Salts

Salt Solutions The salts of weak acids can recombine with water producing basic solutions

Salt Solutions The salts of weak bases can recombine with water producing acidic solutions

Salt Solutions A - + H 2 O HA + OH - B + + H 2 O H + + BOH

Salt or Hydrolysis Problems

Salt Problem Calculate the pH of a 0.20 M solution of NaBz K a = 6.4 x 10 -5

Salt Problem Calculate the pH of a 0.10 M solution of R-NH 3 Cl K b = 2.5 x 10 -5

Drill: Calculate the pH of a 0.18 M solution of KC 2 H 3 O 2 K a = 1.8 x 10 -5

Drill: Calculate the pH of a 0.16 M solution of KC 7 H 5 O 2 K a = 6.4 x 10 -5

Salt Applications Salts of strong acids & weak bases make acidic solutions

Salt Applications Salts of strong bases & weak acids make basic solutions

Salt Applications Salts of strong acids & strong bases make neutral solutions

Predict Relative pH NaAcBaCl 2 KNO 3 NH 4 Br KHSO 4 NH 4 Ac

Predict Relative pH KAcNaCl KClO 2 NH 4 Cl K 2 SO 4 NaI

Anhydrides Compounds without water; that when added to water, form other compounds

Acid Anhydrides Non-metal oxides that form acids when added to water

Basic Anhydrides Metal oxides that form bases when added to water

Predict Relative pH Na 2 OSO 2 NO 2 CO 2 CaOAl 2 O 3

A/B eq, Buffer & Salt Hydrolysis Problems

Calculate the pH of 0.10 M HF. K a HF = 6.5 x 10 -4

7.4 g of Ca(OH) 2 was added to 2.0 L of M H 2 CO 3. Calculate the molarity of all ions present in the solution. K a1 = 4.4 x K a2 = 4.7 x

Calculate the pH of 0.10 M HF in 0.20 M NaF. K a HF = 6.5 x 10 -4

Calculate the pH of 5.0 M KCN. K aHCN = 5.0 x

Calculate [H 3 PO 4 ], [H 2 PO 4 -1 ], [HPO 4 -2 ], [PO 4 -3 ], [K + ], [H + ], & pH of 1.0 M KH 2 PO 4 in 0.50 M K 2 HPO 4. K a1 = 7.5 x K a2 = 6.2 x K a3 = 4.2 x

Calculate pH of: 0.50 M MOH in 0.20 M MCl K b = 5.0 x 10 -5

Calculate pH of: 0.20 M MCl K b = 5.0 x 10 -5

Review of Acid/Base descriptions and Acid/Base, Buffer, & Salt Equilibria

Arhenius, Bronsted- Lowry, & Lewis Acids & Bases

Strong Acids Strong Bases

Acid rxns Base rxns

A/B Equilibrium Constants K W, K A, K B, & pH

Calculate pH of: M HNO M KOH

Calculate pH of: 2.0 M HNO 2 K a = 2.0 x 10 -4

Calculate pH of: 3.0 M HZ in 2.0 M KZ K a HZ = 3.0 x 10 -5

Calculate pH of: 0.20 M KQ K a HQ = 2.0 x 10 -5

150 mL of 0.10 M KOH was added to mL of 0.10 M H 2 CO 3. Calculate [H 2 CO 3 ], [HCO 3 - ], [CO 3 -2 ], [H + ], [OH - ], & pH of the solution. K a1 = 4.4 x K a2 = 4.7 x

Calculate [H 3 A], [H 2 A -1 ], [HA -2 ], [A -3 ], [K + ], [H + ], [OH - ], & pH of 2.0 M KH 2 A. K a1 = 4.0 x K a2 = 5.0 x K a3 = 2.5 x

Calculate pH of: 2.0 M HQ K a = 2.0 x 10 -6

Calculate pH of: 6.0 M HZ in 4.0 M KZ K a HZ = 3.0 x 10 -5

Calculate pH of: 0.20 M KQ K a HQ = 2.0 x 10 -7