Acid-Base Reaction Review
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| acetic acid CH3COOH | strong acid
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| carbonic acid H2CO3 | strong acid
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| hydrogen sulfide H2S | weak acid
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| dihydrogen phosphate ion H2PO4- | weak acid
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| ammonium ion NH4+ | weak acid
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| hydrocyanic acid HCN | weak acid
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| phenol C6H5OH | weak acid
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| bicarbonate ion HCO3- | weak acid
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| hydrogen phosphate ion HPO4 2- | weak acid
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| water H2O | weak acid
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| ethanol C2H5OH | weak acid
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| Iodide ion | Weak Base
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| chloride ion | Weak Base
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| hydgrogen sulfate ion | Weak Base
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| nitrate ion | Weak Base
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| water | Weak Base
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| sulfate ion | Weak Base
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| dihydrogen phosphate ion | Weak Base
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| acetate ion | Weak Base
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| bicarbonate ion | Strong Base
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| hydrogen sulfide ion | Strong Base
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| hydrogen phosphate ion | Strong Base
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| ammonia | Strong Base
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| cyanide ion | Strong Base
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| phenoxide ion | Strong Base
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| carbonate ion | Strong Base
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| phosphate ion | Strong Base
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| hydroxide ion | Strong Base
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| ethoxide ion | Strong Base
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| most important factor determining relative acidities of organic compounds | stability of molecular structure where the greater the electronegativity of anion formed when H is removed the more stable the more acidic
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| how electronegativity, resonance, and inductive effect determine stability of anions | greater electrondegativity, more resonant structures, delocalized negative charge(neg side and pos side) make better acids that want to give up H+ or proton
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| Hydroiiodic acid HI | strong acid
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| hydrochloric acid HCl | strong acid
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| Sulfuric Acid H2SO4 | strong acid
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| Nitric Acid HNO3 | strong acid
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| Hydronium ion H3O+ | strong acid
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| Hydrogen sulfate ion | strong acid
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| Phosporic Acid H3PO4 | strong acid
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| Arrhenius Acid | dissociate in aqueous solution to form hydrogen ions (H+)
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| Arrhenius Base | which dissociate in aqueous solution to form hydroxide (OH−) ions
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| Bronsted-Lowry Acid | ability to "donate" hydrogen ions (H+) or protons
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| Bronsted-Lowry Base | ability to "accept" hydrogen ions (H+) or protons
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| Rules for using curved arrows | Show the change in position of electron pairs where tail is at electron pair and head shows new position showing bond formation or breaking
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| 1st Rule of writing acceptable Resonance Contributing Structures | must have the same number of valence electrons
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| 2nd Rule of writing acceptable Resonance Contributing Structures | must obey the rules of covalent bonding 2e- for H, 2nd Per. 8e- 3rd Per 12e-
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| 3rd Rule of writing acceptable Resonance Contributing Structures | positions of all nuclei must be the same with differences only in distribution of valence e-
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| 4th Rule of writing acceptable Resonance Contributing Structures | must have the same total number of unpaired and paired e-
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| strong acid | an acid that ionises completely in an aqueous solution by losing one proton
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| strong base | compound that is able to deprotonate very weak acids in an acid-base reaction
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| 1st step to determine position of acid-base equilibrium | identify two acids on each side of equation
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| 2nd step to determine position of acid-base equilibrium | determine which acid is the stronger
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| 3rd step to determine position of acid-base equilibrium | identify the stronger base knowing that the stronger acid gives a weaker base
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| 4th step to determine position of acid-base equilibrium | stronger acid and base react to give weaker acid and base therefore equilibrium goes toward the weaker acid and base
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| Acidity of alcohols, water, and carboxylic acid | alcohols weaker than water and much weaker than carboxylic acids
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Created by:
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