c. johannesson i. introduction to acids & bases (p. 453 - 473) ch. 15 & 16 - acids &...
TRANSCRIPT
C. Johannesson
I. Introduction toAcids & Bases
(p. 453 - 473)
I. Introduction toAcids & Bases
(p. 453 - 473)
Ch. 15 & 16 - Acids & BasesCh. 15 & 16 - Acids & Bases
C. Johannesson
A. PropertiesA. Properties
electrolytes electrolytes
turn litmus red
sour taste
react with metals to form H2 gas
slippery to touch
turn litmus blue
bitter taste
ChemASAP
vinegar, milk, soda, apples, citrus fruits
ammonia, lye, antacid, baking soda
C. Johannesson
B. DefinitionsB. Definitions
Arrhenius - In an aqueous solution:
HCl + H2O H3O+ + Cl–
• Acids form hydronium ions (H3O+) (by releasing hydrogen ions into the water)
H
HH H H
H
ClClO O
–+
acid base
C. Johannesson
B. DefinitionsB. Definitions
Arrhenius - In aqueous solution…
• Bases form hydroxide ions (OH-)
NH3 + H2O NH4+ + OH-
H
H
HH H
H
N NO O–+
H
H
H H
base acid
C. Johannesson
B. DefinitionsB. Definitions
Brønsted-Lowry Definitions:
HCl + H2O Cl– + H3O+
• Acids are proton (H+) donors. • Bases are proton (H+) acceptors.
conjugate acidconjugate base
baseacid
C. Johannesson
B. DefinitionsB. Definitions
H2O + HNO3 H3O+ + NO3–
CBCAAB
C. Johannesson
B. DefinitionsB. Definitions
NH3 + H2O NH4+ + OH-
CA CBB A
C. Johannesson
B. DefinitionsB. Definitions
Amphoteric - can be an acid or a base. Monoprotic- an acid that can only donate
one H+
Polyprotic - an acid that can donate more than one H+
C. Johannesson
C. StrengthC. Strength
Strong Acid/Base• 100% ionized in water• strong electrolyte
- +
HCl
HNO3
H2SO4
HBr
HI
HClO4
NaOH
KOH
Ca(OH)2
Ba(OH)2
Acid StrengthAcid Strength
Ternary:• Strong if # oxygen - # hydrogen ≥ 2
• H2SO4
• HNO3
• Weak if not!• H2SO3
• HNO2
LPChem:Wz
Acid StrengthAcid Strength
Binary:• Strong if HCl, HBr, HI• Weak if not!
• H2O
• HF
LPChem:Wz
Base StrengthBase Strength
Bases generally have the formula MOH, where M is a metal:• Strong if M is from Group 1 or “heavy
Group 2” (bottom of Gr2)
• Li, Na, K, Rb, Cs, Fr & Ca, Sr, Ba• Weak if not!
• Mg(OH)2
• AgOHLPChem:Wz
C. Johannesson
C. StrengthC. Strength
Weak Acid/Base• does not ionize completely• weak electrolyte
- +
HF
CH3COOH
H3PO4
H2CO3
HCN
NH3
Strong vs. WeakStrong vs. Weak
Electrolyte:• Conductive in aqueous solution.
Why do we need electrolytes?• Muscle contractions are controlled by
electrical messages of the nervous system. • You sweat out electrolytes during a workout. • They need to be replaced to keep things
working. • And to prevent muscle cramps (from
insufficient electrolyte levels).
LPChem:Wz
- +
Strong vs. WeakStrong vs. Weak
“Strong” substances (both acid and base) dissociate strongly.Dissociate = break into ions
• Acid: HA H+ + A-
• Base: MOH M+ + OH-
Notice the arrows!• These reactions go to completion.
LPChem:Wz
Strong vs. WeakStrong vs. Weak
These reactions go to completion.• This means that a solution of the
“strong acid” HCl doesn’t actually contain any HCl molecules.
• HCl H+ + Cl-
• All the HCl molecules dissociated.• Now it is a solution of H+ and Cl- ions.
(We still label it “HCl” but it’s really H+ + Cl-)
LPChem:Wz
Strong vs. WeakStrong vs. Weak
“Weak” substances (both acid and base) dissociate weakly.
• Acid: HA H⇌ + + A-
• Base: MOH M⇌ + + OH-
Notice the arrows!• These reactions DO NOT go to completion. They are at equilibrium.
LPChem:Wz
Strong vs. WeakStrong vs. Weak
Weak DO NOT go to completion.• This means that a solution of the
“weak acid” HF contains a mixture of HF molecules and H+ and F- ions.
• HF ⇌ H+ + F-
• Only a fraction of the HF molecules dissociated. Now the solution is a mixture of HF molecules, H+ ions and F- ions.
LPChem:Wz
Strong vs. WeakStrong vs. Weak
End result:Strong Acids & Bases dissociate all the
way (making all ions)• and are therefore strong electrolytes
Weak Acids & Bases dissociate part way ⇌ (making only some ions)
• And are therefore weak electrolytes.
LPChem:Wz