Consider the weak bases below and their Kb values: C6H7O- Kb = 1.3 × 10-10 C2H5NH2 Kb = 5.6 × 10-4 C5H5N Kb = 1.7 ×10-9 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

A) C5H5NH+6H7OH 2H5NH B) C6H7OH 5H5NH+ 2H5NH C) C5H5NH+2H5NH3+ 6H7OH D) C6H7OH 2H5NH3+5H5NH+ E) C2H5NH3+5H5NH+ 6H7OH A) C5H5NH+6H7OH 2H5NH B) C6H7OH 5H5NH+ 2H5NH C) C5H5NH+2H5NH3+ 6H7OH D) C6H7OH 2H5NH3+5H5NH+ E) C2H5NH3+5H5NH+ 6H7OH

What is [OH-] for a solution at 25°C that has [H3O+] = 2.35 × 10-3 M?

A) 4.26 × 10-5 M B) 2.35 ×10-11 M C) 4.26 × 10-12 M D) 2.35 × 10-17 M E) 2.35 ×10-3 M A) 4.26 × 10-5 M B) 2.35 ×10-11 M C) 4.26 × 10-12 M D) 2.35 × 10-17 M E) 2.35 ×10-3 M

Below is a representation of an aqueous solution of a weak acid HA at equilibrium.(Each circle represents 1.0 ×10-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are not shown for clarity.) What is Ka of HA?

A) 1.0 ×10-6 B) 6.0 ×10-3 C) 2.5 ×10-4 D) 3.6 ×10-5 E) 1.0 ×10-9 A) 1.0 ×10-6 B) 6.0 ×10-3 C) 2.5 ×10-4 D) 3.6 ×10-5 E) 1.0 ×10-9

In the reaction CaO(s)+ SO2(g) CaSO3(s),

A) O2- acts as a Lewis base,and SO2 acts as a Lewis acid. B) Ca2+ acts as a Lewis base,and SO42- acts as a Lewis acid. C) SO32- acts as a Lewis base,and SO2 acts as a Lewis acid. D) SO2 acts as a Lewis base,and O2- acts as a Lewis acid. E) SO2 acts as a Lewis base,and Ca2+ acts as a Lewis acid. A) O2- acts as a Lewis base,and SO2 acts as a Lewis acid. B) Ca2+ acts as a Lewis base,and SO42- acts as a Lewis acid. C) SO32- acts as a Lewis base,and SO2 acts as a Lewis acid. D) SO2 acts as a Lewis base,and O2- acts as a Lewis acid. E) SO2 acts as a Lewis base,and Ca2+ acts as a Lewis acid.

The acid dissociation constant Ka equals 1.26 × 10-2 for HSO4- and is 5.6 × 10-10 for NH4+. Which statement about the following equilibrium is correct? HSO4-(aq)+ NH3(aq) SO42-(aq)+ NH4+(aq)

A) The reactants will be favored because ammonia is a stronger base than the sulfate anion. B) The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion. C) Neither reactants nor products will be favored because all of the species are weak acids or bases. D) The initial concentrations of the hydrogen sulfate ion and ammonia must be known before any prediction can be made. E) This reaction is impossible to predict,since the strong acid and the weak base appear on the same side of the equation. A) The reactants will be favored because ammonia is a stronger base than the sulfate anion. B) The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion. C) Neither reactants nor products will be favored because all of the species are weak acids or bases. D) The initial concentrations of the hydrogen sulfate ion and ammonia must be known before any prediction can be made. E) This reaction is impossible to predict,since the strong acid and the weak base appear on the same side of the equation.

The substance (CH3CH2)2NH is considered to be

A) a weak acid. B) a weak base. C) a strong acid. D) a strong base. E) a neutral compound. A) a weak acid. B) a weak base. C) a strong acid. D) a strong base. E) a neutral compound.