16-1 chem 102, fall 2012, la tech cth 328 10:00-11:15 am instructor: dr. upali siriwardane e-mail:...
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16-1CHEM 102, Fall 2012, LA TECH
CTH 328 10:00-11:15 am
Instructor: Dr. Upali Siriwardane
e-mail: [email protected]
Office: CTH 311 Phone 257-4941
Office Hours: M,W 8:00-9:00 & 11:00-12:00 am;
Tu, Th, F 8:00 - 10:00am..
Exams: 10:00-11:15 am, CTH 328.
September 27, 2012 (Test 1): Chapter 13
October 18, 2012 (Test 2): Chapter 14 &15
November 13, 2012 (Test 3): Chapter 16 &18
Optional Comprehensive Final Exam: November 15, 2012 :
Chapters 13, 14, 15, 16, 17, and 18
Chemistry 102(001) Fall 2012
16-2CHEM 102, Fall 2012, LA TECH
Chapter 16. Acids and Bases
16.1 The Brønsted-Lowry Concept of Acids and Bases
16.2 Types of acids/bases:Organic Acids and Amines
16.3 The Autoionization of Water
16.4 The pH Scale
16.5 Ionization Constants of Acids and Bases
16.6 Problem Solving Using Ka and Kb
16.7 Molecular Structure and Acid Strength
16.8 Acid-Base Reactions of Salts
16.9 Practical Acid-Base Chemistry
16.10 Lewis Acid and Bases
16-3CHEM 102, Fall 2012, LA TECH
Types of Reactionsa) Precipitation Reactions. Reactions of ionic compounds or
saltsb) Acid/base Reactions. Reactions of acids and basesc) Redox Reactions. reactions of oxidizing & reducing
agents
16-4CHEM 102, Fall 2012, LA TECH
What are Acids &Bases?
Definition?
a) Arrhenius
b) Bronsted-Lowry
c) Lewis
16-5CHEM 102, Fall 2012, LA TECH
Arrhenius, Svante August (1859-1927), Swedish chemist, 1903 Nobel Prize in chemistry
•Acid Anything that produces hydrogen ions in a water solution.
HCl (aq) H+
( aq) + Cl-
( aq)
•Base Anything that producs hydroxide ions in a water solution.
NaOH (aq) Na+
( aq) + OH
- ( aq)
•Arrhenius definitions are limited proton acids and hydroxide bases
to aqueous solutions.
Arrhenius Definitions
16-6CHEM 102, Fall 2012, LA TECH
Expands the Arrhenius definitions to include many bases other than hydroxides and gas phase reactions
Acid Proton donor
Base Proton acceptor
This definition explains how substances like ammonia can act as bases.
Eg. HCl(g) + NH3(g) ------> NH4Cl(s)
HCl (acid), NH3 (base).
NH3(g) + H2O(l) NH4+
+ OH-
Brønsted-Lowry definitions
16-7CHEM 102, Fall 2012, LA TECH
Lewis DefinitionG.N. Lewis was successful in including acid and bases
without proton or hydroxyl ions.
Lewis Acid: A substance that accepts an electron pair.
Lewis base: A substance that donates an electron pair.
E.g. BF3(g) + :NH3(g) F3B:NH3(s)
the base donates a pair of electrons to the acid forming a
coordinate covalent bond common to coordination
compounds. Lewis acids/bases will be discussed later in
detail
16-8CHEM 102, Fall 2012, LA TECH
1) Acids and bases can be defined in several ways. Which definitions of the bases that fits the description below?
a) a compound that produces more OH- ions in water:
b) a proton acceptor:
c) an electron pair donor:
16-9CHEM 102, Fall 2012, LA TECH
Types of Acids and Bases
Binary acids
Oxyacid
Organic acids
Acidic oxides
Basic oxides
Amine
Polyprotic acids
16-10CHEM 102, Fall 2012, LA TECH
Types of Acids and BasesBinary acids: HCl, HBr, HI, H2S
More than two elements: HCN
Oxyacid: HNO3, H2SO4, H3PO4
Polyprotic acids: H2SO4, H3PO4
Organic acids: R-COOH, R= CH3-, CH3CH2-
Acidic oxides: SO3, NO2, CO2,
Basic oxides: Na2O, CaO
Amine: NH3. R-NH2, R= CH3-, CH3CH2- : primary
R2-NH : secondary, R3-N: tertiary
Lewis acids & bases: BF3 and NH3
16-11CHEM 102, Fall 2012, LA TECH
Acidic Oxides
These are usually oxides of non-metallic elements such as P, S and N.
E.g. NO2, SO2, SO3, CO2
They produce oxyacids when dissolved in waterSO3 + H2O ---> H2SO4
CO2 + H2O ---> H2CO3
NO2 + H2O ---> HNO3
16-12CHEM 102, Fall 2012, LA TECH
Basic Oxides
Oxides oxides of metallic elements such as Na, K, Ca. They produce hydroxyl bases when dissolved in water.
e.g. CaO + H2O ---> Ca(OH)2
Na2O + H2O ---> 2 NaOH
16-13CHEM 102, Fall 2012, LA TECH
Protic Acids
Monoprotic Acids: The form protic refers to acidity due to protons. Monoprotic acids have only one acidic proton. e.g. HCl.
Polyprotic Acids: They have more than one acidic proton.
e.g. H2SO4 - diprotic acid
H3PO4 - triprotic acid.
16-14CHEM 102, Fall 2012, LA TECH
Polyprotic Acidsacids where more than one hydrogen per molecule
is released
16-15CHEM 102, Fall 2012, LA TECH
Amines
Class of organic bases derived from ammonia NH3 by replacing hydrogen by organic groups. They are defined as bases similar to NH3 by Bronsted-Lowery or Lewis acid/base definitions.
16-16CHEM 102, Fall 2012, LA TECH
Amines
16-17CHEM 102, Fall 2012, LA TECH
2) Identify types of acids/bases as: binary acids, oxy acids, organic acids, acidic oxides, basic oxides, amine and polyprotic acids.
a) HF b) HBr c) H3PO4
d) H2SO4 e) HNO3 f) R-COOH
g) NO2 h) SO3 j)CaO
k) R-NH2
16-18CHEM 102, Fall 2012, LA TECH
Influence of Molecular Structure on Acid Strength
Binary Hydrides• hydrogen & one other element
Bond Strengths• weaker the bond, the stronger the acid
Stability of Anion• higher the electronegativity, stronger the acid
16-19CHEM 102, Fall 2012, LA TECH
Binary Acids
Compounds containing acidic protons bonded to a more electronegative atom.
e.g. HF, HCl, HBr, HI, H2S
The acidity of the haloacid (HX; X = Cl, Br, I, F)Series increase in the following order: HF < HCl < HBr < HI
16-20CHEM 102, Fall 2012, LA TECH
Oxyacids
Compounds containing acidic - OH groups in the molecule.
Acidity of H2SO4 is greater than H2SO3 because of the extra O (oxygens)
The order of acidity of oxyacids from the a halogen (Cl, Br, or I) shows a similar trend.
HClO4 > HClO3 > HClO2 > HClO
perchloric chloric chlorus hyphochlorus
16-21CHEM 102, Fall 2012, LA TECH
Influence of Molecular Structure on Acid Strength
Oxyacids• hydrogen, oxygen, & one other element
H-O-E• higher the electronegativity on E, stronger the acid as
this weakens the bond between the O and H
16-22CHEM 102, Fall 2012, LA TECH
< <<
<
Oxo Acid
16-23CHEM 102, Fall 2012, LA TECH
3) Which of the following is stronger acid or base:
a) H2SO4 or H2SO3:
b) HCl or HI:
c) HClO or HClO3:
d) H2S or HF:
e) CF3COOH or CH3COOH:
f) CH3COOH or CH3CH2COOH
16-24CHEM 102, Fall 2012, LA TECH
DissociationStrong Acids:
HCl(aq) + H2O(l) H3+O(aq) + Cl-(aq)
H2SO4(aq) + H2O(l) H3+O(aq) + HSO4
-(aq)
Dissociation Equilibrium Weak Acid/base:
H2O(l) + H2O(l) H3+O(aq) + OH-(aq)
This dissociation is called autoionization of water.
HC2H3O2(aq) + H2O(l) H3+O(aq) + C2H3O2
-(aq)
NH3 (aq) + H2O(l) NH4+ + OH-(aq)
Equilibrium constants: Ka, Kb and Kw
16-25CHEM 102, Fall 2012, LA TECH
4) Write equations for the dissociation equilibrium reactions for the following acids and bases in water. Which of these are acid or dissociations?
a) HCl:
b) H2SO4 :
16-26CHEM 102, Fall 2012, LA TECH
4) Write equations for the dissociation equilibrium reactions for the following acids and bases in water. Which of these are acid or dissociations?
c) H2O (autoionization): What is auto ionization?
d) HC2H3O(acetic acid):
e) NH3:
16-27CHEM 102, Fall 2012, LA TECH
Bronsted acid/conjugate base and base/conjugate acid pairs inacid/base equilibria
HCl(aq) + H2O(l) H3+O(aq) + Cl-(aq)
HCl(aq): acid
H2O(l): base
H3+O(aq): conjugate acid
Cl-(aq): conjugate base
H2O/ H3+O: base/conjugate acid pair
HCl/Cl-: acid/conjugate base pair
16-28CHEM 102, Fall 2012, LA TECH
Conjugate acid-base pairs.
Acids and bases that are related by loss or gain of H+ as H3O+
and H2O.
Examples. Acid Base
H3O +
H2O
HC2H3O2 C2H3O2-
NH4 +
NH3
H2SO4 HSO4-
HSO4- SO4
2-
Brønsted-Lowry Definitions
16-29CHEM 102, Fall 2012, LA TECH
Select acid, base, acid/conjugate base pair,base/conjugate acid pair
H2SO4(aq) + H2O(l) H 3+O(aq) + HSO4
-(aq)acid
base
conjugate acid
conjugate base
base/conjugate acid pair
acid/conjugate base pair
16-30CHEM 102, Fall 2012, LA TECH
5) For HOCl write:
a) Dissociation equilibrium reaction for the HOCl:
b) Identify the acid/conjugate base pair:
c) Identify the base/conjugate acid pair:
d) The equilibrium constant expression:
16-31CHEM 102, Fall 2012, LA TECH
Strong Acid vs. Weak AcidsStrong acidcompletely ionizedHydrioidic HI Ka ~ 1011 pKa = -11Hydrobromic HBr Ka ~ 109 pKa = -9Perchloric HClO4 Ka ~ 107 pKa = -7Hyrdrochloric HCl Ka ~ 107 pKa = -7Chloric HClO3 Ka ~ 103 pKa = -3Sulfuric H2SO4 Ka ~ 102 pKa = -2Nitric HNO3 Ka ~ 20 pKa = -1.3Weak acidpartially ionizedHydrofluoric acid HF Ka = 6.6x10-4 pKa = 3.18Formic acid HCOOH Ka = 1.77x10-4 pKa = 3.75Acetic acid CH3COOH Ka = 1.76x10-5 pKa = 4.75Nitrous acid HNO2 Ka = 4.6x10-4 pKa = 3.34Acetyl Salicylic acid C9H8O4 Ka = 3x10-4 pKa = 3.52Hydrocyanic acid HCN Ka = 6.17x10-10 pKa = 9.21
16-32CHEM 102, Fall 2012, LA TECH
Strong Base vs. Weak BaseStrong Basecompletely ionizedLithium hydroxide LiOHSodium hydroxide NaOH
Potassium hydroxide KOH Kb~ 102-103
Rubidium hydroxide RbOHCesium hydroxide CsOHBoarder-line Bases
Magnesium hydroxide Mg(OH)2
Calcium hydroxide Ca(OH)2
Strotium hydroxide Sr(OH)2 Kb~ 0.01 to0.1
Barium hydroxide Ba(OH)2
Weak Basepartially ionized
Ammonia NH3 Kb=1.79x10-5 pKb = 4.74
Ethyl amine CH3CH2NH2 Kb=5.6x10-4 pKb = 3.25
16-33CHEM 102, Fall 2012, LA TECH
•Strong acids Ionize completely in water. HCl, HBr, HI,
HClO3,
HNO3, HClO4, H2SO4.
•Weak acids Partially ionize in water.
Most acids are weak.
•Strong bases Ionize completely in water.
Strong bases are metal hydroxides - NaOH,
KOH
•Weak bases Partially ionize in water.
Acid and Base Strength
16-34CHEM 102, Fall 2012, LA TECH
Common Acids and BasesAcids Formula Molarity*
nitric HNO3 16
hydrochloric HCl 12
sulfuric H2SO4 18
acetic HC2H3O2 18
Bases
ammonia NH3(aq) 15
sodium hydroxide NaOH solid
*undiluted.
16-35CHEM 102, Fall 2012, LA TECH
6. Identify stronger and weaker acids:
16-36CHEM 102, Fall 2012, LA TECH
Autoionization When water molecules react with one another to form ions.
Acids and bases alter the dissociation equilibrium of water based on Le Chaterlier’s principle
Kw = [ H3O+
] [ OH- ]
= 1.0 x 10-14
at 25oC
Note: [H2O] is constant and is included in Kw.
ion product
of water
ion product
of water
H2O(l) + H2O(l) H3O+(aq) + OH-(aq)
(10-7
M) (10-7M)
Autoionization of Water
16-37CHEM 102, Fall 2012, LA TECH
What is pH?
Kw = [H3+O][OH-] = 1 x 10-14
[H3+O][OH-] = 10-7 x 10-7
Extreme cases:
Basic medium
[H3+O][OH-] = 10-14 x 100
Acidic medium
[H3+O][OH-] = 100 x 10-14
pH value is -log[H+]
spans only 0-14 in water.
16-38CHEM 102, Fall 2012, LA TECH
We need to measure and use acids and bases over a very large
concentration range.
pH and pOH are systems to keep track of these very large ranges.
pH = -log[H3O+
]
pOH = -log[OH-]
pH + pOH = 14
Substance pH
1 M HCl 0.0
Gastric juices 1.0 - 3.0
Lemon juice 2.2 - 2.4
Classic Coke 2.5
Coffee 5.0
Pure Water 7.0
Blood 7.35 - 7.45
Milk of Magnesia 10.5
Household ammonia 12.0
1M NaOH 14.0
Substance pH
1 M HCl 0.0
Gastric juices 1.0 - 3.0
Lemon juice 2.2 - 2.4
Classic Coke 2.5
Coffee 5.0
Pure Water 7.0
Blood 7.35 - 7.45
Milk of Magnesia 10.5
Household ammonia 12.0
1M NaOH 14.0
pH and other “p” scales
16-39CHEM 102, Fall 2012, LA TECH
A logarithmic scale used to keep track of the large changes in [H+].
0 7 14
10-14
M 10-7
M 10-14
M
Very Neutral Very
acidic Basic
When you add an acid to, the pH gets smaller.
When you add a base to, the pH gets larger.
pH scale
16-40CHEM 102, Fall 2012, LA TECH
pH of Aqueous Solutions
16-41CHEM 102, Fall 2012, LA TECH
pH, pKw and pOHThe relation of pH, Kw and pOH Kw = [H+][OH-] log Kw = log [H+] + log [OH-] -log Kw= -log [H+] -log [OH-] ; previous equation multiplied by -1 pKw = pH + pOH; pKw = 14 since Kw =1 x 10-14
14 = pH + pOH
pH = 14 - pOH
pOH = 14 - pH
14 = pH + pOH
pH = 14 - pOH
pOH = 14 - pH
16-42CHEM 102, Fall 2012, LA TECH
Measuring pH
Arnold Beckman
inventor of the pH meter
father of electronic instrumentation
16-43CHEM 102, Fall 2012, LA TECH
7. Identify the following as acidic/basic/neutral and estimate/calculate pH.
Solution Acidic/basic/neutral pH of the solution
a) [ H+] > [OH-] and [H+] > 1.0 x 10-7 M : :
b) [H+] < [OH-] and [H+] < 1.0 x 10-7 M : :
c) [H+] = [OH-] = 1.0 x 10-7 M : :
d) [H+] > [OH-] = 1.0 × 10-14 M : :
e) [H+]< [OH-] = 1.0 x 10+7 M : :
16-44CHEM 102, Fall 2012, LA TECH
pH and pOH calculations of acid and base solutions
a) Strong acids/bases
dissociation is complete for strong acid such as HNO3 or base NaOH
[H+] is calculated from molarity (M) of the solution
b) weak acids/bases
needs Ka , Kb or percent(%)dissociation
16-45CHEM 102, Fall 2012, LA TECH
pH of 0.5 M H2SO4 Solution
H2SO4(aq) + H2O(l) H3+O(aq) + HSO4
-(aq)
HSO4-(aq) + H2O(l) H3
+O(aq) + SO42-(aq)
[H3+O][HSO4
-]
H2SO4 ; Ka1 = -------------------
[H2SO4]
[H3+O][SO4
2-]
H2SO4 ; Ka2 = ------------------- ; Ka2 ignored
[HSO4-]
16-46CHEM 102, Fall 2012, LA TECH
H2SO4(aq) + H2O(l) H3+
O(aq) + HSO4-(aq)
the moles of H+
ions in the solution is equal to moles of H2SO4 at the beginning.
[H2SO4] = [H+
] = 0.5 mole/L
pH = -log [H+
]
pH = -log(0.5)
pH = 0.30
pH of 0.5 M H2SO4 Solution
16-47CHEM 102, Fall 2012, LA TECH
1.5 x 10-2 M NaOH.1.5 x 10-2 M NaOH.
NaOH is also a strong base dissociates completely in water.
[NaOH] = [HO- ] = 1.5 x 10-2 mole/L
pOH = -log[HO-]= -log(1.5 x 10-2)
pOH = 1.82
As defined and derived previously:
pKw= pH + pOH; pKw= 14
pH = pKw + pOH
pH = 14 - pOH
pH = 14 - 1.82 ; pH = 12.18
16-48CHEM 102, Fall 2012, LA TECH
8) For a 0.10 M solution of Ba(OH)2.Is it a strong base?
a) How many OH- are in the compound?
b) Calculate the [OH-] and [H+]:
c) pH of the solution:
16-49CHEM 102, Fall 2012, LA TECH
9) Calculate the pH of the strong acid 0.2 M H2SO4.
a) Is it a strong acid?
b) Is it polyprotic acid?
c) Dissociation equilibria:
d) Why second dissociation equilibria is not considered for [H+] concentration?
e) Calculate the [H+]
f) pH of the solution:
16-50CHEM 102, Fall 2012, LA TECH
pH of Mixtures of Strong and Weak Acidsthe presence of the strong acid retards the
dissociation of the weak acid
The pH of the solution is mainly based on the strong acid
Eg. 1.0 M HCl and 1.0 HC2H3O2
HCl(aq) + H2O(l) H3+O(aq) + Cl-(aq)
[
HC2H3O2(aq) + H2O(l) H3+
O(aq) + C2H3O2-(aq)
16-51CHEM 102, Fall 2012, LA TECH
pH of Mixtures of Acids and BasesThe pH of the solution is mainly based on the
excess acid or base present
Eg. 10 mL of 1.0 M HCl and 20 mL 1.0 NaOH
Moles of excess NaOH ( M x L) = 1.0 x 0.001= 0.001
Mixed together volume = 30 mL = 0.030 L
Molarity of excess NaOH = 0.001/0.030= 0.030
Calculate pOH and then pH
[
16-52CHEM 102, Fall 2012, LA TECH
Equilibrium, Constant, Ka & Kb
Ka: Acid dissociation constant for a equilibrium reaction.
Kb: Base dissociation constant for a equilibrium reaction.
Acid: HA + H2O H3+O + A-
Base: BOH + H2O B+ + OH-
[H3+O][ A-] [B+ ][OH-]
Ka = --------------- ; Kb = -----------------
[HA] [BOH]
16-53CHEM 102, Fall 2012, LA TECH
HCl(aq) + H2O(l) H3+O(aq) + Cl-(aq)
[H3+O][Cl-]
Ka= ----------------- [HCl]
[H+][Cl-]
Ka= ----------------- [HCl]
Acid Dissociation Constant
16-54CHEM 102, Fall 2012, LA TECH
Base Dissociation Constant
NH3 + H2O NH4+ + OH-
[NH4+
][OH-]
K =
[NH3]
16-55CHEM 102, Fall 2012, LA TECH
Comparing Kw and Ka & Kb
Any compound with a Ka value greater than Kw of water will be a an acid in water.
Any compound with a Kb value greater than Kw of water will be a base in water.
16-56CHEM 102, Fall 2012, LA TECH
Ionization Constants for Acids
16-57CHEM 102, Fall 2012, LA TECH
WEAKER/STRONGER Acids and Bases & Ka and Kb values
A larger value of Ka or Kb indicates an equilibrium favoring product side.
Acidity and basicity increase with increasing Ka or Kb.
pKa = - log Ka and pKb = - log Kb
Acidity and basicity decrease with increasing pKa or pKb.
16-58CHEM 102, Fall 2012, LA TECH
Which is weaker?a. HNO2 ; Ka= 4.0 x 10-4.
b. HOCl2 ; Ka= 1.2 x 10-2.
c. HOCl ; Ka= 3.5 x 10-8.
d. HCN ; Ka= 4.9 x 10-10.
16-59CHEM 102, Fall 2012, LA TECH
What is Ka1 and Ka2?H2SO4(aq) + H2O(l) H3
+O(aq) + HSO4-(aq)
HSO4-(aq) + H2O(l) H3
+O(aq) + SO42-(aq)
16-60CHEM 102, Fall 2012, LA TECH
H2SO4(aq) + H2O(l) H3+O(aq) + HSO4
-(aq)
HSO4-(aq) + H2O(l) H3
+O(aq) + SO42-(aq)
[H3+O][HSO4
-]
H2SO4 ; Ka1 = -------------------
[H2SO4]
[H3+O][SO4
2-]
H2SO4 ; Ka2 = -------------------
[HSO4-]
Ka Examples
16-61CHEM 102, Fall 2012, LA TECH
HC2H3O2(aq) + H2O(l) H3+O(aq) + C2H3O2
-(aq)
[H+][C2H3O2
-]
H C2H3O2; Ka= ------------------
[H C2H3O2]
NH3 (aq) + H2O(l) NH4+ + OH-(aq)
[NH4+][OH-]
NH3; Kb= --------------
[ NH3]
Ka Examples
16-62CHEM 102, Fall 2012, LA TECH
% Dissociation gives x (amount dissociated) need for pH calculation
Amount dissociated
% Dissoc. = ------------------------- x 100
Initial amount/con.
x
% Dissoc. = --------------------------- x 100
concentration
16-63CHEM 102, Fall 2012, LA TECH
How do you calculate pH of weak acids/bases?
a) From % dissociation
b) From Ka or Kb
What is % dissociation
Amount dissociated
% Dissoc. = ------------------------- x 100
Initial amount
16-64CHEM 102, Fall 2012, LA TECH
How do you calculate % dissociation from Ka or Kb
1.00 M solution of HCN; Ka = 4.9 x 10-10
What is the % dissociation for the acid?
16-65CHEM 102, Fall 2012, LA TECH
1.00 M solution of HCN; Ka = 4.9 x 10-10
First write the dissociation equilibrium equation:
HCN(aq) + H 2O(l) <===> H 3+O(aq) + CN-(aq)
[HCN] [H+ ] [CN- ]Ini. Con. 1.00 M 0.0 M 0.00 M
Cha. Con -x x x
Eq. Con. 1.0 - x x x
[H 3+O ][CN-] x2
Ka = ------------------- = ----------------
[HCN] 1.0 - x
1.00 M solution of HCN; Ka = 4.9 x 10-10
16-66CHEM 102, Fall 2012, LA TECH
1.0 - x ~ 1.00 since x is small
x2
Ka = -----------; Ka = 4.9 x 10-10 = x2
1.0
x = 4.9 x 10-10 = 2.21 x 10 -5
Amount disso. 2.21 x 10 -5
----------------- x 100 =- ------------- x 100 Ini. amount 1.00
% Diss. =2.21 x 10 -5 x 100 = 0.00221 %
1.00 M solution of HCN; Ka = 4.9 x 10-10
16-67CHEM 102, Fall 2012, LA TECH
10) Calculate the % dissociation of 2.00 M solutions of HCN (Ka= 4.9 x 10-10)
a) Dissociation equilibria:
b) ICE setup:
c) Amount dissociated:
d) % dissociation::
16-68CHEM 102, Fall 2012, LA TECH
1 M HF, 2.7% dissociated
Notice the conversion of % dissociation to a fraction (x): 2.7/100=0.027) x=0.027
Calculate the pH of a weak acid from % dissociation
16-69CHEM 102, Fall 2012, LA TECH
HF(aq) + H 2O(l) <===> H 3+O(aq) + F-(aq)
[H+][F-]
Ka = ----------- [HF] [HF] [H+ ] [F- ]Ini. Con. 1.00 M 0.0 M 0.00 MChg. Con -x x xEq.Con. 1.0-0.027 0.027 0.027 pH = -log [H+] pH = -log(0.027) pH = 1.57
Calculate the pH of a weak acid from % dissociation
16-70CHEM 102, Fall 2012, LA TECH
11) Calculate the Ka of if 5.0 M HF, 2.7% dissociated:
a) Dissociation equilibria:
b) ICE setup:
c) Amount dissociated:
d) Ka :
16-71CHEM 102, Fall 2012, LA TECH
Weak acid Equilibria
Example
Determine the pH of a 0.10 M benzoic acid solution at 25 oC if Ka = 6.28 x 10-5
HBz(aq) + H2O(l) H3O+(aq) + Bz-(aq)
The first step is to write the equilibrium expression
Ka = [H3O+
][Bz-]
[HBz]
16-72CHEM 102, Fall 2012, LA TECH
Weak acid Equilibria
HBz H3O+ Bz-
Initial conc., M 0.10 0.00 0.00
Change, DM -x x x
Eq. Conc., M0.10 - x x x
[H3O+] = [Bz-] = x
We’ll assume that [Bz-] is negligible compared to [HBz]. The contribution of H3O+ from water is also negligible.
16-73CHEM 102, Fall 2012, LA TECH
Weak Acid Equilibria
Solve the equilibrium equation in terms of x
Ka = 6.28 x 10-5 =
x = (6.28 x 10-5 )(0.10)
H3O+ = 0.0025 M
pH = 2.60
x2
0.10
16-74CHEM 102, Fall 2012, LA TECH
pH from Ka or Kb
1.00 M solution of HCN; Ka = 4.9 x 10-10
First write the dissociation equilibrium equation:
HCN(aq) + H 2O(l) H 3+O(aq) + CN-(aq)
[HCN] [H+ ] [CN- ]
Ini. Con. 1.00 M 0.0 M 0.00 M
Chg. Con -x x x
Eq. Con. 1.0 - x x x
16-75CHEM 102, Fall 2012, LA TECH
[H 3
+O ][CN-] x2
Ka = --------------- = ----------------
[HCN] 1.0 - x
1.0 - x ~ 1.00 since x is small x2 Ka = -----------; Ka = 4.9 x 10-10 = x2
1.0
x = 4.9 x 10-10 = 2.21 x 10 -5
pH = -log [H+]
pH = -log(2.21 x 10-5)
pH = 4.65
Weak Acid Equilibria
16-76CHEM 102, Fall 2012, LA TECH
The Conjugate Partners of Strong Acids and BasesThe conjugate acid/base of a strong base/acid has
no net effect on the pH of a solution
The conjugate base of a weak acid hydrolyze in water and basic or
pH of a solution > 7.00 E.g. Na+C2H3O2- sodium
acetate
The conjugate acid of a weak base hydrolyze in water and acidic or
pH of a solution < 7.00 E.g NH4Cl
16-77CHEM 102, Fall 2012, LA TECH
12) Calculate the [H+], [OH-] and pH of 0.90 M HC2H3O2; Ka= 1.8 x 10-5.
a) Dissociation equilibria:
b) ICE setup:
c) [H+] and [OH-]:
d) pH:
16-78CHEM 102, Fall 2012, LA TECH
13) Calculate the [H+], [OH-] pOH and pH 5.0 M NH3; Kb = 1.8 x 10-5
a) Dissociation equilibria:
b) ICE setup:
c) [H+] and [OH-]:
d) pOH and pH:
16-79CHEM 102, Fall 2012, LA TECH
14) Calculate the pH of a 0.015 M solution of lactic acid. The Ka for lactic acid is 1.4 x 10-4.
16-80CHEM 102, Fall 2012, LA TECH
15) Calculate the pH of a 0.14 M solution of an acid with Ka = 6.2 x 10-8 (pH = 4.03)