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7.02

7.02. Acids and Bases. Acids and Bases. Three definitions of Acids/Bases: Arrhenius: Increases H + /OH - when added to water Bronsted-Lowry: Proton Donor/Proton acceptor Lewis: Electron Pair Acceptor/Electron Pair Acceptor BF 3  + F −  → BF 4 -. Acids and Bases.

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7.02

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  1. 7.02 Acids and Bases

  2. Acids and Bases • Three definitions of Acids/Bases: • Arrhenius: Increases H+/OH- when added to water • Bronsted-Lowry: Proton Donor/Proton acceptor • Lewis: Electron Pair Acceptor/Electron Pair Acceptor BF3 + F− → BF4-

  3. Acids and Bases • What makes an acid or base a strong acid or base? • “strong” or “weak” refers to the extent to which the acid or base dissociates in water. Strong acids dissociate completely in water. They are 100% ionized.

  4. Acids and Bases • What is a Neutralization Reaction? • When you react an acid and base together, the H+ ion and OH- ion will combine to form water, which is not an acid or a base, but is neutral. • In addition, you will make a salt out of the two counter ions

  5. Acids and Bases • Identify the acid and base in the following reactions, and identify the salt produced: HClO + NH3 → NH4ClO 2 HCl + CaOH → 2 H2O + CaCl2 H2SO4 + 2 NH4OH → (NH4)2SO4 + 2 H2O NH3 + HCl → NH4Cl Ca(OH)2 + H2CO3 → CaCO3 + 2 H2O HClO + NH3 → NH4ClO

  6. Acids and Bases • #1 If it took 24.5 milliliters of 0.35 molar NaOH to neutralize 15.0 milliliters of HNO3, what is the concentration (molarity) of the HNO3?

  7. Acids and Bases • #2 If 40.0 milliliters of 0.15 molar HCl are required to completely neutralize 25.0 milliliters of NH3, what is the concentration of the NH3 solution?

  8. Acids and Bases • #3 If 23.45 milliliters of Ca(OH)2 with an unknown concentration is neutralized by 25.0 milliliters of 0.123 molar HCl, what is the concentration of the Ca(OH)2?

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