ap chem 3.2.4 quiz

Given the reaction:Cu2+(aq) + S2-(aq) CuS(s)What will happen (a) if CuSO4(aq) is added? And (b) if Na2SO4(aq) is added?

(a) More product will form; (b) Nothing

An aqueous solution of 0.25 M silver nitrate, AgNO3, and 0.25 M iron(II) nitrate, Fe(NO3)2, are allowed to come to equilibrium in the following chemical reaction: Ag+(aq) + Fe2+(aq) Fe3 + (aq) + Ag(s) If the equilibrium constant, Kc, for the reaction is 3.0 × 10-3, what is the equilibrium concentration of Fe3+?

1.9 × 10-4 M

For an endothermic dissolution process, which of the following would you observe on cooling a saturated solution by 10 degrees Celsius?

An increase in precipitation

Given the following solubility constants, which list arranges the solutes in order of increasing solubility? CaCO3: Ksp = 2.8×10−9Ca(OH)2: Ksp=5.5×10−6CaSO4: Ksp = 9.1×10−6CaF2: Ksp = 5.3×10−9

CaCO3<CaF2<Ca(OH)2<CaSO4

A, B, C, and D are 4 salts whose Ksp values are 9.21 × 10-8, 7.44 × 10-11, 1.07 × 10-21, and 38.65, respectively. What is the correct arrangement of their solubilities in decreasing order?

D, A, B, C

Which of the following is true of the solubility product constant?

It is an equilibrium constant.

In which of the following cases will there be precipitation

Q>Ksp

Which of the following processes would cause a precipitation reaction to occur?

The addition of a common ion to the solution

What is the relationship between the solubility product constant Ksp and temperature?

When dissolution is endothermic, Ksp increases as the temperature increases.

what is the nature of a solution when it has reached its solubility equilibrium

the solution must be saturated