Monopotassium phosphate

Monopotassium phosphate (MKP) (also, potassium dihydrogen phosphate, KDP, or monobasic potassium phosphate) is the inorganic compound with the formula KH₂PO₄. Together with dipotassium phosphate (K₂HPO₄^.(H₂O)_x) it is often used as a fertilizer, food additive, and buffering agent. The salt often cocrystallizes with the dipotassium salt as well as with phosphoric acid.^[7]

Monopotassium phosphate

Two unit cells of MKP viewed close to the b axis
Names
IUPAC names Potassium dihydrogen phosphate[1]
Other names Potassium phosphate monobasic; Phosphoric acid, monopotassium salt; Potassium biphosphate
Identifiers
CAS Number	7778-77-0 Y
3D model (JSmol)	Interactive image
ChEMBL	ChEMBL1200925 N
ChemSpider	22914 N
ECHA InfoCard	100.029.012
EC Number	231-913-4
E number	E340(i) (antioxidants, ...)
PubChem CID	516951
RTECS number	TC6615500
UNII	4J9FJ0HL51 Y
CompTox Dashboard (EPA)	DTXSID0035667
InChI InChI=1S/3K.H3O4P/c;;;1-5(2,3)4/h;;;(H3,1,2,3,4)/q3*+1;/p-3 Y Key: LWIHDJKSTIGBAC-UHFFFAOYSA-K Y InChI=1/3K.H3O4P/c;;;1-5(2,3)4/h;;;(H3,1,2,3,4)/q3*+1;/p-3 Key: LWIHDJKSTIGBAC-DFZHHIFOAX
SMILES [K+].OP(O)([O-])=O
Properties
Chemical formula	KH 2PO 4
Molar mass	136.086 g/mol
Appearance	Colourless crystals or white granular or crystalline powder[2]
Odor	Odorless [2]
Density	2.338 g/cm3
Melting point	252.6 °C (486.7 °F; 525.8 K) [3]
Boiling point	400 °C (752 °F; 673 K) , decomposes
Solubility in water	22.6 g/100 mL (20 °C) 83.5 g/100 mL (90 °C)
Solubility	Slightly soluble in ethanol
Acidity (pKa)	6.86[4]
Basicity (pKb)	11.9
Refractive index (nD)	1.4864
Structure
Crystal structure	Tetragonal[5]
Space group	I42d
Lattice constant	a = 0.744 nm, b = 0.744 nm, c = 0.697 nm
Hazards
GHS labelling:
Pictograms	[6]
Signal word	Warning[6]
Hazard statements	H315, H319[6]
Precautionary statements	P264, P280, P305+P351+P338, P321, P332+P313, P337+P313[6]
NFPA 704 (fire diamond)	1 0 0
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	3200 mg/kg (rat, oral)
Safety data sheet (SDS)	External MSDS
Related compounds
Other cations	Monosodium phosphate Monoammonium phosphate
Related compounds	Dipotassium phosphate Tripotassium phosphate
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

Single crystals are paraelectric at room temperature. At temperatures below −150 °C (−238 °F), they become ferroelectric.

Structure

Monopotassium phosphate can exist in several polymorphs. At room temperature it forms paraelectric crystals with tetragonal symmetry. Upon cooling to −150 °C (−238 °F) it transforms to a ferroelectric phase of orthorhombic symmetry, and the transition temperature shifts up to −50 °C (−58 °F) when hydrogen is replaced by deuterium.^[8] Heating to 190 °C (374 °F) changes its structure to monoclinic.^[9] When heated further, MKP decomposes, by loss of water, to potassium metaphosphate, KPO
₃, at 400 °C (752 °F).

Symmetry	Space group	№	Pearson symbol	a (nm)	b (nm)	c (nm)	Z	Density (g/cm3)	T (°C, °F, K)
Orthorhombic[8]	Fdd2	43	oF48	1.0467	1.0533	0.6926	8	2.37	< −150 °C, −238 °F, 123 K
Tetragonal[5]	I42d	122	tI24	0.744	0.744	0.697	4	2.34	−150 to 190 °C, −238 to 374 °F, 123 to 463 K
Monoclinic[9]	P21/c	14	mP48	0.733	1.449	0.747	8		190 to 400 °C, 374 to 752 °F, 463 to 673 K

Manufacturing

Monopotassium phosphate is produced by the action of phosphoric acid on potassium carbonate.

Applications

Fertilizer-grade MKP powder contains the equivalent of 52% P
₂O
₅ and 34% K
₂O, and is labeled NPK 0-52-34. MKP powder is often used as a nutrient source in the greenhouse trade and in hydroponics.

As a crystal, MKP is noted for its non-linear optical properties. It is used in optical modulators and for non-linear optics such as second-harmonic generation (SHG).

Also, to be noted is KD*P, potassium dideuterium phosphate, with slightly different properties. Highly deuterated KDP is used in nonlinear frequency conversion of laser light instead of protonated (regular) KDP due to the fact that the replacement of protons with deuterons in the crystal shifts the third overtone of the strong OH molecular stretch to longer wavelengths, moving it mostly out of the range of the fundamental line at approximately 1064 nm of neodymium-based lasers. Regular KDP has absorbances at this wavelength of approximately 4.7–6.3% per cm of thickness while highly deuterated KDP has absorbances of typically less than 0.8% per cm.

Monopotassium phosphate is also used as an ingredient in sports drinks such as Gatorade and Powerade.

In medicine, monopotassium phosphate is used for phosphate substitution in hypophosphatemia.^[10]

Gallery

• 
  A large KDP crystal, used in the form of slices at the National Ignition Facility
• 
  Alternate angle, covered

References

1. "Potassium dihydrogen phosphate".
2. "Commission Regulation (EU) No 231/2012 of 9 March 2012 laying down specifications for food additives listed in Annexes II and III to Regulation (EC) No 1333/2008 of the European Parliament and of the Council Text with EEA relevance". EUR-Lex. E 340 (i) MONOPOTASSIUM PHOSPHATE. Retrieved 19 January 2023.{{cite web}}: CS1 maint: location (link)
3. King, Harold S. J. Am. Chem. Soc. 1927, 49, 6, 1511–1512 https://doi.org/10.1021/ja01405a018
4. Mathews, Christopher K., K. E. Van Holde, Ean R. Appling, and Spencer J. Anthony-Cahill. Biochemistry. Redwood City, CA: Benjamin/Cummings Pub., 1990. Print.
5. Ono, Yasuhiro; Hikita, Tomoyuki; Ikeda, Takuro (1987). "Phase Transitions in Mixed Crystal System K_1−x(NH₄)_xH₂PO₄". Journal of the Physical Society of Japan. 56 (2): 577. Bibcode:1987JPSJ...56..577O. doi:10.1143/JPSJ.56.577.
6. "Potassium Dihydrogen Phosphate". American Elements. Retrieved October 30, 2018.
7. Klaus Schrödter; Gerhard Bettermann; Thomas Staffel; Friedrich Wahl; Thomas Klein; Thomas Hofmann (2012). "Phosphoric Acid and Phosphates". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_465.pub3. ISBN 978-3527306732.
8. Fukami, T. (1990). "Refinement of the Crystal Structure of KH₂PO₄ in the Ferroelectric Phase". Physica Status Solidi A. 117 (2): K93–K96. Bibcode:1990PSSAR.117...93F. doi:10.1002/pssa.2211170234.
9. Itoh, Kazuyuki; Matsubayashi, Tetsuo; Nakamura, Eiji; Motegi, Hiroshi (1975). "X-Ray Study of High-Temperature Phase Transitions in KH₂PO₄". Journal of the Physical Society of Japan. 39 (3): 843. Bibcode:1975JPSJ...39..843I. doi:10.1143/JPSJ.39.843.
10. Gaasbeek, André; Meinders, A. Edo (October 2005). "Hypophosphatemia: an update on its etiology and treatment". The American Journal of Medicine. 118 (10): 1094–1101. doi:10.1016/j.amjmed.2005.02.014. ISSN 0002-9343. PMID 16194637.

External links

• International Chemical Safety Card 1608
• EPA: Potassium dihydrogen phosphate Fact Sheet
• Potassium Phosphate – a Hydroculture Salt