→ REVIEW
PROPERTIES OF ACIDS AND BASES
Acids Bases
- blue → red - red → blue
- low pH - high pH
- conductive (ions) - conductive (ions)
- react with metals - bitter
- sour
Neutral Ionic Neutral Molecular
- conductive if soluble - not conductive
- solid at room temp SATP - any state at SATP (s, l, g)
CONCENTRATION EQUATIONS
pH= -log [H3O+(aq)]
pOH= -log[OH-(aq)]
[H3O+] or [H+]= 10-pH
[OH-]= 10-pOH
⭐︎If needed: 14-pH= pOH
14+pOH= pH
OLD VS MODIFIED ARRHENIUS:
ACIDS AND BASES
Old Modified
Acids Substance that ionizes to produce Acid that donates a proton
H+(aq) ions in solution. (hydrogen) to water to form
→ Any strong acids hydronium ion (H3O+)
Bases Substance that dissociates to Base that accepts the proton
produce OH-(aq) ions in solution (hydrogen) from water to form OH-
OLD VS MODIFIED ARRHENIUS:
WRITING EQUATIONS FOR ACIDS AND BASES
⭐︎Old: same steps as modified but does NOT involve H2O(water) or H3O(hydroxide)
● Acids
1. Write acid reacting with water to produce H3O+(aq)
, 2. Determine the other product → Acids lose a proton (H +)
Bases gain a proton (H-)
Examples → HCl(aq)
Old: HCl(aq) → H+(aq) + Cl-(aq)
Modified: HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq)
→ H2SO4(aq) ~ sulfuric acid
Modified: H2SO4(aq) + H2O(l) → H3O+(aq) + HSO4-(aq)
● Bases
Examples → NH3(aq)
Modified: NH3(aq) + H2O(l) → OH-(aq) + NH4+(aq)
- water donates proton to base
→ NaHCO3(aq)
Modified: Ionic compound splits into ions: Na+ and HCO3-
HCO3-(aq) + H2O(l) → OH-(aq) + H2CO3
→ Strong acids and bases; complete reaction , dissociation
←→ Weak acids and bases; partial reaction, dynamic equilibrium
Example→ Old Arrhenius: CH3COOH(aq) → CH3COOH(aq)
Modified Arrhenius: CH3COOH(aq) ←→ CH3COOH(aq)
RULES FOR NAMING AND FORMULAS FOR ACIDS
● Rules
- Identify the acid by: Hydrogen or attached H+
- All acids are soluble in water: include (aq)
IUPAC Naming System (Compound Name) Classical Naming System (Acid Name)
Aqueous hydrogen _____ide = Hydro_____ic acid
Aqueous hydrogen _____ate = _____ic acid
⭐︎ negative polyatomic: ate → ic acid
Aqueous hydrogen _____ite = _____ous acid
⭐︎ negative polyatomic: ite → ous acid
USING MASS OF ACID/BASE TO CALCULATE:
CONCENTRATION, pH, pOH OF ACID/BASE
SIG DIG RULES FOR pH
pH/pOH [H3O+]/[OH-]
→ NO units, numbers only → Units: mol/L
→ Sig digs: right of the decimal → Sig digs: follow normal rules
PROPERTIES OF ACIDS AND BASES
Acids Bases
- blue → red - red → blue
- low pH - high pH
- conductive (ions) - conductive (ions)
- react with metals - bitter
- sour
Neutral Ionic Neutral Molecular
- conductive if soluble - not conductive
- solid at room temp SATP - any state at SATP (s, l, g)
CONCENTRATION EQUATIONS
pH= -log [H3O+(aq)]
pOH= -log[OH-(aq)]
[H3O+] or [H+]= 10-pH
[OH-]= 10-pOH
⭐︎If needed: 14-pH= pOH
14+pOH= pH
OLD VS MODIFIED ARRHENIUS:
ACIDS AND BASES
Old Modified
Acids Substance that ionizes to produce Acid that donates a proton
H+(aq) ions in solution. (hydrogen) to water to form
→ Any strong acids hydronium ion (H3O+)
Bases Substance that dissociates to Base that accepts the proton
produce OH-(aq) ions in solution (hydrogen) from water to form OH-
OLD VS MODIFIED ARRHENIUS:
WRITING EQUATIONS FOR ACIDS AND BASES
⭐︎Old: same steps as modified but does NOT involve H2O(water) or H3O(hydroxide)
● Acids
1. Write acid reacting with water to produce H3O+(aq)
, 2. Determine the other product → Acids lose a proton (H +)
Bases gain a proton (H-)
Examples → HCl(aq)
Old: HCl(aq) → H+(aq) + Cl-(aq)
Modified: HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq)
→ H2SO4(aq) ~ sulfuric acid
Modified: H2SO4(aq) + H2O(l) → H3O+(aq) + HSO4-(aq)
● Bases
Examples → NH3(aq)
Modified: NH3(aq) + H2O(l) → OH-(aq) + NH4+(aq)
- water donates proton to base
→ NaHCO3(aq)
Modified: Ionic compound splits into ions: Na+ and HCO3-
HCO3-(aq) + H2O(l) → OH-(aq) + H2CO3
→ Strong acids and bases; complete reaction , dissociation
←→ Weak acids and bases; partial reaction, dynamic equilibrium
Example→ Old Arrhenius: CH3COOH(aq) → CH3COOH(aq)
Modified Arrhenius: CH3COOH(aq) ←→ CH3COOH(aq)
RULES FOR NAMING AND FORMULAS FOR ACIDS
● Rules
- Identify the acid by: Hydrogen or attached H+
- All acids are soluble in water: include (aq)
IUPAC Naming System (Compound Name) Classical Naming System (Acid Name)
Aqueous hydrogen _____ide = Hydro_____ic acid
Aqueous hydrogen _____ate = _____ic acid
⭐︎ negative polyatomic: ate → ic acid
Aqueous hydrogen _____ite = _____ous acid
⭐︎ negative polyatomic: ite → ous acid
USING MASS OF ACID/BASE TO CALCULATE:
CONCENTRATION, pH, pOH OF ACID/BASE
SIG DIG RULES FOR pH
pH/pOH [H3O+]/[OH-]
→ NO units, numbers only → Units: mol/L
→ Sig digs: right of the decimal → Sig digs: follow normal rules
