The bearing of these relations, which, it will be noted, concern ‹concentrations of silver-ion›, can best be seen by working with solutions of definite concentrations. If the solution we have just prepared is diluted with water to 200 c.c., a 0.05 molar solution of [(NH_{3})_{2}Ag]NO_{3} is formed. In such a solution, the concentration, [Ag^{+}], of the silver-ion is only 0.0009,[432] whereas in 0.05 molar silver nitrate solution it is 0.0435. It is clear that the reactions of the silver-ion will not be observed as readily in such an ammoniacal solution as in a solution of silver nitrate, which contains the same concentration of ‹total silver›. That such is the case, may be readily demonstrated as follows: the addition of 1 c.c. of molar sodium bromate to 10 c.c. of 0.05 molar silver nitrate immediately forms a heavy precipitate of the moderately difficultly soluble bromate, AgBrO_{3}, while the same addition to 10 c.c. of the 0.05 molar silver-ammonium nitrate solution produces no precipitate whatever (‹exp.›). [p221] A liter of water dissolves 0.025 mole (6 grams) of silver bromate[433] at 18°. If the same degree of ionization be assumed for it as for a 0.025 molar solution of the analogous salt, silver nitrate, AgNO_{3}, 90% of the silver bromate in the saturated solution is ionized. The solubility-product constant then is [Ag^{+}] × [BrO_{3}^{−}] = (0.025 × 0.9)^2 = 0.0005. When 1 c.c. of molar sodium bromate is added to 10 c.c. of 0.05 molar silver nitrate, each salt is ionized 80% in the mixture, and [Ag^{+}] = 0.05 × 0.8 × 10 / 11 = 0.037 and [BrO_{3}^{−}] = (1 × 1 / 11) × 0.8 = 0.072. Then the product of the ion concentrations, [Ag^{+}] × [BrO_{3}^{−}] = 0.037 × 0.072 = 0.0027, is considerably larger than the constant 0.0005 and precipitation follows. But, when 1 c.c. of molar sodium bromate is added to 10 c.c. of a 0.05 molar silver-ammonium nitrate solution, the concentration of silver-ion[434] is 0.00085 and the product of the ion concentrations, [Ag^{+}] × [BrO_{3}^{−}] = 0.00085 × 0.072 = 6E−5, is smaller than the constant; the solution will not be saturated with silver bromate and no precipitate is formed. On the other hand, if 1 c.c. of a 0.1 molar solution of sodium chloride is added to 10 c.c. of 0.05 molar silver-ammonium nitrate solution, a very decided precipitate of silver chloride is formed (‹exp.›). The difference in the action of the sodium bromate and the chloride lies in the fact that silver chloride is 2500 times as insoluble as is silver bromate, and the chloride may be precipitated from solutions containing a ‹very much smaller concentration of the silver-ion› than is required for the precipitation of silver bromate.