Molar mass of table salt. Table salt formula
Table salt is sodium chloride used as a food additive and food preservative. Also used in chemical industry, medicine. Serves the most important raw material for producing caustic soda, soda and other substances. The formula for table salt is NaCl.
Formation of an ionic bond between sodium and chlorine
The chemical composition of sodium chloride is reflected by the conventional formula NaCl, which gives an idea of the equal number of sodium and chlorine atoms. But the substance is not formed by diatomic molecules, but consists of crystals. When an alkali metal reacts with a strong nonmetal, each sodium atom gives up the more electronegative chlorine. Sodium cations Na + and anions of the acidic residue of hydrochloric acid Cl - appear. Oppositely charged particles attract each other, forming a substance with an ionic crystal lattice. Small sodium cations are located between large chlorine anions. The number of positive particles in the composition of sodium chloride is equal to the number of negative ones; the substance as a whole is neutral.
Chemical formula. Table salt and halite
Salts are complex substances of ionic structure, the names of which begin with the name of the acidic residue. The formula for table salt is NaCl. Geologists call a mineral of this composition “halite,” and a sedimentary rock “rock salt.” Outdated chemical term, which is often used in production, is “sodium chloride”. This substance has been known to people since ancient times; it was once considered “white gold”. Modern schoolchildren and students, when reading reaction equations involving sodium chloride, use chemical symbols (“sodium chlorine”).
Let's carry out simple calculations using the formula of the substance:
1) Mr (NaCl) = Ar (Na) + Ar (Cl) = 22.99 + 35.45 = 58.44.
The relative value is 58.44 (in amu).
2) Molar mass is numerically equal to molecular weight, but this quantity has units of measurement g/mol: M (NaCl) = 58.44 g/mol.
3) A 100 g sample of salt contains 60.663 g of chlorine atoms and 39.337 g of sodium.
Physical properties of table salt
Fragile halite crystals are colorless or white. In nature, there are also deposits of rock salt, colored grey, yellow or blue. Sometimes mineral substance has a red tint, which is due to the types and amount of impurities. The hardness of halite is only 2-2.5, glass leaves a line on its surface.
Other physical parameters of sodium chloride:
- smell - absent;
- taste - salty;
- density - 2.165 g/cm3 (20 °C);
- melting point - 801 °C;
- boiling point - 1413 °C;
- solubility in water - 359 g/l (25 °C);
Preparation of sodium chloride in the laboratory
When sodium metal reacts with chlorine gas in a test tube, a substance is formed white- sodium chloride NaCl (table salt formula).
Chemistry provides insight into in various ways obtaining the same connection. Here are some examples:
NaOH (aq) + HCl = NaCl + H 2 O.
Redox reaction between a metal and an acid:
2Na + 2HCl = 2NaCl + H2.
Effect of acid on metal oxide: Na 2 O + 2HCl (aq) = 2NaCl + H 2 O
crowding out weak acid from a solution of its stronger salt:
Na 2 CO 3 + 2HCl (aq) = 2NaCl + H 2 O + CO 2 (gas).
All these methods are too expensive and complex for use on an industrial scale.
Production of table salt
Even at the dawn of civilization, people knew that salting meat and fish lasts longer. Transparent, correct form Halite crystals were used in some ancient countries instead of money and were worth their weight in gold. The search and development of halite deposits made it possible to satisfy the growing needs of the population and industry. The most important natural springs table salt:
- deposits of the mineral halite in different countries;
- water of seas, oceans and salt lakes;
- layers and crusts of rock salt on the banks of salty reservoirs;
- halite crystals on the walls of volcanic craters;
- salt marshes.
The industry uses four main methods for producing table salt:
- leaching of halite from the underground layer, evaporation of the resulting brine;
- mining in ;
- evaporation or brine of salt lakes (77% of the mass of the dry residue is sodium chloride);
- usage by-product desalination of salt waters.
Chemical properties of sodium chloride
In terms of its composition, NaCl is an average salt formed by an alkali and a soluble acid. Sodium chloride is a strong electrolyte. The attraction between ions is so strong that only highly polar solvents can break it. In water, the substance disintegrates, cations and anions (Na +, Cl -) are released. Their presence is due to the electrical conductivity possessed by a solution of table salt. The formula in this case is written in the same way as for dry matter - NaCl. One of the qualitative reactions to the sodium cation is coloration yellow burner flame. To obtain the result of the experiment, you need to collect a little solid salt on a clean wire loop and add it to middle part flame. The properties of table salt are also associated with the peculiarity of the anion, which consists in a qualitative reaction to the chloride ion. When interacting with silver nitrate, a white precipitate of silver chloride precipitates in the solution (photo). Hydrogen chloride is displaced from the salt by stronger acids than hydrochloric acid: 2NaCl + H 2 SO 4 = Na 2 SO 4 + 2HCl. At normal conditions sodium chloride does not undergo hydrolysis.
Areas of application of rock salt
Sodium chloride lowers the melting point of ice, so in winter a mixture of salt and sand is used on roads and sidewalks. She absorbs a large number of impurities, when melting, pollutes rivers and streams. Road salt also accelerates the corrosion process of car bodies and damages trees planted next to roads. In the chemical industry, sodium chloride is used as a raw material to produce large group chemical substances:
- of hydrochloric acid;
- sodium metal;
- chlorine gas;
- caustic soda and other compounds.
In addition, table salt is used in the production of soap and dyes. It is used as a food antiseptic for canning and pickling mushrooms, fish and vegetables. To combat disruptions thyroid gland among the population, the table salt formula is enriched by the addition of safe iodine compounds, for example, KIO 3, KI, NaI. Such supplements support the production of thyroid hormone and prevent endemic goiter.
The importance of sodium chloride for the human body
The formula for table salt, its composition has become vitally important for human health. Sodium ions are involved in the transmission nerve impulses. Chlorine anions are necessary for the production of hydrochloric acid in the stomach. But too much great content table salt in food can lead to high blood pressure and increasing the risk of developing heart and vascular diseases. In medicine with large blood loss patients are given physiological saline solution. To obtain it, 9 g of sodium chloride are dissolved in one liter of distilled water. Human body requires a continuous supply of this substance with food. Salt is excreted through the excretory organs and skin. The average sodium chloride content in the human body is approximately 200 g. Europeans consume about 2-6 g of table salt per day; in hot countries this figure is higher due to higher sweating.
The active ingredient of this product is sodium chloride . The formula for sodium chloride is NaCl, these are white crystals that quickly dissolve in water. Molar mass 58.44 g/mol. OKPD code - 14.40.1.
Saline solution (isotonic) is a 0.9% solution, it contains 9 g of sodium chloride, up to 1 liter of distilled water.
Hypertonic sodium chloride solution is a 10% solution, it contains 100 g of sodium chloride, up to 1 liter of distilled water.
Release form
A 0.9% sodium chloride solution is produced, which can be contained in ampoules of 5 ml, 10 ml, 20 ml. Ampoules are used to dissolve medications for injection.
A solution of sodium chloride 0.9% is also produced in bottles of 100, 200, 400 and 1000 ml. Their use in medicine is practiced for external use, intravenous drips, and enemas.
Sodium chloride solution 10% is contained in bottles of 200 and 400 ml.
With the aim of oral administration tablets of 0.9 g are available.
A nasal spray is also produced in 10 ml bottles.
pharmachologic effect
Sodium chloride is a drug that acts as a rehydrating and detoxifying agent. The medicine is able to compensate for the lack of sodium in the body, subject to the development of various pathologies. Sodium chloride also increases the amount of fluid that circulates in the vessels.
Such properties of the solution are manifested due to the presence in it chloride ions And sodium ions . They are able to penetrate the cell membrane using various transport mechanisms, in particular the sodium-potassium pump. Important role sodium plays a role in signal transmission in neurons, and is also involved in the metabolic process in the kidneys and in the electrophysiological processes of the human heart.
Pharmacopoeia indicates that sodium chloride maintains in extracellular fluid and blood plasma constant pressure. At in good condition body sufficient quantity This compound enters the body with food. But when pathological conditions, in particular, when vomiting , diarrhea , serious burns noted increased secretion from the body of these elements. As a result, the body experiences a deficiency of chlorine and sodium ions, as a result of which the blood becomes thicker and functions are impaired. nervous system, blood flow, convulsions, spasms smooth muscle muscles.
If an isotonic sodium chloride solution is introduced into the blood in a timely manner, its use promotes recovery water-salt balance . But since osmotic pressure solution similar to blood plasma pressure, in vascular bed he doesn't stay long. After administration, it is quickly eliminated from the body. As a result, after 1 hour, no more than half of the injected amount of solution is retained in the vessels. Therefore, in case of blood loss, the solution is not effective enough.
The product also has plasma-substituting and detoxifying properties.
When a hypertonic solution is administered intravenously, an increase in , replenishing the deficiency of chlorine and sodium in the body.
Pharmacokinetics and pharmacodynamics
Excretion from the body occurs mainly through the kidneys. Some sodium is excreted in sweat and feces.
Indications for use
Sodium chloride is a saline solution that is used when the body loses extracellular fluid. Indicated for conditions that lead to limited fluid intake:
- dyspepsia in case of poisoning;
- vomit , ;
- extensive burns;
- hyponatremia or hypochloremia , in which dehydration of the body is noted.
Considering what sodium chloride is, it is used externally to wash wounds, eyes, and nose. The drug is used to moisturize dressings, for inhalation, and for the face.
The use of NaCl is indicated for forced diuresis in case of poisoning, internal bleeding (pulmonary, intestinal, gastric).
It is also indicated in the indications for use of sodium chloride that this is a drug that is used for diluting and dissolving drugs that are administered parenterally.
Contraindications
The use of the solution is contraindicated for the following diseases and conditions:
- hypokalemia , hyperchloremia , hypernatremia ;
- extracellular overhydration , ;
- pulmonary edema , cerebral edema ;
- acute left ventricular failure;
- development of circulatory disorders, in which there is a threat of cerebral and pulmonary edema;
- appointment large doses GCS.
The solution should be prescribed with caution to people who are sick. arterial hypertension , peripheral edema, decompensated chronic heart failure, renal failure in chronic form, preeclampsia , as well as those diagnosed with other conditions that cause sodium retention in the body.
If the solution is used as a diluent for other medications, existing contraindications should be taken into account.
Side effects
The following conditions may develop when using sodium chloride:
- overhydration ;
- hypokalemia ;
- acidosis .
If the drug is used correctly, the development of side effects is unlikely.
If NaCl solution 0.9% is used as a base solvent, then side effects are determined by the properties of the drugs that are diluted in the solution.
When any negative effects you need to immediately report this to a specialist.
Instructions for use of Sodium Chloride (Method and dosage)
The instructions for saline solution (isotonic solution) provide for its administration intravenously and subcutaneously.
In most cases, intravenous drip administration, for which the Sodium Chloride dropper is heated to a temperature of 36-38 degrees. The volume that is administered to the patient depends on the condition of the patient, as well as the amount of fluid that has been lost by the body. It is important to take into account the person’s age and weight.
Average daily dose drug - 500 ml, inject a solution with average speed 540 ml/h. If noted strong degree intoxication, then the maximum volume of medication per day can be 3000 ml. If there is such a need, a volume of 500 ml can be administered at a speed of 70 drops per minute.
Children are given a dose of 20 to 100 ml per day per 1 kg of weight. The dosage depends on body weight and the age of the child. It should be borne in mind that with prolonged use of this medicine it is necessary to monitor the level of electrolytes in plasma and urine.
To dilute drugs that need to be administered by drip, use 50 to 250 ml of sodium chloride per dose of the drug. The characteristics of administration are determined based on the main drug.
The hypertonic solution is administered intravenously.
If the solution is used to immediately compensate for the deficiency of sodium and chlorine ions, 100 ml of the solution is injected dropwise.
To perform a rectal enema to induce defecation, 100 ml of a 5% solution is administered; 3000 ml of an isotonic solution can also be administered throughout the day.
The use of a hypertensive enema is slowly indicated for renal and cardiac edema, increased and for hypertension, it is carried out slowly, 10-30 ml is administered. Such an enema cannot be performed in case of colon erosion and inflammatory processes.
Purulent wounds are treated with a solution according to the regimen prescribed by the doctor. Compresses with NaCl are applied directly to a wound or other lesion on the skin. Such a compress promotes the separation of pus and the death of pathogenic microorganisms.
Nasal spray instilled into the nasal cavity after cleansing it. For adult patients, two drops are instilled into each nostril, for children - 1 drop. It is used for both treatment and prevention, for which the solution is dripped for about 20 days.
Sodium chloride for inhalation used when colds. To do this, the solution is mixed with bronchodilators. Inhalation is carried out for ten minutes three times a day.
If absolutely necessary, saline solution can be prepared at home. To do this, mix a full teaspoon of table salt in one liter of boiled water. If it is necessary to prepare a certain amount of solution, for example, with salt weighing 50 g, appropriate measurements should be taken. This solution can be applied topically, used for enemas, rinses, and inhalations. However, under no circumstances should such a solution be administered intravenously or used for treatment open wounds or eyes.
Overdose
In case of overdose, the patient may feel nausea, suffer from vomiting and diarrhea, he may develop abdominal pain, fever, and rapid heartbeat. Also, with an overdose, indicators may increase, pulmonary edema and peripheral edema may develop, renal failure , muscle cramps , weakness , generalized seizures , coma . If the solution is administered excessively, it may develop hypernatremia .
With excessive intake into the body, it can develop hyperchlorimic acidosis .
If sodium chloride is used to dissolve drugs, then the overdose is mainly associated with the properties of those drugs that are diluted.
If NaCl is inadvertently overinjected, it is important to stop this process and evaluate whether there is more negative symptoms at the patient. Symptomatic treatment is practiced.
Interaction
NaCl is compatible with most medications. It is this property that determines the use of the solution for diluting and dissolving a number of drugs.
When diluting and dissolving, it is necessary to monitor the compatibility of drugs visually, determining whether a precipitate appears during the process, whether the color changes, etc.
When prescribing the drug simultaneously with corticosteroids It is important to constantly monitor the levels of electrolytes in the blood.
When taken in parallel, it decreases hypotensive effect And Spirapril .
Sodium Chloride is incompatible with a leukopoiesis stimulator Filgrastim , as well as with a polypeptide antibiotic Polymyxin B .
There is evidence that isotonic solution increases the bioavailability of drugs.
When diluted with a solution of powdered antibiotics, they are completely absorbed by the body.
Terms of sale
Sold in pharmacies by prescription. If necessary, use the drug to dilute other medications, etc. write out a prescription in Latin.
Storage conditions
The powder, tablets and solution should be stored in a dry place, in a well-closed container, and the temperature should not exceed 25 degrees Celsius. It is important to keep the drug away from children. If the packaging is sealed, freezing does not affect the properties of the drug.
Best before date
There are no restrictions on storing powder and tablets. The solution in 0.9% ampoules can be stored for 5 years; solution in bottles 0.9% - one year, solution in bottles 10% - 2 years. Cannot be used after the shelf life has expired.
special instructions
If an infusion is given, the patient's condition should be carefully monitored, in particular plasma electrolytes. It should be taken into account that in children, due to the immaturity of kidney function, a slowdown in sodium excretion . It is important to determine its plasma concentration before repeated infusions.
It is important to monitor the condition of the solution before administering it. The solution must be transparent and the packaging undamaged. Use the solution for intravenous administration can only be done by a qualified specialist.
Any preparations with Sodium Chloride should only be dissolved by a specialist who can qualifiedly assess whether the resulting solution is suitable for administration. It is important to strictly adhere to all antiseptic rules. Any solution should be administered immediately after its preparation.
The result of the series chemical reactions with the participation of sodium chloride is the formation of chlorine. Electrolysis of molten Sodium Chloride in industry is a method of producing chlorine. If you carry out electrolysis of a solution of Sodium Chloride, you also end up with chlorine. If crystalline Sodium Chloride is treated with concentrated sulfuric acid, the result is hydrogen chloride . and sodium hydroxide can be produced through a chain of chemical reactions. A qualitative reaction to chloride ion is a reaction with.
Analogs
Matches by ATX code 4th level:
U different manufacturers medicines the solution may be produced under a separate name. These are drugs Sodium Chloride Brown , Sodium chloride Bufus , Rizosin , Salin Sodium Chloride Cinco and etc.
Preparations containing sodium chloride are also produced. These are combined saline solutions + sodium chloride, etc.
For children
It is used in accordance with the instructions and under the careful supervision of specialists. The immaturity of renal function in children should be taken into account, therefore reintroduction carried out only after precise definition plasma sodium levels.
During pregnancy and lactation
During pregnancy, a sodium chloride dropper can only be used in pathological conditions. This is toxicosis in the moderate or severe stage, as well. Healthy women receive sodium chloride with food, and its excess can lead to the development of edema.
Reviews
Most reviews are positive, as users write about this product as useful drug. There are especially many reviews about the nasal spray, which, according to patients, is a good remedy for both the prevention and treatment of a runny nose. The product effectively moisturizes the nasal mucosa and promotes healing.
Sodium Chloride price, where to buy
The price of saline solution in ampoules of 5 ml is on average 30 rubles per 10 pcs. Buying sodium chloride 0.9% in a 200 ml bottle costs an average of 30-40 rubles per bottle.
- Online pharmacies in Russia Russia
- Online pharmacies in Ukraine Ukraine
- Online pharmacies in Kazakhstan Kazakhstan
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Structural formula
True, empirical, or gross formula: ClNa
Chemical composition of Sodium Chloride
Molecular weight: 58.443
Sodium chloride or sodium chloride (NaCl) - sodium hydrochloric acid. Known in everyday life as table salt, the main component of which is. Sodium chloride in significant amount found in sea water, giving it a salty taste. It occurs naturally in the form of the mineral halite (rock salt). Pure chloride sodium is colorless crystals, but with various impurities its color can take on a blue, purple, pink, yellow or gray tint.
Occurrence in nature and production
In nature, sodium chloride is found in the form of the mineral halite, which forms deposits of rock salt among sedimentary rocks, layers and lenses on the shores of salt lakes and estuaries, salt crusts in salt marshes and on the walls of volcanic craters and solfataras. Great amount sodium chloride dissolved in sea water. The world's oceans contain 4 × 10 15 tons of NaCl, that is, from every thousand tons of sea water, an average of 1.3 tons of sodium chloride can be obtained. Traces of NaCl are constantly present in the atmosphere as a result of evaporation of seawater spray. In clouds at an altitude of one and a half kilometers, 30% of droplets larger than 10 microns in size contain NaCl. It is also found in snow crystals. It is most likely that man's first acquaintance with salt occurred in lagoons warm seas or on salt lakes, where in shallow water salt water intensively evaporated under the influence high temperature and wind, and salt accumulated in the sediment. In the figurative expression of Pythagoras, “salt was born from noble parents: the sun and the sea.”
Halite
In nature, sodium chloride is most often found in the form of the mineral halite. It has a face-centered cubic lattice and contains 39.34% Na, 60.66% Cl. Others chemical elements impurities included are: Br, N, H, Mn, Cu, Ga, As, I, Ag, Ba, Tl, Pb, K, Ca, S, O. Density 2.1-2.2 g / cm³, and the hardness on the Mohs scale is 2. A colorless transparent mineral with a glassy luster. A common mineral in salt-bearing strata. It is formed during sedimentation in closed reservoirs, and also as a product of distillation on the walls of volcanic craters. Forms strata in sedimentary rocks of lagoonal and marine facies, stock-like bodies in salt domes and the like.
Rock salt
Rock salt is a sedimentary rock from the evaporite group, consisting of more than 90% halite. Halite is also often called rock salt. This sedimentary rock can be colorless or snow-white, but more often it is colored by impurities of clays, talc ( grey colour), iron oxides and hydroxides (yellow, orange, pink, red), bitumen (brown). Rock salt contains chlorides and sulfates of sodium, potassium, magnesium and calcium, bromides, iodides, borates, gypsum, impurities of carbonate-clay material, dolomite, ankerite, magnesite, bitumen and so on. According to the conditions of deposit formation, rock salt is divided into the following types:
- brines from modern salt pools
- saline groundwater
- deposits mineral salts modern salt pools
- fossil deposits (most important for industry).
Sea salt
Sea salt is a mixture of salts (chlorides, carbonates, sulfates, etc.) formed when sea water completely evaporates. The average salt content in sea water is:
When seawater evaporates at temperatures from +20 to +35 °C, the least soluble salts first crystallize in the sediment - calcium and magnesium carbonates and calcium sulfate. Then more soluble sodium and magnesium sulfates, sodium, potassium and magnesium chlorides precipitate, and after them - potassium and magnesium sulfates. The sequence of salt crystallization and the composition of the precipitate may vary slightly depending on temperature, evaporation rate and other conditions. In industry, sea salt is obtained from sea water, mainly by conventional evaporation. It differs significantly from rock salt high content other chemical salts, minerals and various trace elements, primarily iodine, potassium, magnesium and manganese. Accordingly, it differs from sodium chloride in taste - magnesium salts give it a bitter-salty taste. It is used in medicine: in the treatment skin diseases, such as psoriasis. How medicinal substance In pharmacies and regular retail chains, a common product is salt from the Dead Sea. In purified form, this type of salt is also offered in the grocery retail chain - as a natural and iodine-rich food salt.Deposits
Rock salt deposits are found in all geological systems. The most important of them are concentrated in Cambrian, Devonian, Permian and Tertiary deposits. Rock salt makes up thick layered deposits and the cores of vaulted structures (salt domes and stocks), forms layers, lenses, nests and inclusions in other rocks. Among the lake deposits in Russia, the largest are Eltonskoye, Baskunchak in the Caspian region, Lake Kuchukskoye, Lake Kulundinskoye, Ebeity and other lakes in Western Siberia.
Production
In ancient times, the technology of salt extraction was that salt brine (solution) was pulled out by horse drive from mines, which were called “wells” or “windows”, and were quite deep - 60-90 m. The extracted salt solution was poured into a special tank - created , from where it flowed through the holes into lower reservoir, and a system of chutes was fed into wooden towers. There it was poured into large vats, in which the salt was boiled. In Rus', Pomors boiled salt on the coast White Sea and they called her the long-tailed one. In 1137, the Novgorod prince Svyatoslav established a tax on salt pans:
...for the sea from the penis and from the salga in the belly...
White Sea salt, called "moryanka", was traded throughout Russian Empire until the beginning of the 20th century, until it was replaced by cheaper Volga salt. Modern extraction of sodium chloride is mechanized and automated. Salt is produced en masse by evaporating seawater (then called sea salt) or brine from other resources such as salt springs and salt lakes, as well as by developing salt mines and mining rock salt. To extract sodium chloride from seawater, the conditions required are a hot climate with low air humidity, the presence of significant low-lying areas lying below sea level or flooded by tides, low water permeability of the soil of evaporation pools, low precipitation during the season of active evaporation, and the absence of the influence of fresh water. river waters and the presence of developed transport infrastructure. World salt production in 2009 is estimated at 260 million tons. The world's largest producers are China (60.0 million tons), USA (46.0 million tons), Germany (16.5 million tons), India (15.8 million tons) and Canada (14 million tons).
Application
IN Food Industry and cooking
In the food industry and cooking, sodium chloride is used, the purity of which must be at least 97%. It is used as flavoring agent and for canning food products. This sodium chloride has the trade name table salt, sometimes the names food salt, table salt are also used, as well as clarification of the name depending on its origin - rock, sea, and according to the composition of the additives - iodized, fluorinated, etc. This salt is a crystalline bulk product with a salty taste, no taste, no odor (except iodized salt), in which foreign impurities not related to the salt extraction method are not allowed. In addition to sodium chloride, table salt contains small amounts of calcium, magnesium, and potassium salts, which make it hygroscopic and hard. The fewer of these impurities in the salt, the higher its quality. There are varieties: extra, highest, first and second. Mass fraction sodium chloride in varieties, %:
- extra - no less than 99.5;
- highest - 98.2;
- first - 97.5;
- the second - 97.0.
In medicine
An isotonic solution of sodium chloride in water (0.9%) is used as a detoxification agent to correct the state of body systems in case of dehydration, like others medicines. Hypertonic solutions(10% solution) is used as an auxiliary osmotic diuretic for cerebral edema, for raising blood pressure during bleeding, in conditions characterized by a deficiency of sodium and chlorine ions, for poisoning with silver nitrate, for treatment purulent wounds(locally). In ophthalmology as local remedy sodium chloride solution has an anti-edematous effect.
In public utilities. Technical salt
In winter, sodium chloride mixed with other salts, sand or clay - the so-called technical salt - is used as antifreeze against ice. Sidewalks are sprinkled with it, although this negatively affects leather shoes and the technical condition of vehicles due to corrosion processes.
Regeneration of Na-cationite filters
Na-cation exchange filters are widely used in water softening installations of all capacities during water treatment. The cation exchange materials used in modern water treatment plants are mainly glauconite, polymer ion exchange resins and sulfonated carbons. The most common are sulfonic cation exchange resins. Regeneration of Na-cationite filters is carried out with a 6-10% solution of table salt; as a result, the cationite is converted into Na-form and regenerated. The reactions proceed according to the equations: CaR 2 + 2NaCl → 2NaR + CaCl 2 MgR 2 + 2NaCl → 2NaR + MgCl 2
Chemical industry
Salt, along with coal, limestone and sulfur, forms the “big four” mineral products that are essential for the chemical industry. Soda, chlorine, hydrochloric acid, sodium hydroxide, sodium sulfate and sodium metal are obtained from it. In addition, salt is also used for the industrial production of sodium chlorate, which is easily soluble in water, which is a weed killer. The overall equation for the electrolysis reaction of a hot sodium chloride solution: NaCl + 3H 2 O → NaClO 3 + 3H 2
Physical and physico-chemical properties
Melting point +800.8 °C, boiling point +1465 °C. Moderately soluble in water, solubility depends little on temperature: the solubility coefficient of NaCl (in grams per 100 g of water) is 35.9 at +21 °C and 38.1 at +80 °C. The solubility of sodium chloride is significantly reduced in the presence of hydrogen chloride, sodium hydroxide, and metal chloride salts. Dissolves in liquid ammonia and enters into exchange reactions. IN pure form Sodium chloride is not hygroscopic. However, salt is often contaminated with impurities (mainly Ca 2+, Mg 2+ and SO 2- 4 ions), and such salt becomes damp when exposed to air. Crystal hydrate NaCl · 2H 2 O can be isolated at temperatures below +0.15 °C. A mixture of crushed ice and fine powdered sodium chloride is an effective coolant. Thus, a mixture of 30 g of NaCl per 100 g of ice is cooled to a temperature of −20 °C. This happens because the aqueous salt solution freezes at temperatures below 0 °C. Ice, which has a temperature of about 0 °C, melts in such a solution, absorbing heat from the environment.
Dielectric constant of NaCl - 6.3Density and concentration aqueous solutions NaCl
| Concentration, % | Concentration, g/l | Density, g/ml |
|---|---|---|
| 1 | 10,05 | 1,005 |
| 2 | 20,25 | 1,012 |
| 4 | 41,07 | 1,027 |
| 6 | 62,47 | 1,041 |
| 8 | 84,47 | 1,056 |
| 10 | 107,1 | 1,071 |
| 12 | 130,2 | 1,086 |
| 14 | 154,1 | 1,101 |
| 16 | 178,5 | 1,116 |
| 18 | 203,7 | 1,132 |
| 20 | 229,5 | 1,148 |
| 22 | 256 | 1,164 |
| 24 | 283,2 | 1,18 |
| 26 | 311,2 | 1,197 |
Structure
Sodium chloride forms colorless crystals in cubic system, space group Fm3m, cell parameters a = 0.563874 nm, d = 2.17 g/cm 3 . Each of the Cl - ions is surrounded by six Na + ions in an octahedral configuration, and vice versa. If you mentally discard, for example, Na + ions, you will be left with a densely packed cubic structure of Cl - ions, called a face-centered cubic lattice. Na + ions also form a densely packed cubic lattice. Thus, the crystal consists of two sublattices, shifted relative to each other by a half-cycle. The same lattice is characteristic of many other minerals.
In the crystal lattice, ionic chemical bonds predominate between atoms, which is a consequence of the electrostatic interaction of ions of opposite charge.
State educational institution
Higher professional education
"Perm State Pharmaceutical Academy
Federal Agency for Health and Social Development
Russian Federation"
Department of Analytical Chemistry
Course work:
Sodium chloride.
Completed:
student of group 21
Sennikov Anton
Checked:
Kolotova
Nina Vasilievna
Perm, 2010
Analytical reactions of sodium cation 5
Analytical reactions of chloride ion 5
Argentometry 6
Complexometry 6
General information 3
Getting 4
Qualitative analysis 5
Quantitative Analysis 6
Application 7
List of used literature 8
General information.
Chlorié d oń tria - chemical compound NaCl, sodium salt of hydrochloric acid, sodium chloride.
Chloride sodium is known in everyday life as table salt, of which it is the main component. Sodium chloride is found in significant quantities in sea water, creating it salty taste. Occurs naturally as a mineral halite(rock salt).
Pure sodium chloride appears as colorless crystals. But with various impurities, its color can take on a blue, purple, pink, yellow or gray tint.
Sodium chloride forms crystals with cubic symmetry. Larger chlorine ions form a dense cubic packing, in the free nodes of which (at the vertices of the regular octahedron) sodium ions are located.
Moderately soluble in water, solubility depends little on temperature: the solubility coefficient of NaCl (in g per 100 g of water) is 35.9 at 21 ° C and 38.1 at 80 ° C. The solubility of sodium chloride is significantly reduced in the presence of hydrogen chloride, sodium hydroxide , salts - metal chlorides. Dissolves in liquid ammonia and enters into exchange reactions.
Systematic name: sodium chloride / Sodium chloride
Chemical formula: NaCl
Molar mass: 58.44277 g/mol
Physical properties:
Density: 2.165 g/cm 3
Thermal properties:
Melting temperature 800.8 °C
Boiling temperature 1465 °C
Chemical properties:
Solubility in water 35.9 g/100 ml
Receipt.
The first way to produce sodium was the reduction reaction sodium carbonate coal when heating a close mixture of these substances in an iron container to 1000°C:
Na 2 CO 3 +2C=2Na+3CO
Then another way to obtain sodium appeared - electrolysis melt caustic soda or sodium chloride.
3.1. Analytical reactions to sodium cation.
Qualitative analysis.
1) With zinc dioxouranium (VI) acetate to form a yellow crystalline precipitate or yellow crystals of tatra- and octahedral shape:
NaCl + Zn(UO 2) 3 (CH 3 COO) 8 + CH 3 COOH + 9H 2 O ↔
↔ NaZn(UO 2) 3 (CH 3 COO) 9 x 9H 2 O↓ + HCl
2) Coloring the colorless burner flame yellow;
3) Reaction with potassium hexahydroxostibate (V) to form a white crystalline precipitate, soluble in alkalis:
NaCl + K ↔ Na↓ + KCl
In an acidic environment, the reagent is destroyed with the formation of a white amorphous precipitate of metaantimony acid HSbO 3:
K +HCl ↔ KCl + H 3 SbO 4 + 2H 2 O
H 3 SbO 4 ↔ HSbO 3 ↓ + H 2 O
3.2. Analytical reactions for chloride ion.
With a group reagent – AgNO 3 solution:
Methodology: To 2 drops of a solution containing chloride ions, add 1 drop of diluted HNO 3 and 3 drops of AgNO 3 solution. The observed white cheesy precipitate is soluble in NH 4 OH and a saturated solution of (NH 4) 2 CO 3.
The Cl solution is divided into 2 parts: concentrated HNO 3 is added to one until the medium becomes acidic, and a concentrated solution of KJ is added to the other. Precipitation or turbidity of the solution is observed:
Cl + 2HNO 3 ↔ AgCl↓ + 2 NH 4 NO 3
Cl + KJ + 2H 2 O ↔ AgJ↓ + KCl + 2NH 4 OH
Quantitative analysis.
4.1. Argentometry.
Standardization of a 0.05 M solution of silver nitrate against a standard solution of sodium chloride (pipetting method).
NaCl + AgNO 3 → AgCl↓ + NaNO 3
at the end point of titration: K 2 CrO 4 + 2AgNO 3 → Ag 2 CrO 4 ↓ + 2KNO 3
M(NaCl) = 58.44 g/mol
M(AgNO 3) = 169.87 g/mol
Methodology: An aliquot of the prepared standard sodium chloride solution is placed in a titration flask, diluted twice with distilled water, two drops of potassium chromate solution are added and titrated with a silver nitrate solution until the precipitate turns orange-yellow.
4.2. Complexometry.
Standardization of 0.01 M mercuric perchlorate solution to a standard sodium chloride solution (pipetting method)
2NaCl + Hg(ClO 4) 2 ↔ HgCl 2 + 2 NaClO 4
M (NaCl) = 58.44 g/mol
Methodology: The exact volume of a standard sodium chloride solution is placed in a titration flask, 4 drops of diluted nitric acid (1:4), 4 drops of 4 drops of an alcoholic saturated solution of diphenylcarbazone are added and titrated with a 0.01 M solution of mercuric perchlorate until the solution turns pinkish-violet.
5. Application.
If 9 grams of salt are dissolved in 1 liter of water, then its concentration in the resulting solution will be the same as in body fluids and tissues (0.9%). This concentration is called isotonic. More high content sodium chloride in solutions acts as an antimicrobial, stops the processes of fermentation and decay. This is the basis for its use for salting (canning) meat and vegetables.
When taken orally salt enhances the secretion of digestive juices, activates contraction of the stomach and intestines, thins mucus, improves absorption in the gastrointestinal tract. Poisonous in large doses, especially for chickens, pigs, dogs and cats. It is prescribed orally as a flavoring and nutritional substance that improves digestion in the form of a powder mixed with food or in the form of lick salt.
6. List of references.
Klyuchinov N.G. "Inorganic synthesis", Moscow, 1988;
Lurie Yu.Yu. "Handbook of Analytical Chemistry", Moscow, 1979;
Methodical manual on analytical chemistry. "Instrumental analysis methods", Perm, 2004;
Methodical manual on analytical chemistry. "Qualitative chemical analysis", Perm, 2003;
Methodical manual on analytical chemistry. "Quantitative chemical analysis", Perm, 2004;
Rabinovich V.A., Khavin Z.Ya. “A short chemical reference book”, Leningrad, Khimiya, 1977;
Thomas C.F. “Anhydrous synthesis in organic chemistry” (translation from English), Moscow, 1949;
Kharitonov Yu.Ya. “Analytical Chemistry”, in 2 books, Moscow, 2001.
