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Acids & Bases
Definition Acid Base Arrhenius Produces H+^ ions when dissolved in water
Produces OH-^ ions when dissolved in water Bronsted-Lowry Proton (H+) donor Proton (H+) acceptor Lewis Electron pair acceptor Electron pair donor
Strong Acids and Bases Completely Ionize in Water (100% dissociation into ions)
Weak Acids and Bases Ionize Partially in Water
Strong Acids: HCl, HBr, HI, HNO 3 , H 2 SO 4 , HClO 4
Strong Bases: LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH) 2 , Ba(OH) 2 (the “b” hydroxides of Grp. I & II)
Weak Acid Example: HC 2 H 3 O 2 (acetic acid) majority of molecules stay whole
Weak Base Example: NH 3 (ammonia) majority of molecules stay whole
How H+^ (a proton) Reacts with Water
HCl Dissociation
HC 2 H 3 O 2 Dissociation
NH 3 Dissociation +
Net Ionic Equations for Acid-Base Reactions
Strong acids and bases completely ionize, thus write as ions o Strong acid will always produce H+^ (anion spectates) o Strong base will always produce OH-^ (cation spectates) Weak acids and bases mainly stay as whole molecule, thus write complete formulas (no ions) Nonelectrolytes (like water) do not ionize, thus write complete formulas
Examples:
- HClO 4 (aq) + KOH(aq)
- HI(aq) + CH 3 NH 2 (aq)
- HNO 2 (aq) + Ca(OH) 2 (aq)
Acid-Base Calculations
- List the species in the combined solution before any reaction occurs, and decide what reaction will occur.
- Write the balanced net ionic equation for this reaction.
- Calculate the moles of reactants. For reactions in solution, use the volumes of the original solutions and their molarities.
- Determine the limiting reactant where appropriate.
- Calculate the moles of the required reactant or product.
- Convert to grams or volume (of solution), as required.
