of solute - max amount - more than max

Question 25

Solubility rules

Answer 25

Soluble
Na, K, NH4, NO3
SO4 (except Ba Sr Pb Ca Hg2 Ag 2)
Cl, Br, I (except Ag Hg2, Pb, HgI2)
Insoluble
Ag+ (except AgNO3)
O-2 OH- (except NaOH KOH Ba(OH)2 Ca(OH)2
S-2 (except Na K NH4 alkaline, metal ions)
CrO4-2 (except Na K NH4 Ma Ca Al Ni)
CO3-2 PO4-3 (except with Na K NH4)
SO3-2 SiO3-2

Question 26

Aqueous Solution

Answer 26

Solvent is water