Solutions and Solubility (5/10)

Question 1

Solution definition

Answer 1

A homogeneous mixture

• mixture: two substances
• Homogeneous: evenly distributed
• Heterogeneous: not evenly distributed (like a salad)

Question 2

Dissoultion

Answer 2

Minority component (solute) reacts with solvent (majority component)

Question 3

Dissolving

Answer 3

Like dissolves like

-polar amino acids dissolve most readily in polar solvents (like water)

Question 4

Saturation

Answer 4

extent which solute is dissolved in solvent

-adding more solute than what solvent can handle to dissolve will precipitate

Question 5

Supersaturation

Answer 5

Solute concentration>solute solubility

must heat and cool slowly to keep all dissolved. If not, crystallized

Question 6

Electrolyte

Answer 6

Ions conduct electricity in a solution

Question 7

higher temperature for solids

Answer 7

higher solubility in endothermic reactions

Question 8

Higher temperature for gases

Answer 8

lowers solubility for gases

Question 9

Solubility rules: alkali metals

Answer 9

All soluble in water

Question 10

Solubility rules: Nitrates

Answer 10

All soluble in water

Question 11

Solubility rules: Halides

Answer 11

soluble in water except when combined with silver, lead, or mercury

Question 12

Solubility rules: Sulfates

Answer 12

Souble in water except when combined with calcium, silver, lead, etc

Question 13

Solubility rules: Carbonate, phosphate, sulfide

Answer 13

Insoluble except when combined with sodium carbonate or ammonium phosphate

Question 14

Solubility rules: Hydroxides and metal oxides

Answer 14

Insoluble except if combined with alkali metals

Question 15

Molarity

Answer 15

moles of solute/Liters of solution

Question 16

Molality

Answer 16

Moles of solute/Kg of solvent

Question 17

High concentration of solute

Answer 17

Impacts volume

Molarity does not equal molality

Question 18

Colligative properties

Answer 18

Properties changing solely with the concentration of solute in solution

Question 19

Normality

Answer 19

Equivalents of solute/ Liters of solution

Question 20

Calculating normality

Answer 20

(molarity of acid) x (acidic protons per molecule)

molarity of base) x (hydroxide ions per molecule

Question 21

Solubility equilibria

Answer 21

balance between reactant and balanced species

Question 22

Ksp expression

Answer 22

Product ions only

high value = large concentration of dissolved ions (high solubility)

Question 23

Insolubility

Answer 23

No compound is truly insoluble

Question 24

Molar solubility

Answer 24

Ksp/[cation] = [anion]

number of moles that need to dissolved for the solution to be saturated

Question 25

A saturated aqueous solution when at equilibrium is…

Answer 25

The rates of dissolution and precipitation are equal

Question 26

Common ion effect

Answer 26

solubility of an ionic species decreases when one of its component ions is already present in solution

Question 27

Example of the common ion effect

Answer 27

AgCl –> Ag+ + Cl-
external Cl- is the common ion which moves closer to saturation before Ag+ can dissolve because it takes up solvent so we decrease the solubility of Ag

Question 28

Coordination complex

Answer 28

complex ion

takes external ions and adds them to something else to allow reactants to dissolve better