Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases...

Acid/Base Definitions Arrhenius Model

Acids produce hydrogen ions in aqueous solutions

Bases produce hydroxide ions in aqueous solutions

Bronsted-Lowry Model Acids are proton donors Bases are proton acceptors

Lewis Acid Model Acids are electron pair acceptors Bases are electron pair donors

Acid DissociationAcid Dissociation

HA H+ + A-

Acid Proton Conjugate

base

][

]][[

HA

AHKa

Alternately, H+ may be written in its hydrated form, H3O+ (hydronium ion)

Dissociation of Strong AcidsDissociation of Strong AcidsStrong acids are assumed to dissociate completely in solution.

Large Ka or small Ka?Reactant favored or product favored?

Dissociation Constants: Strong Dissociation Constants: Strong AcidsAcids

Acid Formul

a Conjugate

Base Ka

Perchloric HClO4 ClO4- Very large

Hydriodic HI I- Very large

Hydrobromic HBr Br- Very large

Hydrochloric HCl Cl- Very large

Nitric HNO3 NO3- Very large

Sulfuric H2SO4 HSO4- Very large

Hydronium ion H3O+ H2O 1.0

Strength of oxyacids

• The more oxygen hooked to the central atom, the more acidic the hydrogen.

• HClO4 > HClO3 > HClO2 > HClO

• Remember that the H is attached to an oxygen atom.

• The oxygens are electronegative

• Pull electrons away from hydrogen

Strength of oxyacidsStrength of oxyacids

Electron Density

Cl O H


Electron Density

Cl O HO


Cl O H

O

O

Electron Density

Strength of oxyacids

Cl O H

O

O

O

Electron Density

Dissociation of Weak AcidsDissociation of Weak AcidsWeak acids are assumed to dissociate only slightly (less than 5%) in solution.

Large Ka or small Ka?Reactant favored or product favored?

Dissociation Constants: Weak Dissociation Constants: Weak AcidsAcids

Acid Formula Conjugate Base

Ka

Iodic HIO3 IO3- 1.7 x 10-1

Oxalic H2C2O4 HC2O4- 5.9 x 10-2

Sulfurous H2SO3 HSO3- 1.5 x 10-2

Phosphoric H3PO4 H2PO4- 7.5 x 10-3

Citric H3C6H5O7 H2C6H5O7- 7.1 x 10-4

Nitrous HNO2 NO2- 4.6 x 10-4

Hydrofluoric HF F- 3.5 x 10-4

Formic HCOOH HCOO- 1.8 x 10-4

Benzoic C6H5COOH C6H5COO- 6.5 x 10-5

Acetic CH3COOH CH3COO- 1.8 x 10-5

Carbonic H2CO3 HCO3- 4.3 x 10-7

Hypochlorous HClO ClO- 3.0 x 10-8

Hydrocyanic HCN CN- 4.9 x 10-10

Self-Ionization of WaterSelf-Ionization of Water

H2O + H2O H3O+ + OH-

At 25, [H3O+] = [OH-] = 1 x 10-7

Kw is a constant at 25 C:

Kw = [H3O+][OH-]

Kw = (1 x 10-7)(1 x 10-7) = 1 x 10-14 = [Ka][Kb]

Calculating pH, Calculating pH, pOHpOHpH = -log10(H3O+)

pOH = -log10(OH-)

Relationship between pH and Relationship between pH and pOHpOH pH + pOH = 14

Finding [HFinding [H33OO++], [OH], [OH--] from pH, pOH] from pH, pOH

[H3O+] = 10-pH

[OH-] = 10-pOH

pH and pOH Calculations

H + O H -

pH pO H

[O H -] = 1 x 10 - 1 4

[H + ]

[H + ] = 1 x 10 - 1 4

[O H -]

p O H = 14 - p H

p H = 14 - p O H

pOH

= -l

og[O

H- ]

pH =

-log

[H+

]

[OH

- ] = 1

0-pO

H

[H+

] = 1

0-pH

A Weak Acid Equilibrium A Weak Acid Equilibrium ProblemProblem

What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-

5 ?

Step #1: Write the dissociation equation

HC2H3O2 (aq) + H2O(l) C2H3O2-(aq) + H+

(aq)



5 ?

Step #2: ICE it!

HC2H3O2 C2H3O2- + H+

II

CC

EE

0.50 0 0

- x +x +x

0.50 - x xx



5 ?

Step #3: Set up the law of mass action


0.50 - x xxEE

)50.0()50.0(

))((108.1

25 x

x

xxx



5 ?

Step #4: Solve for x, which is also [H+]


0.50 - x xxEE

)50.0(108.1

25 x

x [H+] = 3.0 x 10-3 M



5 ?

Step #5: Convert [H+] to pH


0.50 - x xxEE

pH = - log (3.0 x 10-3) = 2.52

Dissociation of Strong Dissociation of Strong BasesBases

Strong bases are metallic hydroxides Group I hydroxides (NaOH, KOH) are

very soluble Group II hydroxides (Ca, Ba, Mg, Sr)

are less soluble pH of strong bases is calculated

directly from the concentration of the base in solution

MOH(s) M+(aq) + OH-(aq)

Reaction of Weak Bases with Reaction of Weak Bases with WaterWater

The base reacts with water, producing The base reacts with water, producing its conjugate acid and hydroxide ion:its conjugate acid and hydroxide ion:

CH3NH2 + H2O CH3NH3+ + OH- Kb = 4.38 x 10-

4

4 3 3

3 2

[ ][ ]4.38 10

[ ]b

CH NH OHK x

CH NH

KKbb for Some Common Weak for Some Common Weak BasesBases

Base Formula Conjugate Acid

Kb

Ammonia NH3 NH4+ 1.8 x 10-5

Methylamine CH3NH2 CH3NH3+ 4.38 x 10-4

Ethylamine C2H5NH2 C2H5NH3+ 5.6 x 10-4

Diethylamine (C2H5)2NH (C2H5)2NH2+ 1.3 x 10-3

Triethylamine (C2H5)3N (C2H5)3NH+ 4.0 x 10-4

Hydroxylamine HONH2 HONH3+

1.1 x 10-8

Hydrazine H2NNH2 H2NNH3+

3.0 x 10-6

Aniline C6H5NH2 C6H5NH3+

3.8 x 10-10

Pyridine C5H5N C5H5NH+ 1.7 x 10-9

Many students struggle with identifying weak bases and their conjugate acids.What patterns do you see that may help you?

Reaction of Weak Bases with Reaction of Weak Bases with WaterWater

The generic reaction for a base The generic reaction for a base reacting with water, producing its reacting with water, producing its conjugate acid and hydroxide ion:conjugate acid and hydroxide ion:

B + H2O BH+ + OH-

[ ][ ]

[ ]b

BH OHK

B

A Weak Base Equilibrium A Weak Base Equilibrium ProblemProblem

What is the pH of a 0.50 M solution of ammonia, NH3, Kb = 1.8 x 10-5 ?

Step #1: Write the equation for the reaction

NH3 + H2O NH4+ + OH-



Step #2: ICE it!

II

CC

EE

0.50 0 0

- x +x +x

0.50 - x xx



Step #3: Set up the law of mass action

0.50 - x xxEE

)50.0()50.0(

))((108.1

25 x

x

xxx




Step #4: Solve for x, which is also [OH-]

0.50 - x xxEE

)50.0(108.1

25 x

x [OH-] = 3.0 x 10-3 M




Step #5: Convert [OH-] to pH

0.50 - x xxEE



pOH = - log (3.0 x 10-3) = 2.52

pH = 14 - pOH = 11.48

Acid-Base Properties of SaltsAcid-Base Properties of Salts

Type of Salt Examples

Comment pH of solution

Cation is from a strong base, anion from a strong acid

KCl, KNO3

NaCl NaNO3

Both ions are neutral

Neutral

These salts simply dissociate in water:

KCl(s) K+(aq) + Cl-(aq)




Cation is from a strong base, anion from a weak acid

NaC2H3O2

KCN, NaF

Cation is neutral, Anion is basic

Basic

C2H3O2- + H2O HC2H3O2 + OH-

base acid acid base

The basic anion can accept a proton from water:




Cation is the conjugate acid of a weak base, anion is from a strong acid

NH4Cl,

NH4NO3

Cation is acidic, Anion is neutral

Acidic

NH4+(aq) NH3(aq) + H+(aq)

Acid Conjugate Proton base

The acidic cation can act as a proton donor:




Cation is the conjugate acid of a weak base, anion is conjugate base of a weak acid

NH4C2H3O2

NH4CN

Cation is acidic, Anion is basic

See below

IF Ka for the acidic ion is greater than Kb for the basic ion, the solution is acidic

IF Kb for the basic ion is greater than Ka for the acidic ion, the solution is basic

IF Kb for the basic ion is equal to Ka for the acidic ion, the solution is neutral

Acid-Base Properties of SaltsAcid-Base Properties of SaltsType of Salt Exampl

esComment pH of

solutionCation is a highly charged metal ion; Anion is from strong acid

Al(NO3)2

FeCl3

Hydrated cation acts as an acid; Anion is neutral

Acidic

Step #1: AlCl3(s) + 6H2O Al(H2O)6

3+(aq) + Cl-(aq) Salt water Complex ion anion

Step #2: Al(H2O)6

3+(aq) Al(OH)(H2O)52+(aq) + H+(aq)

Acid Conjugate base Proton

Effect of Structure on Acid-Effect of Structure on Acid-Base Base

PropertiesProperties

Hydrated metals

• Highly charged metal ions pull the electrons of surrounding water molecules toward them.

• Make it easier for H+ to come off.

Al+3 OH

H

Acid-Base Properties of Oxides

• Non-metal oxides dissolved in water can make acids.

• SO3 (g) + H2O(l) H2SO4(aq)

• Ionic oxides dissolve in water to produce bases.

• CaO(s) + H2O(l) Ca(OH)2(aq)

What is the concentration of H3O+ in pure water?

1. 1.00 x 10–7 M

2. 7.00 M3. 1.00 x 10-14 4. 1.00 x 107 M5. 7.00 x 10-14

[H+] = 8.26 x 10–5 M, what is the pH of the solution?

1.2.162.4.1 3.4.084.4.0835.8.024

Which of the following is a conjugate acid/base pair?1. HCl/OCl-

2. H2SO4/SO42-

3. NH4+/NH3

4. H3O+/OH-

5. none of these

Which of the following indicates the most basic solution?1. [H+] = 1 × 10–10 M 2. pOH =6.7 3. [OH–] = 7 × 10–5 M 4. pH = 4.2 5. At least two of the

solutions are equally basic.

Dissolving Na2SO4 in water will create a ______ solution.

1. Acidic2. Basic3. Neutral4. Cannot be

determined.

Calculate the pH of a 0.17 M solution of HOCl, Ka = 3.5 10-8.

1.4.112.8.233.9.894.1.005.3.77

Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases...

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