Unit 7 Chapter 16 and 17

Review of Acids and Bases

Conjugate Acid-Base Pairs

The Autoionization of Water

The pH Scale

Strong Acids and Bases

Weak Acids

Calculating K a from pH

Using K a to calculate pH

Polyprotic Acids

Weak Bases

Using K b to Calculate [OH-]

The Relationship Between K a and K b

Acid-Base Properties of Salts

Using pH to Determine the Concentration of a Salt

Acid-Base Behavior and Chemical Structure

Lewis Acids and Bases

Additional Aspects of Aqueous Chapter 17

The Common Ion Effect

Buffer Solutions

Calculating the pH of a Buffer

Adding Strong Acids or Bases to Buffers

Acid Base-Titrations

Effect of K a on titration curves

Solubility Equilibria

Factors that Affect Solubility

Precipitation

A solution contains 0.2 M Ba 2+ and 0.2 M Ca 2+. Which of the following CrO 4 2- concentrations will precipitate as much Ba 2+ as possible with out precipitating any CaCrO 4 ?(The K sp of BaCrO 4 = 1 x and the K sp of CaCrO 4 = 7 x ) (A) 3.5 x M (B) 7 x M (C) 1.5 x M (D) 5 x M (E) 7 x M

(A) NH 3 and CH 3 COOH (B) KOH and NH 3 (C) HCl and KCl (D) H 3 PO 4 and KH 2 PO 4 (E) NH 3 and NH 4 Cl 18.) The solution with the highest pH 19.) The solution with the lowest pH 20.) The solution with the pH closest to neutral 21.) A buffer with a basic pH 22.) A buffer with an acidic pH

What is the [H+] in a 0.02 M nitrous acid (HNO 2 ) solution? (K a for HNO 2 is 4.5 x ) (A) 2.25 x (B) 3.0 x (C) 5.1 x (D) 9.0 x (E) 2.6 x 10 -7

BaF 2 is slightly soluble in water. The addition of dilute HF to a saturated solution of BaF 2 at equilibrium is expected to: (A) Raise the pH (B) React with BaF 2 to produce hydrogen gas (C) increase the solubility of BaF 2 (D) Decrease the solubility of BaF 2 (E) produce no change in the solution

At 25 o C, an aqueous solution with a pH of 6 has a hydroxide concentration [OH-], of: (A) 1 x M (B) 1 x M (C) M (D) 6 M (E) 8 M