Ionic Equilibria

The solubility product expression for tin(II) hydroxide, Sn(OH)₂, is

• [Sn²⁺][OH^-]

• [Sn²⁺]²[OH^-]

• [Sn²⁺][OH^-]²

• [Sn²⁺]³[OH^-]

Consider the following solubility data for various chromates at 25^oC.

Ag₂CrO₄, K_sp = 9.0 x 10^-12

BaCrO₄, K_sp = 2.0 x 10^-10

PbCrO_4, K_sp = 1.8 x 10^-14

The chromate that is the most soluble in water at 25^oC on a molar basis is:

• Ag₂CrO₄

• BaCrO₄

• PbCrO₄

• impossible to determine

The molar solubility of PbBr₂ is 2.17 x 10^-3 M at a certain temperature. Calculate K_sp for PbBr₂.

• 6.2 x 10^-6

• 6.4 x 10^-7

• 4.1 x 10^-8

• 3.4 x 10^-6

The solubility of silver sulfate in water at 100^oC is approximately 1.4 g per 100 mL. What is the solubility product of this salt at 100^oC?

• 8.3 x 10^-6

• 3.5 x 10^-7

• 5.7 x 10^-8

• 3.6 x 10^-4

What is the molar solubility, s, of Ba₃(PO₄)₂ in terms of K_sp?

• s = K_sp^1/2

• s = K_sp^1/5

• s = [K_sp/27]^1/5

• s = [K_sp/108]^1/5

For Cu(OH)₂, K_sp = 1.6 x 10^-19. What is the molar solubility of Cu(OH)₂?

• 3.4 x 10^-7 M

• 6.4 x 10^-7 M

• 2.7 x 10^-11 M

• 5.1 x 10^-10 M

Ag₃PO₄ would be least soluble at 25^oC in

• 0.1 M AgNO₃

• 0.1 M HNO₃

• pure water

• 0.1 M Na₃PO₄

The molar solubility of PbCl₂ in 0.20 M Pb(NO₃)₂ solution is:

• 1.7 x 10^-4 M

• 9.2 x 10^-3 M

• 1.7 x 10^-5 M

• 4.6 x 10^-3 M

When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will precipitate if Q_sp _____ K_sp, and will continue to precipitate until Q_sp _____ K_sp.

• is greater than; equals

• is less than; is greater than

• is less than; equals

• equals; is less than

Which of the following pairs of compounds gives a precipitate when aqueous solutions of them are mixed? Assume that the concentrations of all compounds are 1.0 M immediately after mixing.

• CuBr₂ and K₂CO₃

• HNO₃ and NH₄I

• BaCl₂ and KClO₄

• Na₂CO₃ and H₂SO₄