Transcript 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:

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
BF3 + F− → BF4-
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.
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
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
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?
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?
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?