Solubility

Question 1

Are compounds labeled insoluble generally somewhat soluble?

Answer 1

yes, not a lot, but a small amount

Question 2

Are the solubility or sparingly soluble compounds analogous to weak acids/bases?

Answer 2

yes, they react a little, but not a lot

Question 3

What is solubility?

Answer 3

maximum amount of a solute you can dissolve in a given amount of solvent. Units are typically given as mass/volume

Question 4

What is molar solubility?

Answer 4

same as solubility, but units are given in moles instead of mass. Units are typically given as moles/volume

Question 5

What is Ksp?

Answer 5

solubility product

Question 6

What is the % dissociation, solubility, K value, and what side is favoured?
NaCl (s) → Na+ (aq) + Cl- (aq)?

Answer 6

100% dissociated
Soluble (dissolves)
K = [Na+][Cl-]/[NaCl]
K >1
Favours reactants

Question 7

Does K value products or reactants when K is less than 1?

Answer 7

products

Question 8

What do you measure the concentration of a solid by?

Answer 8

mol/L → g/L

Question 9

What is the mass/volume for a solid?

Answer 9

density (𝝆)

Question 10

Is the concentration fixed for solids?

Answer 10

yes

Question 11

How does the density stay the same when stuff is being lost into solution?

Answer 11

The number is not changing because mass is being lost along with volume
Concentration stays the same

Question 12

What is the Ksp equation of AgCl (s) –> Ag+ + Cl-

Answer 12

Ksp = [Ag+][Cl-]

Question 13

What are the factors of Ksp?

Answer 13

Constant at constant temperature, changes with changing temperature
Small Ksp values means less soluble
Larger Ksp values means more soluble
Bi2S3 (s) 2Bi+3 (aq) + 3S-2 (aq)
Ksp = [Bi2+]2[S-2]3

Question 14

What is Qsp?

Answer 14

[A+][B-] not at equilibrium

Question 15

What is it when Qsp<Ksp?

Answer 15

More ions can dissolve
No precipitate formed
Proceeding towards products

Question 16

What is it when Qsp>Ksp?

Answer 16

Too many ions in solution
A precipitate forms
Proceeding towards reactants

Question 17

What is electrochemistry?

Answer 17

converting chemical energy to electrical energy or vice versa

Question 18

What are the 2 types of electrochemical cells?

Answer 18

Voltaic (galvanic) cells and electrolytic

Question 19

What is a voltaic (galvanic) cell?

Answer 19

convert chemical energy to electric energy
Spontaneouss, 𝚫G < 0

Question 20

What is an electrolytic cell?

Answer 20

convert electric energy to chemical energy
Non-spontaneous, 𝚫G > 0

Question 21

What is an acid-base reaction?

Answer 21

transferring/sharing 2e- at a time

Question 22

What is a redox reaction?

Answer 22

transferring 1e- at a time
One species loses electrons and the other gains them

Question 23

What are the 2 kinds of redox reactions?

Answer 23

oxidation and reduction

Question 24

What is an oxidation reaction?

Answer 24

losing electrons

Question 25

What is a reduction reaction?

Answer 25

gaining electrons

Question 26

What are the rules for assigning oxidation states?

Answer 26

1) Atoms in their elemental form have O.N.(oxidation numbers) = 0 2) For monatomic ions the O.N. = ion charge 3) The sum of O.N. for the atoms in a compound = 0. The sum of O.N. of atoms in polyatomic ions = charge on the polyatomic ion

Question 27

What are electrodes?

Answer 27

conductors that move electrons

Question 28

What are the two types of electrodes?

Answer 28

inert and active

Question 29

What is an inert electrode?

Answer 29

not involved in reactions

Question 30

What is an active electrode?

Answer 30

involved in the reactions

Question 31

What is an anode (-)?

Answer 31

the electrode where oxidation takes place

Question 32

What is a cathode (+)?

Answer 32

the electrode where reduction takes place

Question 33

What is electromotive force equal to?

Answer 33

Electromotive Force= Potential (E)=Voltage (V)

Question 34

What is potential (E)?

Answer 34

Potential is the strength of the electron flow

Question 35

What are the units for potential?

Answer 35

volts (V)

Question 36

What are the equations to find volts?

Answer 36

1V = 1 J/C J = V x C

Question 37

What is the current (i) equation?

Answer 37

Current (i) = C/s = Ampere (A)

Question 38

What are standard reduction potentials?

Answer 38

No zero point for potential Can calculate changes in potential (the height of something) Define a standard that we define as having zero potential

Question 39

What happens to the compound when E0 is more positive?

Answer 39

reduced

Question 40

What happens to compound when E0 is more negative?

Answer 40

oxidized

Question 41

What do strong oxidizing agents want to do?

Answer 41

steal electrons

Question 42

What do strong reducing agents want to do?

Answer 42

give away electrons

Question 43

What is the Ecell equation?

Answer 43

E0cell = E0cathode - E0anode

Question 44

What is the more positive value in reduction potential?

Answer 44

cathode

Question 45

Will E0cell always be positive?

Answer 45

yes (𝚫G <0)

Question 46

What is the relationship between in Faraday's constant?

Answer 46

𝚫G and Ecell

Question 47

What does 𝚫G equal in Faraday's constant?

Answer 47

Ecell x charge

Question 48

What does J equal in Faraday's constant?

Answer 48

V x C

Question 49

What does 1V equal in Faraday's constant?

Answer 49

1J/C

Question 50

What is the charge on 1e-?

Answer 50

-1.602 x 10^-19 C

Question 51

What is the charge on 1 mole of e?

Answer 51

-1.602 x 10^-19 C x 6.022 x 10^23

Question 52

What is Faraday's constant (F)?

Answer 52

96485 C/mol

Question 53

What is the Faraday's constant equation?

Answer 53

𝚫G = -nFEcell

Question 54

What does 𝚫G = -nFEcell equal?

Answer 54

𝚫G0 = -RT ln K

Question 55

What does -nFEcell equal?

Answer 55

-RT ln K

Question 56

What does E0cell equal?

Answer 56

RT/nF ln K

Question 57

What are batteries?

Answer 57

devices that convert chemical energy to electrical energy (voltaic cell)

Question 58

What are rechargeable batteries?

Answer 58

the reactions are reversible and providing electrical energy, the chemical reactants are regenerated and can be used again