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Potassium hydroxide

Potassium hydroxide
Crystal structure of KOH
Pellets of potassium hydroxide
Names
IUPAC name
Potassium hydroxide
Other names
  • Caustic potash
  • Lye
  • Potash lye
  • Potassia
  • Potassium hydrate
  • KOH
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.013.802 Edit this at Wikidata
EC Number
  • 215-181-3
E number E525 (acidity regulators, ...)
RTECS number
  • TT2100000
UNII
UN number 1813
  • InChI=1S/K.H2O/h;1H2/q+1;/p-1 checkY
    Key: KWYUFKZDYYNOTN-UHFFFAOYSA-M checkY
  • InChI=1/K.H2O/h;1H2/q+1;/p-1
    Key: KWYUFKZDYYNOTN-REWHXWOFAT
  • [K+].[OH-]
Properties
KOH
Molar mass 56.105 g·mol−1
Appearance white solid, deliquescent
Odor odorless
Density 2.044 g/cm3 (20 °C)[1]
2.12 g/cm3 (25 °C)[2]
Melting point 410[3][4] °C (770 °F; 683 K)
Boiling point 1,327 °C (2,421 °F; 1,600 K)
85 g/100 mL (-23.2 °C)
97 g/100 mL (0 °C)
121 g/100 mL (25 °C)
138.3 g/100 mL (50 °C)
162.9 g/100 mL (100 °C)[1][5]
Solubility soluble in alcohol, glycerol
insoluble in ether, liquid ammonia
Solubility in methanol 55 g/100 g (28 °C)[2]
Solubility in isopropanol ~14 g / 100 g (28 °C)
Acidity (pKa) 14.7[6]
−22.0·10−6 cm3/mol
1.409 (20 °C)
Thermochemistry
65.87 J/mol·K[2]
79.32 J/mol·K[2][7]
-425.8 kJ/mol[2][7]
-380.2 kJ/mol[2]
Hazards
GHS labelling:
GHS05: CorrosiveGHS07: Exclamation mark[8]
Danger
H290, H302, H314[8]
P280, P305+P351+P338, P310[8]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard ALK: Alkaline
3
0
1
ALK
Flash point nonflammable
Lethal dose or concentration (LD, LC):
273 mg/kg (oral, rat)[10]
NIOSH (US health exposure limits):
PEL (Permissible)
 none[9]
REL (Recommended)
 C 2 mg/m3[9]
IDLH (Immediate danger)
 N.D.[9]
Safety data sheet (SDS) ICSC 0357
Related compounds
Other anions
 Potassium hydrosulfide
Potassium amide
Other cations
 Lithium hydroxide
Sodium hydroxide
Rubidium hydroxide
Caesium hydroxide
Related compounds
 Potassium oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Potassium hydroxide is an inorganic compound with the formula KOH, and is commonly called caustic potash.

Along with sodium hydroxide (NaOH), KOH is a prototypical strong base. It has many industrial and niche applications, most of which utilize its caustic nature and its reactivity toward acids. An estimated 700,000 to 800,000 tonnes were produced in 2005. KOH is noteworthy as the precursor to most soft and liquid soaps, as well as numerous potassium-containing chemicals. It is a white solid that is dangerously corrosive.[11]

Properties and structure

KOH exhibits high thermal stability. Because of this high stability and relatively low melting point, it is often melt-cast as pellets or rods, forms that have low surface area and convenient handling properties. These pellets become tacky in air because KOH is hygroscopic. Most commercial samples are ca. 90% pure, the remainder being water and carbonates.[11] Its dissolution in water is strongly exothermic. Concentrated aqueous solutions are sometimes called potassium lyes. Even at high temperatures, solid KOH does not dehydrate readily.[12]

Structure

At higher temperatures, solid KOH crystallizes in the NaCl crystal structure. The  OH− group is either rapidly or randomly disordered so that it is effectively a spherical anion of radius 1.53 Å (between Cl− and F− in size). At room temperature, the OH− groups are ordered and the environment about the K+ centers is distorted, with K+−OH− distances ranging from 2.69 to 3.15 Å, depending on the orientation of the OH group. KOH forms a series of crystalline hydrates, namely the monohydrate KOH · H2O, the dihydrate KOH · 2H2O and the tetrahydrate KOH · 4H2O.[13]

Reactions

Solubility and desiccating properties

About 112 g of KOH dissolve in 100 mL water at room temperature, which contrasts with 100 g/100 mL for NaOH.[14] Thus on a molar basis, KOH is slightly more soluble than NaOH. Lower molecular-weight alcohols such as methanol, ethanol, and propanols are also excellent solvents. They participate in an acid-base equilibrium. In the case of methanol the potassium methoxide (methylate) forms:[15]

KOH + CH3OH → CH3OK + H2O

Because of its high affinity for water, KOH serves as a desiccant in the laboratory. It is often used to dry basic solvents, especially amines and pyridines.

As a nucleophile in organic chemistry

KOH, like NaOH, serves as a source of OH−, a highly nucleophilic anion that attacks polar bonds in both inorganic and organic materials. Aqueous KOH saponifies esters:

KOH + RCOOR' → RCOOK + R'OH

When R is a long chain, the product is called a potassium soap. This reaction is manifested by the "greasy" feel that KOH gives when touched; fats on the skin are rapidly converted to soap and glycerol.

Molten KOH is used to displace halides and other leaving groups. The reaction is especially useful for aromatic reagents to give the corresponding phenols.[16]

Reactions with inorganic compounds

Complementary to its reactivity toward acids, KOH attacks oxides. Thus, SiO2 is attacked by KOH to give soluble potassium silicates. KOH reacts with carbon dioxide to give potassium bicarbonate:

KOH + CO2 → KHCO3

Manufacture

Historically, KOH was made by adding potassium carbonate to a strong solution of calcium hydroxide (slaked lime). The salt metathesis reaction results in precipitation of solid calcium carbonate, leaving potassium hydroxide in solution:

Ca(OH)2 + K2CO3 → CaCO3 + 2 KOH

Filtering off the precipitated calcium carbonate and boiling down the solution gives potassium hydroxide ("calcinated or caustic potash"). This method of producing potassium hydroxide remained dominant until the late 19th century, when it was largely replaced by the current method of electrolysis of potassium chloride solutions.[11] The method is analogous to the manufacture of sodium hydroxide (see chloralkali process):

2 KCl + 2 H2O → 2 KOH + Cl2 + H2

Hydrogen gas forms as a byproduct on the cathode; concurrently, an anodic oxidation of the chloride ion takes place, forming chlorine gas as a byproduct. Separation of the anodic and cathodic spaces in the electrolysis cell is essential for this process.[17]

Uses

KOH and NaOH can be used interchangeably for a number of applications, although in industry, NaOH is preferred because of its lower cost.

Catalyst for hydrothermal gasification process

In industry, KOH is a good catalyst for hydrothermal gasification process. In this process, it is used to improve the yield of gas and amount of hydrogen in process. For example, production of coke (fuel) from coal often produces much coking wastewater. In order to degrade it, supercritical water is used to convert it to the syngas containing carbon monoxide, carbon dioxide, hydrogen and methane. Using pressure swing adsorption, we could separate various gases and then use power-to-gas technology to convert them to fuel.[18] On the other hand, the hydrothermal gasification process could degrade other waste such as sewage sludge and waste from food factories.

Precursor to other potassium compounds

Many potassium salts are prepared by neutralization reactions involving KOH. The potassium salts of carbonate, cyanide, permanganate, phosphate, and various silicates are prepared by treating either the oxides or the acids with KOH.[11] The high solubility of potassium phosphate is desirable in fertilizers.

Manufacture of soft soaps

The saponification of fats with KOH is used to prepare the corresponding "potassium soaps", which are softer than the more common sodium hydroxide-derived soaps. Because of their softness and greater solubility, potassium soaps require less water to liquefy, and can thus contain more cleaning agent than liquefied sodium soaps.[19]

As an electrolyte

Potassium carbonate, formed from the hydroxide solution leaking from an alkaline battery
Potassium carbonate, formed from the hydroxide solution leaking from an alkaline battery

Aqueous potassium hydroxide is employed as the electrolyte in alkaline batteries based on nickel-cadmium, nickel-hydrogen, and manganese dioxide-zinc. Potassium hydroxide is preferred over sodium hydroxide because its solutions are more conductive.[20] The nickel–metal hydride batteries in the Toyota Prius use a mixture of potassium hydroxide and sodium hydroxide.[21] Nickel–iron batteries also use potassium hydroxide electrolyte.

Food industry

In food products, potassium hydroxide acts as a food thickener, pH control agent and food stabilizer. The FDA considers it generally safe as a direct food ingredient when used in accordance with Good Manufacturing Practices.[22] It is known in the E number system as E525.

Niche applications

Like sodium hydroxide, potassium hydroxide attracts numerous specialized applications, virtually all of which rely on its properties as a strong chemical base with its consequent ability to degrade many materials. For example, in a process commonly referred to as "chemical cremation" or "resomation", potassium hydroxide hastens the decomposition of soft tissues, both animal and human, to leave behind only the bones and other hard tissues.[23] Entomologists wishing to study the fine structure of insect anatomy may use a 10% aqueous solution of KOH to apply this process.[24]

In chemical synthesis, the choice between the use of KOH and the use of NaOH is guided by the solubility or keeping quality of the resulting salt.

The corrosive properties of potassium hydroxide make it a useful ingredient in agents and preparations that clean and disinfect surfaces and materials that can themselves resist corrosion by KOH.[17]

KOH is also used for semiconductor chip fabrication (for example anisotropic wet etching).

Potassium hydroxide is often the main active ingredient in chemical "cuticle removers" used in manicure treatments.

Because aggressive bases like KOH damage the cuticle of the hair shaft, potassium hydroxide is used to chemically assist the removal of hair from animal hides. The hides are soaked for several hours in a solution of KOH and water to prepare them for the unhairing stage of the tanning process. This same effect is also used to weaken human hair in preparation for shaving. Preshave products and some shave creams contain potassium hydroxide to force open the hair cuticle and to act as a hygroscopic agent to attract and force water into the hair shaft, causing further damage to the hair. In this weakened state, the hair is more easily cut by a razor blade.

Potassium hydroxide is used to identify some species of fungi. A 3–5% aqueous solution of KOH is applied to the flesh of a mushroom and the researcher notes whether or not the color of the flesh changes. Certain species of gilled mushrooms, boletes, polypores, and lichens[25] are identifiable based on this color-change reaction.[26]

Safety

Potassium hydroxide is a caustic alkali and its solutions range from irritating to skin and other tissue in low concentrations, to highly corrosive in high concentrations. Eyes are particularly vulnerable, and dust or mist is severely irritating to lungs and can cause pulmonary edema.[27] Safety considerations are similar to those of sodium hydroxide.

The caustic effects arise from being highly alkaline, but if potassium hydroxide is neutralised with a non-toxic acid then it becomes a non-toxic potassium salt. It is approved as a food additive under the code E525.

Potassium hydroxide spillage, stained red by phenolphthalein

See also

References

  1. ^ a b Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton, Florida: CRC Press. p. 4-80. ISBN 0-8493-0486-5.
  2. ^ a b c d e f "potassium hydroxide". chemister.ru. Archived from the original on 18 May 2014. Retrieved 8 May 2018.
  3. ^ Otto, H.W; Seward, R.P. (1964). "Phase equilibria in the potassium hydroxide-sodium hydroxide system". J. Chem. Eng. Data. 9 (4): 507–508. doi:10.1021/je60023a009.
  4. ^ Seward, R.P; Martin, K.E. (1949). "The melting point of potassium hydroxide". J. Am. Chem. Soc. 71 (10): 3564–3565. doi:10.1021/ja01178a530.
  5. ^ Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand. Retrieved 2014-05-29.
  6. ^ Popov, K.; et al. (2002). "7Li, 23Na, 39K and 133Cs NMR comparative equilibrium study of alkali metal cation hydroxide complexes in aqueous solutions. First numerical value for CsOH formation". Inorganic Chemistry Communications. 3 (5): 223–225. doi:10.1016/S1387-7003(02)00335-0. ISSN 1387-7003. Retrieved October 20, 2018.
  7. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
  8. ^ a b c Sigma-Aldrich Co., Potassium hydroxide. Retrieved on 2014-05-18.
  9. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0523". National Institute for Occupational Safety and Health (NIOSH).
  10. ^ Chambers, Michael. "ChemIDplus - 1310-58-3 - KWYUFKZDYYNOTN-UHFFFAOYSA-M - Potassium hydroxide [JAN:NF] - Similar structures search, synonyms, formulas, resource links, and other chemical information". chem.sis.nlm.nih.gov. Archived from the original on 12 August 2014. Retrieved 8 May 2018.
  11. ^ a b c d Schultz, Heinz; Bauer, Günter; Schachl, Erich; Hagedorn, Fritz; Schmittinger, Peter (2005). "Potassium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim, Germany: Wiley-VCH. doi:10.1002/14356007.a22_039. ISBN 978-3-527-30673-2.
  12. ^ Holleman, A. F; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 978-0-12-352651-9.
  13. ^ Wells, A.F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press. ISBN 978-0-19-855370-0.
  14. ^ Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand. Retrieved 2014-05-29.
  15. ^ Platonov, Andrew Y.; Kurzin, Alexander V.; Evdokimov, Andrey N. (2009). "Composition of Vapor and Liquid Phases in the Potassium Hydroxide + Methanol Reaction System at 25 °С". J. Solution Chem. 39 (3): 335–342. doi:10.1007/s10953-010-9505-1. S2CID 97177429.
  16. ^ W. W. Hartman (1923). "p-Cresol". Organic Syntheses. 3: 37. doi:10.15227/orgsyn.003.0037; Collected Volumes, vol. 1, p. 175.
  17. ^ a b Römpp Chemie-Lexikon, 9th Ed. (in German)
  18. ^ Chen, Fu; Li, Xiaoxiao; Qu, Junfeng; Ma, Jing; Zhu, Qianlin; Zhang, Shaoliang (2020-01-13). "Gasification of coking wastewater in supercritical water adding alkali catalyst". International Journal of Hydrogen Energy. 45 (3): 1608–1614. Bibcode:2020IJHE...45.1608C. doi:10.1016/j.ijhydene.2019.11.033. ISSN 0360-3199. S2CID 213336330.
  19. ^ K. Schumann; K. Siekmann (2005). "Soaps". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a24_247. ISBN 978-3527306732.
  20. ^ D. Berndt; D. Spahrbier (2005). "Batteries". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_343. ISBN 978-3527306732.
  21. ^ "Toyota Prius Hybrid 2010 Model Emergency Response Guide" (PDF). Toyota Motor Corporation. 2009. Archived from the original (PDF) on 2012-03-20.
  22. ^ "Compound Summary for CID 14797 - Potassium Hydroxide". PubChem.
  23. ^ Green, Margaret (January 1952). "A RAPID METHOD FOR CLEARING AND STAINING SPECIMENS FOR THE DEMONSTRATION OF BONE". The Ohio Journal of Science. 52 (1): 31–33. hdl:1811/3896.
  24. ^ Thomas Eisner (2003). For the Love of Insects. Harvard University Press. p. 71.
  25. ^ Elix, J.A.; Stocker-Wörgötter, Elfie (2008). "Chapter 7: Biochemistry and secondary metabolites". In Nash III, Thomas H. (ed.). Lichen Biology (2nd ed.). New York: Cambridge University Press. pp. 118–119. ISBN 978-0-521-69216-8.
  26. ^ Testing Chemical Reactions Archived 2009-10-15 at the Wayback Machine at MushroomExpert.com
  27. ^ "Hazardous Substance Fact Sheet: Potassium Hydroxide" (PDF). New Jersey Department of Health. Retrieved 7 October 2024.
Quelle: https://en.wikipedia.org/wiki/Potash_lye