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Ferric Chloride
Introduction
Ferric chloride is an inorganic chemical with the formula $\mathrm{FeCl_{3}}$ that has a wide range of industrial, medicinal, & laboratory applications. Iron (πΌπΌπΌ) chloride or Iron trichloride is its IUPAC term. It is a dangerous substance that is very corrosive & acidic. The anhydrous substance is a potent dehydrating agent. Even though human poisoning is uncommon, consumption of $\mathrm{FeCl_{3}}$ can result in significant morbidity & lead fatality. Even though chlorine is a nonmetal & iron is a metal, it is a covalent complex. Because chlorine is more electronegative than iron, it draws a shared electron pair towards itself in $\mathrm{FeCl_{3}}$, while iron receives a partial positive charge.
What is Ferric Chloride?
It is an inorganic chemical made up of iron with an oxidation state of +3. The compound, often known as Molysite, is a solid that ranges in colour from orange to brown-black. It has the chemical formula $\mathrm{FeCl_{3}}$. In general, $\mathrm{FeCl_{3}}$ is very weakly soluble in water. $\mathrm{FeCl_{3}}$ solutions are either colourless or light brown. Human tissues & other metals are both corroded by $\mathrm{FeCl_{3}}$ solution. The non-combustible $\mathrm{FeCl_{3}}$ solution is utilised in sewage treatments & water cleaning.
Properties of Ferric Chloride
The physical & chemical properties of ferric chloride are as follows.
Physical Properties
Anhydrous $\mathrm{FeCl_{3}}$ is made up of octahedral centres that are linked together by two coordinating chloride ligands.
Light-reflecting crystals are dark green, whereas light-transmitting crystals are purple-red.
In contrast to anhydrous forms of the compound, aqueous solutions are often colourless or yellow.
Organic solvents such as diethyl ether & methanol are very soluble in the compound. Ethyl acetate does not dissolve it.
Heat is emitted when mixed with water, indicating that the process is exothermic. When $\mathrm{FeCl_{3}}$ is dissolved in water, it forms an acidic mixture.
| Property | Value |
|---|---|
| Ferric Chloride | $\mathrm{FeCl_{3}}$ |
| Molecular Weight | 162.204 π/πππ (anhydrous) |
| Density | 2.90 π/ππ3 (anhydrous) |
| M.P. | 307.6Β°C |
| B.P. | 316Β°C |
| Odour | Faint π»πΆπ |
| Colour | Orange to brown-black |
Chemical Properties
The $\mathrm{FeCl_{3}}$ -water reaction
The reaction of $\mathrm{FeCl_{3}}$ with water is exothermic, which means that heat is produced. This reaction yields a very acidic solution.
Ferric chloride heating
When $\mathrm{FeCl_{3}}$ is heated to 350 β, a unique πΉπ compound known as iron oxychloride is created.
Ferric chloride reaction with carboxylate anions
The compound rapidly interacts with carboxylate anions or oxalates to form salt compounds like tartrate & citrate.
$\mathrm{FeCl_{3}}$ reaction with alkali metal alkoxides
Iron alkoxide compounds are formed when the compound reacts with alkali metal alkoxides. The complexes might be dimeric or trimeric.
Ferric chloride-chlorobenzene reaction
When the compound interacts with chlorobenzene, a di-substituted compound known as dichlorobenzene is formed. This process produces hydrochloric acid & ferrous chloride as by-products.
$$\mathrm{2FeCl_{3}\:+\:c_{6}H_{5}Cl\:\rightarrow\:2FeCl_{2}\:+\:C_{6}H_{5}CL_{2}\:+\:HCl}$$
$\mathrm{FeCl_{3}}$ reaction with organometallic compounds
The compound reacts with organometallic complexes like methyl lithium. In the existence of ether, $\mathrm{FeCl_{3}}$ combines with methyl lithium to form lithium tetrachloroferrate(πΌπΌπΌ), a greenish-yellow complex. In the existence of excess methyl lithium, the reaction progresses & produces lithium tetrachloroferrate (πΌπΌ).
$$\mathrm{2FeCl_{3}\:+\:LiCH_{3}\:\rightarrow\:FeCl_{3}\:+\:LiFeCl_{4}\:+\:CH_{3}}$$
Reduction-oxidation reactions of ferric chloride
Because the compound is a moderate oxidising agent, it participates in a variety of redox processes.
$\mathrm{CuCl_{2}}$ is formed when ferric chloride oxidises πΆπ’πΆπ.
Iron(πΌπΌ) chloride is formed through the comproportionation reaction of ferric chloride & iron.
Preparation of Ferric Chloride
The iron & chlorine reaction.
Iron ore reaction with HCl
Ferrous chloride-chlorine reaction
Oxygen-ferrous chloride reaction
$$\mathrm{2Fe\:+\:3Cl_{2}\:\rightarrow\:2FeCl_{3}}$$
$$\mathrm{Fe_{3}O_{4}\:+*\:8HCl\:\rightarrow\:FeCl_{2}\:+\:2FeCl_{3}\:+\:4H_{2}O}$$
$$\mathrm{2FeCl_{2}\:+\:Cl_{2}\:\rightarrow\:2FeCl_{3}}$$
$$\mathrm{4FeCl_{2}\:+\:O_{2}\:+\:4HCl\:\rightarrow\:4FeCl_{3}\:+\:2H_{2}O}$$
Ferric Chloride Test
This test is used to evaluate whether phenol is present in a particular sample. Sulfinic acids, Enols, oximes, & hydroxamic acids produce favourable effects. The Folin-Ciocalteu test can be used to determine the amount of phenol in a sample.
Dissolve the substance in a solution of water & ethanol.
Add a few drops of dilute ferric chloride.
If the colour of the substance changes to red, green, purple, or blue, it identifies the existence of phenols.
If the substance is insoluble in water, dissolve it in dichloromethane $\mathrm{(CH_{2}Cl_{2})}$ with a little amount of pyridine $\mathrm{(C_{5}H_{5}N)}$
Applications of Ferric Chloride
It is utilised in wastewater treatment & water cleaning.
Many organic processes employ $\mathrm{FeCl_{3}}$ as a catalyst. Friedel crafts alkylation & aromatic compound chlorination are two instances.
In the colourimetric examination of phenols, ferric chloride is utilised.
It is also used in veterinary medicine to treat overgrown animal claws that cause bleeding.
It may also test for gamma-hydroxybutyric acid & gamma-butyrolactone.
In several reactions, it is utilised as a drying reagent.
It is utilised in pattern welding by bladesmiths & craftspeople.
It is employed in the removal of the aluminium coating from mirrors.
It is employed in the etching of complicated medical equipment.
Conclusion
Iron chloride is another name for ferric chloride. It is a chemical complex with the chemical formula $\mathrm{FeCl_{3}}$ . It has a lower melting temperature than its boiling temperature, which is roughly 315Β°C. When the compound is dissolved in water, it undergoes hydrolysis & emits heat in an otherwise exothermic reaction. It is made in factories by reacting dry chlorine with scrap iron at temperatures ranging from 500 to 700Β°C. It dissolves into a light brown aqueous solution with a mildly hydrochloric acid odour. It is extremely corrosive to most metals & is almost certainly harmful to tissues.
FAQs
1. Is Ferric Chloride a kind of electrolyte?
It is a very corrosive acid. As a result, it can function as an electrolyte component
2. Can Ferric Chloride be thrown away?
Water has a negative reaction with $\mathrm{FeCl_{3}}$. It is not recommended to dispose of the drain
3. Is $\mathrm{FeCl_{3}}$ basic or acidic?
The pH of the compound is two, which is lower than the neutral pH of seven. As a result, the chemical has an acidic pH.
4. What exactly is the distinction between Ferric Chloride & Iron (π°π°) Chloride?
Unlike $\mathrm{FeCl_{3}}$, Iron (πΌπΌ) Chloride has been specifically employed in the flocculation of sulphide or chlorate-containing wastewater. It is also employed in organic production as a reagent.
5. Name the chemical tests which should be performed to differentiate between the Benzoic acid & Phenol compounds?
Ferric chloride test- When neutral $\mathrm{FeCl_{3}}$ is added to both solutions, phenol interacts with it to create an iron-phenol compound, resulting in a violet colour, whereas benzoic acid does not.
