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Sour taste-lemons, asprins
Acids contain hydrogen (react with metals to give H2)
Acids change color dyes (acid/base indicators)
Acids react with bases to produce "salts" and water
Acids are electrolytes (will conduct electricity in water) |
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| Traditional (Arrhenius) Acids |
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Contan H and ionize to form H+
HNO3 + H2O --> H30+ + NO3- |
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Molecue or ion that is proton donor
HCl + H2O --> H3O+ + Cl-
(Bronsted/ Arrhenius Acid)
HCl + NH3 --> NH4+ + Cl-
(Bronsted Acid ONLY)
H2O + NH3 --> NH4+ + OH-
(Bronsted Acid ONLY) |
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| Less tahn 100% ionization, weak electrolyte |
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| Sulfuric Acid, Hydrochloric Acid |
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Hydrogen bonded to more electronegative element
Prefix: Hydro
Root: Root name of second element
Suffix: -ic
HCl: Hydro-chlor-ic acid
HI: Hydro-iod-ic acid
H2S: Hydro-sulfur-ic acid |
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Hydrogen, Oxygen, and a thrid element
Polyatomic ion root with suffix (-ate to -ic, -ite to -ous)
Hydrogen Sulfate--Sulfuric Acid
Hydrogen Chlorite--Chlorous Acid
Hydrogen Periodate--Periodic Acid
Hydrogen Hypobromite--Hypobromous Acid
Hydrogen Dichromate--Dichromic Acid |
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Bases have a bitter taste
Dilute aqueous solutions of bases feel slippery
Bases change the color of dyes (acid/base indicators)
Bases react with acids to produce "salts" and water.
Bases are electrolytes (will conduct electricity in solution) |
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| Traditional (Arrhenius) Base |
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| Substance that contains hydroxide ions (OH-) and dissociates to give hydroxide ions in aqueous solution, ionic compound (metal hydroxide) alkaline solution--basic solution |
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Molecule or ion that is proton acceptor
HCl + NH3 --> NH4+ +Cl
(HCl-Bronsted Acid/ NH3-Bronsted Base) |
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| Strong electrolyte, Group I and II metal with hydroxide |
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| Ammonia (NH3) produces low concentration of OH- |
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| Species formed when Bronsted base gains a proton |
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| Species that remains after a Bronsted acid has given up a proton |
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| Bronsted Acid + Bronsted Base <--> Conjugate Acid + Conjugate base |
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| Bronsted Acid + Bronsted Base <--> Conjugate Acid + Conjugate Base |
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| HC2H3O2 + H2O <--> H3O + + C2H3O2 |
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| Bronsted Acid (WEAK) + Bronsted Base (WEAK) <--> Conjugate Acid (STRONGER) + Conjugate Base (STRONGER) |
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| HClO4 + H2O <--> H30+ + ClO4- |
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| Bronsted Acid (STRONGER) + Bronsted Base (STRONGER) <--> Conjugate Acid (WEAK) + Conjugate Base (WEAK) |
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| Conclusions from Bronsted definitions of acids and bases |
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Stronger Acid---Weaker conjugate base
Stronger Base---Weaker conjugated acid
Proton transfer reactions favor production of the weaker acid and the weaker base |
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| Any peices that can act as an acid or base, water is an example |
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| Acid/Base Reaction in Metals |
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| Zn + H2SO4 --> Zn SO4 + H2 |
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| Acid/ Base Reaction in Metal Oxides |
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| CuO + H2SO4 --> CuSO4 + H2O |
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| Acid/Base Reaction in Carbonates |
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| CaCO3 + 2HCl --> CaCl2 + CO2 + H2O |
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| Acid/Base Reactions in Nonmetal Oxides |
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Definition
CO2 + 2NaOH --> Na2CO3 + H2O
CO2 + H2O --> H2CO3 |
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Separation of IONIC compounds to produce ions
NaOH --> Na+ + OH- |
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Separation of COVALENT compounds to produce ions
NH3 + H2O <--> NH4+ + OH- |
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H2O + H2O <--> H3O + OH-
(Amphoteric/ Amphiteric)
At Equilibrium! |
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Equilibrium constant for water
[H3O+][OH-]
Kw=1x10^-14 M^2 |
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When finding just pH
When finding grams or L and pH |
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Use the easy way
Use Stoichiometry |
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| When finding [OH-] in a pH problem |
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Excess/ Total Volume in Liters
(Molarity) |
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| Capable of reacting chemically either as an acid or as a base |
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