Chapter 18, Problem 91E

Refer to the K_sp value from Table 17.2 to calculate the solubility of iron(ll) hydroxide in pure water in grams per 100.0 ml of solution.

Table 17.2 Selected Solubility-Product Constants (K_sp) at 25 ?C

Compound	Formula	Ksp	Compound	Formula	Ksp
Barium fluoride	BaF2	2.45 × 10−5	Lead(II) chloride	PbCl2	1.17 × 10−5
Barium sulfate	BaSO4	1.07 × 10−10	Lead(II) bromide	PbBr2	4.67 × 10−6
Calcium carbonate	CaCO3	4.96 × 10−9	Lead(II) sulfate	PbSO4	1.82 × 10−8
Calcium fluoride	CaF2	1.46 × 10−10	Lead(II) sulfide	PbS	9.04 × 10−29
Calcium hydroxide	Ca(OH)2	4.68 × 10−6	Magnesium carbonate	MgCO3	6.82 × 10−6
Calcium sulfate	CaSO4	7.10 × 10−5	Magnesium hydroxide	Mg(OH)2	2.06 × 10−13
Copper(II) sulfide*	CuS	1.27 × 10−36	Silver chloride	AgCl	1.77 × 10−10
Iron(II) carbonate	FeCO3	3.07 × 1011	Silver chromate	Ag2CrO4	1.12 × 10−12
Iron(II) hydroxide	Fe(OH)2	4.87 × 10−17	Silver bromide	AgBr	5.36 × 10−13
Iron(II) sulfide*	FeS	3.72 × 10−19	Silver iodide	AgI	8.51 × 10−17

*Sulfide equilibrium is of the type: $\text{MS}\left(s\right)+{\text{ H}}_{\text{2}}\text{O}\left(l\right)\rightleftharpoons {\text{M}}^{\text{2}+}\left(aq\right)+{\text{ HS}}^{+}\left(aq\right)+{\text{ OH}}^{–}\left(aq\right)$ .