organic chem tutor and additional information; chem 2

strong acids

HCl

HBr

HI

HNO3

HClO4

H2SO4

the stronger the acid,

the weaker the conjugate base

acids have

a hydrogen in front

bases have

a hydroxide ion

hydrogen next to a metal:

base

NH3

base

hydrogen next to a nonmetal

acid

H+

acid

H-

base

Arrhenius definition of an acid:

release H+ ions in a solution

Arrhenius definition of a base:

release OH- in a solution

bronsted-lowry definition of an acid

proton donor

bronsted-lowry

in an equation, if a compound has accepted an H on the right side of the equation

in an equation, if a compound has lost an H on the right side of the equation, it is a

Acid

acids donate the proton. the conjugate acid is the one who

accepts it

bases accept a proton. the conjugate base is the one who

loses the hydrogen

conjugate base

lost a hydrogen

conjugate acid

gained a hydrogen

acids turn into

conjugate bases

bases turn into

conjugate acids

what is the conjugate acid of H2O?

add H+. go up in charge too.

H3O+

what is the conjugate base of H2O?

lose an H+. go down in charge too.

OH-

pH<7

acidic

pH>7

basic

HF is a

weak acid

NH4+ is a

weak acid

HCl is a

strong acid

HCN is a

weak acid

HBr is a

strong acid

HClO4 is a

strong acid

HNO2 is a

weak acid

HC2H3O2 is a

weak acid

H2SO4 is a

strong acid

HI is a

strong acid

oxyacids:

more oxygen atoms, more acidic

H2SO4>H2SO3

strong acid/base equations contain how many arrows?

1

weak acid/base equations contain how many arrows?

2

KOH is a

strong base

strong bases -OH

Li, Na, K, Rb, Cs

strong bases -(OH)2

Be, Mg, Ca, Ba, Sr

A

F- is a

weak base

NO2- is a

weak base

CN- is a

weak base

OH is a

strong base

O^-2 is a

strong base

H- is a

strong base

HSO3- is a

weak base

the less hydrogens on an atom, the more

basic it is

a stronger base will produce a

weaker conjugate base

acids turn blue litmus paper

red

bases turn red litmus paper

blue

can acids and bases conduct electricity in a solution?

yes

lewis acids are

e-pair acceptors

lewis bases are

e- pair donors

acids taste

sour

bases taste

bitter and feel slippery

weak acids and bases are weak

electrolytes

amphoteric

water.

can act as an acid or base

Kw

auto-ionization constant for water

dependent on temp (bc it is an equilibrium constant)

T ^, Kw

^

Kw = at 25C

1×10^-14

Kw=

Ka*Kb= 1×10^-14

NaCl is a

neutral salt

percent ionization for ICE table problems: acids

x (H+)/ [HA]initial *100%

percent ionization for ICE table problems: bases

x (OH-)/ [A-]initial *100%

if Kb, Ka, or Kc have an exponent of -5, you can assume

.1-x or anything similar is just .1 or the constant!

what is the pH of a .4 M NH4Cl solution? Kb of NH3 is 1.8×10^-5.

• NH₄Cl is a salt of a weak base (NH₃) and a strong acid (HCl).

• It dissociates completely in water:

  NH4​Cl→NH4+​ + Cl−

• The NH₄⁺ ion is acidic and will hydrolyze in water:

  NH4+ ​+ H2​O⇌NH3 ​+ H3​O+ *** use this equation!

since we’re given concentration of the weak acid originally, use Ka.

Ka*Kb= Kw= 1×10^-14.

continue !

what is the pH of a 1.5 M NaF solution? Ka of HF is 7.2×10^-4.

NaF>Na+ + F-

F- + H2O >< HF + OH- ** USE THIS EQ FOR THE ICE TABLE!

since we are given initial concentration of our weak base (F), use Kb!

find from Kb*Ka= Kw= 1×10^-14

continue!

the conjugate base of a strong acid is

neutral

the conjugate base of a weak acid is

basic

NH4+

acidic

Al+3

acidic

Cl-

neutral

F-

basic

Br-

neutral

Pb+4

acidic

I-

neutral

NO2-

basic

Fe3+

acidic

Cu+2

acidic

SO3^(2-)

basic

C2H3O2-

basic

NO3-

neutral

CN-

basic

ClO4-

neutral

SO4^(2-)

neutral

CO3^(2-)

basic

alkali metals

neutral

H-

basic

OH-

basic

O^(-2)

basic

O-

basic

KCl

neutral (contains an alkali metal and Cl)

NaOH

Basic (contains Na which is neutral but OH is basic)

NH4Cl

Acidic (NH4+ is acidic and Cl- is neutral)

AlBr3

acidic (Al3+ is acidic and Br is neutral)

NaF

basic (Na is neutral and F is basic)