Calcium nitrate

Names
Other names

* Kalksalpeter
* Norgessalpeter
* nitrocalcite
* Norwegian salpeter
* lime nitrate

Identifiers

CAS Number

* 10124-37-5 Y
* 13477-34-4 (tetrahydrate) Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:64205

ChEMBL |

* ChEMBL3183960

ChemSpider |

* 23336 Y

EC Number |

* 233-332-1

PubChem CID

* 24963

RTECS number |

* EW2985000

UNII |

* NF52F38N1N Y
* O8T8H4NBBR (tetrahydrate) Y

UN number | 1454

InChI

* InChI=1S/Ca.2NO3/c;2*2-1(3)4/q+2;2*-1 Y

Key: ZCCIPPOKBCJFDN-UHFFFAOYSA-N Y

* InChI=1/Ca.2NO3/c;2*2-1(3)4/q+2;2*-1

Key: ZCCIPPOKBCJFDN-UHFFFAOYAF

SMILES

* [Ca+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O

Properties

Chemical formula

| Ca(NO

Molar mass |

* 164.088 g/mol (anhydrous)
* 236.15 g/mol (tetrahydrate)

Appearance  | colorless solid (hygroscopic)
Density |

* 2.504 g/cm3 (anhydrous)
* 1.896 g/cm3 (tetrahydrate)

Melting point |

* 561 °C (1,042 °F) (anhydrous)
* 42.7 °C (108.9 °F) (tetrahydrate)

Boiling point |

* decomposes (anhydrous)
* 132 °C (270 °F) (tetrahydrate)

Solubility in water

* anhydrous:

* 1212 g/L (20 °C (68 °F))
* 2710 g/L (40 °C (104 °F))

* tetrahydrate:

* 1050 g/L (0 °C (32 °F))
* 1290 g/L (20 °C (68 °F))
* 3630 g/L (100 °C (212 °F))

Solubility |

* soluble in ammonia
* almost insoluble in nitric acid

Solubility in ethanol |

* 51.4 g/100 g (20 °C (68 °F))
* 62.9 g/100 g (40 °C (104 °F))[citation needed]

Solubility in methanol |

* 134 g/100 g (10 °C (50 °F))
* 144 g/100 g (40 °C (104 °F))
* 158 g/100 g (60 °C (140 °F))[citation needed]

Solubility in acetone | 33.08 g/100g (anhydrous, 25 °C (77 °F))[1]
Acidity (pKa)  | 6.0

Magnetic susceptibility (χ)

| −45.9×10−6 cm3/mol
Structure

Crystal structure

| cubic (anhydrous)
monoclinic (tetrahydrate)
Hazards
Safety data sheet | ICSC 1037
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H272, H302, H315, H319

GHS precautionary statements

| P210, P220, P221, P264, P270, P280, P301+312, P302+352, P305+351+338, P310, P321, P330, P332+313, P337+313, P362, P370+378, P501
NFPA 704 (fire diamond)  |

Flash point | Non-flammable
Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 302 mg/kg (rat, oral)
Related compounds

Other anions

* Calcium sulfate
* Calcium chloride

Other cations

* Magnesium nitrate
* Strontium nitrate
* Barium nitrate

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

N verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Calcium nitrate is an inorganic compound with the formula Ca(NO

2. It forms hydrates Ca(NO

2 * xH
2O. The anhydrous compound, which is rarely encountered, absorbs moisture from the air to give the tetrahydrate. Both anhydrous and hydrated forms are colourless salts. Hydrated calcium nitrate, also called Norgessalpeter (Norwegian salpeter), is mainly used as a component in fertilizers, but it has other applications. Nitrocalcite is the name for a mineral which is a hydrated calcium nitrate that forms as an efflorescence where manure contacts concrete or limestone in a dry environment as in stables or caverns. A variety of related salts are known including calcium ammonium nitrate decahydrate and calcium potassium nitrate decahydrate.[2]

## Contents

* 1 Production and reactivity
* 2 Applications
* 2.1 Use in agriculture
* 2.2 Waste water treatment
* 2.3 Concrete
* 2.4 Latex coagulant
* 2.5 Cold packs
* 2.6 Molten salts for heat transfer and storage
* 3 References

## Production and reactivity

Norgessalpeter was synthesized at Notodden, Norway in 1905 by the Birkeland–Eyde process. Most of the world's calcium nitrate is now made in Porsgrunn. It is produced by treating limestone with nitric acid, followed by neutralization with ammonia:

CaCO
3 \+ 2 HNO
3 → Ca(NO

2 \+ CO
2 \+ H

It is also an intermediate product of the Odda Process:

5(PO

3OH + 10 HNO
3 → 3 H
3PO
4 \+ 5 Ca(NO

2 \+ H

It can also be prepared from an aqueous solution of ammonium nitrate, and calcium hydroxide:

2 NH
4NO
3 \+ Ca(OH)
2 → Ca(NO

2 \+ 2 NH
4OH

Like related alkaline earth metal nitrates, calcium nitrate decomposes upon heating (starting at 500 °C (932 °F)) to release nitrogen dioxide:[2]

2 Ca(NO

2 → 2 CaO + 4 NO
2 \+ O
2 ΔH = 369 kJ/mol

## Applications

### Use in agriculture

The fertilizer grade (15.5-0-0 + 19% Ca) is popular in the greenhouse and hydroponics trades; it contains ammonium nitrate and water, as the "double salt" 5Ca(NO

2 * NH
4NO
3 * 10H2O. This is called calcium ammonium nitrate and often the name calcium nitrate prill is used as it always comes in a prilled (granular) form. Formulations lacking ammonia are also known: Ca(NO

2 * 4H2O (11.9-0-0 + 16.9 Ca) and the water-free 17-0-0 + 23.6 Ca. A liquid formulation (9-0-0 + 11 Ca) is also offered. An anhydrous, air-stable derivative is the urea complex Ca(NO

2 * 4[OC(NH

2], which has been sold as Calurea.[3]

Calcium nitrate is also used to control certain plant diseases. For example, dilute calcium nitrate (and calcium chloride) sprays are used to control bitter pit and cork spot in apple trees.[4]

### Waste water treatment

Waste water treatment unit

Calcium nitrate is used in waste water pre-conditioning for odour emission prevention. The waste water pre-conditioning is based on establishing an anoxic biology in the waste water system. In the presence of nitrate, the metabolism for sulfates stops, thus preventing formation of hydrogen sulfide.[5] Additionally, easily degradable organic matter is consumed, which otherwise can cause anaerobic conditions downstream as well as odour emissions itself. The concept is also applicable for surplus sludge treatment.[6]

### Concrete

Calcium nitrate is used in concrete admixtures to accelerate setting. This use with concrete and mortar is based on two effects. The calcium ion accelerates formation of calcium hydroxide and thus precipitation and setting. This effect is used also in cold weather concreting agents as well as some combined plasticizers.[7] The nitrate ion leads to formation of iron hydroxide, whose protective layer reduces corrosion of the concrete reinforcement.[8]

### Latex coagulant

Calcium nitrate is a very common coagulant in latex production, especially in dipping processes. Dissolved calcium nitrate is a part of the dipping bath solution. The warm former is dipped into the coagulation liquid and a thin film of the dipping liquid remains on the former. When now dipping the former into the latex the calcium nitrate will break up the stabilization of the latex solution and the latex will coagulate on the former.[9]

### Cold packs

The dissolution of calcium nitrate tetrahydrate is highly endothermic (cooling). For this reason, calcium nitrate tetrahydrate is sometimes used for regenerable cold packs.[2]

### Molten salts for heat transfer and storage

Calcium nitrate can be used as a part of molten salt mixtures. Typical are binary mixtures of calcium nitrate and potassium nitrate or ternary mixtures including also sodium nitrate.[10][11][better source needed] Those molten salts can be used to replace thermo oil in concentrated solar power plants for the heat transfer, but mostly those are used in heat storage.[citation needed]

## References

1. ↑ Norwitz, George; Chasan, David E. (1968-05-01). "Application of Infrared Spectroscopy to the Analysis of Inorganic Nitrates" (PDF). Defense Technical Information Centre. https://apps.dtic.mil/sti/pdfs/AD0673124.pdf. Retrieved 2023-01-21.
2. ↑ 2.0 2.1 2.2 "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. 2002. doi:10.1002/14356007.a17_265.
3. ↑ https://archive.org/details/yoa1938/page/497/mode/2up?q=cal-urea Soils and Men, Yearbook of Agriculture 1938, United States Department of Agriculture, p. 497.
4. ↑ "Bitter Pit and Cork Spot". UW-Madison, Dept of Horticulture. https://hort.uwex.edu/articles/bitter-pit-and-cork-spot/.
5. ↑ Bentzen, G; Smith, A; Bennett, D; Webster, N; Reinholt, F; Sletholt, E; Hobson, J (1995). "Controlled dosing of nitrate for prevention of H2S in a sewer network and the effects on the subsequent treatment process". Water Science and Technology 31 (7): 293. doi:10.1016/0273-1223(95)00346-O.
6. ↑ Einarsen, A.M.; ÆeesØy, A.; Rasmussen, A. I.; Bungum, S.; Sveberg, M. (2000). "Biological prevention and removal of hydrogen sulphide in sludge at Lillehammer Wastewater Treatment Plant". Water Sci. Technol. 41 (6): 175–187. doi:10.2166/wst.2000.0107.
7. ↑ Justines, H. (2010) "Calcium Nitrate as a Multifunctional Concrete Admixture" Concrete Magazine, Vol 44, No. 1, p.34. ISSN 0010-5317
8. ↑ Al-Amoudi, Omar S.Baghabra; Maslehuddin, Mohammed; Lashari, A.N; Almusallam, Abdullah A (2003). "Effectiveness of corrosion inhibitors in contaminated concrete". Cement and Concrete Composites 25 (4–5): 439. doi:10.1016/S0958-9465(02)00084-7.
9. ↑ Dafader, N. C.; Jolly, Y. N.; Haque, M. E.; Akhtar, F.; Ahmad, M. U. (April 1999). "The Role of Coagulants on the Preparation of Dipped film from Radiation Vulcanized Natural Rubber Latex". Polymer-Plastics Technology and Engineering 38 (2): 267–274. doi:10.1080/03602559909351576.
10. ↑ European Patent Application EP0049761: Use of a ternary mixture of salts as a heat transmitting medium and/or as a heat storage medium. http://www.freepatentsonline.com/EP0049761A1.html
11. ↑ WIPO Patent Application WO/2014/044652: Use of a calcium potassium nitrate salt for the manufacture of a heat transfer fluid. http://www.freepatentsonline.com/WO2014044652A1.html

* v
* t
* e

Calcium compounds

* CaAl2O4
* CaB6
* CaBr2
* Ca(BrO3)2
* CaC2
* CaCN2
* Ca(CN)2
* CaCO3
* CaC2O4
* CaCl2
* Ca(ClO)2
* Ca(ClO3)2
* CaCrO4
* CaF2
* CaH2
* Ca(HCO3)2
* CaH2S2O6
* CaI2
* Ca(IO3)2
* Ca(MnO4)2
* CaN6
* Ca(NO3)2
* CaO
* CaO2
* Ca(OH)2
* CaP
* CaS
* CaSO3
* CaSO4
* CaSe
* CaSi
* CaSi2
* CaTiO3
* Ca2P2O7
* Ca2SiO4
* Ca3Al2O6
* Ca3(AsO4)2
* Ca3(BO3)2
* Ca3(C6H5O7)2
* Ca3N2
* Ca3P2
* Ca4(PO4)2O
* Ca3(PO4)2
* Ca(H2PO4)2
* CaHPO4
* C36H70CaO4

* v
* t
* e

Salts and covalent derivatives of the nitrate ion

HNO3 |  |  |  | He

|
|
|
|

LiNO3 | Be(NO3)2 | B(NO3)−4 | C  | NO−3,
NH4NO3 | O  | FNO3 | Ne
NaNO3 | Mg(NO3)2 | Al(NO3)3 | Si  | P  | S  | ClONO2 | Ar
KNO3 | Ca(NO3)2 | Sc(NO3)3 | Ti(NO3)4 | VO(NO3)3 | Cr(NO3)3 | Mn(NO3)2 | Fe(NO3)3,
Fe(NO3)2 | Co(NO3)2,
Co(NO3)3 | Ni(NO3)2 | Cu(NO3)2 | Zn(NO3)2 | Ga(NO3)3 | Ge  | As  | Se  | Br  | Kr
RbNO3 | Sr(NO3)2 | Y(NO3)3 | Zr(NO3)4 | Nb  | Mo  | Tc  | Ru  | Rh  | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In  | Sn  | Sb(NO3)3 | Te  | I  | Xe(NO3)2
CsNO3 | Ba(NO3)2 |  | Hf  | Ta  | W  | Re  | Os  | Ir  | Pt  | Au  | Hg2(NO3)2,
Hg(NO3)2 | Tl(NO3)3,
TlNO3 | Pb(NO3)2 | Bi(NO3)3
BiO(NO3) | Po  | At  | Rn
FrNO3 | Ra(NO3)2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La(NO3)3 | Ce(NO3)3,
Ce(NO3)4 | Pr  | Nd(NO3)3 | Pm  | Sm  | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy  | Ho  | Er  | Tm  | Yb  | Lu
Ac(NO3)3 | Th(NO3)4 | Pa  | UO2(NO3)2 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

0.00

(0 votes)

Original source: https://en.wikipedia.org/wiki/Calcium nitrate. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Calcium_nitrate&oldid=4310019"
*[CID]: Compound ID
*[H272]: May intensify fire: oxidizer
*[H302]: Harmful if swallowed
*[H315]: Causes skin irritation
*[H319]: Causes serious eye irritation
*[P210]: Keep away from heat/sparks/open flames/hot surfaces – No smoking
*[P220]: Keep/Store away from clothing/…/combustible materials
*[P221]: Take any precaution to avoid mixing with combustibles
*[P264]: Wash … thoroughly after handling
*[P270]: Do not eat, drink or smoke when using this product
*[P280]: Wear protective gloves/protective clothing/eye protection/face protection
*[P301+312]: IF SWALLOWED: Call a POISON CENTER or doctor/physician if you feel unwell
*[P302+352]: IF ON SKIN: Wash with soap and water
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P310]: Immediately call a POISON CENTER or doctor/physician
*[P321]: Specific treatment (see … on this label)
*[P330]: Rinse mouth
*[P332+313]: If skin irritation occurs: Get medical advice/attention
*[P337+313]: Get medical advice/attention
*[P362]: Take off contaminated clothing and wash before reuse
*[P370+378]: In case of fire: Use … for extinction
*[P501]: Dispose of contents/container to …
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template