Review of Acids, Bases,

1
Review of Acids, Bases, Salts
2
Arrhenius Acid

• Has H in the formula
• Produces H as the only positive ion in solution

3
Formula of an Acid

• Inorganic formula starts with H
• Organic formula ends with COOH

4
Properties of Acids

• Sour Taste
• Electrolytes
• React with bases to form a salt H2O
• Turn litmus RED
• React with most metals to produce H2(g)

5
Ionization of an Acid

• HCl ? H Cl-

or
HCl H2O ? H3O Cl-
6
Arrhenius Base

• Has OH in the formula
• Produces OH- as the only negative ion in solution

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Formula of a Base

• Has format MOH
• M is a metal

8
Properties of Bases

• Bitter Taste
• Slippery Feel
• Electrolytes
• React with acids to form a salt H2O
• Turn litmus BLUE

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Ionization of a Base

• NaOH ? Na OH-

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Ionization of NH3

• NH3 H2O ? NH4 OH-

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Formula of a Salt

• Metal Nonmetal

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Write the formula of potasium sulfate

• K (SO4)2-

K2SO4
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Electrolytes

• Solutions conduct they contain ions
• Acids (HX), bases (MOH), salts (MX) are
  electrolytes

14
NONelectrolytes

• Solutions of covalent compounds (all nonmetals).
  They do NOT conduct.

15
Identify the electrolytes
Yes - B
Yes - B

• LiOH
• CH3COOH
• C6H12O6
• NaNO3
• H2SO4
• CH3OH
• Ca(OH)2
• HCl
• C8H18

• Al(OH)3
• HNO3
• CH3CH2COOH
• K2SO4
• CH3CHOHCH3
• CH3OCH3
• H3PO4
• Mg(OH)2
• CH3CH2OH

Yes - A
Yes - A
Yes - A
No
Yes - S
Yes - S
Yes - A
No
No
No
Yes - A
Yes - B
Yes - A
Yes - B
No
No
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pH scale

• 0-14
• Acidic 0 to 7,
• Neutral 7
• Basic 7-14

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Most acidic on pH scale

• pH 0

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Most basic on pH scale

• pH 14

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OH-

• Hydroxide ion

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H

• Hydrogen ion
• or
• Proton

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H3O

• Hydronium ion. Interchangeable with H.

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Acidic Solution

• H ? OH-

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Basic Solution

• OH- ? H

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If the pH changes from 3 to 5, how does the H
change?

• The pH changes by 2, so the H changes by 102
  or 100X. Since the pH went up, it became LESS
  acidic.
• The new solution has a H 100 times less than
  the original solution.

25
How can pH be safely tested?

• Instrumental use pH meter
• Indicators use a series of indicators to narrow
  down the pH range
• Test acids with metals (NOT Cu, Ag, or Au)

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Bronsted-Lowry Acid

• Proton Donor

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Bronsted-Lowry Base

• Proton Acceptor

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Bronsted-Lowry Acids Bases

• HCl H2O ? H3O Cl-

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Strong Acids Bases

• Complete or almost complete ionization.

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Weak Acids Bases

• Ionization occurs only to a slight extent, a few
  percent.

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Reactions of Acids with Metals

• Metal Acid ? H2(g) salt

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Zn(s) HCl ? ?
Zn(s) 2HCl ? H2(g) ZnCl2
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Al(s) HCl ? ?
2Al(s) 6HCl ? 3H2(g) 2AlCl3
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Neutralization Reactions

• Acid Base ? Salt H2O

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Net Ionic Equation for Neutralization Reactions

• H OH- ? H2O

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At neutralization

• Moles H Moles OH-

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Molarity (M)

• Molarity Moles solute

Liters of soln
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Titration Equation

• MaVa MbVb

This equation works when the number of Hs on the
acid EQUALS the number of OHs on the base!
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Titration Equation

• naMaVa nbMbVb

This equation works when the number of Hs on the
acid does NOT equal the number of OHs on the
base! na number of acidic Hs in acid. nb
number of OHs in base.
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pH

• -logH or logH3O

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pOH

• -logOH-

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pOH pH

• 14

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OH- X H

• 1.0 X 10-14

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If the H 1 X 10-3

1. The pH
2. The pOH
3. The OH-

3
11
1 X 10-11
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Indicator

• Substance that changes color over a narrow pH
  range.

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Molarity H2SO4 Vs. Molarity H

• H2SO4 ? 2H SO42-
• H 2H2SO4
• 2M H2SO4 ? 4M H

47
What is the concentration of a hydrochloric acid
solution if 50.0 mL of a 0.250 M KOH solution are
needed to neutralize 20.0 mL of the HCl solution
of unknown concentration?

• MaVa MbVb
• X(20.0 mls) .250M(50.0mls)

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Acid 1.50 M Base ? M
Final Volume 16.07 24.25
Initial Volume 5.45 4.05
Amount Used



10.62 20.20
(1.50 M)(10.62 mls) X(20.20 mls)