Aluminum oxide - Al2O3. Physical properties: aluminum oxide is a white amorphous powder or very hard white crystals. Molecular weight = 101.96, density - 3.97 g / cm3, melting point - 2053 ° C, boiling point - 3000 ° C.
Chemical properties: aluminum oxide exhibits amphoteric properties - the properties of acidic oxides and basic oxides, and reacts with both acids and bases. Crystalline Al2O3 is chemically passive, amorphous is more active. Interaction with acid solutions gives average aluminum salts, and with base solutions - complex salts - metal hydroxoaluminates:
When aluminum oxide is fused with solid metal alkalis, double salts are formed - metaaluminates(anhydrous aluminates):
Aluminum oxide does not interact with water and does not dissolve in it.
Receipt: aluminum oxide is obtained by the method of aluminum reduction of metals from their oxides: chromium, molybdenum, tungsten, vanadium, etc. - metallothermy, open Beketov:
Application: aluminum oxide is used for the production of aluminum, in the form of a powder - for refractory, chemically resistant and abrasive materials, in the form of crystals - for the manufacture of lasers and synthetic precious stones (rubies, sapphires, etc.), colored with impurities of other metal oxides - Cr2O3 ( red), Ti2O3 and Fe2O3 (blue).
Aluminum hydroxide - A1 (OH) 3. Physical properties: aluminum hydroxide - white amorphous (gel-like) or crystalline. Almost insoluble in water; molecular mass- 78.00, density - 3.97 g / cm3.
Chemical properties: a typical amphoteric hydroxide reacts:
1) with acids, forming medium salts: Al(OH)3 + 3НNO3 = Al(NO3)3 + 3Н2О;
2) with alkali solutions, forming complex salts - hydroxoaluminates: Al(OH)3 + KOH + 2H2O = K.
When Al(OH)3 is fused with dry alkalis, metaaluminates are formed: Al(OH)3 + KOH = KAlO2 + 2H2O.
Receipt:
1) from aluminum salts under the action of an alkali solution: AlCl3 + 3NaOH = Al(OH)3 + 3H2O;
2) decomposition of aluminum nitride with water: AlN + 3H2O = Al(OH)3 + NH3?;
3) passing CO2 through a solution of the hydroxo complex: [Al(OH)4]-+ CO2 = Al(OH)3 + HCO3-;
4) action on Al salts with ammonia hydrate; Al(OH)3 is formed at room temperature.
62. General characteristics of the chromium subgroup
Elements chromium subgroups occupy an intermediate position in the series of transition metals. They have high melting and boiling points, free places in electronic orbitals. Elements chromium And molybdenum have an atypical electronic structure - they have one electron in the outer s-orbital (as in Nb from the VB subgroup). These elements have 6 electrons in the outer d- and s-orbitals, so all orbitals are half-filled, that is, each has one electron. With such an electronic configuration, the element is particularly stable and resistant to oxidation. Tungsten has a stronger metallic bond than molybdenum. The oxidation state of the elements of the chromium subgroup varies greatly. Under proper conditions, all elements exhibit a positive oxidation state from 2 to 6, the maximum oxidation state corresponding to the group number. Not all oxidation states of the elements are stable, chromium has the most stable - +3.
All elements form the MVIO3 oxide; oxides with lower oxidation states are also known. All elements of this subgroup are amphoteric - they form complex compounds and acids.
Chrome, molybdenum And tungsten in demand in metallurgy and electrical engineering. All metals under consideration are covered with a passivating oxide film when stored in air or in an oxidizing acid medium. By removing the film by chemical or mechanical means, it is possible to increase the chemical activity of metals.
Chromium. The element is obtained from chromite ore Fe(CrO2)2 by reducing with coal: Fe(CrO2)2 + 4C = (Fe + 2Cr) + 4CO?.
Pure chromium is obtained by reducing Cr2O3 with aluminum or by electrolysis of a solution containing chromium ions. By recovering chromium by electrolysis, chromium plating can be obtained, which is used as decorative and protective films.
Chromium is used to produce ferrochromium, which is used in the production of steel.
Molybdenum. Obtained from sulfide ore. Its compounds are used in the production of steel. The metal itself is obtained by reducing its oxide. By calcining molybdenum oxide with iron, ferromolybdenum can be obtained. Used for the manufacture of threads and tubes for winding furnaces and electrical contacts. Steel with the addition of molybdenum is used in the automotive industry.
Tungsten. Received from the oxide extracted from the enriched ore. Aluminum or hydrogen is used as a reducing agent. The resulting tungsten in the powder idea is subsequently molded under high pressure and heat treatment (powder metallurgy). In this form, tungsten is used to make filaments, added to steel.
Aluminum- element of the 13th (III) group of the periodic table of chemical elements with atomic number 13. It is designated by the symbol Al. Belongs to the group of light metals. Most common metal and third most common chemical element V earth's crust(after oxygen and silicon).
Aluminium oxide Al2O3- in nature, it is common as alumina, a white refractory powder, close to diamond in hardness.
Aluminum oxide is a natural compound that can be obtained from bauxites or by thermal decomposition of aluminum hydroxides:
2Al(OH)3 = Al2O3 + 3H2O;
Al2O3 is an amphoteric oxide, chemically inert due to its strong crystal lattice. It does not dissolve in water, does not interact with solutions of acids and alkalis, and can only react with molten alkali.
At about 1000°C, it intensively interacts with alkalis and alkali metal carbonates to form aluminates:
Al2O3 + 2KOH = 2KAlO2 + H2O; Al2O3 + Na2CO3 = 2NaAlO2 + CO2.
Other forms of Al2O3 are more active, they can react with solutions of acids and alkalis, α-Al2O3 interacts only with hot concentrated solutions: Al2O3 + 6HCl = 2AlCl3 + 3H2O;
The amphoteric properties of aluminum oxide are manifested when interacting with acidic and basic oxides with the formation of salts:
Al2O3 + 3SO3 = Al2(SO4)3 (basic properties), Al2O3 + Na2O = 2NaAlO2 (acidic properties).
Aluminum hydroxide, Al(OH)3- connection of aluminum oxide with water. White gelatinous substance, poorly soluble in water, has amphoteric properties. Obtained by the interaction of aluminum salts with aqueous solutions of alkali: AlCl3 + 3NaOH \u003d Al (OH) 3 + 3NaCl
Aluminum hydroxide is a typical amphoteric compound, freshly obtained hydroxide dissolves in acids and alkalis:
2Al(OH)3 + 6HCl = 2AlCl3 + 6H2O. Al(OH)3 + NaOH + 2H2O = Na.
When heated, it decomposes, the dehydration process is rather complicated and can be schematically represented as follows:
Al(OH)3 = AlOOH + H2O. 2AlOOH = Al2O3 + H2O.
Aluminates - salts formed by the action of alkali on freshly precipitated aluminum hydroxide: Al (OH) 3 + NaOH \u003d Na (sodium tetrahydroxoaluminate)
Aluminates are also obtained by dissolving metallic aluminum (or Al2O3) in alkalis: 2Al + 2NaOH + 6H2O = 2Na + ZH2
Hydroxoaluminates are formed by the interaction of Al (OH) 3 with an excess of alkali: Al (OH) 3 + NaOH (wt) = Na
aluminum salts. Almost all aluminum salts can be obtained from aluminum hydroxide. Almost all aluminum salts are highly soluble in water; aluminum phosphate is poorly soluble in water.
In an aluminum salt solution, an acid reaction is shown. An example is the reversible effect of aluminum chloride with water:
AlCl3 + 3H2O "Al (OH) 3 + 3HCl
Many aluminum salts are of practical importance. For example, anhydrous aluminum chloride AlCl3 is used in chemical practice as a catalyst in oil refining
Aluminum sulfate Al2(SO4)3 18H2O is used as a coagulant in the purification of tap water, as well as in the production of paper.
Double aluminum salts are widely used - alum KAl (SO4) 2 12H2O, NaAl (SO4) 2 12H2O, NH4Al (SO4) 2 12H2O, etc. - have strong astringent properties and are used in skin tanning, as well as in medical practice as a hemostatic agent.
Application- Due to a set of properties, it is widely used in thermal equipment. - Aluminum and its alloys retain strength at ultra-low temperatures. Due to this, it is widely used in cryogenic technology. - aluminum is an ideal material for the manufacture of mirrors. - In production building materials as a gas-forming agent. - Aluminizing imparts corrosion and scale resistance to steel and other alloys; - Aluminum sulfide is used for the production of hydrogen sulfide.
As a restorer- As a component of thermite, mixtures for aluminothermy - In pyrotechnics. - Aluminum is used to restore rare metals from their oxides or halides. (Aluminothermy)
Aluminothermy.- a method for obtaining metals, non-metals (as well as alloys) by reducing their oxides with metallic aluminum.
aluminum hydroxide(English) aluminum hydroxide), aluminum hydroxide, Al(OH) 3- in medicine, an antacid.
Aluminum hydroxide - international non-proprietary name of the drug
Aluminum hydroxide is the international non-proprietary name (INN) of the drug. According to the ATC, aluminum hydroxide belongs to the section "A02A Antacids", the group "A02AB Aluminum preparations" and has the code A02AB01. Aluminum hydroskid - antacid
Currently, aluminum hydroxide as a one-component drug in the treatment of acid-dependent diseases is practically not used. It is most often used in combination with magnesium compounds. Like other aluminum compounds, it has a fixing effect.
Aluminum hydroxide, as an antacid, is the so-called "non-absorbable antacid" (see the figure on the right; Ivashkin V.T. and others). The effect of non-absorbable antacids develops more slowly than that of absorbable ones, but lasts longer, up to 2.5-3 hours. But the main advantage of non-absorbable antacids is the absence of the “acid rebound” phenomenon, which consists in an increase in acid production after the end of the drug (Bordin D.S.).
Aluminum hydroxide causes a slow decrease in stomach acidity, therefore, with an accelerated passage through the stomach, the antacid effect does not have time to fully develop.
The electronic configuration of the external level of aluminum … 3s 2 3p 1 .
In the excited state, one of the s-electrons passes to a free cell of the p-sublevel, this state corresponds to valence III and the oxidation state +3.
There are free d-sublevels in the outer electron layer of the aluminum atom. Due to this, its coordination number in compounds can be not only 4 ([A1 (OH) 4] -), but also 6 - ([A1 (OH) 6] 3-).
Being in nature
The most common metal in the earth's crust, the total aluminum content in the earth's crust is 8.8%.
It does not occur in free form in nature.
The most important natural compounds are aluminosilicates:
white clay Al 2 O 3 ∙ 2SiO 2 ∙ 2H 2 O, feldspar K 2 O ∙ Al 2 O 3 ∙ 6SiO 2, mica K 2 O ∙ Al 2 O 3 ∙ 6SiO 2 ∙ H 2 O
From others natural forms finding aluminum highest value have bauxites A1 2 Oz ∙ nH 2 O, minerals corundum A1 2 Oz and cryolite A1Fz ∙3NaF.
Receipt
At present, aluminum is produced in industry by electrolysis of aluminum oxide Al 2 O 3 in a cryolite melt.
The process of electrolysis is ultimately reduced to the decomposition of Al 2 Oz by electric current
2A1 2 Oz \u003d 4A1 + 3O 2 (950 0 C, A1Fz ∙3NaF, electric current)
Liquid aluminum is released at the cathode:
A1 3+ + 3e-=Al0
Oxygen is released at the anode.
Physical properties
Lightweight, silvery white, ductile metal, conducts well electricity and warm.
In air, aluminum is covered with the thinnest (0.00001 mm), but very dense oxide film, which protects the metal from further oxidation and gives it a matte appearance.
Aluminum is easily drawn into wire and rolled into thin sheets. Aluminum foil (thickness 0.005 mm) is used in the food and pharmaceutical industry for packaging products and preparations.
Chemical properties
aluminum is highly active metal, slightly inferior in activity to the elements of the beginning of the period - sodium and magnesium.
1. aluminum easily combines with oxygen at room temperature, while an oxide film is formed on the aluminum surface (A1 2 O 3 layer). This film is very thin (≈ 10 -5 mm), but strong. It protects aluminum from further oxidation and is therefore called a protective film.
4Al + 3O 2 \u003d 2Al 2 O 3
2. when interacting with halogens, halides are formed:
with chlorine and bromine, the interaction occurs already at ordinary temperature, with iodine and sulfur - when heated.
2Al + 3Cl 2 = 2AlCl 3
2Al + 3S \u003d Al 2 S 3
3. At very high temperatures, aluminum also combines directly with nitrogen and carbon.
2Al + N 2 = 2AlN aluminum nitride
4Al + 3C \u003d Al 4 C 3 aluminum carbide
Aluminum does not react with hydrogen.
4. aluminum is quite resistant to water. But if the protective effect of the oxide film is removed mechanically or by amalgamation, then an energetic reaction occurs:
2Al + 6H 2 O \u003d 2Al (OH) 3 + 3H 2
5. interaction of aluminum with acids
From razb. acids (HCl, H 2 SO 4) aluminum interacts with the formation of hydrogen.
2Al + 6HCl = 2AlCl 3 + 3H 2
In the cold, aluminum does not interact with concentrated sulfuric and nitric acid.
Interacts with conc. sulfuric acid when heated
8Al + 15H 2 SO 4 = 4Al 2 (SO 4) 3 + 3H 2 S + 12H 2 O
Aluminum reacts with dilute nitric acid to form NO
Al + 4HNO 3 \u003d Al (NO 3) 3 + NO + 2H 2 O
6. interaction of aluminum with alkalis
Aluminum, like other metals that form amphoteric oxides and hydroxides, interacts with alkali solutions.
Aluminum under normal conditions, as already noted, is covered with a protective film of Al 2 O 3 . Under the action of alkali aqueous solutions on aluminum, the layer of aluminum oxide A1 2 O 3 dissolves, and aluminates are formed - salts containing aluminum in the composition of the anion:
A1 2 O 3 + 2NaOH + 3H 2 O \u003d 2Na
Aluminum, devoid of a protective film, interacts with water, displacing hydrogen from it.
2Al + 6H 2 O \u003d 2Al (OH) 3 + 3H 2
The resulting aluminum hydroxide reacts with an excess of alkali, forming tetrahydroxoaluminate
Al (OH) 3 + NaOH \u003d Na
The overall equation for the dissolution of aluminum in aqueous solution alkalis:
2Al + 2NaOH + 6H 2 O \u003d 2Na + 3H 2
Aluminum oxide A1 2 O 3
White solid, insoluble in water, melting point 2050 0 С.
Natural A1 2 O 3 - the mineral corundum. Transparent colored corundum crystals - red ruby - contains an admixture of chromium - and blue sapphire - an admixture of titanium and iron - gems. They are also obtained artificially and used for technical purposes, for example, for the manufacture of parts for precision instruments, stones in watches, etc.
Chemical properties
Aluminum oxide exhibits amphoteric properties
1. interaction with acids
A1 2 O 3 + 6HCl \u003d 2AlCl 3 + 3H 2 O
2. interaction with alkalis
A1 2 O 3 + 2NaOH - 2NaAlO 2 + H 2 O
Al 2 O 3 + 2NaOH + 5H 2 O \u003d 2Na
3. When a mixture of oxide of the corresponding metal with aluminum powder is heated, a violent reaction occurs, leading to the release of free metal from the taken oxide. The reduction method with Al (aluminum) is often used to obtain a number of elements (Cr, Mn, V, W, etc.) in a free state
2A1 + WO 3 \u003d A1 2 Oz + W
4. interaction with salts having a strongly alkaline environment due to hydrolysis
Al 2 O 3 + Na 2 CO 3 \u003d 2 NaAlO 2 + CO 2
Aluminum hydroxide A1(OH) 3
A1(OH) 3 is a voluminous white gelatinous precipitate, practically insoluble in water, but easily soluble in acids and strong alkalis. It therefore has an amphoteric character.
Aluminum hydroxide is obtained by the exchange reaction of soluble aluminum salts with alkalis.
AlCl 3 + 3NaOH = Al(OH) 3 ↓ + 3NaCl
Al 3+ + 3OH - \u003d Al (OH) 3 ↓
This reaction can be used as a qualitative reaction for the Al 3+ ion
Chemical properties
1. interaction with acids
Al(OH) 3 + 3HCl = 2AlCl 3 + 3H 2 O
2. when interacting with strong alkalis, the corresponding aluminates are formed:
NaOH + A1(OH)3 = Na
3. thermal decomposition
2Al(OH) 3 \u003d Al 2 O 3 + 3H 2 O
aluminum salts undergo hydrolysis by the cation, the medium is acidic (pH< 7)
Al 3+ + H + OH - ↔ AlOH 2+ + H +
Al(NO 3) 3 + H 2 O↔ AlOH(NO 3) 2 + HNO 3
Soluble salts aluminum and weak acids undergo complete (irreversible hydrolysis)
Al 2 S 3 + 3H 2 O \u003d 2Al (OH) 3 + 3H 2 S
Application in medicine and national economy aluminum and its compounds.
The lightness of aluminum and its alloys and high resistance to air and water determine their use in mechanical engineering and aircraft construction. As a pure metal, aluminum is used to make electrical wires.
Aluminum foil (thickness 0.005 mm) is used in the food and pharmaceutical industry for packaging products and preparations.
Aluminum oxide Al 2 O 3 - is part of some antacids (for example, Almagel), used for increased acidity of gastric juice.
KAl (SO 4) 3 12H 2 O - potassium alum is used in medicine for the treatment of skin diseases, as a hemostatic agent. It is also used as a tannin in the leather industry.
(CH 3 COO) 3 Al - Burov's liquid - 8% solution of aluminum acetate has an astringent and anti-inflammatory effect, in high concentrations it has moderate antiseptic properties. It is used in diluted form for rinsing, lotions, for inflammatory diseases of the skin and mucous membranes.
AlCl 3 - used as a catalyst in organic synthesis.
Al 2 (SO 4) 3 18 H 2 0 - used in water purification.
Control questions to fix:
1. What is the highest valency of the oxidation state of the elements of III A group. Explain in terms of the structure of the atom.
2. Name the most important boron compounds. What is a qualitative reaction to a borate ion?
3. What Chemical properties have aluminum oxide and hydroxide?
Mandatory
Pustovalova L.M., Nikanorova I.E. . Inorganic chemistry. Rostov-on-Don. Phoenix. 2005. -352p. ch. 2.1 p. 283-294
Additional
1. Akhmetov N.S. General and inorganic chemistry. M.: Higher school, 2009.- 368s.
2. Glinka N.L. general chemistry. KnoRus, 2009.-436 p.
3. Erokhin Yu.M. Chemistry. Textbook for students. Middle professional education - M .: Academy, 2006.- 384s.
Electronic resources
1. Open chemistry: a complete interactive chemistry course for students of schools, lyceums, gymnasiums, colleges, students. technical universities: version 2.5-M.: Physicon, 2006. Electronic optical disk CD-ROM
2. .1C: Tutor - Chemistry, for applicants, high school students and teachers, 1C CJSC, 1998-2005. Electronic optical disc CD-ROM
3. Chemistry. Fundamentals of theoretical chemistry. [Electronic resource]. URL: http://chemistry.narod.ru/himiya/default.html
4. Digital library teaching materials in chemistry [Electronic resource]. URL: http://www.chem.msu.su/rus/elibrary/
Thank you
aluminum hydroxide also called aluminum hydroxide, has antacid properties (reduces the acidity of gastric juice), and therefore is used in medical practice for the symptomatic treatment of diseases of the stomach or duodenum. This substance has been used in medicine for quite a long period of time, but at present it is being replaced by more modern drugs of the antacid group. However, in many cases, aluminum hydroxide is still the optimal drug in many respects, so it is necessary to know its properties and therapeutic effects well.
Aluminum hydroxide - a brief description of the substance, its properties and methods of application
Aluminum hydroxide is a chemical compound that is included in the list of medical products of the group antacids. All antacids reduce the acidity of gastric juice, thereby eliminating heartburn, a feeling of heaviness, discomfort and pain in the abdomen after eating, and are also used for the complex treatment of gastric and duodenal ulcers, gastroesophageal reflux, etc. Aluminum hydroxide, being an antacid , also reduces the acidity of gastric juice and, accordingly, can be used to treat the above conditions and diseases. In countries former USSR aluminum hydroxide is often referred to as a substance called algeldrate (aluminum oxide monohydrate) , which is not entirely correct, since the chemical structure of these compounds is different. So, aluminum hydroxide is, in fact, an alkali, and algeldrate is an oxide containing an additional water molecule. Therefore, from the standpoint of academic science, and from a practical point of view, these substances should not be combined into one, because they have different chemical and physical properties. Moreover, in the anatomical-therapeutic-chemical classification of medicinal substances, algeldrate and aluminum hydroxide are also separated and have different codes, as a result of which they should not be combined. We will also not combine algeldrate and aluminum hydroxide into one substance, and consider the properties of only the first compound, so as not to create confusion.
Currently, aluminum hydroxide is practically not used as an independent antacid in medical practice, because, firstly, it has a number of very unpleasant side effects, and secondly, because modern, more effective drugs with better tolerance have appeared. As a rule, aluminum hydroxide is used in medical practice in combination with magnesium hydroxide, since the latter improves the tolerance of the aluminum compound. In the CIS countries, there are only a few preparations containing aluminum hydroxide as active substance- these are Rokzhel (Rokgel) and Aluminum hydroxide-Rivopharm. In the US and Europe, there is a wider range of preparations containing aluminum hydroxide and used in medical practice to this day.
However, many may argue that aluminum hydroxide is included in many modern antacid preparations as one of the active ingredients along with other substances, such as magnesium hydroxide. This opinion is not entirely correct, since modern preparations do not contain aluminum hydroxide, but algeldrate, which is simply often considered the same substance as aluminum hydroxide. But, as we have already said, algeldrate and aluminum hydroxide are different chemical compounds that should not be combined into one.
Aluminum hydroxide, despite its shortcomings, is included in the list of medicinal substances and, although not often, is used in practical medicine. Therefore, we will consider its properties and application rules.
So, aluminum hydroxide is a loose powder, practically insoluble in water, but capable of forming a gel-like structure. It is precisely due to the ability to form a gel-like structure that aluminum hydroxide powder for medical use shaken with water, receiving a suspension for oral administration. The substance has antacid, adsorbent and enveloping properties.
Aluminum hydroxide is usually used orally to treat diseases of the digestive tract associated with increased acidity of gastric juice, such as peptic ulcer of the stomach or duodenum, gastritis, esophagitis, colitis, etc.
Somewhat less often, aluminum hydroxide is used to eliminate hyperphosphatemia ( elevated level phosphates in the blood) against the background of renal failure. The fact is that aluminum hydroxide binds excess phosphates in the intestines, which, in case of kidney failure, are not excreted from the body in a normal volume, thereby, as it were, helping the kidneys to remove these salts.
In addition, in rare cases, aluminum hydroxide is used externally as an astringent for skin diseases.
Inside aluminum hydroxide, as a rule, is taken in the form of a suspension, which is a powder thoroughly loosened in water. In rare cases, if it is impossible to prepare a suspension, aluminum hydroxide is taken orally directly in powder form.
Externally, aluminum hydroxide is used only in powder, sprinkling it on the affected areas of the skin.
Medicines containing aluminum hydroxide
In the CIS countries, there are only two medicinal products containing aluminum hydroxide as an active substance - these are Rokzhel (Rokgel) and Aluminum hydroxide-Rivofarm. In Europe and the USA, there is a much wider range of drugs with aluminum hydroxide as the only active substance, such as Alternagel, Amphojel, Aloh-Gel, etc. There are significantly more drugs that contain algeldrate as one of the active components on the market of the CIS countries, since they are more effective, safe and modern. To facilitate orientation, here is a list of antacid preparations present on the pharmaceutical market of the CIS countries containing algeldrate as an active substance:
- Ajiflux (algeldrate + magnesium hydroxide) tablets;
- Almagel, Almagel A and Almagel Neo (algeldrate + magnesium hydroxide) - suspension;
- Altacid (algeldrate + magnesium hydroxide) - suspension and chewable tablets;
- Alumag (algeldrate + magnesium hydroxide) tablets;
- Gastracid (algeldrate + magnesium hydroxide) tablets;
- Maalox and Maalox mini (algeldrate + magnesium hydroxide) tablets and suspension;
- Palmagel (algeldrate + magnesium hydroxide) oral gel;
- Simalgel VM (algeldrate + magnesium hydroxide + simethicone) oral suspension.
Therapeutic action
Aluminum hydroxide has three main pharmacological properties:- Antacid action;
- adsorbent action;
- Enveloping action.
In the intestines, aluminum is not absorbed, but forms insoluble salts - phosphates, which provoke constipation. Therefore, when using only aluminum hydroxide as an antacid, laxatives should be taken. Constipation can be eliminated by the complex intake of aluminum hydroxide in combination with magnesium hydroxide, which, as a rule, is successfully done.
adsorbent property aluminum hydroxide lies in its ability to bind hydrochloric acid molecules and, thereby, neutralize them, enhancing the antacid effect based on a chemical reaction.
enveloping property aluminum hydroxide lies in its ability to be evenly distributed over the gastric mucosa, forming a thin protective film on it, protecting it from the damaging effects of both hydrochloric acid and certain types of food.
Thus, aluminum hydroxide is used as a symptomatic remedy to eliminate various unpleasant sensations caused by increased acidity of gastric juice. Since the acidity of gastric juice can be increased not only in severe serious diseases, but also against the background of functional disorders, aluminum hydroxide cannot be considered a drug only for the treatment of pathology, since it can also be used exclusively as a symptomatic remedy to eliminate discomfort.
Separately, it should be said about one more property of aluminum hydroxide, which is also used in medical practice. So, this substance, getting from the stomach to the intestines, binds phosphates, forming insoluble salts with them and removing them from the body along with feces. The ability of aluminum hydroxide to remove phosphates from the body is used in the complex therapy of renal failure, in which, on the contrary, these salts accumulate and cause various disorders. After all, phosphates are normally excreted mainly by the kidneys, and in case of renal failure, respectively, these salts are not removed from the body in the required volume and accumulate. The use of aluminum hydroxide allows you to remove excess phosphate from the body and, thereby, improve the well-being of a person suffering from kidney failure.
Indications for use
Aluminum hydroxide is indicated for use as part of the complex therapy of the following diseases, as well as to eliminate dyspeptic symptoms: - Esophagitis;
- Reflux esophagitis;
- Acute gastritis;
- Chronic gastritis with high acidity of gastric juice;
- Acute duodenitis;
- Peptic ulcer of the stomach or duodenum during an exacerbation;
- Symptomatic ulcers or erosions on the mucous membranes of the digestive tract;
- Hernia of the esophageal opening of the diaphragm;
- Acute pancreatitis;
- Hyperphosphatemia (increased levels of phosphate in the blood);
- Functional disorders of the intestines (for example, irritable bowel syndrome, etc.);
- Colitis;
- Symptoms of dyspepsia in diseases of the stomach or intestines (for example, a feeling of discomfort, heaviness and pain in the stomach, heartburn, belching sour, etc.);
- Symptoms of dyspepsia (for example, a feeling of discomfort, heaviness and pain in the stomach, heartburn, sour belching, etc.) that occur after diet errors, drinking alcohol, smoking, coffee, etc.
Instructions for use of aluminum hydroxide
Rules for the use of aluminum hydroxide suspension
Aluminum hydroxide is usually sold as an oral suspension in sealed bottles. However, this substance in some cases (usually on request) can also be purchased in powder form. Accordingly, the rules for applying suspension and aluminum hydroxide powder are different. Considering that in the CIS countries it is possible to purchase both forms of aluminum hydroxide, we will consider the rules and methods for using both powder and suspension. So, aluminum hydroxide suspension is intended for oral administration. In diseases of the esophagus, stomach and duodenum as part of complex therapy for adults and children, it is recommended to take 1-2 teaspoons of the suspension 4-6 times a day, 1-2 hours after meals and at night. This means that the drug should be drunk 1-2 hours after each meal and additionally at night, before going to bed. In diseases of the intestines and stomach ulcers, it is recommended to take a suspension of aluminum hydroxide not after, but 30 minutes before meals.
In addition, if necessary, a suspension of aluminum hydroxide can be drunk between meals to eliminate emerging heartburn or other symptoms of dyspepsia. The duration of the suspension in diseases of the digestive tract varies and ranges from 4 weeks to 3 months. In each specific case, the question of the duration of application of the suspension of aluminum hydroxide is decided individually, depending on the rate of normalization of health.
If a person does not have diseases of the digestive tract in the acute stage, but periodically symptoms of dyspepsia appear, such as heartburn, heaviness, discomfort and pain in the abdomen, etc., then he can take a suspension of aluminum hydroxide occasionally. This means that the suspension should be taken in 1 - 2 teaspoons only when the person has unpleasant symptoms of dyspepsia.
With hyperphosphatemia that occurs against the background of renal failure, the dosage of aluminum hydroxide suspension is selected individually, focusing on the level of phosphorus in the blood.
If a person is to undergo any procedure that can irritate the mucous membranes of the stomach, esophagus or duodenum (for example, taking strong alcoholic drinks, spicy foods, etc.), then aluminum hydroxide suspension can be taken for prophylaxis 1-2 teaspoons 15 - 30 minutes before manipulation.
It should be remembered that the maximum allowable daily dosage of aluminum hydroxide is 12 teaspoons or 6 tablespoons. This maximum allowable daily amount of the suspension should not be exceeded, as this can lead to a violation of the water and electrolyte balance and persistent constipation.
It is also necessary to shake the vial with the suspension well each time before measuring the required amount of the drug in order to mix the precipitate that has formed.
Rules for the application of aluminum hydroxide powder
Aluminum hydroxide powder as an antacid can be taken orally in pure form or prepared from it in suspension. To prepare a suspension of 4 g of powder, pour 96 ml of distilled water and mix well until a homogeneous cloudy liquid is formed. A self-prepared suspension is taken in the same way as a pharmacy one, that is, 1-2 teaspoons of the suspension 4-6 times a day 1-2 hours after meals for diseases of the esophagus and stomach, and 30 minutes before meals for intestinal pathology. Aluminum hydroxide in powder form is recommended to be taken only occasionally to relieve symptoms of dyspepsia (heartburn, pain, heaviness and discomfort in the abdomen). If these symptoms of dyspepsia occur, it is recommended to take one tablespoon of the powder with a glass of water.
For long-term therapy of diseases of the digestive tract, aluminum hydroxide should be used in the form of a suspension, not a powder. Occasional intake of the powder is allowed if, for some reason, it was not possible to purchase the suspension. In such cases, take a tablespoon of powder instead of suspension.
For the treatment of skin diseases, aluminum hydroxide powder is used in its pure form. Powder sprinkle the affected areas with a thin layer several times a day. In addition, aluminum hydroxide powder can be used as a powder to reduce perspiration. As an antiperspirant, aluminum hydroxide is common in English-speaking countries.
special instructions
If within 10 days of taking aluminum hydroxide the symptoms of dyspepsia do not decrease or their severity increases, then you should immediately stop using the drug and consult a doctor.The intake of aluminum hydroxide and other drugs should be separated in time by 2 hours, since the antacid worsens the absorption of drugs. That is, any other medications should be taken two hours before or after taking aluminum hydroxide. In the case of fluoroquinolones (for example, Tavanic, Lomefloxacin, Levofloxacin, Ciprofloxacin, etc.), intake with aluminum hydroxide should be separated by 4 hours.
In the presence of violations of the liver should not take aluminum hydroxide for more than 8 weeks.
Since aluminum hydroxide removes phosphates from the body, with prolonged use, the drug can provoke hypophosphatemia ( low level phosphate in the blood). Therefore, with long-term intake of aluminum hydroxide, it is necessary to include foods rich in phosphates in the diet, such as meat, fish, seafood, canned milk, cheeses, carbonated drinks, etc.
Overdose
An overdose of aluminum hydroxide is possible despite the fact that the substance is not absorbed into the systemic circulation and does not have any pharmacological effects on various organs and systems. Overdose due to accumulation in the intestinal lumen a large number aluminum compounds, which cause various disorders in the functioning of this organ. An overdose of aluminum hydroxide is manifested by the following symptoms:- Persistent constipation;
- Abdominal pain;
- Narrowing of the intestinal lumen up to the formation of obstruction;
- Hypophosphatemia (deficiency of phosphorus in the blood);
Influence on the ability to control mechanisms
Aluminum hydroxide does not affect the operation of the central nervous system, therefore, against the background of its use, a person can engage in any type of activity that requires an increased speed of reactions and concentration of attention.Interaction with other drugs
Aluminum hydroxide leads to an increase in the concentration of Quinidine in the blood, therefore, with their simultaneous use, the dosage of the latter should be reduced.Aluminum hydroxide impairs the absorption and, accordingly, the severity of the therapeutic effect of the following drugs:
- Acetylsalicylic acid (Aspirin, etc.);
- Bisphosphonates;
- Histamine blockers (
