POTASSIUM IODIDE KI

Properties of potassium iodide KI:

White, when stored on the light turn yellow. Readily soluble in water (without hydrolysis). Does not form Crystalline hydrates. Typical reducing agent. An aqueous solution of KI chemically dissolves potassium iodide by complexation.


Molar mass g/mol 166.00
Density g/cm3 3.115
Melting point °C 681

Obtaining potassium iodide KI:

2K + E2 = 2KE (normal temp.; E = F, Cl, Вr, I).

2KOH + FeI2 = 2KI + Fe(OH)2↓ (in the atmosphere N2)

2KOH(diluted) + 2AgNO3 = Ag2O↓ + H2O + 2KNO3.

KIO3 + 3 H2O2 = KI + 3O2↑ + 3H2O (in diluted HNO3).


Chemical reactions with potassium iodide KI:

KI (diluted) + 6H2O = [K(H2O)6]+ + I- (pH=7).

8KI (solid) + 9H2SO4 (conc.) = 4I2↓ + H2S↑ + 4H2O + 8KHSO4 (30-50° C).

KI + 2 H2O + O2 → (time) → 4KOH + I2↓ + K[I(I)2] (normal temp., on the light)

4KI + 4 HCl(diluted) + O2 = 2I2↓ + 4KCl + 2H2O (normal temp., on the light).

2KI + E2 = 2KE + I2↓ (E = Cl, Br).

KI + 3 H2O + 3Cl2 (gas) = HIO3 + KCl + 5HCl

KI (conc.) + 6KOH(conc.) + 3Cl2 (gas) = KIO3↓ + 6KCl + 3H2O.

KI (solition) + I2 = K[I(I)2](solution) (yellow).

10KI + 8H2SO4 (diluted) + 2KMnO4 = 5I2↓ + 2MnSO4 + 8H2O + 6K2SO4

6KI + 7H2SO4 (diluted) + K2Cr2O7 = Cr2(SO4)3 + 3I2↓ + 7H2O + 4K2SO4.

2KI + H2SO4 (diluted.) + H2O2 = I2↓ + K2SO4 + 2H2O

2KI + 2 H2SO4 (diluted) + 2KNO2 = 2K2SO4 + I2↓ +  2NO ↑ + 2H2O.

2KI + Fe2(SO4)3 = I2↓ + 2FeSO4 + K2SO4 (in the diluted H2SO4).

2KI + 2 CuSO4 + K2SO3 + H2O=2 CuI↓ + 2K2SO4 + H2SO4 (in the dark).

KI + 3 H2O → Electrolysis → 3H2↑(cathode) + KIO3(anode).


 

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The six states of matter are: Plasmas, Gases, Liquids, Solids, Bose-Einstein Condensates and Fermionic Condensates.