ca(oh)2

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Calcium hydroxide
Calcium hydroxide
Names
IUPAC name

Calcium hydroxide

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Other names
  • Slaked lime
  • Milk of lime
  • Calcium(II) hydroxide
  • Pickling lime
  • Hydrated lime
  • Portlandite
  • Calcium hydrate
  • Calcium dihydroxide
Identifiers

CAS Number

  • 1305-62-0 check

3D model (JSmol)

  • Interactive image
  • Interactive image
ChEBI
  • CHEBI:31341 check
ChemSpider
  • 14094 check
ECHA InfoCard 100.013.762 Edit this at Wikidata
EC Number
  • 215-13
E number E526 (acidity regulators, ...)

Gmelin Reference

846915
KEGG
  • D01083 check

PubChem CID

  • 14777
RTECS number
  • EW2800000
UNII
  • PF5DZW74VN check

CompTox Dashboard (EPA)

  • DTXSID7034410 Edit this at Wikidata

InChI

  • InChI=1S/Ca.2H2O/h;2*1H2/q+2;;/p-2 check

    Key: AXCZMVOFGPJBDE-UHFFFAOYSA-L check

  • InChI=1/Ca.2H2O/h;2*1H2/q+2;;/p-2

    Key: AXCZMVOFGPJBDE-NUQVWONBAD

SMILES

  • [Ca+2].[OH-].[OH-]

  • [OH-].[OH-].[Ca+2]

Properties

Chemical formula

Ca(OH)2
Molar mass 74.093 g/mol
Appearance White powder
Odor Odorless
Density 2.211 g/cm3, solid
Melting point 580 °C (1,076 °F; 853 K) (loses water, decomposes)

Solubility in water

  • 1.89 g/L (0 °C)
  • 1.73 g/L (20 °C)
  • 0.66 g/L (100 °C)
  • (retrograde solubility, i.e., unusually decreasing with T)

Solubility product (Ksp)

5.02×10−6 [1]
Solubility
  • Soluble in glycerol and acids.
  • Insoluble in ethanol.[citation needed]
Acidity (pKa) 12.63 (first OH), 11.57 (second OH)[2][3] [clarification needed]

Magnetic susceptibility (χ)

−22.0·10−6 cm3/mol

Refractive index (nD)

1.574
Structure

Crystal structure

Hexagonal, hP3[4]

Space group

P3m1 No. 164

Lattice constant

a = 0.35853 nm, c = 0.4895 nm

Thermochemistry

Std molar
entropy (S298)

83 J·mol−1·K−1[5]

Std enthalpy of
formation fH298)

−987 kJ·mol−1[5]
Hazards
GHS labelling:

Pictograms

GHS05: Corrosive GHS07: Exclamation mark

Signal word

Danger

Hazard statements

H314, H335, H402

Precautionary statements

P261, P280, P305+P351+P338
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 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code

3

Flash point Non-flammable
Lethal dose or concentration (LD, LC):
7340 mg/kg (oral, rat)
7300 mg/kg (mouse)
NIOSH (US health exposure limits):

PEL (Permissible)

TWA 15 mg/m3 (total) 5 mg/m3 (resp.)[7]

REL (Recommended)

TWA 5 mg/m3[7]

IDLH (Immediate danger)

N.D.[7]
Safety data sheet (SDS) [6]
Related compounds

Other cations

Magnesium hydroxide
Strontium hydroxide
Barium hydroxide

Related bases

Calcium oxide
Supplementary data page
Calcium hydroxide (data page)

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

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Infobox references

Calcium hydroxide (traditionally called slaked lime) is an inorganic compound with the chemical formula Ca(OH)2. It is a colorless crystal or white powder and is produced when quicklime (calcium oxide) is mixed with water. It has many names including hydrated lime, caustic lime, builders' lime, slaked lime, cal, and pickling lime. Calcium hydroxide is used in many applications, including food preparation, where it has been identified as E number E526. Limewater, also called milk of lime, is the common name for a saturated solution of calcium hydroxide.

Properties[edit]

Calcium hydroxide is poorly soluble in water, with a retrograde solubility increasing from 0.66 g/L at 100 °C to lớn 1.89 g/L at 0 °C. With a solubility product Ksp of 5.02×10−6 at 25 °C[1][clarification needed], its dissociation in water is large enough that its solutions are basic according to lớn the following dissolution reaction:

Ca(OH)2 → Ca2+ + 2 OH

At ambient temperature, calcium hydroxide (portlandite) dissolves in water to lớn produce an alkaline solution with a pH of about 12.5. Calcium hydroxide solutions can cause chemical burns. At high pH values due to lớn a common-ion effect with the hydroxide anion, its solubility drastically decreases. This behavior is relevant to lớn cement pastes. Aqueous solutions of calcium hydroxide are called limewater and are medium-strength bases, which react with acids and can attack some metals such as aluminium[citation needed] (amphoteric hydroxide dissolving at high pH), while protecting other metals, such as iron and steel, from corrosion by passivation of their surface. Limewater turns milky in the presence of carbon dioxide due to lớn the formation of insoluble calcium carbonate, a process called carbonatation:

Ca(OH)2 + CO2 → CaCO3 + H2O

When heated to lớn 512 °C, the partial pressure of water in equilibrium with calcium hydroxide reaches 101 kPa (normal atmospheric pressure), which decomposes calcium hydroxide into calcium oxide and water:[8]

Ca(OH)2 → CaO + H2O

Calcium hydroxide reacts with hydrogen chloride to lớn first give calcium hydroxychloride and then calcium chloride.

Structure, preparation, occurrence[edit]

SEM image of fractured hardened cement paste, showing plates of calcium hydroxide and needles of ettringite (micron scale)

Calcium hydroxide adopts a polymeric structure, as tự all metal hydroxides. The structure is identical to lớn that of Mg(OH)2 (brucite structure); i.e., the cadmium iodide motif. Strong hydrogen bonds exist between the layers.[9]

Calcium hydroxide is produced commercially by treating (slaking) lime with water:

CaO + H2O → Ca(OH)2

In the laboratory it can be prepared by mixing aqueous solutions of calcium chloride and sodium hydroxide. The mineral size, portlandite, is relatively rare but can be found in some volcanic, plutonic, and metamorphic rocks. It has also been known to lớn arise in burning coal dumps.

The positively charged ionized species CaOH+ has been detected in the atmosphere of S-type stars.[10]

Retrograde solubility[edit]

According to lớn Hopkins and Wulff (1965),[11] the decrease of calcium hydroxide solubility with temperature was known since the works of Marcellin Berthelot (1875)[12] and Julius Thomsen (1883)[13] (see Thomsen–Berthelot principle), when the presence of ions in aqueous solutions was still questioned. Since, it has been studied in detail by many authors, a.o., Miller and Witt (1929)[14] or Johnston and Grove (1931)[15] and refined many times (e.g., Greenberg and Copeland (1960);[16] Hopkins and Wulff (1965);[11] Seewald and Seyfried (1991);[17] Duchesne and Reardon (1995)[18]).

The reason for this rather uncommon behavior is that the dissolution of calcium hydroxide in water involves an entropy decrease, due to lớn the ordering of water molecules around the doubly charged calcium ion, This counter-intuitive temperature dependence of the solubility is referred to lớn as "retrograde" or "inverse" solubility. The variably hydrated phases of calcium sulfate (gypsum, bassanite and anhydrite) also exhibit a slight retrograde solubility due to lớn the presence of the calcium ion. However, other calcium salts lượt thích calcium chloride show an increase in solubility since the enthalpy change is larger and dominates the không tính phí energy change during dissolution. In all cases, the dissolution is exothermic.[citation needed]

Uses[edit]

Calcium hydroxide is commonly used to lớn prepare lime mortar.

One significant application of calcium hydroxide is as a flocculant, in water and sewage treatment. It forms a fluffy charged solid that sida in the removal of smaller particles from water, resulting in a clearer product. This application is enabled by the low cost and low toxicity of calcium hydroxide. It is also used in fresh-water treatment for raising the pH of the water ví that pipes will not corrode where the base water is acidic, because it is self-regulating and does not raise the pH too much.[citation needed]

It is also used in the preparation of ammonia gas (NH3), using the following reaction:

Ca(OH)2 + 2 NH4Cl → 2 NH3 + CaCl2 + 2 H2O

Another large application is in the paper industry, where it is an intermediate in the reaction in the production of sodium hydroxide. This conversion is part of the causticizing step in the Kraft process for making pulp.[9] In the causticizing operation, burned lime is added to lớn green liquor, which is a solution primarily of sodium carbonate and sodium sulfate produced by dissolving smelt, which is the molten size of these chemicals from the recovery furnace.[citation needed]

In orchard crops, calcium hydroxide is used as a fungicide. Applications of 'lime water' prevent the development of cankers caused by the fungal pathogen Neonectria galligena. The trees are sprayed when they are dormant in winter to lớn prevent toxic burns from the highly reactive calcium hydroxide. This use is authorised in the European Union and the United Kingdom under Basic Substance regulations.[19]

Calcium hydroxide is used in dentistry, primarily in the specialty of endodontics.

Food industry[edit]

Because of its low toxicity and the mildness of its basic properties, slaked lime is widely used in the food industry:

  • In USDA certified food production in plants and livestock[20]
  • To clarify raw juice from sugarcane or sugar beets in the sugar industry (see carbonatation)
  • To process water for alcoholic beverages and soft drinks
  • To increase the rate of Maillard reactions (pretzels)[21]
  • Pickle cucumbers and other foods
  • To make Chinese century eggs
  • In maize preparation: removes the cellulose hull of maize kernels (see nixtamalization)
  • To clear a brine of carbonates of calcium and magnesium in the manufacture of salt for food and pharmaceutical uses
  • In fortifying (Ca supplement) fruit drinks, such as orange juice, and infant formula
  • As a digestive aid (called Choona, used in India in paan, a mixture of areca nuts, calcium hydroxide and a variety of seeds wrapped in betel leaves)
  • As a substitute for baking soda in making papadam
  • In the removal of carbon dioxide from controlled atmosphere produce storage rooms
  • In the preparation of mushroom growing substrates[22]

Native American uses[edit]

Dry untreated maize (left), and treated maize (right) after boiling in water with calcium hydroxide (15 ml, or 1 tbsp, lime for 500 g of corn) for 15 minutes

In Nahuatl, the language of the Aztecs, the word for calcium hydroxide is nextli. In a process called nixtamalization, maize is cooked with nextli to lớn become nixtamal, also known as hominy. Nixtamalization significantly increases the bioavailability of niacin (vitamin B3), and is also considered tastier and easier to lớn digest. Nixtamal is often ground into a flour, known as masa, which is used to lớn make tortillas and tamales.[citation needed]

In chewing coca leaves, calcium hydroxide is usually chewed alongside to lớn keep the alkaloid stimulants chemically available for absorption by the body toàn thân. Similarly, Native Americans traditionally chewed tobacco leaves with calcium hydroxide derived from burnt mollusc shells to lớn enhance the effects. It has also been used by some indigenous American tribes as an ingredient in yopo, a psychedelic snuff prepared from the beans of some Anadenanthera species.[23]

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Asian uses[edit]

Calcium hydroxide is typically added to lớn a bundle of areca nut and betel leaf called "paan" to lớn keep the alkaloid stimulants chemically available to lớn enter the bloodstream via sublingual absorption.

It is used in making naswar (also known as nass or niswar), a type of dipping tobacco made from fresh tobacco leaves, calcium hydroxide (chuna or soon), and wood ash. It is consumed most in the Pathan diaspora, Afghanistan, Pakistan, India and Bangladesh. Villagers also use calcium hydroxide to lớn paint their mud houses in Afghanistan, Pakistan and India.

Health risks[edit]

Unprotected exposure to lớn Ca(OH)2, as with any strong base, can cause severe skin irritation, chemical burns, blindness, lung damage or rashes.[6]

See also[edit]

  • Baralyme (carbon dioxide absorbent)
  • Cement
  • Lime mortar
  • Lime plaster
  • Plaster
  • Magnesium hydroxide (less alkaline due to lớn a lower solubility product)
  • Soda lime (carbon dioxide absorbent)
  • Whitewash
  • On Food and Cooking

References[edit]

  1. ^ a b John Rumble (18 June 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
  2. ^ "Sortierte Liste: pKb-Werte, nach Ordnungszahl sortiert. – Das Periodensystem online".
  3. ^ ChemBuddy dissociation constants pKa and pKb
  4. ^ Petch, H. E. (1961). "The hydrogen positions in portlandite, Ca(OH)2, as indicated by the electron distribution". Acta Crystallographica. 14 (9): 950–957. doi:10.1107/S0365110X61002771.
  5. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
  6. ^ a b "MSDS Calcium hydroxide" (PDF). Archived from the original (PDF) on 25 March 2012. Retrieved 21 June 2011.
  7. ^ a b c NIOSH Pocket Guide to lớn Chemical Hazards. "#0092". National Institute for Occupational Safety and Health (NIOSH).
  8. ^ Halstead, P.. E.; Moore, A. E. (1957). "The Thermal Dissociation of Calcium Hydroxide". Journal of the Chemical Society. 769: 3873. doi:10.1039/JR9570003873.
  9. ^ a b Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
  10. ^ Jørgensen, Uffe G. (1997), "Cool Star Models", in nài Dishoeck, Ewine F. (ed.), Molecules in Astrophysics: Probes and Processes, International Astronomical Union Symposia. Molecules in Astrophysics: Probes and Processes, vol. 178, Springer Science & Business Media, p. 446, ISBN 079234538X.
  11. ^ a b Hopkins, Harry P..; Wulff, Claus A. (1965). "The solution thermochemistry of polyvalent electrolytes. I. Calcium hydroxide". The Journal of Physical Chemistry. 69 (1): 6–8. doi:10.1021/j100885a002. ISSN 0022-3654.
  12. ^ Berthelot, M. (1875). Dissolution des acides et des alcalis. [Dissolution of acids and alkalis]. In: Annales de Chimie et de Physique. Vol. 4, pp. 445–536.
  13. ^ Thomsen J. (1883). Thermochemische untersuchungen [Thermochemical studies]. Vol. III, Johann Ambrosius Barth Verlag, Leipzig.
  14. ^ Miller, L. B.; Witt, J. C. (1929). "Solubility of calcium hydroxide". The Journal of Physical Chemistry. 33 (2): 285–289. doi:10.1021/j150296a010. ISSN 0092-7325.
  15. ^ Johnston, John.; Grove, Clinton. (1931). "The solubility of calcium hydroxide in aqueous salt solutions". Journal of the American Chemical Society. 53 (11): 3976–3991. doi:10.1021/ja01362a009. ISSN 0002-7863.
  16. ^ Greenberg, S. A.; Copeland, L. E. (1960). "The thermodynamic functions for the solution of calcium hydroxide in water". The Journal of Physical Chemistry. 64 (8): 1057–1059. doi:10.1021/j100837a023. ISSN 0022-3654.
  17. ^ Seewald, Jeffrey S.; Seyfried, William E. (1991). "Experimental determination of portlandite solubility in H2O and acetate solutions at 100–350 °C and 500 bars: Constraints on calcium hydroxide and calcium acetate complex stability". Geochimica et Cosmochimica Acta. 55 (3): 659–669. Bibcode:1991GeCoA..55..659S. doi:10.1016/0016-7037(91)90331-X. ISSN 0016-7037.
  18. ^ Duchesne, J.; Reardon, E.J. (1995). "Measurement and prediction of portlandite solubility in alkali solutions". Cement and Concrete Research. 25 (5): 1043–1053. doi:10.1016/0008-8846(95)00099-X. ISSN 0008-8846.
  19. ^ European Union (13 May 2015). "COMMISSION IMPLEMENTING REGULATION (EU) 2015/762 of 12 May năm ngoái approving the basic substance calcium hydroxide in accordance with Regulation (EC) No 1107/2009 of the European Parliament and of the Council concerning the placing of plant protection products on the market, and amending the Annex to lớn Commission Implementing Regulation (EU) No 540/2011". Retrieved 12 May 2022.
  20. ^ Pesticide Research Institute for the USDA National Organic Program (23 March 2015). "Hydrated Lime: Technical Evaluation Report" (PDF). Agriculture Marketing Services. Retrieved 17 July 2019.
  21. ^ Borsook, Alec (6 August 2015). "Cooking with Alkali". Nordic Food Lab.
  22. ^ "Preparation of Mushroom Growing Substrates". North American Mycological Association. Retrieved 8 July 2021.
  23. ^ de Smet, Peter A. G. M. (1985). "A multidisciplinary overview of intoxicating snuff rituals in the Western Hemisphere". Journal of Ethnopharmacology. 3 (1): 3–49. doi:10.1016/0378-8741(85)90060-1. PMID 3887041.

External links[edit]

  • National Lime Association. "Properties of typical commercial lime products. Solubility of calcium hydroxide in water" (PDF). lime.org. Retrieved 18 June 2021.
  • National Organic Standards Board Technical Advisory Panel (4 April 2002). "NOSB TAP Review: Calcium Hydroxide" (PDF). Organic Materials Review Institute. Archived from the original (.PDF) on 31 October 2007. Retrieved 5 February 2008.
  • CDC – NIOSH Pocket Guide to lớn Chemical Hazards – Calcium Hydroxide
  • MSDS Data Sheet