Hubbry Logo
Zinc phosphateZinc phosphateMain
Open search
Zinc phosphate
Community hub
Zinc phosphate
logo
7 pages, 0 posts
0 subscribers
Be the first to start a discussion here.
Be the first to start a discussion here.
Zinc phosphate
Zinc phosphate
Zinc phosphate
View on Wikipedia
from Wikipedia
Zinc phosphate
Zinc phosphate
Zinc phosphate
Names
IUPAC name
Zinc phosphate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.040 Edit this at Wikidata
RTECS number
  • TD0590000
UNII
  • InChI=1S/2H3O4P.3Zn/c2*1-5(2,3)4;;;/h2*(H3,1,2,3,4);;;/q;;3*+2/p-6 checkY
    Key: LRXTYHSAJDENHV-UHFFFAOYSA-H checkY
  • InChI=1/2H3O4P.3Zn/c2*1-5(2,3)4;;;/h2*(H3,1,2,3,4);;;/q;;3*+2/p-6
    Key: LRXTYHSAJDENHV-CYFPFDDLAR
  • [Zn+2].[Zn+2].[Zn+2].[O-]P([O-])(=O)[O-].[O-]P([O-])([O-])=O
Properties
H4O12P2Zn3
Molar mass 454.11 g·mol−1
Appearance white solid
Density 3.998 g/cm3
Melting point 900 °C (1,650 °F; 1,170 K)
Boiling point 158 °C (316 °F; 431 K)
insoluble
−141.0·10−6 cm3/mol
1.595
Structure
monoclinic
Thermochemistry
−2891.2 ± 3.3
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 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
2
0
0
Flash point Non-flammable
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Zinc phosphate is an inorganic compound with the formula Zn3(PO4)2. This white powder is widely used as a corrosion resistant coating on metal surfaces either as part of an electroplating process or applied as a primer pigment (see also red lead). It has largely displaced toxic materials based on lead or chromium, and by 2006 it had become the most commonly used corrosion inhibitor.[1][2] Zinc phosphate coats better on a crystalline structure than bare metal, so a seeding agent is often used as a pre-treatment. One common agent is sodium pyrophosphate.[3]

Minerals

[edit]

Natural forms of zinc phosphate include minerals hopeite and parahopeite. A somewhat similar mineral is natural hydrous zinc phosphate called tarbuttite, Zn2(PO4)(OH). Both are known from oxidation zones of Zn ore beds and were formed through oxidation of sphalerite by the presence of phosphate-rich solutions. The anhydrous form has not yet been found naturally.

Use

[edit]

Dentistry

[edit]

Zinc phosphate cement is the classic dental cement par excellence. It is commonly used for luting permanent metal and zirconium dioxide[4][5][6][7][8][9] restorations and as a base for dental restorations. Zinc phosphate cement is used for cementation of inlays, crowns, bridges, and orthodontic appliances and occasionally as a temporary restoration.

It is prepared by mixing zinc oxide (ZnO) and magnesium oxide (MgO) powders with a liquid consisting principally of phosphoric acid, water, and buffers. It is the standard cement to measure against. It has the longest track record of use in dentistry.

In recent years, newer adhesive cements on a different chemical basis have been added (e.g. glass ionomer cement), but they have not displaced the classic phosphate cement, which continues to hold its own in the dental market with its simple and safe processing and good price-performance ratio. Zinc phosphate cement has only a low flexural strength and it does not stick to the dentin (it is a cement and not an adhesive).

Zinc phosphate cement has high compressive strength, low film thickness, minimal setting shrinkage and thermal expansion and is biocompatible. Compared to other luting materials such as glass ionomer cement or composites, zinc phosphate cement is less sensitive to moisture. The excess produced during the cementation of dental restorations can be easily removed.

Zinc phosphate cement has a high adhesive capacity to the tooth, metal, or even zirconium oxide.

Despite its strong acidity, zinc phosphate cement does not damage the pulp (or the tooth nerve) during the setting phase. It is therefore used as liner to protect the pulp under composite fillings.

Well-known dental brands in Germany and the world for zinc phosphate cement are Harvard cement and Hoffmann's cement. Otto Hoffmann invented this cement in 1892 and had it patented. Until the beginning of the First World War, he had a worldwide monopoly position with his cement.

References

[edit]
[edit]
Revisions and contributorsEdit on WikipediaRead on Wikipedia

Zinc phosphate

View on Grokipedia
from Grokipedia
Zinc phosphate is an with the Zn₃(PO₄)₂ and a molecular weight of 386.1 g/mol, typically appearing as a white, odorless crystalline powder. It is sparingly soluble in and commonly used in its pure form or as hydrates like the tetrahydrate. This compound occurs naturally in minerals such as hopeite and tarbuttite, and it is produced industrially for various applications. In , zinc phosphate serves as one of the oldest and most reliable luting , valued for its high (around 55-110 MPa), low solubility in oral fluids, and neutral after setting, which minimizes pulpal irritation. The forms through an acid-base reaction between oxide powder and liquid, resulting in a aluminophosphate matrix that provides strong mechanical retention for crowns, bridges, and orthodontic appliances. Despite its lack of chemical adhesion to tooth structure, it remains a standard due to its durability and ease of use when properly mixed. Beyond , zinc is widely employed as an anticorrosion in primers and paints, forming a protective layer on metal surfaces like to inhibit through chemical conversion. This application enhances the and longevity of coatings in industrial settings, such as automotive and marine environments, due to its non-toxic nature compared to alternatives like lead-based . It also finds use in as a bulking agent and in some glass enamels for improved chemical durability. Regarding safety, zinc phosphate exhibits low acute oral toxicity (LD50 >5000 mg/kg in rats) and is generally biocompatible in set dental forms, though freshly mixed versions can be mildly cytotoxic to pulp cells. It is classified as very toxic to aquatic life, necessitating careful handling to prevent environmental release.

Properties

Physical properties

Zinc phosphate appears as a white, odorless crystalline powder. Its is 386.11 g/mol. The compound has a of 3.998 g/cm³ at 15 °C. Zinc phosphate decomposes at approximately 900 °C without melting. The following properties refer to the anhydrous form unless otherwise specified. It is practically insoluble in (Ksp ≈ 10^{-36} at 25 °C).

Chemical properties

Zinc phosphate is an ionic compound with the formula Zn₃(PO₄)₂, consisting of Zn²⁺ cations and PO₄³⁻ anions, formed as a salt from zinc oxide and . The compound exhibits high chemical stability in neutral and alkaline environments, maintaining its structure without significant degradation under ambient conditions. In strong acidic media, however, zinc phosphate decomposes, releasing and soluble zinc species through and dissolution of the lattice. Aqueous suspensions of zinc phosphate display slightly acidic values, typically around 6-7, attributable to the of Zn²⁺ ions according to the equilibrium Zn²⁺ + H₂O ⇌ ZnOH⁺ + H⁺, where the hydrolysis constant K_h ≈ 10^{-9} (pK_h ≈ 9). Zinc phosphate is non-flammable and does not support combustion under standard conditions. It lacks significant activity at ambient temperatures and pressures, remaining inert toward atmospheric oxygen or common reductants without external catalysts.

Structure and production

Crystal structure

Zinc phosphate, with the chemical formula , exists in several polymorphic forms in its state, each characterized by distinct s that influence its stability and applications. The α-form, which is the most commonly studied polymorph, crystallizes in the monoclinic system with C2/c (No. 15). The unit cell parameters for this form are a = 8.14 , b = 5.63 , c = 15.04 , and β = 105.1°, containing four formula units (Z = 4). In this structure, the lattice is composed of a three-dimensional framework where ions occupy two types of tetrahedral sites coordinated by oxygen atoms, with average Zn–O bond lengths of approximately 1.96–1.98 . The phosphate groups form slightly distorted PO₄ tetrahedra with average P–O bond lengths of about 1.53 , linking the zinc tetrahedra through shared vertices to create a dense, interconnected network. A β-polymorph of anhydrous Zn₃(PO₄)₂ has also been identified, crystallizing in the monoclinic space group P2₁/c (No. 14) with unit cell parameters a = 9.393 Å, b = 9.170 Å, c = 8.686 Å, and β = 125.73°. This form features zinc ions in tetrahedral and pentacoordinate environments, with one site tetrahedrally coordinated by four oxygen atoms and two sites pentacoordinate by five oxygen atoms, interconnected by PO₄ tetrahedra, though the specific arrangement leads to differences in thermal stability compared to the α-form. Other polymorphs, such as the γ-form, exhibit related monoclinic structures but with variations in cation coordination, including some five- or six-coordinated zinc sites in solid solutions. These structural features, particularly the coordination of zinc by phosphate oxygen atoms, contribute to the compound's rigidity and its role in corrosion-resistant coatings and cements. In nature, anhydrous Zn₃(PO₄)₂ does not occur; instead, zinc phosphate is found primarily in hydrated forms, such as the mineral hopeite, Zn₃(PO₄)₂·4H₂O. Hopeite crystallizes in the orthorhombic system with Pnma (No. 62), featuring unit cell parameters a ≈ 10.63 , b ≈ 18.37 , and c ≈ 5.02 . Its structure consists of layers of [Zn(PO₄)] units interconnected by hydrated zinc octahedra, with molecules stabilizing the framework through hydrogen bonding. A triclinic polymorph, parahopeite, represents another hydrated variant but shares similar tetrahedral zinc-phosphate coordination motifs. These hydrated structures underscore the compound's tendency to incorporate in natural settings, contrasting with the synthetic anhydrous forms used industrially.

Synthesis

Zinc phosphate, an important used in various applications, has seen significant development in its synthesis methods since the late . Initially explored for dental cements around , its production as an anticorrosive gained prominence in the early , particularly as a safer alternative to lead-based pigments in paints and coatings. By the early , regulatory pressures on lead led to widespread replacement of lead chromates and red lead with zinc phosphate in anticorrosive formulations, driven by its non-toxic profile and effective performance. A common laboratory method for synthesizing zinc phosphate involves the reaction of zinc oxide with . The balanced equation is: 3ZnO+2H3PO4→Zn3(PO4)2+3H2O3\text{ZnO} + 2\text{H}_3\text{PO}_4 \rightarrow \text{Zn}_3(\text{PO}_4)_2 + 3\text{H}_2\text{O} This acid-base reaction typically occurs in an aqueous medium at controlled temperatures, often around 60-80°C, to yield the dihydrate form, Zn₃(PO₄)₂·2H₂O, which can be filtered, washed, and dried. The process allows for high purity when using reagent-grade precursors, and variations in and heating duration influence the and hydration state of the product. In industrial production, zinc phosphate is frequently prepared via from solutions of salts, such as or , and alkali metal phosphates like . For example, mixing (ZnSO₄) with (Na₃PO₄) results in the insoluble zinc phosphate precipitating out, followed by , washing to remove soluble byproducts, and if product is desired. This method is scalable and cost-effective, utilizing readily available industrial chemicals, and is optimized for pigment-grade material with specific particle sizes (typically 5-20 μm) to enhance dispersibility in coatings. To promote the formation of crystalline structures during synthesis, particularly for applications requiring adherent coatings, seeding agents such as are employed. These agents facilitate on substrates, leading to uniform, crystalline zinc phosphate layers rather than amorphous deposits, improving the overall quality and performance of the synthesized material. Synthesis conditions are often tailored to achieve the orthorhombic of hopeite, the common polymorph of zinc phosphate.

Natural occurrence

Minerals

Zinc phosphate minerals are rare secondary phases that occur in the oxidized zones of zinc ore deposits, where they form through the weathering of primary zinc sulfides in the presence of phosphate ions. Hopeite, with the composition Zn₃(PO₄)₂·4H₂O, crystallizes in the orthorhombic system and typically appears as colorless to white or yellowish prismatic crystals with a vitreous to pearly luster. It is notably found at the type locality of (Vieille Montagne), , as well as in (Broken Hill), ; Broken Hill, , ; and the Tip Top Mine in the Black Hills, South Dakota, . Parahopeite is a triclinic polymorph of hopeite, sharing the same formula Zn₃(PO₄)₂·4H₂O, and forms transparent, colorless to golden-brown tabular or prismatic crystals. It was first identified at the type locality of , , and occurs at additional sites such as Martins Well, , and the and areas in , . Tarbuttite, a related hydroxy with the formula Zn₂(PO₄)(OH), adopts a triclinic and manifests as colorless, white, or tinted (yellow, green, or brown) fibrous or radiating aggregates with a vitreous luster. It is reported from its type locality at (), , as well as , , and , , . These zinc phosphate minerals are infrequently encountered due to their specific formation conditions and are often associated with other secondary zinc species like hemimorphite and in such deposits.

Geological formation

Zinc phosphate minerals primarily form as secondary phases in the oxidized zones of ore deposits, where primary (ZnS) undergoes under atmospheric conditions. This process involves the oxidation of minerals, releasing ions (Zn²⁺) into solution, which then react with ions derived from circulating fluids to precipitate hydrated phosphates. Such formations are commonly observed in deposits, like those at , , where oxidative alteration creates favorable conditions for phosphate mineralization. The geochemical interaction driving this precipitation occurs when phosphate-rich encounters mobilized zinc ions from the of and associated sulfides. In these environments, phosphates may originate from the dissolution of nearby or other P-bearing , or from external inputs like guano-derived solutions, leading to the and deposition of zinc phosphate phases at low temperatures. This secondary enrichment is enhanced in zones of high water-table fluctuation, where evaporative concentration promotes crystallization. Zinc phosphates also develop as secondary minerals in arid, phosphate-bearing geological settings, such as complex pegmatites and hydrothermal s. In pegmatites, late-stage hydrothermal fluids rich in interact with primary silicates or oxides, altering them through metasomatic processes to form assemblages. Similarly, in hydrothermal systems, fluid circulation along fractures facilitates the remobilization and redeposition of and , often in environments with limited moisture that favor persistent secondary phases. For instance, minerals like hopeite emerge in such contexts as products of these interactions. No primary anhydrous zinc phosphate minerals are known to occur in , with all documented examples being hydrated secondary formed under surface or near-surface conditions.

Applications

Corrosion inhibition

Zinc phosphate is widely employed as a primer pigment in anticorrosive paints and as a in the phosphating process applied to and aluminum surfaces to enhance resistance. In paint formulations, it serves as an inhibitive that improves the protective performance of organic coatings, with optimal loading around 30% by volume in systems. For metal pretreatment, the phosphating process involves immersing or spraying the substrate in a zinc phosphate solution, forming a polycrystalline layer that promotes for subsequent paints or serves as a standalone barrier. The inhibition mechanism of involves both physical and chemical actions. Physically, it creates an insoluble barrier layer that limits the of corrosive like and oxygen to the metal substrate. Chemically, ions adsorb onto the metal surface, passivating it by forming a protective film that inhibits active sites for ; this is often enhanced by slight in aqueous environments, releasing inhibitive . In phosphating applications, a seeding step using colloidal agents like titanium conditions the surface to promote uniform crystalline film growth, ensuring better coverage and durability on substrates such as galvanized or aluminum. Due to the toxicity and carcinogenic risks of traditional inhibitors like chromates and , zinc phosphate has become the predominant non-toxic alternative in corrosion-protective coatings since the early . This shift was driven by regulatory pressures to eliminate , positioning zinc phosphate as a safer option that maintains effective inhibition without environmental hazards. Electrochemical principles underpin zinc phosphate's rust prevention on ferrous and non-ferrous substrates. It primarily inhibits the anodic dissolution of the base metal by elevating the corrosion potential and reducing the rate of iron or aluminum oxidation through phosphate adsorption. Cathodically, it suppresses oxygen reduction reactions by blocking access to the surface, thereby minimizing galvanic corrosion in chloride environments like 3.5% NaCl solutions. These effects result in significantly lower corrosion currents compared to uncoated metals.

Dental cements

Zinc phosphate cement, one of the earliest dental restorative materials, was invented in 1892 by German chemist Otto Hoffmann, marking a significant advancement in luting agents for . This cement is formed through an acid-base reaction between a powder primarily composed of zinc oxide and a phosphoric acid-based liquid, resulting in a durable matrix suitable for clinical use. Well-known commercial formulations include Harvard Cement and Hoffmann's Cement, which have been staples in dental practice for over a century. The composition of zinc phosphate cement consists of a powder containing approximately 90% zinc oxide (ZnO) and 3-10% (MgO), with minor additives like silica for enhanced handling. The liquid component is a buffered solution (33-38% concentration), incorporating water and metallic salts such as aluminum or zinc phosphates to moderate the exothermic setting reaction and reduce initial acidity. When mixed, the ZnO reacts with the acid to form zinc phosphate crystals (Zn₃(PO₄)₂·4H₂O) embedded in an amorphous zinc aluminophosphate matrix, providing mechanical stability without chemical bonding to tooth structure. Key properties of zinc phosphate include high , typically ranging from 70 to 100 MPa, which supports its role in load-bearing restorations. It exhibits a low film thickness of less than 25 μm, ensuring intimate adaptation between restorations and prepared teeth while meeting ISO 9917-1 standards for luting cements. The material demonstrates good , with studies showing minimal impact on gingival fibroblasts and pulp cells compared to resin-based alternatives, making it suitable for intraoral placement. Additionally, its closely matches (approximately 11 × 10⁻⁶/°C), minimizing stress at the restoration interface, though it has moderate (0.1-0.2% in ) that requires careful moisture control during placement. In dental applications, zinc phosphate cement is primarily used as a luting agent for cementing crowns, bridges, inlays, and onlays, providing reliable retention through mechanical interlocking. It also serves as a temporary filling material for short-term restorations and as a pulp liner or base under amalgam or composite fillings to protect against thermal and chemical insults. These uses leverage its radiopacity (comparable to dentin) for easy radiographic visualization and its neutral pH after setting (around 6.5-7.0), which reduces pulpal irritation over time. Despite the rise of adhesive cements, zinc phosphate remains a gold standard for non-adhesive luting in metal-based prosthetics due to its proven longevity and ease of manipulation.

Other uses

Zinc phosphate serves as a surface treating agent in the automotive and industries, where it is applied as a to metal components to enhance and . In automotive applications, such as assemblies and parts, zinc phosphate coatings provide a crystalline layer that improves resistance and serves as a base for subsequent oiling or processes. In , it is used on components like electric panels to prepare surfaces for electrostatic , leveraging its corrosion-inhibiting properties in a brief pretreatment step. As an additive in phosphate fertilizers, zinc phosphate contributes to zinc supplementation in , particularly in soils where phosphorus applications are common. When is incorporated into ammoniated phosphate fertilizers, it forms zinc phosphate compounds like hopeite, which supply essential micronutrients to crops but require management to maintain and . Recent research indicates that lowering the of these fertilizers increases the of zinc phosphate, improving uptake in and supporting higher crop yields in zinc-deficient regions. Zinc phosphate plays a role in flame-retardant composites, where its content promotes char formation and thermal stability during combustion. In composites, poly( ) acts as an effective additive, decomposing to form protective residues like that reduce peak heat release rates by up to 71% compared to unmodified . Similarly, when combined with in matrices such as , enhances limiting oxygen index values and suppresses smoke production, contributing to overall in composite materials. Zinc phosphate is used in cosmetics as a white pigment with potential as a bulking agent due to its opacity and profile. It is also incorporated into glass enamels to improve chemical durability, particularly in formulations like zinc phosphate glasses for protective coatings.

Safety and toxicity

Health effects

Zinc phosphate exhibits low , with an oral LD50 greater than 5,000 mg/kg in rats, indicating it is not highly hazardous via in single exposures. Exposure to zinc phosphate powder can cause mild to moderate irritation to the skin and eyes upon direct contact, manifesting as redness, itching, or discomfort that typically resolves without lasting damage. Inhalation of zinc phosphate dust poses a risk of irritation, potentially leading to coughing, , or throat discomfort in occupational settings with poor ventilation. In dental applications, zinc phosphate cement initially presents an acidic environment with a of 2-4 due to the component, but it neutralizes to a of approximately 5-6 within 24 hours as the reaction completes, minimizing pulpal irritation and supporting without causing tissue damage. Chronic exposure to zinc phosphate is generally associated with low risk due to its insolubility and limited , though excessive long-term inhalation or ingestion could contribute to zinc accumulation, potentially leading to symptoms such as , , or interference with absorption in sensitive individuals. Overall, zinc phosphate demonstrates good in biomedical contexts, with studies showing no significant toward osteoblast-like cells, affirming its safety for prolonged contact in approved uses.

Environmental considerations

Zinc phosphate, when released into the environment through industrial effluents or disposal, contributes to phosphate runoff that promotes in bodies by providing excess nutrients that stimulate algal blooms and deplete oxygen levels. This process disrupts aquatic ecosystems, leading to hypoxic conditions harmful to and other organisms. As a source of zinc, a heavy metal, zinc phosphate poses risks of pollution in aquatic environments, where zinc ions can bioaccumulate in organisms such as algae, invertebrates, and fish, magnifying toxicity through the food chain. Studies have shown that zinc from such compounds accumulates in freshwater species like and Selenastrum capricornutum, potentially impairing reproduction and growth at concentrations as low as 250 μg/L. Regulatory frameworks address these impacts through restrictions on phosphate compounds to curb environmental release. Under the EU REACH regulation, zinc phosphate is registered but subject to evaluation for environmental hazards, while broader phosphate limits in detergents—capped at 0.5 g phosphorus per wash—aim to reduce eutrophication risks from related phosphorus sources. Industry trends favor replacements like calcium strontium phosphosilicates or sodium silicates, which offer corrosion inhibition with lower heavy metal content and reduced ecological persistence. Zinc phosphate exhibits low solubility in neutral conditions, limiting immediate environmental mobility, but it slowly leaches zinc and phosphate ions in acidic soils, such as those affected by , potentially increasing to plants and . This leaching behavior underscores the need for controlled disposal to prevent long-term and degradation.

References

  1. https://pubchem.ncbi.nlm.nih.gov/compound/Zinc-Phosphate
  2. http://www.rjor.ro/wp-content/uploads/2023/10/ZINC-BASED-DENTAL-CEMENTS-PROPERTIES-APPLICATIONS-AND-ADVANCEMENTS.pdf
  3. https://dentaleducationhub.com/zinc-phosphate-cement-an-overview/
  4. https://pmc.ncbi.nlm.nih.gov/articles/PMC5554035/
  5. https://pmc.ncbi.nlm.nih.gov/articles/PMC9953316/
  6. https://www.chemicalbook.com/ChemicalProductProperty_EN_CB6236647.htm
  7. https://www.sciencemadness.org/smwiki/index.php/Zinc_phosphate
  8. https://yadda.icm.edu.pl/baztech/element/bwmeta1.element.baztech-db1bbee3-ef36-479d-b446-2e21d7a6d8e9/c/Mineralogia_2023_Bajda.pdf
  9. https://www.sigmaaldrich.com/US/en/sds/aldrich/587583
  10. https://www.sciencedirect.com/science/article/abs/pii/S0304386X01001487
  11. https://cdnsciencepub.com/doi/10.1139/v65-058
  12. https://cdnsciencepub.com/doi/10.1139/v67-376
  13. https://www.sciencedirect.com/science/article/abs/pii/0025540881902889
  14. https://atamankimya.com/sayfalar.asp?LanguageID=2&cid=3&id=8&id2=13203
  15. https://www.minsocam.org/ammin/AM61/AM61_987.pdf
  16. https://rruff.geo.arizona.edu/doclib/mm/vol36/MM36_621.pdf
  17. https://ipen.org/sites/default/files/documents/switchmed_technical_guidelines_for_replacing_lead_in_anticorrosive_paint.pdf
  18. https://patents.google.com/patent/US4207301A/en
  19. https://taylorandfrancis.com/knowledge/Engineering_and_technology/Chemical_engineering/Zinc_phosphate/
  20. https://www.cambridge.org/core/journals/mineralogical-magazine-and-journal-of-the-mineralogical-society/article/on-hopeite-and-other-zinc-phosphates-and-associated-minerals-from-the-broken-hill-mines-northwestern-rhodesia/86E5F3A67817256A6F5F2AD57CD795B1
  21. https://www.mindat.org/min-1999.html
  22. https://www.dakotamatrix.com/mineralpedia/6245/hopeite
  23. https://www.mindat.org/min-3092.html
  24. https://www.mindat.org/min-3892.html
  25. https://www.sciencedirect.com/topics/earth-and-planetary-sciences/phosphate-mineral
  26. https://rruff.geo.arizona.edu/doclib/MinMag/Volume_50/50-355-33.pdf
  27. https://pubs.usgs.gov/bul/1135a/report.pdf
  28. https://www.sciencedirect.com/science/article/abs/pii/S0269749111005616
  29. https://pubs.usgs.gov/bul/1252d/report.pdf
  30. https://scholarworks.uno.edu/cgi/viewcontent.cgi?article=4293&context=td
  31. https://www.jgeosci.org/content/jgeosci.185_wlodek.pdf
  32. https://pubs.geoscienceworld.org/eurjmin/article/30/5/1007/531473/Secondary-Zn-bearing-phosphate-minerals-associated
  33. https://rruff.geo.arizona.edu/doclib/am/vol95/AM95_397.pdf
  34. https://pubs.acs.org/doi/10.1021/acsomega.2c07853
  35. https://www.sciencedirect.com/science/article/pii/S0010938X12005677
  36. https://www.valencesurfacetech.com/services/chemical-processing/zinc-phosphate/
  37. https://www.usbr.gov/research/publications/download_product.cfm?id=2609
  38. https://www.paint.org/coatingstech-magazine/articles/the-two-pillars-of-surface-preparation/
  39. https://www.sciencedirect.com/science/article/abs/pii/S0300944015000995
  40. https://hoffmann-dental.com/unternehmen/der-pionier-der-dentalindustrie/?lang=en
  41. https://hoffmann-dental.com/wp-content/uploads/2022/10/Hoffmann-Dental-Katalog-Englisch.pdf
  42. https://www.sciencedirect.com/science/article/abs/pii/S0008884697002238
  43. https://www.sciencedirect.com/topics/chemistry/zinc-phosphate-cement
  44. https://www.fda.gov/media/182280/download
  45. https://www.celljournal.org/article_250085.html
  46. https://pmc.ncbi.nlm.nih.gov/articles/PMC9961919/
  47. https://pocketdentistry.com/8-dental-cements/
  48. https://dentistry.co.uk/2021/07/05/a-dental-students-guide-toluting-cements/
  49. https://next.henkel-adhesives.com/us/en/articles/zinc-phosphating.html
  50. http://www.phosphating.net/zinc-phosphating.html
  51. https://acsess.onlinelibrary.wiley.com/doi/10.1002/saj2.20744
  52. https://phys.org/news/2024-11-fine-tuning-fertilizers-boost-crop.html
  53. https://www.sciencedirect.com/science/article/abs/pii/S0141391016301926
  54. https://pubs.acs.org/doi/10.1021/acsomega.1c00882
  55. https://www.sciencedirect.com/science/article/abs/pii/S0272884213011917
  56. https://scholarsmine.mst.edu/masters_theses/2444/
  57. https://echa.europa.eu/registration-dossier/-/registered-dossier/14696/7/3/2
  58. https://www.sigmaaldrich.com/AT/de/sds/aldrich/587583
  59. https://www.shofu.com/wp-content/uploads/HY-Bond-Zinc-Phosphate-Cement-Powder-SDS-US-Version-12.pdf
  60. https://www.atsdr.cdc.gov/toxprofiles/tp60.pdf
  61. https://www.knowyourh2o.com/outdoor-4/phosphates-in-the-environment
  62. https://www.sciencedirect.com/science/article/pii/S2667010023000574
  63. https://www.epa.gov/sites/default/files/2018-12/documents/ambient-wqc-zinc.pdf
  64. https://www.sciencedirect.com/science/article/pii/0043135487901047
  65. https://pubs.acs.org/doi/full/10.1021/es00135a005
  66. https://echa.europa.eu/substance-information/-/substanceinfo/100.033.683
  67. https://www.phosphonates.org/index.php/regulations
  68. https://www.specialchem.com/coatings/guide/corrosion-inhibitors
  69. https://www.sciencedirect.com/science/article/pii/S0045653521013874
  70. https://link.springer.com/article/10.1007/s42729-024-01908-5
Add your contribution
Related Hubs
User Avatar
No comments yet.