ch. 17 &19 test

Question 1

the common ion effect

Answer 1

whenever a weak electrolyte and a strong electrolyte containing a common ion are together in solution, the weak electrolyte ionizes less than if would if it were alone in solution.

Question 2

buffers

Answer 2

solutions of a weak conjugate acid-base pair that resist drastic changes in pH

Question 3

henderson-hasselback equation

Answer 3

pH=pKa+log([A-]/[HA])

Question 4

addition of a strong acid or a strong base to a buffer is…

Answer 4

a neutralization reaction

Question 5

titration of a strong acid w/ a strong base

Answer 5

S

Question 6

titration of a strong base w/ a strong acid

Answer 6

backwards S

Question 7

titration of a weak acid w/ a strong base

Answer 7

S shifts up

Question 8

more soluble salt

Answer 8

has an anion that is the conjugate base of a weak acid.

Question 9

unchanged solubility salt

Answer 9

has anion that is the conjugate base of a string acid

Question 10

complex ion formation

Answer 10

metal ions can act as lewis acids and form complex ions with lewis base in the solvent

Question 11

formation of what increases the solubility of certain salts?

Answer 11

complex ions

Question 12

Amphoterism

Answer 12

amphoteric oxides and hydroxides are soluble in strong acids or base, because they can act either as acids or bases

Question 13

metals with amphoterism behavior

Answer 13

Al^+3, Cr^+3, Zn^+3, and Sn^+2

Question 14

Q=Ksp

Answer 14

the system is at equilibrium and the solution is saturated

Question 15

Q<Ksp

Answer 15

more solid can dissolve, no precipitate forms

Question 16

Q>Ksp

Answer 16

a precipitate will form

Question 17

first law of thermodynamics

Answer 17

energy cannot be created or destroyed

Question 18

enthalpy

Answer 18

is the heat absorbed or released by a system during a constant-pressure process

Question 19

entropy

Answer 19

is a measure of the randomness in a system

Question 20

spontaneous process

Answer 20

proceed without any outside assistance

Question 21

experimental factors that affect spontaneous processes

Answer 21

temperature and pressure

Question 22

reversible process

Answer 22

the system changes so that the system and surroundings can be returned to the original state by exactly reversing the process. this maximizes work done by a system on the surroundings

Question 23

irreversible process

Answer 23

cannot be undone by exactly reversing the change to the system or cannot have the process exactly followed in reverse.

Question 24

second law of thermodynamics

Answer 24

the entropy of the universe increases in any spontaneous process.

Question 25

entropy equation

Answer 25

ΔS= Sfinal-Sinitial or ΔS=qrev/T(constant T)

Question 26

reversible process

Answer 26

ΔS univ=ΔSsys +ΔSsurr=0

Question 27

irreversible process

Answer 27

ΔS univ=ΔSsys +ΔSsurr>0

Question 28

microstate

Answer 28

a single possible arrangement of position nd kinetic energy of molecules

Question 29

Boltzman equation

Answer 29

S=klnW

Question 30

entropy increases with

Answer 30

the number if microstates of a system

Question 31

translational

Answer 31

movement of the entire molecule from one place to another

Question 32

vibrational

Answer 32

periodic motion of atoms within a molecule

Question 33

rotational

Answer 33

rotation of the molecule about an axis

Question 34

the number of microstates possible for a system increase with

Answer 34

- an increase in volume - an increase in temperature - an increase in the number of atoms/molecules

Question 35

entropy of a system increases for process where

Answer 35

- gases form from either solids or liquids - liquids or solutions form from solids - the number of gas molecules increases during a chemical reaction

Question 36

factors that affect entropy

Answer 36

1. physical state 2. amount of substance more ->greater 3. temp. higher->greater 4. vol./pressure: higher vol. lower pressure -> greater 5. size: larger -> greater

Question 37

third law of thermodynamics

Answer 37

the entropy of a pure crystalline substance at absolute zero is 0.

Question 38

entropy change equation

Answer 38

ΔS= ΣΔS^o(products)- ΣΔS^o(reactants)

Question 39

ΔS^o

Answer 39

is the standrad moalr entropy and n and m coefficients of the balanced chemical equation

Question 40

ΔS^o bullet points

Answer 40

- is not zero for the elements - values of (g) > (l) > (s) - increase with molar mass and number of atoms

Question 41

ΔSsurr=

Answer 41

-ΔH/T

Question 42

Gibbs free energy

Answer 42

enthalpy and entropy can be used to predict whether a reaction is spontaneous using the states function ΔG

Question 43

ΔG=

Answer 43

ΔH-TΔS

Question 44

ΔG>0

Answer 44

the forward reaction is spontaneous

Question 45

ΔG=0

Answer 45

the system is at equilibrium

Question 46

ΔG<0

Answer 46

the reaction is non spontaneous but spontaneous in the reverse direction

Question 47

ΔG^o=

Answer 47

ΣΔGf^o(products)- ΣΔGf^o(reactants)

Question 48

when -ΔH & +ΔS

Answer 48

spontaneous at all temperatures

Question 49

when +ΔH & -ΔS

Answer 49

non spontaneous at all temperatures

Question 50

when -ΔH & -ΔS

Answer 50

Spontaneous at low Temp; nonspontaneous at high temp

Question 51

when +ΔH & +ΔS

Answer 51

spontaneous at high temp; nonspontaneous at low temp