Unit 4 Chem Ii

Front 1

reactant quotient

Back 1

Predicts the direction of the reaction (Q).
Q=Keq the system is at equilibrium

Q>Keq there is too much product. has to shift to left to get more reactant too much excess product

Q< Keq there is too much reactant has to shift to right to get more product get rid of excess reactant

Front 2

solubility product

Back 2

Keq for the dissolution of the an insoluble salt (Ksp)

Front 3

2 ways to use Ksp

Back 3

1) to find the equilibrium concentrations of ions in saturated solutions

2) To predict when precipitate will form in reaction

Front 4

ICE table

Back 4

Initial concentrations

Change- how do amounts change to reach equilibrium

Equilibrium- What are the equilibrium concentrations

Front 5

LeChatelier's principal

Back 5

when a system at equilibrium is disturbed , the system will shift in a direction that reestablishes equilibrium

Front 6

disturbances to equilibrium include

Back 6

adding more reactant, removing some reactant, adding product, removing product, changing temp., changing container volume (for gas), adding inert gas, adding catalyst

Front 7

If pressure increases, a system will shift to theside of the reaction with the ______ moles of gas.

Back 7

fewest

Front 8

If pressure decreases, a system will shift to theside of the reaction with the _____ moles of gas.

Back 8

most

Front 9

acid (Arrhenius definition)

Back 9

a substance thatincreases the concentration of H+ (or protons, orH3O+, or H5O2+, or H9O4+) when dissolved in water.

Front 10

H3O+

Back 10

hydronium ion

Front 11

base (Arrhenius definition)

Back 11

a substance thatincreases concentration of OH− in water solution.

Front 12

Be sure you can name the following bases:

Back 12

NaOH KOH Ca(OH)2 Sr(OH)2 Al(OH)3

Front 13

CH3OH and C2H5OH are not bases –they are _______

Back 13

alcohols

Front 14

acid properties

Back 14

• are corrosive (react with metal, skin, and paper).• taste sour (stomach acid, vinegar, citric acid).• ionize in water to increase [H+].• neutralize bases.

Front 15

Bases properties

Back 15

• are corrosive (caustic).• taste bitter or chalky.• feel slippery on the skin.• ionize in H2O or react with H2O to increase [OH−]• neutralize acids.

Front 16

Arrhenius acids and bases neutralize each otherbecause

Back 16

H+ + OH− → H2O

Front 17

Brønsted-Lowry acid

Back 17

a proton (H+) donor.

Front 18

Brønsted-Lowry base

Back 18

a proton acceptor

Front 19

conjugate acid

Back 19

Brønsted-Lowry base afteraddition of H+

Front 20

conjugate base

Back 20

Brønsted-Lowry acid after lossof H+

Front 21

amphoteric substance

Back 21

a substance that caneither accept or donate a proton.

Front 22

The Keq for an acid dissociation is called the ________ and is represented as ______ .

Back 22

acid dissociation constant

Ka

Front 23

Monoprotic acids only have

Back 23

one Ka

Front 24

Polyprotic acids have ___________

Back 24

have two or more Ka values (onefor each ionization or dissociation step).

Front 25

diprotic acids have

Back 25

2 Ka

Front 26

Stronger acids produce ________ conjugate bases.

Back 26

weaker

Front 27

Weaker acids produce _________ conjugate bases.

Back 27

stronger

Front 28

Because this process produces ions where therewere none before, it’s called the ______________

Back 28

autoionization of water.

Front 29

The equilibrium constant for this process is calledthe ______________ or ________________forwater, Kw.

Back 29

ion product, autoionization constant

Front 30

pH scale for acid

Back 30

1-7

Front 31

pH scale for base

Back 31

7-14

Front 32

know seven strong acids

Back 32

HCl chloric acid

HBr Bromic acid

HI iodic acid

HNO3 nitric acid

HClO3 chloric acid

HClO4 perchloric acid

H2SO4 sulfuric acid

Front 33

Strong bases include

Back 33

• soluble hydroxides (Group 1 hydroxides plusCa(OH)2, Sr(OH)2, and Ba(OH)2).• soluble oxides such as Na2O or K2O.• soluble hydrides such as NaH.• soluble amides such as NaNH2.

Front 34

strong acids have a Keq ______.

weak acids have a Keq________.

Back 34

larger than one, less than one

Front 35

acid dissociationconstant

Back 35

The Keq for an acid dissociation. Represented as Ka.

Monoprotic acids have one Ka.Polyprotic acids have two or more Ka values (onefor each ionization or dissociation step).

Front 36

When comparing binary acids containing elementson the same row, the acid containing the more ____________ element will be stronger.

Back 36

electronegative, across to right of row

Front 37

When comparing binary acidscontaining elements in the samefamily, the acid containing the_________ atom will be stronger.

Back 37

larger, down column

Front 38

The more electronegative the ___________ is, thestronger the oxyacid is. The more ____ the stronger

Back 38

central atom, >^ on periodic table, the more Oxygens

Front 39

higher Ka = _________acid

lower Ka = ________ acid

Back 39

stronger, weaker

Front 40

higher pKa = _______ acid

lower pKa = ________ acid

Back 40

weaker, stronger

Front 41

Lewis acid –

Lewis base –

Back 41

an electron-pair acceptor.

an electron-pair donor.

Front 42

Metal ions can accept pairs of electrons to form___________.

Back 42

complex ions

Front 43

buffer

Back 43

a solution thatresists changes in pH when H+or OH−ions are added.

A buffer usually consists of aweak acid and its conjugatebase. Buffers therefore havecomponents that can neutralizeeither added H+ or added OH−.