10.At a certain temperature, the solubility of strontium arsenate, Sr3(AsO4)2, is 0.0520 g/L. What is the Ksp of this salt at this temperature?

11.The Ksp of magnesium carbonate, MgCO3, is 6.82 × 10-6. Calculate the solubility of this compound in g/L.

12.The Ksp of calcium hydroxide, Ca(OH)2, is 5.02 × 10-6. Calculate the solubility of this compound in g/L.

13.At 22 °C an excess amount of a generic metal hydroxide M(OH)2 is mixed with pure water. The resulting equilibrium solution has a pH of 10.36. What is the Ksp of the salt at 22 °C?

14. Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12× 10-12. What is the solubility (in mol/L) of silver chromate

(a) in 1.50 M potassium chromate aqueous solution?

(b) in 1.50 M silver nitrate aqueous solution?

(c) in pure water?

15.The Ksp of CaSO4 is 4.93× 10-5. Calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na2SO4(aq) at 25 °C.

18.Above what Fe2 concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 9.18? The Ksp of Fe(OH)2 is 4.87×10-17.

19.Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0380 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, Ksp, can be found here.

What percentage of the Ca2 (aq) can be precipitated from the Ag (aq) by selective precipitation?

21.A 0.170-mole quantity of NiCl2 is added to a liter of 1.20 M NH3 solution. What is the concentration of Ni2 ions at equilibrium? Assume the formation constant* of Ni(NH3)62 is 5.5 × 108.

24. Write the balanced chemical equation for each of these reactions. Include phases.

When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms.

However, when additional aqueous hydroxide is added the precipitate redissolves forming a soluble [Pb(OH)4]2-(aq) complex ion.