Medicinal Chemistry

Aluminium Hydroxideoccurrence

Aluminum hydroxide is a hydroxide salt type of aluminum. It is usually utilized as a medication, and can be found in acid neutralizers for the treatment of indigestion, gastritis, and peptic ulcers. It might likewise be utilized to lessen the retention of phosphorus in individuals with kidney failure. It is dangerous and even lethal. It harms every single distinctive kind of tissues, and is somewhat less lethal than lead or mercury.

Properties

It is free from odour, white in colour and not crystal like structure, change into liquid from solid on 300 ‘C, cannot be dissolved in aqueous medium and alcohol but can be dissolve in acidic and basic mediums because it contains both Acidic-Basic properties at ones.

Preparation of Aluminium Hydroxide

Commercially aluminium hydroxide is prepared by Bayer Process. In this process bauxite is dissolved in sodium hydroxide at 270C temperature. The bauxite residue and waste solid are removed from the solution. From the remaining solution of sodium aluminate, aluminium hydroxide is precipitated. By Potash Alum and sodium carbonateAl(OH)3 is prepared by the reaction of Potassium Alum with sodium carbonate. In 150 mi of water, 100g sodium carbonate and 100g potassium alum are dissolved separately. Filter both of the solutions and then heat them till boiling. Hot alum solution is then poured into hot sodium carbonate solution with constant stirring. 100ml of hot water is also added additionally. Aluminium hydroxide precipitates are formed.

These precipitates are drained and mixed with 200ml of hot water. The precipitates are again decanted and washed with hot water. The washing is repeated till it gives no positive reaction for sulphate ions with barium chloride. Aluminium hydroxide is then filtered and dried at 40C. Thus white, amorphous, tasteless and odorless powder is obtained. 2KAl (SO4)2 + 3NO2CO3 + 2H2O  3Na2SO4 + K2SO4 + 2Al(OH)3 + 3CO2By sol-gel methodThis method is used for ultra-fine Al(OH)3 preparation. Aluminium hydroxide is prepared by the hydrolysis of aluminium salts and alkoxides in water. Al reacts with-OH group and form Al(OH)3 which is then precipitated out.

Applications

Aluminum hydroxide has an excellent assortment of use in synthetic industry, a portion of these utilizations are as plastic, elastic, polymer and epoxy sap filler, fire resistant, added substance for glass and paper. In drug store, it is utilized as an acid neutralizer for the gastritis and ulcer treatment and it is likewise an added substance in a few immunizations and fills in as excipient in the generation of a few medications. Be that as it may, aluminum hydroxide is generally utilized as crude material in the generation of alumina (aluminum oxide) to create aluminum metal.

Ammonium Chlorideoccurrence

In other words, it is called as “salmiac or sal ammoniac. It is an inorganic salt found in the human urine. It has an imperative biochemical capacity keeping up the pH. It is found in mineralogical developments and in this shape it is called as “SALT AMMONIAC. ” It has additionally been found in some volcanic vents and slag. The mineral is usually shaped on consuming coal dumps from build-up of coal inferred gasses.

Properties

It is whitish crystal like solid material, easily dissolved in water, it is free from smell, having salt-like taste, can be changed into liquid from solid by heating at 662’C.

Preparation of Ammonium Chloride

Commercially Aluminium chloride is prepared by the reaction of aluminium metal with hydrogen chloride. It is an exothermic reaction and it takes place at 650-750 C. 2Al + 6HCL  2AlCl3 + 3H2By Aluminium metal and Iron chlorideIron chloride react with the surface of solid aluminium at 500C and produce aluminium chloride. The gaseous mixture of aluminium chloride and iron chloride is then cooled to transform them in solid phases. Then in separated sealing container, separate aluminium chloride from this mixture at 150C for 5 hours.

FeCl3 + Al  AlCl3 + Fe2

Applications

The principle use of ammonium chloride is as a nitrogen source in composts (comparing to 90% of the world creation of ammonium chloride, for example, chloroammonium phosphate. The principle crops prepared along these lines are rice and wheat in Asia. Ammonium chloride was utilized in fireworks in the eighteenth century however was superseded by more secure and less hygroscopic synthetics. Its motivation was to give a chlorine contributor to upgrade the green and blue hues from copper particles in the fire. It had an auxiliary use to give white smoke, yet its prepared twofold deterioration response with potassium chlorate creating the exceptionally insecure ammonium chlorate made its utilization extremely suspect. It is utilized as a diuretic for individuals with edema or Läennex ailments. A measurements of nine grams for each day is prescribed. Ammonium chloride acts by expanding the renal discharge of chloride. In the meantime, likewise utilized as an acidifier, as this salt outcomes in expanded acridity groupings of free hydrogen particles. Ammonium chloride, handles an expectorant, bothering the mucosa that is causing the incitement of the organs of the bronchial mucosa. In the region of pharmacokinetics, ammonium chloride, retains from the GI tract for a time of five to six hours after ingestion. Additionally, this salt is utilized for delivering dry cells of tin in zinc process and exciting procedures. In different enterprises it is utilized as transition for fastening and metal oxide remover. It is additionally utilized in materials and earthenware. Utilization of ammonium chloride ought to be under therapeutic supervision and with earlier enrollment as it might be destructive for a few people, for example, the individuals who have been determined to have cirrhosis or liver infection. This salt ought to never be utilized as treatment of metabolic alkalosis since it can cause an absence of control in renal brokenness. Whenever devoured without following set up a doctor can have reactions, for example, cerebral pain, laziness, gastica disturbance, spewing, loose bowels, anorexia, tetany, and among different sicknesses.

Sodium Carbonateoccurrence

Soda ash, also called sodium carbonate (Na2CO3), is an alkali compound produced by refining the mineral trona or naturally exicting sodium carbonate-bearing brines (both referred to as natural soda ash), the mineral nahcolite (referred to as natural sodium bicarbonate, from which soda ash can be formed), or manufactured from any of several chemical processes then called as synthetic soda ash.

Sodium carbonate is a white crystalline powder, molecular weight is 105. 988 g/mol, density of is 2. 54g/ml, melting point is 8510c, Na2co3 is hygroscopic in nature. It dissolves rapidly in water and form carbonic acid (weakly acidic) and sodium hydroxide (strong base), thus the aqueous solution of Na2co3 is strong base, which react with acids violently. When Na2co3 is heated to high temperature, it decompose and release fumes of disodium oxide (Na2Co3)

Preparation

Process of refining includes many steps to produce soda ash from trona ore. First step consists of the crushing and screening of raw ore from mine. The obtained material is then fed to rotary calciners and then heated. In this process, the trona decomposes to form crude soda ash, which is then dissolved in water. The insoluble shales are separated from the solution by passing through settling and filtration steps, and the resulting insoluble tailings are taken back into the mine and refilled. The soda ash solution is treated to remove organic materials, and obtained yield is a high-purity saturated solution of sodium carbonate. Next, the solution is fed to crystallizers where water is evaporated and sodium carbonate monohydrate crystals are obtained. The industry-familiar term "mono-process" originates from this step of processing. The crystals are dewatered and washed using cyclones and centrifuges, and the solution is recycled to the evaporator units for further recovery of soda ash. The monohydrate crystals are fed to rotary kilns where they are dried to finished soda ash. Finally, product is screened as a final step to assure purity.

Application

Sodium carbonate mainly used as:

• Water softener in laundry, in hard water it competes with Mg+ and Ca+ ion and prevent the binding of these ions with detergent.
• Food processing aid
• pH modifier
• electrolyte
• It is also used in the manufacturing of:
• glass
• pulp and paper
• Many other chemicals i. e. sodium silicate & sodium phosphate
• soap & detergent
• In chemical industry Na2co3 is used as an alkaline agent.
• It is used in reticulation (the process of photography.
• In brick industry it is used as a wetting agent.

Magnesium Carbonte

• Magnesium carbonate is a white, yellowish, grayish-white or brown crystalline solid or crystalline powder.
• Molecular weight is 84. 313 g/mol
• Density 3. 31 g/cm3
• Particularly insoluble in water, acetone and ethanol
• Soluble in acid

Occurrence

Magnesium carbonate, is an inorganic salt found as a white solid. Several hydrated and basic forms of magnesium carbonate also exist as minerals. The most common magnesium carbonate forms are the anhydrous salt called magnesite (MgCO3) and the di, tri, and pentahydrates known as barringtonite (MgCO3*2 H2O), nesquehonite (MgCO3*3 H2O), and lansfordite (MgCO3*5 H2O), respectively. Some basic forms such as artinite (MgCO3*Mg(OH)2*3 H2O), hydromagnesite (4 MgCO3*Mg(OH)2*4 H2O), and dypingite (4 MgCO3* Mg(OH)2*5 H2O).

Properties

it is free from any odor, whitish-crystal like material, can absorb water from surroundings, 3D structure, cannot dissolves in an aqueous medium, change into liquid form at 350 ‘C.

Preparation

Magnesium carbonate is ordinarily obtained by mining the mineral magnesite. Seventy percent of the world's supply is mined and prepared in China. Magnesium carbonate can be prepared in laboratory by reaction between any soluble magnesium salt and sodium bicarbonate: MgCl2(aq) + 2NaHCO3(aq) → MgCO3(s) + 2NaCl(aq) + H2O(l) + CO2(g)

High purity industrial routes include a path through magnesium bicarbonate, which can be formed by combining a slurry of magnesium hydroxide and carbon dioxide at high pressure and moderate temperature. The bicarbonate is then vacuum dried, causing it to lose carbon dioxide and a molecule of water, results in formation of high purity magnesium carbonate.

Mg(OH)2 + 2 CO2 → Mg(HCO3)2Mg(HCO3)2 → MgCO3 + CO2 + H2O

Application

Magnesium carbonate is used In flooring, Fire proofing, fire extinguishing compositions, Cosmetics, Dusting powder & toothpaste. Color retention in foodsIn pharmaceuticals it is used as an antacid in medicine.

Lithium Carbonate

It is a lithium salt of carbonate. It is an inorganic compound having formula i. e. Li2CO3. It is an important medication used in health system to treat bipolar disorder.

Occurrence

It is found as a natural mineral as well as extracted from the ores by using hot water.

Properties

no smell, change into liquid at 724 ‘C, very much similar to Na because of charge and size, can easily dissolve in acidic medium but not in water, in order to enhance it’s solubility in water we must use Hot-Water.

Preparation

It is widely extracted from minerals but can also be prepared by chemical synthesis. By the reaction of lithium chloride or lithium hydroxide with sodium carbonate yields the precipitates of lithium carbonate. It is extracted from pegmatite crystals and brine pools. By the reaction of lithium per oxide with carbon dioxide, it can also be prepared.

Application

It is used as an industrial chemical to make glass which is useful in ovenware, It is used in preparation of ceramic glaze and lithium ion battery cathodes. It can be used as a solvent for bladder stones,It treats mania, gout, urinary tract infections, headache and depression.

Silver Nitrateoccurance

Silver nitrate is an adaptable precursor to numerous other silver mixes. It was once called lunar acidic in light of the fact that silver was called luna by the old chemists, who trusted that silver was related with the moon. It was otherwise called the stone of damnation since it is exceptionally destructive.

Properties

The chemical formula of silver nitrate is AgNO3, and its molar mass is 169. 87 g/mol. It is a salt, and its synthetic structure comprises of the silver cation (Ag+) and the nitrate particle (NO3-). Silver nitrate is found as a white scentless strong with a thickness of 4. 35 g/mL, melt at 210 °C and boil at 440 °C. It is water solvent and non-hygroscopic. Dissimilar to numerous other silver salts, it isn't photosensitive. It is an oxidizing specialist and is very receptive as the nitrate particle can be effectively supplanted by different groups. Along these lines, it is a valuable beginning material for making a wide range of silver mixes including silver halides, silver oxide, and so forth, and in addition diverse metal nitrates, for example, copper nitrate. Silver nitrate is genuinely steady to light and warmth, yet breaks down when warmed to higher temperatures to give metallic silver alongside poisonous NO2 gas.

Preparation

To make silver nitrate, fill a glass compartment with concentrated nitric acid and wrap some aluminum wire around a bit of silver, leaving a tail to later expel the silver from the acid, if important. Next, put the aluminum-wrapped silver into the nitric acid, warm the acid until the silver begins to air bubbles and hold up until the point when the silver has totally disintegrated. Give the solution a chance to remain for a couple of days until the point that it totally vanishes, leaving loads of silver nitrate precious stones.

Applications

Silver nitrate is vitally used as a disinfectant, in the mechanical readiness of other silver salts. It is utilized either in stick frame as lunar harsh (or acidic pencil),The stick is utilized for expelling warts and granulation tissue and for closing up wounds and ulcerations. It is powerful against gonococcal microbes and might be connected to the eyes of babies to guarantee against visual impairment from gonorrhea. Unadulterated silver nitrate is utilized in the synthesis of silver salts, like colloidal silver mixes utilized in solution and silver halides utilized In photographic emulsions.