Sodium hydroxide

Sodium hydroxide
General
Systematic name	Sodium hydroxide
Other names	Lye, Caustic Soda
Molecular formula	NaOH
Molar mass	40.0 g/mol
Appearance	White flakes
CAS number	^*
Properties
Density and phase	2.1 g/cm³, solid
Solubility in water	111 g/100 ml (20°C)
Melting point	323°C (596 K)
Boiling point	1390°C (1663 K)
Basicity (pK_b)	0.2
Hazards
MSDS	External MSDS
EU classification	Corrosive (C)
R-phrases
S-phrases	, , ,
NFPA 704
Flash point	Non-flammable.
Supplementary data page
Structure and properties	n, ε_r, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Related compounds
Other anions	Sodium chloride Sodium sulfate.
Other cations	Potassium hydroxide Calcium hydroxide
Related bases	Ammonia, lime.
Related compounds	Chlorine
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Chemical infobox

Sodium hydroxide (Na OH), also known as lye or caustic soda, is a caustic metallic base. It is widely used in industry, mostly as a strong chemical base in the manufacture of pulp and paper, textiles, drinking water, and detergents. Worldwide production in 1998 was around 45 million tonnes. Sodium hydroxide is also the most common base used in chemical laboratories.

General properties

Pure sodium hydroxide is a white solid, available in pellets, flakes, granules, and also 50% saturated solution. It is very deliquescent and also readily absorbs carbon dioxide from the air, so it should be stored in an airtight container. It is very soluble in water with liberation of heat. It also dissolves in ethanol and methanol, though it exhibits lower solubility in these solvents than does potassium hydroxide. It is insoluble in ether and other non-polar solvents. A sodium hydroxide solution will leave a yellow stain on fabric and paper.

Chemical properties

Sodium hydroxide is completely ionic, containing sodium ions and hydroxide ions. The hydroxide ion makes sodium hydroxide a strong base which reacts with acids to form water and the corresponding salts, e.g., with hydrochloric acid, sodium chloride is formed:

NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

In general such reactions are represented by one simple net ionic equation:

OH⁻(aq) + H⁺(aq) → H₂O

This type of reaction releases heat when a strong acid is used. Such acid-base reactions can also be used for titrations, and indeed this is a common way for measuring the concentration of acids. Related to this is the reaction of sodium hydroxide with acidic oxides. The reaction of carbon dioxide has already been mentioned, but other acidic oxides such as sulfur dioxide (SO₂) also react completely. Such reactions are often used to "scrub" harmful acidic gases (like SO₂) and prevent their release into the atmosphere.

2 NaOH + CO₂ → Na_{2_CO₃} + H₂O

Sodium hydroxide slowly reacts with glass to form sodium silicate, so glass joints and stopcocks exposed to NaOH have a tendency to "freeze". Flasks and glass-lined chemical reactors are damaged by long exposure to hot sodium hydroxide, and the glass becomes frosted. Sodium hydroxide does not attack iron or copper, but many other metals such as aluminium, zinc and titanium are attacked rapidly. In 1986 an aluminium road tanker in the UK was mistakenly used to transport 25% sodium hydroxide solution, causing pressurisation of the contents and damage to the tanker. For this same reason aluminium pans should never be cleaned with lye.

2 Al(s) + 6 NaOH(aq) → 3 H₂ (g) + 2 Na₃AlO₃(aq)

Many non-metals also react with sodium hydroxide, giving salts. For example phosphorus forms sodium hypophosphite, while silicon gives sodium silicate.

Unlike NaOH, the hydroxides of most metals are insoluble, and therefore sodium hydroxide can be used to precipitate metal hydroxides. One such hydroxide is aluminium hydroxide, used as a gelatinous floc to filter out particulate matter in water treatment. Aluminium hydroxide is prepared at the treatment plant from aluminium sulfate by reaction with NaOH:

6 NaOH(aq) + Al₂(SO₄)₃(aq) → 2 Al(OH)₃(s) + 3 Na₂SO₄(aq)

Sodium hydroxide reacts readily with carboxylic acids to form their salts, and it is even a strong enough base to form salts with phenols. NaOH can also be used for the base-driven hydrolysis of esters (as is saponification), amides and alkyl halides. However, the limited solubility of NaOH in organic solvents means that the more soluble KOH is often preferred.

Manufacture

In 1998, total world production was around 45 million tonnes. Of this, both North America and Asia contributed around 14 million tonnes, and Europe produced around 10 million tonnes.

Methods of production

Sodium hydroxide is produced (along with chlorine and hydrogen) via the chloralkali process. This involves the electrolysis of an aqueous solution of sodium chloride. The sodium hydroxide builds up at the cathode, where water is reduced to hydrogen gas and hydroxide ion:

2 Na⁺ + 2 H₂O + 2 e⁻ → H₂ + 2 NaOH

To produce NaOH it is necessary to prevent reaction of the NaOH with the chlorine, this is typically done in one of three ways, of which the membrane cell process is, economically, the most viable.

Mercury cell process – sodium metal forms as an amalgam at a mercury cathode; this sodium is then reacted with water to produce NaOH. There have been concerns about mercury releases, although modern plants claim to be safe in this regard.
Diaphragm cell process – uses a steel cathode, and reaction of NaOH with Cl₂ is prevented using a porous diaphragm.
Membrane cell process – similar to the diaphragm cell process, with a Nafion membrane to separate the cathode and anode reactions. It is less expensive than the diaphragm cell process, and it produces a higher quality of NaOH.

An older method for sodium hydroxide production was the LeBlanc process, which produced sodium carbonate, followed by roasting to create carbon dioxide and sodium oxide. This method is no longer used, but it helped to establish sodium hydroxide as an important commodity chemical.

Major producers

In the United States, the major producer of sodium hydroxide is the Dow Chemical Company, which has annual production around 3.7 million tonnes from sites at Freeport, Texas and Plaquemine, Louisiana. Other major US producers include Oxychem, PPG, Olin, Pioneer Companies, Inc. (PIONA), and Formosa. All of these companies use the chloralkali process.

Uses

General applications

Sodium hydroxide is the principal strong base used in the chemical industry. In bulk it is most often handled as an aqueous solution, since solutions are cheaper and easier to handle. It is used to drive for chemical reactions and also for the neutralization of acidic materials.it can be used also as a neutralizing agent in petroleum refining

Experiment

Sodium hydroxide has also been used in conjunction with zinc for creation of the famous "Gold pennies" experiment. A penny is boiled in a solution of NaOH together with some granular zinc metal, the color of the penny will turn silver in about 45 seconds. The penny is then held in the flame of a burner for a few seconds and it turns golden. The reason this happens is that granular zinc dissolves in NaOH to form Zn(OH)₄^2-. This zincate ion becomes reduced to metallic zinc on the surface of a copper penny. Zinc and copper when heated in a flame form brass.

Use in chemical analysis

In analytical chemistry, sodium hydroxide solutions are often used to measure the concentration of acids by titration. Since NaOH is not a primary standard, solutions must first be standardised by titration against a standard such as KHP. Burettes exposed to NaOH should be rinsed out immediately after use to prevent "freezing" of the stopcock!

Soap making

Soap making via saponification is the most traditional chemical process using sodium hydroxide. The Arabs began producing soap in this way in the 7th century, and the same basic process is still used today. It was also featured in Fight Club, a novel and film.

Biodiesel

For the manufacture of biodiesel, sodium hydroxide is used as a catalyst for the transesterification of methanol and triglycerides. This only works with anhydrous sodium hydroxide, because water and lye would turn the fat into soap which would be tainted with methanol.

It is used more often than potassium hydroxide because it costs less, and a smaller quantity is needed for the same results. Another alternative is sodium silicate.

Aluminum etching

Strong bases attack aluminium. This can be useful in etching through a resist or in converting a polished surface to a satin-like finish, but without further passivation such as anodizing or allodizing the surface may become corroded, either under normal use or in severe atmospheric conditions.

Food preparation

Food uses of lye include washing or chemical peeling of fruits and vegetables, chocolate and cocoa processing, caramel color production, poultry scalding, soft drink processing, and thickening ice cream. Olives are often soaked in lye to soften them, while pretzels and German lye rolls are glazed with a lye solution before baking to make them crisp.

Specific foods processed with lye include:

The Scandinavian delicacy known as lutefisk (from lutfisk, "lye fish").
Hominy is dried maize (corn) kernels reconstituted by soaking in lye-water. These expand considerably in size and may be further processed by cooking in hot oil and salting to form corn nuts
Hominy is also known in some areas of the Southeastern United States, as the breakfast food grits, dried and ground into a coarse powder. They are prepared by boiling in water,with the addition of butter and other ingredient to suit the tastes of the preparer.
Sodium hydroxide is also the chemical that causes gelling of egg whites in the production of Century eggs.
German pretzels are poached in a boiling sodium hydroxide solution before baking, which contributes to their unique crust.

Domestic uses

Sodium hydroxide is used in the home as an agent for unblocking drains, provided as a dry crystal (e.g. "Drāno") or as a thick liquid gel. The chemical mechanism employed is the conversion of grease to a form of soap, and so forming a water soluble form to be dissolved by flushing; also decomposing complex molecules such as the protein of hair. Such drain cleaners (and their acidic versions) are highly caustic and should be handled with care (see precautions).

Tissue Digestion

This is a process that was used with farm animals at one time. This process involves the placing of a carcass into a sealed chamber, which then puts the carcass in a mixture of lye and water, which breaks chemical bonds keeping the body intact. This eventually turns the body into a coffee-like liquid, and the only solid remains are bone hulls, which could be crushed between one's fingertips. This seems as if it could be an ecologically friendly way of getting rid of remains when compared with cremation.

Precautions

Gloves and eye protection should be worn when using sodium hydroxide, since there is a high danger of causing chemical burns, permanent injury or scarring, and blindness. A PVC apron is also recommended when concentrated solutions or the solid form are used. It should be stored well away from strong acids such as battery acid. It can create enough heat to ignite flammables (such as alcohols), so it should be added slowly in biodiesel processors. Vinegar is a mild acid that will neutralize lye, a strong base, but do not use vinegar or any other acid to neutralize a strong base that has contacted the skin; this will generate heat and cause a heat burn as well. If lye makes contact with the skin, rinse well with copious amounts of water.

This danger was shown in a scene of the 1999 movie Fight Club, where the character Tyler Durden puts it on the protagonist's freshly kissed hand to create a lip-shaped scar, symbolizing their commitment to the plan that makes up the movie's plot.

External links

References

N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.
Heaton, A. (1996) An Introduction to Industrial Chemistry, 3rd edition, New York:Blackie. ISBN 0-7514-0272-9.
Kirk-Othmer Encyclopedia of Chemical Technology 5th edition (online, account needed), John Wiley & Sons. Accessed November 21st, 2005.

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