Silver chloride hydroxide + AgCl

Use the information in Table 1.1 to classify the following ionic compounds as soluble or insoluble in water (a) zinc acetate, Zn(CH3C02)2 (b) iron(III) chloride, FeCl3 (c) silver chloride, AgCl (d) copper(II) hydroxide, Cu(OEf)2. 

Electrode of the second kind — Electrodes of the second kind [i-ii] contain a metal, a poorly soluble compound of this metal (which is usually a salt but it may be oxide or hydroxide as well), and an electrolyte which can establish a solubility equilibrium with the precipitate. Typical examples are Ag(s) AgCl(s) KCl(aq), Hg(l) Hg2Cl2(s) KCl(aq), Hg(l) HgO(s) NaOH(aq), Hg(l) HgS04(s) H2S04(aq). The solubility equilibrium, e.g., for the silver chloride electrode, is as follows... 

The silver ammonia complex, Ag(NH8)2, is sufficiently stable for ammonium hydroxide to dissolve precipitated silver chloride by re-ducing the concentration of silver ion, [Ag+], below the value required for precipitation by the solubility product of AgCl. A satisfactory test for silver ion is the formation with chloride ion of a precipitate which is soluble in ammonium hydroxide. 

Calculate the molar solubilities, concentrations of the constiment ions, and solubilities in grams per liter for (a) silver chloride, AgCl = 1.8 X 10-1 ), inc hydroxide, Zn(OH)2... 

Chlorid—AgCl—143.4—formed when HCl or a chlorid is added to a solution containing silver. It is white turns violet and black in sunlight volatilizes at 260° (500° F.) sparingly soluble in HCl soluble in solutions of the alkaline chlorids, hyposul-flds, and cyanids, and in ammonium hydroxid. It crystallizes in octahedra on exposure of its ammoniacal solution. 

---