Silver chloride is described as a white crystalline chemical compound having the formula AgCl. Silver chloride, present in the test tube, turns into purplish quickly, especially in the case of sunny laboratory due to the silver chloride being split up into both chlorine and silver. Silver chloride can be prepared when the sodium chloride compound is added to the silver nitrate solution; there occurs a white precipitate of silver chloride. Silver chloride is also an example of a well-known salt stain, which is used to impart an amber colour to the glass.
Chloro silver is the other name of silver chloride.
Let us look at the properties of silver chloride as follows.
Let us look at the physical properties of silver chloride.
Let us look at the chemical properties of silver chloride.
Silver chloride undergoes a decomposition reaction in the presence of sunlight to produce chlorine and silver. The chemical reaction for the same can be given as follows:
AgCl → Ag + Cl
Silver chloride reacts with a base same as ammonia, forming a complex compound known as chloride ion and Silver diammo ion. The chemical reaction for the same can be given as follows:
AgCl + 2NH3 → [Ag(NH3)2]+ + Cl–
The solid adopts the structure of fcc NaCl, where every Ag+ ion is surrounded by an octahedron of 6 chloride ligands. Similarly, AgBr and AGF crystallize. However, crystallography depends on the crystallization condition, majorly in the free silver ion concentration.
[Image will be Uploaded Soon]
Silver chloride is given as unusual, where in that, unlike most of the chloride salts, it contains very low solubility. It can be synthesized easily by the process of metathesis, which is combining an aqueous solution of silver nitrate (soluble) with a soluble chloride salt, like cobalt(II) chloride or sodium chloride. The formed silver chloride will precipitate immediately.
Let us look at the important uses of silver chloride as listed below.
Silver chloride's low solubility makes it a useful addition to pottery glazes for the formation of "Inglaze lustre".
It has been used as an antidote for mercury poisoning, assisting in mercury elimination.
Silver chloride is also used:
to make a photographic paper because it reacts with photons to produce a latent image via photoreduction
in the photochromic lenses, again taking advantage of its reversible conversion to Ag metal
wound healing products and in bandages
to create amber, brown, and yellow shades in the manufacturing of stained glass
as an infrared transmissive optical component since it can be hot-pressed into lens shapes and window
As an antimicrobial agent:
for the long-term preservation of drinking water in water tanks
in a few personal deodorant products
Due to the dissociation constant, if we notice the rows of the periodic table, chlorine falls above the iodine which means, it makes stronger ions, and we also know that strong ions contain high dissociation. Moreover, higher dissociation is also known as higher reactivity.
Another way to look at it is from the acid-base point of view.
The base of silver is weak, whereas chlorine acid is strong. When the weak base reacts with a strong acid, it forms acidic salt. It means the salt that produces acidic ph, currently (ammonia), becomes a base when dissolved in water. Thus, chlorine from AgCl reacts with NH₃ to produce NH₄-Cl. Even though the AgCl holds a poor dissociation but the ionized Cl reacts with ammonia and disturbs the equilibrium present between Ag+n Cl-. Hence, more AgCl dissociates to maintain the equilibrium until all the Agcl is consumed.
Furthermore, the acid of iodine and the silver base is weak. Therefore, weak acid reacts with the weak base to form neutral salt with poor dissociation. We can also confirm it by the fact that the solubility of AgI is poorer than the AgCl.
No, though AgCl and NaCl seem to be similar, the Ag ion's effective nuclear charge is much more compared to the Na+ ion. Thus, according to the Fajan law, it polarizes chloride anion and forms the bond between them more covalently (in NaCl, Na holds an overall positive charge, and chloride holds a negative charge. Hence, there is no electron present between Cl and Na, and thus it is not covalent. Whereas in Cl and Ag, as polarization occurs, the electron residing on Cl- gets towards the Ag+ ion. Therefore, some amount of electric charge comes between Cl- and Ag+ ion and this forms a covalent bond.
Q1. What are the Uses of Silver Chloride?
Answer: AgCl contains many antiseptic and disinfectant properties and can also be used in mercury poisoning treatment. This compound finds usage in wound healing materials, antimicrobials, water treatment, antidotes, and personal deodorants. At low concentrations, Silver chloride is not harmful and can also be used in disinfectant and medical applications.
Q2. Explain the Health Hazards of Silver Chloride.
Answer: If silver chloride is ingested, it can cause digestive tract discomfort. At the same time, the intake of soluble silver salts can induce argyria, which is characterized by permanent blue-grey skin pigmentation, eyes, and mucous membranes. Also, silver compounds ingestion can lead to stiffness, abdominal pain, shock, and seizures.
Q3. Explain the Synthesizing Process of Silver Chloride.
Answer: The combination of aqueous solutions of sodium chloride and silver nitrate is an easy method of synthesizing the silver chloride compound. It is also formed by reacting the cobalt (II) chloride with the silver nitrate. This is general precipitation for silver nitrate reaction to soluble chloride salts, and it is not unique to cobalt alone.
Q4. List the Important Uses of Silver Chloride.
Answer: Some of the uses of silver chloride can be listed as follows:
The most effective method of water-activated battery uses magnesium as anode and silver chloride as a positive electrode.
It can be used in polishing mirrors, electroplating, and making alloys.
It can also be used as an antidote that reacts with the poison to form a harmless chemical compound.
It is used in medicines.
Silver salts are used in photographic films.