acids 2 ph below 7 turns litmus paper red taste sour reacts with metals to produce h 2 (g) generally...
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The Chemistry of Acids and Bases
The Chemistry of Acids and Bases
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Acids
2
pH below 7turns litmus paper red
taste sour
reacts with metals to produce H2(g)
generally starts with a hydrogen ion
[H+] > [OH-] HCl
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3
Bases
pH greater than 7turns litmus paper blue
taste bitter
feel slippery
generally contains a hydroxide ion
[H+] < [OH-] NaOH
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4
Both Acids and Bases
an electrolyte
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Acidic, Basic, and Neutral Solutions
Type of Solutio
n
pH Ranges
[H+] versus [OH-]
Example
Acidic Below 7 [H+] > [OH-]Orange JuiceBattery Acid
Your Stomach
Neutral Equals EXACTLY 7
[H+] = [OH-] DistilledWater
Basic Above 7 [H+] < [OH-]Bleach
Sea WaterBlood
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Indicators
Indicators are compounds that have one color in acidic solutions and another in basic.
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Litmus Paper
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
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Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
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Acid Nomenclature Flowchart
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BINARY ACIDS
HBr (aq)
Hydrobromic Acid
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TERNARY ACIDS
POLYATOMIC IONS
PURE FORMS
TERNARY ACIDS
SO42- H2SO4 H2SO4(aq)
Sulfuric acidSO3
2- H2SO3 H2SO3(aq)
Sulfurous Acid
Naming Ternary Acids
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Naming Bases
Use the same rules as for ions (name the cation, then name the anion)
NaOH
Ca(OH)2
KOH
Sodium hydroxideCalcium hydroxide
Potassium hydroxide
polyatomic
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Some Common Acids and Bases and their Household Uses.
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What are Acids and Bases?
There are two common definitions todescribe acids and bases:
1. Arrhenius acids and bases2. Bronsted-Lowry acids and bases
These are basically the same although they state different things.
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Definitions for Acids & Bases
Arrhenius Brønsted-Lowry
Definition for Acids
Definition for Bases
Key Examples
a proton producer in an aqueous solution
a proton donor
a hydroxide producer in an aqueous solution
a proton acceptor
Acid – HCl
Base - NaOH
Acid – HCl
Base – NH3
H+ = proton
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Arrhenius Acids and Bases Definitions
1. Arrhenius Acid
acids in water produce hydronium ions, (H3O+, H+)
HNO3(aq) H+(aq) + NO3-
2. Arrhenius Base
bases in water produce hydroxide ions, (OH-)
KOH(s) K+(aq) + OH-(aq)
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HCl + H2O Cl– + H3O+
• Acids are proton (H+) donors. • Bases are proton (H+) acceptors.
conjugate acid
conjugate base
baseacid
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Bronsted-Lowry Definitions
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Bronsted-Lowry
Come in Pairs
General equation
HA(aq) + H2O(l) A-(aq) + H3O+(aq)
Acid + Base Conjugate base + Conjugate acid This is an equilibrium.
B(aq) + H2O(l) BH+(aq) + OH-(aq)
Base + Acid Conjugate acid +Conjugate base This is an equilibrium.
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What to Focus On?
Arrhenius was the most restrictive definition. This definition required:
the solutions to be aqueous and
a base to contain a hydroxide (OH-) ion.
Bronsted-Lowry’s definition is the most commonly used. It is helpful to remember:
acids tend to “lose“ an H+ ion, while
bases tend to “gain“ an H+ ion.
Under this definition, ammonia (NH3) is considered a base even though it is NOT an Arrhenius base.
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Examples HCl(aq) + KOH(s) KCl(aq) + H2O(l)
3 Ca(OH)2(aq) + 2 H3PO4(aq) Ca3(PO4)2(s) + H2O(l)
F-(aq) + H2O(l) HF(aq) + OH-(aq)
HCO3
-(aq) + H2O(l) CO32-(aq) + H3O+(aq)
NH4
+(aq) + CO32-(aq) NH3(aq) + HCO3
-(aq)
acid base
base acid
base acid
acid base
acid base
conjugate
acid
conjugate
base
conjugate
base
conjugate
acid
conjugate
base
conjugate
acid
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Remember Electrolytes?
Na+
NaCl
Na+ Cl-
Cl-
C6H12O6
C6H12O6
C6H12O6
Ionic Covalent
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Acids and bases are both strong or weak electrolytes (conduct electricity)• Electrolytes = dissociate (break apart into ions) when dissolved
• Strong = completely Weak = partially Non = not at all
H+
HC2H3
O2
H+
C2H3O21-
C2H3O21- H
+
H-Cl
H+
Cl-
Cl-
Weak Strong
Lots of IonsOnly a few Ions
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Strong Electrolytes
Notice that all of the ions are separated or dissociated.
WORD DESCRIPTION Completely breaks
apart into its ions Are good conductors
of electricity Will produce a bright
light bulb Examples of Acids and
Bases that are Strong Electrolytes
Strong Acids Strong BasesH2SO4 NaOH
HCl Ba(OH)2
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Notice that only some of the ions are separated or dissociated.
Weak Electrolytes
WORD DESCRIPTION Partially breaks apart
into its ions Are poor conductors of
electricity Will produce a dim light
bulb Examples of Acids and
Bases that are Weak Electrolytes
Weak AcidHC2H3O2 (Vinegar)
Weak BaseNH3 (Ammonia)
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Strong BasesThe hydroxides of the
Group I and Group II
LiOH - lithium hydroxide NaOH - sodium hydroxide KOH - potassium hydroxide *Ca(OH)2 - calcium hydroxide
*Sr(OH)2 - strontium hydroxide
*Ba(OH)2 - barium hydroxide
What makes a strong acid or a strong base?
Strong electrolytes make strong acids and bases
Strong Acids
HCl - hydrochloric acid HBr - hydrobromic acid HI - hydroiodic acid HNO3 - nitric acid
H2SO4 - sulfuric acid HClO4 - perchloric acid
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pH Concept
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pH ScalePouvoir hydrogéne (hydrogen power)
Is a scale to measure the acidity of a sample, Range: 0 -14
1 14
Highly acidic Very basic (not acidic)
neutral
7
Acids 0-7 Bases 7-14Neutral = 7.0
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Relationships between pH, [H+], and [OH-]
As pH increases… The [H+] (increases or decreases). The [OH-] (increases or decreases). The solution becomes more (acidic or
basic).
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Relationships between pH, [H+], and [OH-]
What happens as pH decreases?
As pH decreases… The [H+] (increases or decreases). The [OH-] (increases or decreases). The solution becomes more (acidic or
basic).
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The pH Scale
The value of pH is unitless.
Solutions with a pH less than 7 are acidic and solutions greater than 7 are basic.
If a solution is equal to 7 it is neutral.
Here is a typical pH scale.
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pH of Common Substances
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pH is a Logarithmic Scale
Logarithm –The number of times a base must be multiplied by itself to reach a given number
yx blog# of multiples
Base
# you’re trying to reach
pH is a Logarithmic Scale
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pH Calculations
Given Solving for
Formula to Use
[H+] pH pH = - log[H+]
[OH-] pOH pOH = - log[OH-]
[H+] is the concentration of H+ ions, in mol/L.
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Logarithms
Use your calculator! If you have a log button, you’re all set.
Each calculator can have its own method for entering logs.
If you don’t know what to do your calculator manual should give examples.
+
-1
/
x
0
2 3
4 5 6
7 8 9
.
CE
EE
log
ln
1/x
x2
cos tan
1.44939 E -2
9 - 43
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Logarithms
If your calculator has a ln button -
• Don’t use it.• Its for taking natural logs.• This is different than base 10.
+
-1
/
x
0
2 3
4 5 6
7 8 9
.
CE
EE
log
ln
1/x
x2
cos tan
1.44939 E -2
9 - 44
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Calculating pH
If [H+] is written in scientific notation and has a coefficient of 1, then the pH of the solution equals the absolute value of the exponent
Ex. 1.0 x 10-4 M
pH = 4.0
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Problem 1:
If [H+] = 3.40 x 10-5 M, what is the pH?Given UnknownEquation[H+] = 3.40 x 10-5 M pH pH = - log[H+]
Solve:
pH = -log (3.40 x 10-5)
pH = 4.47
Calculating pH
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Problem 2:
If [H+] = 1 X 10-10, what is the pH?
Given Unknown Equation[H+] = 1 X 10-10 pH pH = -
log[H+]
Solve:pH = - log 1 X 10-10
pH = - (- 10)pH = 10
Calculating pH
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Problem 3:
If [H+] = 1.8 X 10-5, what is the pH?
Given Unknown Equation[H+] = 1.8 X 10-5 pH pH = -
log[H+]
Solve:pH = - log 1.8 X 10-5
pH = - (- 4.74)pH = 4.74
Calculating pH
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Problem 1:If [OH-] = 2.30 x 10-12 M, what is the pOH?
Given Unknown Equation
[OH-] = 2.30 x 10-12 M pOH pOH = - log[OH-]
Solve:pOH = -log (2.3 x 10-12)
pOH = 11.6
Calculating pOH
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If [OH-] is written in scientific notation and has a coefficient of 1, then the pOH of the solution equals the absolute value of the exponent
Problem 2:
If [OH-] = 1.0 x 10-9 M, what is the pH?pOH = 9.0
Calculating pOH
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WHAT’S IN A GLASS OF WATER?
distilled
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Distilled H2O at the Molecular LevelWhat’s in a glass of distilled water?
• Water Molecules (H2O)
• Hydronium Ions (H3O+)• Hydroxide Ions (OH-)
What’s happens in the glass of water?
H2O + H2O H⇆ 3O+ + OH-
This is called the self-ionization of water.
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WaterWater ionizes- falls apart into ions.
H2O ® H+ + OH-.
Only a small amount.
[H+ ] = [OH-] = 1 x 10-7M
A neutral solution.
In water Kw = [H+ ] x [OH-] = 1 x 10-14
Kw is called the ion product constant.
pH + pOH = 14Amphoteric
a molecule or ion that can react as an acid as well as a baseEx: H2O, NH3
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Calculating pOH from pH
If the pH is 3.25, what is the pOH?Given pH = 3.25
UnknownpOH ?
Equation pH + pOH = 14
Substitute and solve :
3.25 + pOH = 14
3.25 + (- 3.25) +pOH = 14 (- 3.25)
pOH = 10.8
Problem 1:
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What is the pH of a solution if [OH-] = 4.0 x 10-11 M?
Given [OH-] = 4.0 x 10-11 M
UnknownpH?
Equation
pH + pOH = 14
Step 1: Find pOHpOH = -log [OH] pOH= -log[4.0 x 10-11 ] = 10.4
Step 2: Calculate pHpH + pOH= 14; pH = 14 – 10.4 pH = 3.6
Calculating pH from pOH
Problem 2:
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Looking at the Math
Given Solving for
Formula to Use
pH [H+]
pOH [OH-]pOHOH 10][
pHH 10][
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If the pH of Coke is 3.12, [H+] = ???[
[H+] = 10-3.12 = 7.6 x 10-4 M
*** to find antilog on your calculator, look for “Shift” or “2nd function” and then the log button
KnownpH = 3.12
Unknown[H+] ?
Analysis[H+] = 10 -pH
Substitute and solve :
Calculating [H+] from pH
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Calculating [H+] from pH
The pH of an unknown solution is 6.00. What is its [H+]?
KnownpH = 6.00
Unknown[H+] ?
Analysis[H+] = 10 -pH
Substitute and solve :
[H+] = 1x 10 -6 M
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A solution has a pH of 8.5. What is the Molarity of hydrogen ions in the solution?
Calculating [H+] from pH
KnownpH = 8.5
Unknown[H+] ?
Analysis[H+] = 10 -pH
Substitute and solve :
[H+] = 10-8.5
3.16 X 10-9 M
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Acid-Base Reactions or Neutralization Reactions
acid + base water + salt
1. HBr(aq) + NaOH(aq)
2. H2SO4(aq) + KOH(aq)
3. H3PO4(aq) + Ba(OH)2(aq)
* Double replacement reactions
H2O + NaBr
H2O + K2SO4
H2O + Ba3(PO4)2