Inorganic Chem 2 Exam 3

Front 1

Le Chatelier's principle

Back 1

when a system in chemical equilibrium is disturbed by a change of temperature, pressure, or concentration, the system shifts in equilibrium to counteract change

Front 2

when you remove moles of something in an equilibrium reaction, what will happen

Back 2

it will go towards that to counteract change

Front 3

If pressure is increased by decreasing volume, what will happen in an equilibrium reaction?

Back 3

reaction will shift to direction with fewer moles

Front 4

Kc=

Back 4

[right side]^stoich coef*...///[left side]^stoich coef

Front 5

equilibrium increase in temp

Back 5

-products increased in increase in temp when endothermic reaction
-products increased in decrease of temp in exothermic reaction

Front 6

Arrhenius acid and base

Back 6

acid: dissolved in water increases amount of hydronium ions

base: increase amount of hydronium ions when dissolved in water

Front 7

Bronsted-Lowry acid and base

Back 7

acid: donates a proton in a proton transfer reaction

base: accepts a proton in a proton transfer reaction

Front 8

Lewis acid and base

Back 8

acid: species that can form a covalent bond by accepting an electron pair from another species

base: a species that can form a covalent bond by donating an electron pair to another species

Front 9

6 strong acids and bases

Back 9

acids: HClO4, H2SO4, HI, HBr, HCl, HNO3

bases: Hydroxides in group 1 and 2 except berryillium

Front 10

An acid base reaction will normally go in the dirrection of what?

Back 10

the weaker acid

Front 11

In general how does acid strenth relate to the periodic table for H-X acid?

Back 11

acid strength increases going right and down

Front 12

In general how does acid strength relate to the periodic table for oxoacids (H-O-Y)?

Back 12

For a species differing only in Y, acid strength will increase as electronegativety increases with Y.

Front 13

polarity

Back 13

when bonded electrons spend more time near one atom than another

Front 14

electronegativety

Back 14

a measure of the ability of an atom in a molecule to draw bonding electrons to itself: increase up and right

Front 15

for oxoacids (H-O-Y), what happens when there are more oxygens? (exclude OH group)

Back 15

acid strength increases with addition of Oxygens

Front 16

The acid strength of the anion relates how to its parent ion

Back 16

negative charge is weaker acid

Front 17

self ionization

Back 17

two like molecules react to give ions

Front 18

ion-product of water equation

Back 18

Kw= [H30+][OH-]=1.0E-14 at 25degC

Front 19

concentration of H30+ in basic, neutral, and acid solution

Back 19

acidic>1.0E-7 M
neutral= 1.0E-7 M
basic< 1.0E-7 M

Front 20

pH equation

Back 20

pH= -log [H3O+]

Front 21

PH of following: stomach acid, Vinegar, Milk, Seawater, Blood, Household ammonia

Back 21

stomach acid: 1.0
Vinegar: 2.5
Milk: 6.4
Seawater: 7.0-8.3
Blood: 7.4
Household ammonia: 11.9

Front 22

pH and pOH equation?

Back 22

pH + pOH= 14.00

Front 23

best indicator?

Back 23

bromthymol blue

Front 24

methyl red

Back 24

red under pH4, orange after

Front 25

bromthymol blue

Back 25

egg color up to 6
light blue at 7
dark blue 8-14

Front 26

phenolphyline

Back 26

clear up until 8, pink at 9 and beyond

Front 27

conjugate acid-base pair

Back 27

two species in an acid base reaction: differ by the loss or gain of a proton

Front 28

acid reacting with water to produce hydronium ion and the conjugate base ion

Back 28

acid ionization or acid dissociation

Front 29

acid ionization constant

Back 29

equilibrium constant for the ionization of a weak acid

Ka

Front 30

why do strong acids not have Ka?

Back 30

they dissociate 100% complete

Front 31

degree of ionization

Back 31

weak electrolyte is the fraction of molecules that react with water to give ions

Front 32

degree of ionization can be exspressed also how?

Back 32

percent ionization

Front 33

if Ka is less than E-3 what?

Back 33

ignore any additions or subtractions of x in ICE equation

Front 34

Polyprotic acid

Back 34

more than 1 H+

Front 35

second ionization constant is generally what compared to the first?

Back 35

much smaller

Front 36

base ionization constant

Back 36

base-ionization constant for a weak base

Front 37

hydrolysis of an ion

Back 37

reaction of an ion with water to produce the conjugate acid and OH- or conjuage base and H30+

Front 38

salt of a strong base and a strong acid

Back 38

gives a neutral aqueous solution: NaCl

Front 39

salt of a strong base and weak acid

Back 39

gives a basic solution: NaCN

Front 40

weak base and stong acid

Back 40

acid solution: NH4Cl

Front 41

weak base and weak acid

Back 41

compare Ka of Cation with Kb of anion: larger number either means basic or acidic

NH4CHO2

NH4+ Ka larger than CH02- Kb

Front 42

Ka and Kb equation

Back 42

Ka * Kb = Kw

Front 43

common ion effect

Back 43

shift in an ionic equilibrium caused by the addition of a solute that provides an ion that takes part in the equilibrium.

Front 44

buffer

Back 44

solution of weak acid and conjugate base: has ability to resist any change in pH to some extent

Front 45

Ksp

Back 45

solubility product constant is the equilibrium constnat for the solubility of equilibrium of a slightly soluble ionic compound

Front 46

Ksp depends on what?

Back 46

temp

Front 47

Qc<Kc
Qc=Kc
Qc>Kc

Back 47

Qc<Kc, forward direction
Qc=Kc at equilibrium
Qc>Kc reverse direction

Front 48

Fractional precipitation

Back 48

technique of separating two or more ions from a solution by adding a reactant that precipitates first one ions, then another, and so forth