POTASSIUM CHLORIDE KCl

Properties of potassium chloride KCl:

Sylvite. White, melts and boils without decomposition. Moderately soluble in water (without hydrolysis). Does not form сrystalline hydrates. Poorly soluble in concentrated hydrochloric acid, liquid ammonia. A weak reducing agent.Participates in exchange reactions. Main part (along with NaCl) of natural deposits of sylvite.


Obtaining potassium cloride KCl:

2 K + 2 НСl (diluted) = 2 KСl + H2↑.

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

KОН + НСl (diluted) = KСl + H2O

KОН + HNO3 (diluted) = KNO3 + H2O.

KОН (conc.) + NH4Cl (conc.) = KCl + NH3↑ + H2O (boiling).

K2CO3 + 2 HCl (diluted) = 2 KCl + CO2↑ + H2O.

K2SO4 + BaE2 = BaSO4 ↓ + 2KE (E = Сl-, OH-).


Chemical reactions with potassium cloride KCl:

KCl (diluted) + 6 H2O = [K(H2O)6](+) + Cl(-) (pH = 7).

2 KCl (solid) + H2SO4 (conc.) = K2SO4 + 2 HCl↑ (boiling).

KCl + KHSO4 = K2SO4 + HCl (450-700°C).

10KCl(solid) + 8H2SO4(conc., hot) + 2KMnO4=5Cl2↑ + 2MnSO4 + 6K2SO4 + 8H2O.

KСl (conc.) + NaClO4 (saturated) = KClO4 ↓ + NaCl (10°C).

2 KCl (liquid) → Electrolysis → 2K(cathode) + Cl2↑(anode).

2 KCl + 2H2O → Electrolysis → H2↑(cathode) + Cl2↑(anode) + 2KОН

2 KCl (melt) (on Hg-cathode) → Electrolysis 2 K (cathode) + Cl2↑(anode).

KCl + 3H2O → Electrolysis 3 H2↑ (cathode) + KClO3(anode)[40-60°C].


 

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