Potassium Iodide Cr...

Potassium Iodide Crystals KI

Potassium Iodide Crystals KI

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1 Kilogram

Negotiable

  • Min.Order :1 Kilogram
  • Purity: 99.9999%
  • Payment Terms : T/T,,MoneyGram

Keywords

Kalium iodide KCN suppliers crystal pottasium KI

Quick Details

  • Appearance:white crystalline solid
  • Application:Potassium iodide is used in photography, in the preparation of silver(I) iodide for high speed photographic film:
  • PackAge:Buyer's request
  • ProductionCapacity:10000|Kilogram|Day
  • Storage:as per buyer's request
  • Transportation:Air, sea

Superiority:

Potassium iodide behaves as a simple ionic salt, K+I−. Since the iodide ion is a mild reducing agent, I− is easily oxidised to I2 by powerful oxidising agents such as chlorine:

2 KI( aq) + Cl2(aq) → 2 KCl + I2(aq)

Even air will oxidize iodide as evidenced by the observation of a purple extract when KI is rinsed with dichloromethane. Under acidic conditions, KI is oxidised even more easily, due to the formation ofhydroiodic acid (HI), which is a powerful reducing agent.

KI forms I3− when combined with elemental iodine.

KI(aq) + I2( s) → KI3(aq)

Unlike I2, I3− salts can be highly water-soluble. I2 and I3− have virtually identical redox potentials (0.535 and 0.536 V vs NHE, respectively), i.e. they are both mild oxidants relative to H2. Therefore, this reaction allows the iodine to be used in aqueous solutions for redox titrations.

Potassium iodide also serves in some organic reactions as a source of iodide ion (see "uses" below).

Details:

Potassium iodide behaves as a simple ionic salt, K+I−. Since the iodide ion is a mild reducing agent, I− is easily oxidised to I2 by powerful oxidising agents such as chlorine:

2 KI( aq) + Cl2(aq) → 2 KCl + I2(aq)

Even air will oxidize iodide as evidenced by the observation of a purple extract when KI is rinsed with dichloromethane. Under acidic conditions, KI is oxidised even more easily, due to the formation ofhydroiodic acid (HI), which is a powerful reducing agent.

KI forms I3− when combined with elemental iodine.

KI(aq) + I2( s) → KI3(aq)

Unlike I2, I3− salts can be highly water-soluble. I2 and I3− have virtually identical redox potentials (0.535 and 0.536 V vs NHE, respectively), i.e. they are both mild oxidants relative to H2. Therefore, this reaction allows the iodine to be used in aqueous solutions for redox titrations.

Potassium iodide also serves in some organic reactions as a source of iodide ion (see "uses" below).

 

 

Systematic name Potassium iodide
Other names Kalium iodide,
knollide, potide
Molecular formula KI
Molar mass 166.00 g/mol
Appearance white crystalline solid
CAS number [7681-11-0]
Properties
Density and phase 3.13 g/cm3, solid
Solubility in water 128 g/100 ml (6 °C)
Melting point 681 °C (954 K)
Boiling point 1330 °C (1600 K)
Acidity (pKa)  
Alkilinity (pKb)  
Structure
Molecular shape  
Coordination geometry  
Crystal structure  
Dipole moment    D

 

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