PRODUCTS

SODIUM BICARBONATE

Sodium Bicarbonate has an alkaline taste, loses carbon dioxide at 270°C (518 °F) and is used in food preparation.
Sodium bicarbonate also finds use as a medicine,a butter preservative, in ceramics,and to prevent timber mold.
Sodium bicarbonate is a white, crystalline, and odorless powder with a slightly alkaline taste.

CAS Number: 144-55-8
Molecular Formula: CHNaO3
Molecular Weight: 84.01
EINECS Number: 205-633-8

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Sodium bicarbonate, which is the compound commonly called baking soda, exists as a white, odorless, crystalline solid.
Sodium Bicarbonate occurs naturally as the mineral nahcolite, which derives its name from its chemical formula by replacing the “3” in NaHCO3 with the ending “lite.”
The world’s main source of nahcolite is the Piceance Creek Basin in western Colorado, which is part of the larger Green River formation.

Sodium bicarbonate is extracted using solution mining by pumping hot water through injection wells to dissolve the nahcolite from the Eocene beds where it occurs 1,500 to 2,000 feet below the surface.
The dissolved sodium bicarbonate is pumped to the surface where it is treated to recover NaHCO3 from solution.
Sodium bicarbonate, NaHC03, also known as sodium acid carbonate and baking soda, is a white water-soluble crystalline solid.

Sodium Bicarbonate is an inorganic compound with the chemical formula NaHCO₃, also known as baking soda.
It naturally occurs as the mineral nahcolite, which can be found in deposits of soda ash.
Sodium bicarbonate acts as a weak base and reacts easily with acids to produce carbon dioxide gas.

When heated, it decomposes into sodium carbonate (Na₂CO₃), water, and carbon dioxide.
This ability to release gas makes it extremely useful in both household and industrial applications.
It is highly soluble in water and creates a mildly basic solution when dissolved.

This property helps neutralize acids and stabilize pH levels in various environments.
Because of this, sodium bicarbonate is widely used in medicine, food processing, and cleaning products.
Sodium bicarbonate (IUPAC name: sodium hydrogencarbonate), commonly known as baking soda or bicarbonate of soda (or simply "bicarb", especially in the UK), or salaratus, is a chemical compound with the formula NaHCO3. It is a salt composed of a sodium cation (Na+) and a bicarbonate anion (HCO−3).

Sodium bicarbonate is a white solid that is crystalline but often appears as a fine powder.
Sodium Bicarbonate has a slightly salty, alkaline taste resembling that of sodium carbonate ("washing soda").
The natural mineral form is nahcolite, although it is more commonly found as a component of the mineral trona.

As it has long been known and widely used, the salt has many different names such as baking soda, bread soda, cooking soda, brewing soda and bicarbonate of soda and can often be found near baking powder in stores.
The term baking soda is more common in the United States, while bicarbonate of soda is more common in Australia, the United Kingdom, and New Zealand.
Abbreviated colloquial forms such as sodium bicarb, bicarb soda, bicarbonate, and bicarb are common.

The prefix bi- in "bicarbonate" comes from an outdated naming system predating molecular knowledge.
Sodium Bicarbonate is based on the observation that there is twice as much carbonate (CO2−3) per sodium in sodium bicarbonate (NaHCO3) as there is in sodium carbonate (Na2CO3).
The modern chemical formulas of these compounds now express their precise chemical compositions which were unknown when the name bi-carbonate of potash was coined (see also: bicarbonate).

Sodium bicarbonate occurs as an odorless, white, crystalline powder with a saline, slightly alkaline taste.
The crystal structure is monoclinic prisms.
Grades with different particle sizes, from a fine powder to free-flowing uniform granules, are commercially available.

White crystalline powder or granules; monoclinic crystals; density 2.20 g/cm3; decomposes around 50°C, begins to lose carbon dioxide; converts to sodium carbonate at 100°C; soluble in water, 10g/100 mL at 20°C; slowly decomposes to CO2 and Na2CO3 in aqueous solution at ambient temperature; decomposes to Na2CO3 in boiling water; aqueous solution slightly alkaline; pH of 0.1M solution at 25°C is about 8.3; insoluble in alcohol; decomposes in acids.
Most sodium bicarbonate in the United States is made synthetically by the reaction of sodium carbonate solution (Na2CO3) with carbon dioxide: Na2CO3(aq) + H2O(l) + CO2(g) → 2NaHCO3(aq).

Sodium Bicarbonate can also be produced using the Solvay process, which uses ammonia, carbon dioxide, and salt to produce sodium bicarbonate according to the following series of reactions: 2NH3(g) + CO2(g) + H2O(l) → (NH4)2CO3(aq)
(NH4)2CO3(aq) + CO2(g) + H2O(l) → 2NH3HCO3(aq)
NH4HCO3(aq) + NaCl(aq) → NaHCO3(s) + NH4Cl(aq).

Sodium bicarbonate reacts with acids, acidic salts, and many alkaloidal salts, with the evolution of carbon dioxide. Sodium bicarbonate can also intensify the darkening of salicylates.
In powder mixtures, atmospheric moisture or water of crystallization from another ingredient is sufficient for sodium bicarbonate to react with compounds such as boric acid or alum.
In liquid mixtures containing bismuth subnitrate, sodium bicarbonate reacts with the acid formed by hydrolysis of the bismuth salt.

In solution, sodium bicarbonate has been reported to be incompatible with many drug substances such as ciprofloxacin, amiodarone, nicardipine, and levofloxacin.
Sodium bicarbonate is a key ingredient in baking powders and leavening agents.
When combined with an acid like vinegar or lemon juice, it releases carbon dioxide.

This gas causes dough to expand, giving baked goods their soft and fluffy texture.
Sodium Bicarbonate is also used to neutralize acidity in food and beverages.

For example, it helps reduce the sour taste in tomato sauces or acidic drinks.
In food preservation, it maintains freshness by balancing pH and preventing spoilage.

Melting point:>300 °C (lit.)
Boiling point:851 °C
Density:2.16 g/mL at 25 °C (lit.)
Bulk density:1000 kg/m³
Refractive index:1.500
Storage temperature:2–8 °C
Solubility:H₂O — 1 M at 20 °C, clear, colorless
Form:Solution (7.5%)
Color:White
Specific gravity:2.159
pH range:7.8–8.2
pH:8.27 (1 mM solution); 8.22 (10 mM solution); 8.02 (100 mM solution)
pKa:(1) 6.37, (2) 10.25 (carbonic, at 25 °C)
Odor:Odorless
Water solubility:9 g/100 mL (20 °C)
Decomposition:50 °C
Merck:14,8583
BRN:4153970
BCS class:1
Stability:Stable
LogP:-4.010 (estimated)

Sodium bicarbonate is manufactured either by passing carbon dioxide into a cold saturated solution of sodium carbonate, or by the ammonia–soda (Solvay) process, in which first ammonia and then carbon dioxide is passed into a sodium chloride solution to precipitate sodium bicarbonate while the more soluble ammonium chloride remains in solution.
In nature, sodium bicarbonate occurs almost exclusively as either nahcolite or trona.
Trona is more common, as nahcolite is more soluble in water and the chemical equilibrium between the two minerals favors trona.

Significant nahcolite deposits are in the United States, Botswana and Kenya, Uganda, Turkey, and Mexico.
The biggest trona deposits are in the Green River basin in Wyoming.
In medicine, sodium bicarbonate acts as an antacid to relieve heartburn and indigestion.

Sodium bicarbonate neutralizes excess stomach acid, providing quick relief from discomfort.
It is available in tablets, powders, or as an injectable solution for medical emergencies.
Doctors sometimes use sodium bicarbonate in intravenous solutions to treat acidosis.

It helps restore the body's normal pH when it becomes too acidic.
This is especially important in patients with kidney problems or metabolic disorders.
Sodium bicarbonate can also be used as a mouthwash or toothpaste additive.

Sodium bicarbonate helps whiten teeth, reduce bad breath, and maintain oral hygiene.
Its mild abrasiveness removes stains without damaging tooth enamel.
Sodium bicarbonate is an excellent cleaning and deodorizing agent.

It can remove stains, neutralize odors, and absorb moisture.
When mixed with water or vinegar, it becomes a powerful, non-toxic cleaner for household surfaces.
It is often sprinkled in refrigerators, carpets, or shoes to eliminate bad smells.

The compound reacts with acidic odors, turning them into neutral salts and water.
Because of its non-corrosive nature, it is safe for use on metals, fabrics, and plastics.
In laundry, it helps soften water and enhance the cleaning power of detergents.

It also keeps colors bright and prevents unpleasant odors in washing machines.
Many natural cleaning products use sodium bicarbonate as their main active ingredient.
Baking soda: A white solid formed either by passing an excess of carbon dioxide through sodium carbonate or hydroxide solution, or by precipitation when cold concentrated solutions of sodium chloride and ammonium hydrogencarbonate are mixed.

Sodium hydrogencarbonate decomposes on heating to give sodium carbonate, carbon dioxide, and water With dilute acids, it yields carbon dioxide.
Sodium bicarbonate is used as a constituent of baking powder, in effervescent beverages, and in fire extinguishers.
Its aqueous solutions are alkaline as a result of salt hydrolysis. Sodium hydrogencarbonate forms monoclinic crystals.

Sodium bicarbonate is an amphoteric compound.[33] Aqueous solutions are mildly alkaline due to the formation of carbonic acid and hydroxide ion: HCO−3 + H2O → H
2CO3 + OH−
Sodium bicarbonate can sometimes be used as a mild neutralization agent and a safer alternative to strong bases like sodium hydroxide.

Reaction of sodium bicarbonate and an acid produces a salt and carbonic acid, which readily decomposes to carbon dioxide and water: NaHCO3 + HCl → NaCl + H2O + CO2
H2CO3 → H2O + CO2(g)
Sodium bicarbonate reacts with acetic acid (found in vinegar), producing sodium acetate, water, and carbon dioxide: NaHCO3 + CH3COOH → CH3COONa + H2O + CO2(g)

Sodium bicarbonate reacts with bases such as sodium hydroxide to form carbonates: NaHCO3 + NaOH → Na2CO3 + H2O
At temperatures from 80–100 °C (176–212 °F), sodium bicarbonate gradually decomposes into sodium carbonate, water, and carbon dioxide.
The conversion is faster at 200 °C (392 °F): 2 NaHCO3 → Na2CO3 + H2O + CO2

Most bicarbonates undergo this dehydration reaction.
Further heating converts the carbonate into the oxide (above 850 °C/1,560 °F): Na2CO3 → Na2O + CO2

The generation of carbon dioxide and water partially explain the fire-extinguishing properties of NaHCO3, although other factors like heat absorption and radical scavenging are more significant.
Sodium bicarbonate, neutralises gastric acid with the production of carbon dioxide. Bicarbonate not involved in that reaction is absorbed and in the absence of a deficit of bicarbonate in the plasma, bicarbonate ions are excreted in the urine, which is rendered alkaline, and there is an accompanying diuresis.

Storage:
When heated to about 50℃, sodium bicarbonate begins to dissociate into carbon dioxide, sodium carbonate, and water; on heating to 250–300℃, for a short time, sodium bicarbonate is completely converted into anhydrous sodium carbonate.
However, the process is both time- and temperature-dependent, with conversion 90% complete within 75 minutes at 93°C.
The reaction proceeds via surface-controlled kinetics; when sodium bicarbonate crystals are heated for a short period of time, very fine needleshaped crystals of anhydrous sodium carbonate are formed on the sodium bicarbonate surface.

The effects of relative humidity and temperature on the moisture sorption and stability of sodium bicarbonate powder have been investigated.
Sodium bicarbonate powder is stable below 76% relative humidity at 25℃ and below 48% relative humidity at 40℃.
At 54% relative humidity, the degree of pyrolytic decarboxylation of sodium bicarbonate should not exceed 4.5% in order to avoid detrimental effects on stability.

At ambient temperatures, aqueous solutions slowly decompose with partial conversion into the carbonate; the decomposition is accelerated by agitation or heat.
Aqueous solutions begin to break up into carbon dioxide and sodium carbonate at about 20°C, and completely on boiling.
Aqueous solutions of sodium bicarbonate may be sterilized by filtration or autoclaving.

To minimize decomposition of sodium bicarbonate by decarboxylation on autoclaving, carbon dioxide is passed through the solution in its final container, which is then hermetically sealed and autoclaved.
The sealed container should not be opened for at least 2 hours after it has returned to ambient temperature, to allow time for the complete reformation of the bicarbonate from the carbonate produced during the heating process.
Aqueous solutions of sodium bicarbonate stored in glass containers may develop deposits of small glass particles.

Sediments of calcium carbonate with traces of magnesium or other metal carbonates have been found in injections sterilized by autoclaving; these are due to impurities in the bicarbonate or to extraction of calcium and magnesium ions from the glass container.
Sedimentation may be retarded by the inclusion of 0.01–0.02% disodium edetate.
Sodium bicarbonate is stable in dry air but slowly decomposes in moist air and should therefore be stored in a well-closed container in a cool, dry place.

Uses:
Sodium bicarbonate, used in the formof baking soda and baking powder, is the most common leavening agent.
When baking soda,which is an alkaline substance, is added to a mix, it reacts with an acid ingredient to producecarbon dioxide.
The reaction can be represented as: NaHCO3(s) + H+ → Na+(aq) + H2O(l) +CO2(g), where H+ is supplied by the acid.

Baking powders contain baking soda as a primaryingredient along with acid and other ingredients.
Depending on the formulation, bakingpowders can produce carbon dioxide quickly as a single action powder or in stages, as with adouble-action powder.
Baking soda is also used as a source of carbon dioxide for carbonatedbeverages and as a buffer.

In addition to baking, baking soda has numerous household uses.
Sodium bicarbonate is used as a generalcleanser, a deodorizer, an antacid, a fire suppressant, and in personal products such as toothpaste.
Sodium bicarbonate is a weak base in aqueous solution, with a pH of about 8.

Thebicarbonate ion (HCO3-) has amphoteric properties, which means it can act as either an acidor a base.
This gives baking soda a buff ering capacity and the ability to neutralize both acidsand bases.
Food odors resulting from acidic or basic compounds can be neutralized with bakingsoda into odor-free salts.

Because sodium bicarbonate is a weak base, it has a greater abilityto neutralize acid odors.
The second largest use of sodium bicarbonate, accounting for approximately 25% of totalproduction, is as an agricultural feed supplement.
In cattle it helps maintain rumen pH andaids fiber digestibility; for poultry it helps maintain electrolyte balance by providing sodiumin the diet, helps fowl tolerate heat, and improves eggshell quality.

Sodium bicarbonate is used in the chemical industry as a buff ering agent, a blowingagent, a catalyst, and a chemical feedstock.
Sodium bicarbonate is used in the leather tanningindustry for pretreating and cleaning hides and to control pH during the tanning process.Heating sodium bicarbonate produces sodium carbonate, which is used for soap and glassmaking.
Sodium bicarbonate is incorporated into pharmaceuticals to serve as an antacid, abuff ering agent, and in formulations as a source of carbon dioxide in eff ervescent tablets.

Drychemical type BC fire extinguishers contain sodium bicarbonate (or potassium bicarbonate).
Other uses of bicarbonate include pulp and paper processing, water treatment, and oil welldrilling.
Sodium bicarbonate is usually administered orally in order to regulate the serum pH.

Imbalances of the plasma pH can be due to problems occurring in the kidneys such as renal tubular acidosis.
Within the kidneys, blood is filtered before it passes through the tubular part of the nephrons where re-absorption or secretion of important salts and others takes place.
In renal tubular acidosis, the kidneys either fail to filter or secrete acid ions (H+) from the plasma (secretion takes place in the distal tubule), or to recover bicarbonate ions (HCO3-) from the filtrate (passive re-absorption takes place in the proximal tubule, active re-absorption at the distal tubule), which is necessary to balance the pH.

In the view of this mode of action, the pharmaceutically active component of sodium bicarbonate is the bicarbonate anion, but the cation Na+ is responsible for solubility and compatibility.
Sodium Bicarbonate is a leavening agent with a ph of approxi- mately 8.5 in a 1% solution at 25°c.
Sodium bicarbonate functions with food grade phosphates (acidic leavening compounds) to release carbon dioxide which expands during the baking process to provide the baked good with increased volume and tender eating qualities.

Sodium bicarbonate is also used in dry-mix beverages to obtain carbonation, which results when water is added to the mix containing the sodium bicarbonate and an acid.
Sodium bicarbonate is a component of baking powder.
Sodium bicarbonate is also termed baking soda, bicarbonate of soda, sodium acid carbonate, and sodium hydrogen carbonate.

Sodium bicarbonate manufacture of many sodium salts; source of CO2; ingredient of baking powder, effervescent salts and beverages; in fire extinguishers, cleaning Compounds.
In cooking, baking soda is primarily used in baking as a leavening agent.
When it reacts with acid or is heated, carbon dioxide is released, which causes expansion of the batter and forms the characteristic texture and grain in cakes, quick breads, soda bread, and other baked and fried foods. When an acid is used, the acid–base reaction can be generically represented as follows: NaHCO3 + H+ → Na+ + CO2 + H2O

Acidic materials that induce this reaction include hydrogen phosphates, cream of tartar, lemon juice, yogurt, buttermilk, cocoa, and vinegar.
Baking soda may be used together with sourdough, which is acidic, making a lighter product with a less acidic taste.
Since the reaction occurs slowly at room temperature, mixtures (cake batter, etc.) can be allowed to stand without rising until they are heated in the oven.

Heat can also by itself cause sodium bicarbonate to act as a raising agent in baking because of thermal decomposition, releasing carbon dioxide at temperatures above 80 °C (180 °F), as follows: 2 NaHCO3 → Na2CO3 + H2O + CO2
When used this way on its own, without the presence of an acidic component (whether in the batter or by the use of a baking powder containing acid), only half the available CO2 is released (one CO2 molecule is formed for every two equivalents of NaHCO3).
Additionally, in the absence of acid, thermal decomposition of sodium bicarbonate also produces sodium carbonate, which is strongly alkaline and gives the baked product a bitter, soapy taste and a yellow color.

Baking powder, also sold for cooking, contains around 30% of bicarbonate, and various acidic ingredients that are activated by the addition of water, without the need for additional acids in the cooking medium.
Many forms of baking powder contain sodium bicarbonate combined with calcium acid phosphate, sodium aluminium phosphate, or cream of tartar.
Baking soda is alkaline; the acid used in baking powder avoids a metallic taste when the chemical change during baking creates sodium carbonate.

Sodium bicarbonate is often used in conjunction with other bottled water food additives to add taste.
Its European Union E number is E500.
Sodium bicarbonate is one of the main components of the common "black snake" firework.

The effect is caused by the thermal decomposition, which produces carbon dioxide gas to produce a long snake-like ash as a combustion product of the other main component, sucrose.
Sodium bicarbonate also delays combustion reactions through the release of carbon dioxide and water, both of which are flame retardants, when heated.
Sodium bicarbonate has weak disinfectant properties and it may be an effective fungicide against some organisms.

Sodium bicarbonate can be used to extinguish small grease or electrical fires by being thrown over the fire, as heating of sodium bicarbonate releases carbon dioxide.
However, it should not be applied to fires in deep fryers; the sudden release of gas may cause the grease to splatter.
Sodium bicarbonate is used in BC dry chemical fire extinguishers as an alternative to the more corrosive monoammonium phosphate in ABC extinguishers.

The alkaline nature of sodium bicarbonate makes it the only dry chemical agent, besides Purple-K, that was used in large-scale fire suppression systems installed in commercial kitchens.
Sodium bicarbonate has several fire-extinguishing mechanisms that act simultaneously.
It decomposes into water and carbon dioxide when heated, an endothermic reaction that deprives the fire of heat.

In addition, it forms intermediates that can scavenge the free radicals which are responsible for the propagation of fire.
With grease fires specifically, it also has a mild saponification effect, producing a soapy foam that can help smother the fire.
Sodium bicarbonate reacts spontaneously with acids, releasing CO2 gas as a reaction product.

Sodium bicarbonate is commonly used to neutralize unwanted acid solutions or acid spills in chemical laboratories.
Sodium bicarbonate is not appropriate to use sodium bicarbonate to neutralize base even though it is amphoteric, reacting with both acids and bases.
Sodium bicarbonate is taken as a sports supplement to improve muscular endurance.

Studies conducted mostly in males have shown that sodium bicarbonate is most effective in enhancing performance in short-term, high-intensity activities.
Sodium bicarbonate can prevent the growth of fungi when applied on leaves, although it will not kill the fungus.
Excessive amounts of sodium bicarbonate can cause discolouration of fruits (two percent solution) and chlorosis (one percent solution).

Sodium bicarbonate is also commonly used as a free choice dietary supplement in sheep to help prevent bloat.
Sodium bicarbonate mixed with water can be used as an antacid to treat acid indigestion and heartburn.
Its reaction with stomach acid produces salt, water, and carbon dioxide: NaHCO3 + HCl → NaCl + H2O + CO2(g)

A mixture of sodium bicarbonate and polyethylene glycol dissolved in water and taken orally, is an effective gastrointestinal lavage preparation and laxative prior to gastrointestinal surgery, gastroscopy, etc.
Intravenous sodium bicarbonate in an aqueous solution is sometimes used for cases of acidosis, or when insufficient sodium or bicarbonate ions are in the blood.
In cases of respiratory acidosis, the infused bicarbonate ion drives the carbonic acid/bicarbonate buffer of plasma to the left, and thus raises the pH.

For this reason, sodium bicarbonate is used in medically supervised cardiopulmonary resuscitation.
Infusion of bicarbonate is indicated only when the blood pH is markedly low (< 7.1–7.0).
HCO3− is used for treatment of hyperkalemia, as it will drive K+ back into cells during periods of acidosis.

Since sodium bicarbonate can cause alkalosis, it is sometimes used to treat aspirin overdoses.
Aspirin requires an acidic environment for proper absorption, and a basic environment will diminish aspirin absorption in cases of overdose.
Sodium bicarbonate has also been used in the treatment of tricyclic antidepressant overdose.

Sodium bicarbonate can also be applied topically as a paste, with three parts baking soda to one part water, to relieve some kinds of insect bites and stings (as well as accompanying swelling).
Some alternative practitioners, such as Tullio Simoncini, have promoted baking soda as a cancer cure, which the American Cancer Society has warned against due to both its unproven effectiveness and potential danger in use.
Edzard Ernst has called the promotion of sodium bicarbonate as a cancer cure "one of the more sickening alternative cancer scams I have seen for a long time".

Sodium bicarbonate can be added to local anaesthetics, to speed up the onset of their effects and make their injection less painful.[47] It is also a component of Moffett's solution, used in nasal surgery.[48]
Sodium bicarbonate has been proposed that acidic diets weaken bones.
One systematic meta-analysis of the research shows no such effect.

Another also finds that there is no evidence that alkaline diets improve bone health, but suggests that there "may be some value" to alkaline diets for other reasons.
Antacid (such as baking soda) solutions have been prepared and used by protesters to alleviate the effects of exposure to tear gas during protests.
Similarly to its use in baking, sodium bicarbonate is used together with a mild acid such as tartaric acid as the excipient in effervescent tablets: when such a tablet is dropped in a glass of water, the carbonate leaves the reaction medium as carbon dioxide gas (HCO3− + H+ → H2O + CO2↑ or, more precisely, HCO3− + H3O+ → 2 H2O + CO2↑).

This makes the tablet disintegrate, leaving the medication suspended and/or dissolved in the water together with the resulting salt (in this example, sodium tartrate).
Sodium bicarbonate is also used as an ingredient in some mouthwashes.
Sodium bicarbonate has anticaries and abrasive properties.[54] It works as a mechanical cleanser on the teeth and gums, neutralizes the production of acid in the mouth, and also acts as an antiseptic to help prevent infections.

Sodium bicarbonate in combination with other ingredients can be used to make a dry or wet deodorant.
Sodium bicarbonate may be used as a buffering agent, combined with table salt, when creating a solution for nasal irrigation.
It is used in eye hygiene to treat blepharitis.

This is done by adding a teaspoon of sodium bicarbonate to cool water that was recently boiled followed by gentle scrubbing of the eyelash base with a cotton swab dipped in the solution.
Sodium bicarbonate is used as a cattle feed supplement, in particular as a buffering agent for the rumen.
Sodium bicarbonate is used in a process to remove paint and corrosion called sodablasting.

As a blasting medium, sodium bicarbonate is used to remove surface contamination from softer and less resilient substrates such as aluminium, copper, or timber that could be damaged by silica sand abrasive media.
A manufacturer recommends a paste made from baking soda with minimal water as a gentle scouring powder.
Such a paste can be useful in removing surface rust because the rust forms a water-soluble compound when in a concentrated alkaline solution.

Cold water should be used since hot-water solutions can corrode steel.
Sodium bicarbonate attacks the thin protective oxide layer that forms on aluminium, making it unsuitable for cleaning this metal.
A solution of baking soda in warm water will remove the tarnish from silver when the silver is in contact with a piece of aluminium foil.

Baking soda is commonly added to washing machines as a replacement for water softener and to remove odors from clothes.
When diluted with warm water, it is also almost as effective in removing heavy tea and coffee stains from cups as sodium hydroxide.
Sodium bicarbonate is an inorganic salt used as a buffering agent and a pH adjuster, it also serves as a neutralizer.

Sodium bicarbonate is used in skin-smoothing powders.
Sodium bicarbonate is generally used in pharmaceutical formulations as a source of carbon dioxide in effervescent tablets and granules.
Sodium bicarbonate is also widely used to produce or maintain an alkaline pH in a preparation.

In effervescent tablets and granules, sodium bicarbonate is usually formulated with citric and/or tartaric acid; combinations of citric and tartaric acid are often preferred in formulations as citric acid alone produces a sticky mixture that is difficult to granulate, while if tartaric acid is used alone, granules lose firmness.
When the tablets or granules come into contact with water, a chemical reaction occurs, carbon dioxide is evolved, and the product disintegrates.
Melt granulation in a fluidized bed dryer has been suggested as a one-step method for the manufacture of effervescent granules composed of anhydrous citric acid and sodium bicarbonate, for subsequent compression into tablets.

Tablets may also be prepared with sodium bicarbonate alone since the acid of gastric fluid is sufficient to cause effervescence and disintegration.
Sodium bicarbonate is also used in tablet formulations to buffer drug molecules that are weak acids, thereby increasing the rate of tablet dissolution and reducing gastric irritation.
The effects of tablet binders, such as polyethylene glycols, microcrystalline cellulose, silicified microcrystalline cellulose, pregelatinized starch, and povidone, on the physical and mechanical properties of sodium bicarbonate tablets have also been investigated.

Additionally, sodium bicarbonate is used in solutions as a buffering agent for erythromycin, lidocaine, local anesthetic solutions, and total parenteral nutrition (TPN) solutions.
In some parenteral formulations, e.g. niacin, sodium bicarbonate is used to produce a sodium salt of the active ingredient that has enhanced solubility.
Sodium bicarbonate has also been used as a freeze-drying stabilizer and in toothpastes.

Sodium bicarbonate has been used as a gas-forming agent in alginate raft systems and in floating, controlledrelease oral dosage forms for a range of drugs.
Tablet formulations containing sodium bicarbonate have been shown to increase the absorption of paracetamol, and improve the stability of levothyroxine.
Sodium bicarbonate has also been included in formulations of vaginal bioadhesive tablets and in carbon dioxide releasing suppositories.

Therapeutically, sodium bicarbonate may be used as an antacid, and as a source of the bicarbonate anion in the treatment of metabolic acidosis.
Sodium bicarbonate may also be used as a component of oral rehydration salts and as a source of bicarbonate in dialysis fluids; it has also been suggested as a means of preventing radiocontrast-induced nephrotoxicity.
Sodium bicarbonate is used in food products as an alkali or as a leavening agent, e.g. baking soda.

Safety Profile:
Low toxicity by ingestion, an experimental teratogen.
A nuisance dust, human systemic effects: changes in potassium levels, increased urine volume, metabolic acidosis, nausea or vomiting, respiratory changes, sodium level changes.
Sodium bicarbonate is used in a number of pharmaceutical formulations including injections and ophthalmic, otic, topical, and oral preparations.

Sodium bicarbonate is metabolized to the sodium cation, which is eliminated from the body by renal excretion, and the bicarbonate anion, which becomes part of the body’s bicarbonate store.
Any carbon dioxide formed is eliminated via the lungs.
Administration of excessive amounts of sodium bicarbonate may thus disturb the body’s electrolyte balance, leading to metabolic alkalosis or possibly sodium overload with potentially serious consequences.

The amount of sodium present in antacids and effervescent formulations has been sufficient to exacerbate chronic heart failure, especially in elderly patients.
Orally ingested sodium bicarbonate neutralizes gastric acid with the evolution of carbon dioxide and may cause stomach cramps and flatulence.
When used as an excipient, sodium bicarbonate is generally regarded as an essentially nontoxic and nonirritant material.