case of argentometry. The solubility product, Ksp, for AgCl in water is at room temperature, which indicates that only 1.9 mg (that is, ) of AgCl will dissolve per liter of water. The chloride content of an aqueous solution can be determined quantitatively by weighing the precipitated AgCl, which conveniently is non-hygroscopic, since AgCl is one of the few transition metal chlorides that is unreactive toward water. Interfering ions for this test are bromide and iodide, as well as a variety of ligands (see silver halide). For AgBr and AgI, the Ksp values are 5.2 x 10−13 and 8.3 x 10−17, respectively. Silver bromide (slightly yellowish white) and silver iodide (bright yellow) are also significantly more photosensitive than is AgCl. AgCl quickly darkens on exposure to light by disintegrating into elemental chlorine and metallic silver. This reaction is used in photography and film. Uses The silver chloride electrode is a common reference electrode in electrochemistry. Silver chloride's low solubility makes it a useful addition to pottery glazes for the production of "Inglaze lustre". Silver chloride has been used as an antidote for mercury poisoning, assisting in the elimination of mercury. Silver chloride is used: to make photographic paper since it reacts with photons to form latent image and via photoreduction in photochromic lenses, again taking advantage of its reversible conversion to Ag metal in bandages and wound healing products to create yellow, amber, and brown shades in stained glass manufacture as an infrared transmissive optical component as it can be hot-pressed into window and lens shapes as an antimicrobial agent: in some personal deodorant products for long-term preservation of drinking water in water tanks See also Photosensitive glass References Chlorides Silver compounds Metal halides Coordination complexes Photographic chemicals Light-sensitive chemicals Rock salt crystal structure