Solutions

Question 1

Are all mixtures solutions?

Answer 1

No

Question 2

Are all solutions mixtures?

Answer 2

Yes

Question 3

When is solvation exothermic?

Answer 3

When the new interactions are stronger than the old ones

Question 4

What kind of temperature favors solubility of gas in liquid?

Answer 4

Lower temp

Question 5

When is solvation endothermic?

Answer 5

When new interactions are weaker than old

Question 6

When is endothermic solvation favored?

Answer 6

At higher temperatures

Question 7

Ideal solution

Answer 7

Enthalpy of the dissolution/solvation = 0

Question 8

Spontaneous processes do what to Gibb’s free energy?

Answer 8

Reduce Gibb’s free energy

Question 9

Nonspontaneous processes do what to Gibb’s free energy

Answer 9

Increase Gibb’s free energy

Question 10

Breaking bonds is

Answer 10

Endothermic

Question 11

Making bonds is

Answer 11

Exothermic

Question 12

Solubility

Answer 12

Maximum amount of the substance that can be dissolved in a particular solvent at a given temperature

Question 13

Above what solubility are solutes considered soluble?

Answer 13

Above 0.1 M

Question 14

Solubility rules

Answer 14

NH4+ and Group 1 are water soluble
Nitrates and Acetates are soluble
Cl, Br, I excluding F are soluble except for Ag, Pb, Hg2
All sulfates are soluble except Ca, Sr, Ba, Pb
All metal oxides are insoluble except alkali, ammonium, CaO, SrO,BaO
All hydroxides are insoluble except for alkali metals, ammonium, Ca, Sr, Ba
Carbonates, phosphates, sulfides, sulfites are insoluble except alkali metals and ammonium

Question 15

Complex ion/Coordinated compound

Answer 15

a molecule in which a cation is bonded to at least one electron donoor moleules called ligands

Question 16

Coordinate covalent bonds

Answer 16

Hold complexes together where an electron donor pair (Lewis base) and acceptor (Lewis acid) form a Lewis acid-base adducts

Question 17

Chelation

Answer 17

Central cation bonded to same ligand in multiple places in a complex

Question 18

Concentration of solution after dilution

Answer 18

MV=MV

Question 19

Normality

Answer 19

mols solute/kg solvent

Question 20

Saturation point

Answer 20

Equilibrium in creating a solution where solute concentration is max for given temp and pressure

Question 21

Change in free energy at equilibrium

Answer 21

0

Question 22

Solubility product constant

Answer 22

Ksp

Question 23

Ksp equation

Answer 23

Ksp=[A^n+]^m[B^m-]^n

Question 24

Would a Ksp have a denominator?

Answer 24

No

Question 25

What happens to the Ksp as temperature rises for gas solutes?

Answer 25

Decreases

Question 26

What happens to the Ksp as temperature rises for gas solutes?

Answer 26

Increases

Question 27

Ksp at higher pressures for gases

Answer 27

Larger

Question 28

Ksp at lower pressures for gases

Answer 28

Higher

Question 29

Ion product (IP)

Answer 29

Similar to Q

Question 30

Unsaturated

Answer 30

IP

Question 31

Supersaturated

Answer 31

IP>Ksp

Question 32

Ksp equations used for what kind of problems?

Answer 32

Sparingly/insoluble

Question 33

Sparingly soluble salt formula MX has what Ksp?

Answer 33

x^2

Question 34

Sparingly soluble salt formula MX^2 has what Ksp?

Answer 34

4x^3

Question 35

Sparingly soluble salt formula MX3

Answer 35

27x^4

Question 36

Relative Ksp of complex?

Answer 36

High

Question 37

Kf

Answer 37

Formation constant of complexes | If very high, the final concentration of the complex ion will be very near to the limiting reagent

Question 38

Common ion effects

Answer 38

Reduced solubility due to same ion already in solution | No effect on solubility product constant, only on molar solubility of salt

Question 39

Colligative properties

Answer 39

Dependent on the concentration of dissolved particles but not their chemical identity

Question 40

Colligative property examples

Answer 40

Vapor pressure depression Boiling point elevation Freezing point depression Osmotic pressure

Question 41

Raoult's law

Answer 41

Vapor pressure depression caused by solutes in solution | As solute is added to solvent, vapor pressure decreases proportionally

Question 42

Raoult's law expression

Answer 42

PA=XAPA not PA=vapor pressure when solutes are present XA=mol fraction of solvent A PA not=vapor pressure of solvent A in pure state

Question 43

Lowering of solution's vapor pressure means

Answer 43

Higher boiling point

Question 44

Boiling point elevation

Answer 44

When a nonvolatile solute is dissolved in a solvent to create a solution, boiling point greater than pure solvent

Question 45

Boiling point depression

Answer 45

Temperature where vapor pressure of the liquid equals ambient pressure More energy/higher temp needed to to get vapor pressure to reach ambient pressure

Question 46

Boiling point depression expression

Answer 46

Delta(T)=iKbm i=van't Hoff factor=number of particles in which a compound dissociates (NaCl=2) Kb=proportionality constant of the solvent m=molality Temperature in Kelvin

Question 47

Density of water

Answer 47

1 g/mL

Question 48

Freezing point depression

Answer 48

More temperature must be removed to create lattice structure

Question 49

Freezing point depression equation

Answer 49

Delta T f=iKfm i=van t'Hoff Kf=proportionality constant m=molality Temperature in Kelvin

Question 50

What is the effect of adding salt to roads?

Answer 50

Doesn't change the rate of melting | Decreases the rate of freezing

Question 51

Osmotic pressure

Answer 51

Sucking pressure genenrated by solutions in which water is drawn into the solution Must be applied to counteract attraction of water molecules for the solution

Question 52

Osmotic pressure equation

Answer 52

II=iMRT i=van't Hoff

Question 53

What predicts that Rasoult's Law will apply?

Answer 53

When solute-solute, solvent-solvent, solute-solvents are all very similar

Question 54

Bond breaking

Answer 54

Endothermic

Question 55

Bond making

Answer 55

Exothermic

Question 56

Charge density

Answer 56

Which ions form higher charge numbers