POTASSIUM CARBONATE K2CO3

Properties potassium carbonate K2CO3:

Potash. White. Melts without decomposition, on further heating decomposes. Very soluble in water (strong hydrolysis on the anion), creates a high alkaline environment. Reacts with acids, non-metals, oxides of nonmetals. Participates in exchange reactions.


Molar mass g/mol 138.20
Density g/cm3 2.428
Melting point °C 891

Obtaining potassium carbonate K2CO3:

4 KO2 + 3 C (graphite) = 2 K2CO3 + CO2 (30° C).

4 KO2 + 2 CO2(humidity) = 2 K2CO3 + 3O2 (normal temp.).

2 KO2 + CO = K2CO3 + O2 (50° C).

2 KOH (conc.) + EO2 = K2EO3 + H2O (E = C, S),

KOH + CO2 = KHCO3↓ (in ethanol).

2 KHCO3 = K2CO3 + CO2 + H2O (100-400° C).

KHCO3 + KOH conc.) = K2CO3 + H2O.

K2SO4 + Ca(OH)2 + 2 CO = 2KHCOO + CaSO4 (200° C, pressure),

2KHCOO + O2 = K2CO3 + CO2 + H2O (700° C).


Chemical reactions with potassium carbonate K2CO3:

K2CO3 = K2O + CO2 (t > 1200° C).

K2CO3 - 1.5 H2O = K2CO3 + 1.5 H2O (100-150° C, vacuum).

K2CO3 (diluted) + 12H2O = 2 [K(H2O)6]+ + CO32-,

CO32- + H2O ↔ HCO3- + OH-.

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

K2CO3 (saturated) + 2 HClO4 (conc., cold) = 2 KClO4↓ + H2O + CO2↑.

3 K2CO3 (conc.) + 2 H3PO4 (diluted) = 2 K3PO4 + 3 H2O + 3 CO2 ↑.

K2CO3 + 2 HF (diluted) = 2 KF + H2O + CO2↑,

K2CO3 + 4 HF(conc.) = 2 KHF2 + H2O + CO2↑.

K2CO3 + H2O + CO2 = 2 KHCO3 (30-40° C).

K2CO3 (diluted)+ H2O + 2 SO2 = 2 KHSO3 + CO2↑.

K2CO3 + Ca(OH)2 (saturated) = CaCO3 ↓ + 2 KOH.

3 K2CO3 (conc., hot) + 3E2 = 5KE + KEO3 + 3 CO2↑ (E = Cl, Br, I).

3 K2CO3 + 3 H2O (hot) + 2AlCl3 = 2 Al(OH)3↓ + 3 CO2↑ + 6 KCl.

3 K2CO3 + H2O + 2 FeBr3 = 6 KBr + 2 FeO(OH)4 + 3 CO2↑ (boiling).

K2CO3 + BaS2O6 = K2S2O6 + BaCO3↓.

K2CO3 + C (coke) + CaCN2 = 2 KCN + CaCO3 (900° C).

K2CO3 + C (NH2)2O = 2 KOCN + 2 H2O (40 °C).


 

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