Ca No2 2 Compound Name
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| ECHA InfoCard | 100.034.008 |
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| Chemical formula | Ca(NO 2 ) 2 |
| Density | 2.26 grand/cmiii |
| Melting point | 390 °C (734 °F; 663 K) |
| Hazards | |
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| Pictograms |      |
| Bespeak give-and-take | Danger |
| Risk statements | H272, H301, H302, H311, H319, H340, H361, H371, H372, H373, H410 |
| Precautionary statements | P201, P202, P210, P220, P221, P260, P264, P270, P273, P280, P281, P301+P310, P301+P312, P302+P352, P305+P351+P338, P308+P313, P309+P311, P312, P314, P321, P322, P330, P337+P313, P361, P363, P370+P378, P391, P405, P501 |
| Except where otherwise noted, data are given for materials in their standard country (at 25 °C [77 °F], 100 kPa). Infobox references | |
Calcium nitrite is an inorganic chemical compound with the chemical formula Ca(NO
two )
ii . In this compound, every bit in all nitrites, nitrogen is in a +three oxidation state. It has many applications such equally antifreeze, rust inhibitor of steel and wash heavy oil.[ane]
Backdrop [edit]
At room temperature and pressure, the compound is an odorless white or light yellowish pulverisation. Information technology is freely soluble in water with a density of 2.26 g/cm3. Its melting bespeak is of 390 °C and information technology is stable under ordinary conditions of use and storage. It is also characterized for its strong oxidizing character.[ii] Nitrite (III) is a stronger oxidizer than nitrate (Five) considering at valence III information technology has less electrons to recover than nitrate at valence V and so the number of electrons to capture is lower. This facilitates the electronic transfer and increases the kinetic of the oxidation reaction.
Synthesis [edit]
Calcium nitrite tin be produced by different synthesis processes. I is by reacting hydrated lime with NOX gas, which typically comes from a nitric acid plant. At the acid plant, ammonia is burned to produce the NOX gas for acid besides equally calcium nitrite.[3]
Likewise, it tin can be prepared as detailed beneath, forming a solution of sodium nitrite and calcium nitrate; cooling the solution to precipitate sodium nitrate; forming a double salt of calcium nitrite/calcium hydroxide; and in the presence of water, decomposing double salt to grade a solution of calcium nitrite and insolubilize calcium hydroxide. Essentially the part of calcium hydroxide is to carry calcium nitrite; calcium hydroxide forms the insolubilized double salt which can be used to separate from calcium nitrite portions from the solution. Later, the double salt is dissolved liberating calcium nitrite and regenerating the calcium hydroxide.[4]
one. Precipitation of double table salt
- Ca(NO
2 )
2 + Ca(OH)
two + H
2 O → Ca(NO
2 )
2 •Ca(OH)
2 •H
two O
2. Liberation of calcium nitrite
- Ca(NO
ii )
2 •Ca(OH)
2 •H
2 O--H
two O → Ca(NO
2 )
2 (aq) + Ca(OH)
2 + H
ii O
Uses [edit]
Calcium nitrite has a slap-up multifariousness of uses. It tin exist use as antifreeze due to its high solubility, either in solution or pulverisation. It can promote the hydration of minerals in cement using this antifreeze at sub freezing temperature, the operative temperature can be reduced to −twenty °C. It also work equally metallic corrosion inhibitor, so it can protect steel in physical buildings and structures from rust, to extend life of specific buildings.[five] Nitrite's success equally a corrosion inhibitor for the protection of embedded steel in reinforced physical comes from the "smart" behavior of the AFm phase (AFm is shorthand for a family of hydrated calcium aluminate hydrate phases: aluminate-ferrite-monosubstituent phases); normally it stores nitrite in preference to sulfate, carbonate, and hydroxyl ions and so that the nitrite concentrations of pore fluid are depression. However, if chloride ingress occurs in service (from body of water water or de-icing common salt), the AFm undergoes ion exchange, gaining chloride and forming Friedel'due south salt (Cl-AFm), while releasing soluble nitrite ions to the pore fluid. Equally a upshot, the aqueous ratio of [NO2 −]/[Cl−] increases which assures corrosion inhibition of embedded steel.[6] The corrosion inhibition machinery of nitrite in concrete is twofold: on i mitt, the concentration of the very corrosive chloride anions (responsible for the pitting corrosion of steel rebars) in the concrete pore h2o decreases subsequently their uptake into the AFm phases and on the other hand, nitrites as well oxidize the Iron2+ ions present effectually the corroding rebars leading to the precipitation of poorly soluble iron oxy-hydroxides onto the steel surface contributing to its passivation.
Calcium nitrite is widely used in concrete for loftier-rise construction, highways, bridges, railroads, airports, and large-scale hydraulics. Information technology also might enable coastal areas to utilise chloride-containing sea sand in concrete.[7]
Calcium nitrite is also used as a heavy oil detergent and in pharmaceuticals, dyes and metallurgy industries. It can substitute for sodium nitrite, a production often used as a heat transfer fluid in thermal free energy storage units for big air-conditioning or process cooling applications.
Safety [edit]
It is a poisonous inorganic oxidiser, which can non be mixed with organic ammonium salt, acid or cyanide. It has to be kept in heat-proof place, because when the temperature is higher than 220 °C it volition reduce and decompose into nitrous oxide. During transportation it is important to protect information technology from rain and insolation, and protect its package from breakage. Also, the warehouse should be ventilated and dry.[five]
See likewise [edit]
- Calcium nitrate
References [edit]
- ^ "Calcium nitrite". Retrieved six October 2012.
- ^ "Calcium nitrite MSDS canvas; Manufacturers". Retrieved vi October 2012.
- ^ "Calcium nitrite; a definition". Archived from the original on 17 July 2009. Retrieved 6 October 2012.
- ^ Gaidis, James Thou.; Arnold Grand. Rosenberg (23 September 1980). "Process for forming calcium nitrite". U.s.a. Patent.
- ^ a b "Calcium nitrite". Archived from the original on fourteen January 2013. Retrieved half dozen October 2012.
- ^ Balonis, Magdalena; Glasser, Fredrik P. (2011). "Calcium nitrite corrosion inhibitor in Portland cement: Influence of nitrite on chloride binding and mineralogy". Journal of the American Ceramic Lodge. 94 (7): 2230–2241. doi:x.1111/j.1551-2916.2010.04362.x. ISSN 0002-7820.
- ^ "Nitrous acid calcium". Archived from the original on 31 January 2012. Retrieved 6 October 2012.
Ca No2 2 Compound Name,
Source: https://en.wikipedia.org/wiki/Calcium_nitrite
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