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Comment: Almost all the content is about Sodium perborate, which already has an article. The little mention of potassium perforate is only supported by an unreliable reference. Graeme Bartlett (talk) 23:26, 21 December 2025 (UTC)
Perborates are a group of inorganic salts that contain the perborate anion [B₂O₄(OH)₄]²⁻ known for their roles as detergents and bleaching agents derived from perboric acid structurally: H₂B₂O₄(OH)₄ (simplified: HBO₃·H₂O₂), having more oxygens than standard orthoborate (as a baseline) making it a strong oxidizer, they exist usually in hydrated forms (usually monohydrate and tetrahydrate) and there is no stable isolable anhydrous salts.[1]
Perborate Salts
editthe two Alkali Perborates (Potassium perborate, Sodium perborate) are known to be white crystalline solids or powders both having similar bleaching and oxidizing properties
Sodium Perborates ( Na₂B₂O₄(OH)₄ )
editSodium Perborates are mainly in two stable forms:
Sodium Perborate monohydrate is the form with most heat stability between the two Sodium Perborates, the most common industrially for bleaching and disinfecting. reported to decompose at ~95-105°C (~200-215° F) (). with a molar mass of approximately 99.815 g/mol.[2]
While Sodium perborate tetrahydrate decomposes at ~63°C (~145 °F). with a molar mass of 153.86 g/mol[2] making it less seen in detergents and bleaching agents since it retains less effectivness than Sodium perborate monohydrate at high temperatures.
Potassium Perborates ( K₂B₂O₄(OH)₄ )
editPotassium Perborates are also found in the same hydration forms as Sodium Perborates:
Potassium Perborate monohydrate is the stablest form among all alkali perborates it decomposes at ~150 °C (~302 °F) with a molar mass of 115.92 g/mol[3]
Potassium Perborate tetrahydrate is decomposes at the lowest among Potassium Perborates with a decomposition temperature of ~70-80 °C (~160-175 °F) and a molar mass of ~153.9 g/mol . (citation needed)
History
editDiscovery:
editSodium perborate was first obtained independently in 1898 by Tanatar and by Melikoff & Pissadewsky.[4]
Industrial synthesis:
editIn 1904, Otto Liebknecht developed a synthesis method that enabled large‑scale production.[5]
Commercialization:
editThis discovery paved the way for the detergent Persil (launched in 1907), which used sodium perborate as a self‑acting bleaching agent.[5]
Applications
editSodium perborate was widely used as a bleaching agent in detergents and cleaning products.[6] and It also found applications in toothpaste and cosmeticsformulations due to its antiseptic and disinfectant properties.[7] When dissolved in water, sodium perborate releases hydrogen peroxide, providing bleaching and deodorizing effects. [6]
Environmental and safety concerns
editLaws:
editthe EU tightly restricted the use of perborates in detergents and banned them in cosmetics due to their classification as CMR substances (carcinogenic, mutagenic, or reprotoxic), precisely reprotoxic And Omnibus Act VIII (2025) Updates the EU Cosmetics Regulation, adjusting Annex II (do not be confused with Annex II: Kyoto Protocol) banning sodium perborate in personal care products from 1 May 2026. (in Entry 1397)[8]
Enviorment Hazards:
Perborates release active oxygen and boron compounds, which can accumulate in soil and water and harmful to aquatic organisms at elevated concentrations.[9]
Fish LC50 values (for sodium perborate) : 51–125 mg/L
Daphnia magna LC50 values: 11–30 mg/L
Algae LC50 values: 3.3–20 mg/L
highlighting enviormental concerns especially for aquatic ecosystems[10]
Consumer safety:
Using Perborates in toothpaste or cosmetics raises ethical issues because of their reprotoxic properties.[11]
Oxidizing power:
Salts like sodium perborate is noncombustible but mixtures with organic material may ignite and burn fiercely.[12]
Chemical Properties
edit| Names | |
|---|---|
| IUPAC name
Peroxoborates | |
| Properties | |
| [B₂O₄(OH)₄]²⁻ salts (commonly NaBO₃·nH₂O, KBO₃·nH₂O) | |
| Molar mass | Varies by salt and hydration (NaBO₃·H₂O = 99.815 g/mol; NaBO₃·4H₂O = 153.86 g/mol) |
| Appearance | White crystalline solids |
| Odor | Odorless |
| Density | ~1.6–1.7 g/cm³ (hydrated salts) |
| Melting point | Decomposes before melting |
| Soluble in water | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards |
Strong oxidizers; irritants; classified as CMR substances in EU |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions |
Borates, Percarbonates |
Other cations |
Sodium, Potassium |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
information may vary slightly
- ↑ https://www.atamanchemicals.com/sodium-perborate_u25998/?lang=EN.
{{cite web}}: Missing or empty|title=(help) - 1 2 "Sodium perborate", Wikipedia, 2025-12-11, retrieved 2025-12-21
- ↑ "potassium perborate monohydrate | 28876-88-2". ChemicalBook. Retrieved 2025-12-21.
- ↑ "Properties of NaBO3". www.webqc.org. Retrieved 2025-12-21.
- 1 2 "Sodium perborate - Evonik Industries". history.evonik.com. Retrieved 2025-12-21.
- 1 2 "Sodium Perborate – Applications, Safety, and Handling Guide". 2025-01-03. Retrieved 2025-12-21.
- ↑ "The Multifaceted Applications of Sodium Perborate Tetrahydrate Beyond Cleaning". www.nbinno.com. Retrieved 2025-12-21.
- ↑ Lai, Chiara (2025-05-21). "The EU is banning new substances in cosmetics - Omnibus Act VIII". COSlaw.eu - Guiding through EU Cosmetics Regulations. Retrieved 2025-12-20.
- ↑ "Registration Dossier - ECHA". echa.europa.eu. Retrieved 2025-12-21.
- ↑ "Perboric acid, sodium salt, mono and tetrahydrate". HERA Project - CEFIC. Retrieved 2025-12-21.
- ↑ "Substance Information - ECHA". echa.europa.eu. Archived from the original on 2024-06-23. Retrieved 2025-12-21.
- ↑ "SODIUM PERBORATE | CAMEO Chemicals | NOAA". cameochemicals.noaa.gov. Retrieved 2025-12-20.