1 some properties of acids þ produce h + (as h 3 o + ) ions in water (the hydronium ion is a...
TRANSCRIPT
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Some Properties of Acids
Produce H+ (as H3O+) ions in water (the hydronium ion is a
hydrogen ion attached to a water molecule)
Taste sour
React with metals to produce hydrogen gas
Electrolytes
React with bases to form a salt and water
pH is less than 7
Turns blue litmus paper to red
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What do acids do?
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Some Common Acids
HCl hydrochloric acid
HNO3 nitric acid
H2SO4 sulfuric acid
H3PO4 phosphoric acid
H2CO3 carbonic acid
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Strong Acids
• Strong acids completely ionize in water.
• For every mole of acid, there will be 1 mole of H+, so the concentration of H+ will be the same as the concentration of the acid.
• For Example:
HCl H+ + Cl- [0.03 M] [0.03M] [0.03 M]
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Strong Acids
HCl, HI, HBr, HNO3, H2SO4,
HClO4
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Weak Acids
• All weak acids form equilibrium systems in solution.
• For example:
H2CO3 (aq) <======> H+ (aq) + HCO3(aq)
• Since we have an equilibrium system, an equilibrium constant (Ka) can be written:
Ka = __[H+] [A-]___
[HA]
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Some Properties of Bases
Produce OH- ions in water
Taste bitter, chalky
Are electrolytes
Feel soapy, slippery
React with acids to form salts and water
pH greater than 7
Turns red litmus paper to blue “Basic Blue”
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Some Common Bases
NaOH sodium hydroxide lye
KOH potassium hydroxide liquid soap
Ba(OH)2 barium hydroxide stabilizer for plastics
Mg(OH)2 magnesium hydroxide “MOM” Milk of
magnesia
Al(OH)3 aluminum hydroxide Maalox (antacid)
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Strong Bases
• Strong bases completely ionize in water.
• For every mole of a base, there will be 1 mole of OH-, so the concentration of OH- will be the same as the concentration of the base.
• For Example:
NaOH Na+ + OH- [0.03 M] [0.03M] [0.03 M]
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Strong Bases
NaOH, KOH, LiOH, RbOH, CsOH, Ca(OH)2, Ba(OH)2,
Sr(OH)2
Strong bases completely ionized in water.
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HNO3, HCl, H2SO4 and HClO4 are among the only known strong acids.
Strong versus Weak Strong versus Weak Acids/BasesAcids/Bases
The strength of an acid (or base) is determined by the amount of IONIZATION.
The strength of an acid (or base) is determined by the amount of IONIZATION.
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Categorizing Acids/Bases: Categorizing Acids/Bases: Weak versus StrongWeak versus Strong
• Weak acids and bases do not completely ionize in water.
• Strong acids and bases completely ionize in water.
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Acids and Bases Acids and Bases TheoriesTheoriesAcids and Bases Acids and Bases TheoriesTheories
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Arrhenius Acids and Bases
• Acids – produce H+ ions (or hydronium ions H3O+)
• Bases – produce OH- ions
• (problem: some bases don’t have hydroxide ions!)
1515Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water
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Brønsted – Lowry Acids and Bases
• Acids – proton donor
• Bases – proton acceptor
• A “proton” is really just a hydrogen atom that has lost it’s electron!
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A Brønsted-Lowry acid is a proton donorA Brønsted-Lowry base is a proton acceptor
acidconjugate
basebase conjugate
acid
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Bronsted-Lowry Definition
a. NH3(g) + H3O+(aq) → NH4
+(aq) + H2O
b. CH3OH(l) + NH2-(aq) → CH3O-
(aq) + NH3(g)
c. OH-(aq) + H3O+
(aq) → H2O + H2O
1919Lewis Acids and Lewis Acids and BasesBases
Lewis acid - a Lewis acid - a substance that substance that accepts an accepts an electron pairelectron pair
Lewis base - a Lewis base - a substance that substance that donates an donates an electron pairelectron pair
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The pH Scale
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Calculating pH and pOH
pH = -log [H+] pOH = -log [OH-]
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pHpH [H+][H+] [OH-][OH-] pOHpOH
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Neutralization
• Acid + Base– Ex:
HCl + NaOH NaCl + H2O
HNO3 + KOH KNO3 + H2O
• Neutralizations always result in a ________ and __________.
saltwater
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Base Ex.
Closing
Acid, Base, or Both?
Slippery
Soap
Tastes sour
Ca(OH)2
Conducts electricity
Corrosive to skin
Examples include citrus
fruits.
H2SO4
HNO3
Forms the H3O+ ion when
dissolved in water
Ionizes in water.
HCl
Litmus paper turns red
Forms the OH ion when
dissolved in water
pH < 7
pH > 7
Baking soda
Bitter taste
NaOH