SODIUM CHLORIDE NaCl

Properties of sodium chloride NaCl:

Salt, halite. White, slightly hygroscopic, water absorption increases sharply in the presence of natural impurities, such as magnesium salts. Melts and boils without decomposition. Moderately soluble in water (without hydrolysis), the solubility is slightly dependent on temperature, but strongly reduced in the presence of HCl, NaOH, chlorides of metalls. Dissolves in liquid ammonia. A weak reducing agent. Participates in the exchange reactions. The main component of natural deposits of rock salt, sylvite, brine of salt lakes.


Obtaining sodium chloride NaCl:

2 Na + 2 HСl (diluted) = 2 NaCl + H2↑.

2 Na + E2 = 2NaE (normal temp., E = F, Cl, Вr, I).

NaOH + HСl (diluted) = NaCl + H2O.

NaOH (conc.) + NH4Cl(conc.) = NaCl + NH3↑ + H2O (boiling).

Na2CO3 + 2 HСl (diluted) = 2NaCl + CO2↑ + H2O.

Na2SO4 + BaE2 = BaSO4↓ + 2NaE (E = Cl-, OH-).


Reactions with sodium chloride NaCl:

NaCl-2H2O ↔ NaСl (saturated) + 2H2O (until +0,15° С)

NaCl-2H2O = NaCl + 2 H2O (normal temp., in dry air).

NaCl (diluted) + 4H2O = [Na(H2O)4](+) + Сl(-) (pH7).

NaCl (solid) + H2SO4 (conc.) = NaHSO4 + HCl↑ (to 50° С)

2 NaCl (solid) + H2SO4 (conc.) = Na2SO4 + 2HCl↑ (boiling).

NaCl + NaHSO4 = Na2SO4 + HCl (450-800° С).

2NaCl(solid)+4H2SO4(conc.)+PbO2=Cl2↑+Pb(HSO4)2+2NaHSO4+2H2O(normal temp.)

2NaCl(solid)+2H2SO4(conc.)+MnO2=Cl2↑+MnSO4+Na2SO4+2H2O (100°C).

10NaCl(solid) + 8H2SO4(conc.,hot) + 2KMnO4(solid) = 5Cl2↑ + 2MnSO4 + 5Na2SO4 + K2SO4 + 8H2O.

NaCl (saturated) + AgNO2 (saturated) = NaNO2 + AgCl↓

NaCl (diluted) + AgNO3 = NaNO3 + AgCl4.

NaCl (saturated) + H2O + NH3 + CO2 = NaHCO3↓ + NH4Cl.

NaCl + AlCl3 = Na[AlCl4] (until 300 ° C)

2 NaCl(melt) →Electrolysis→ 2Na (cathode) + Сl2↑ (anode).

2 NaCl + 2H2O →Electrolysis→ H2↑ (cathode) + Сl2↑ (anode) + 2NaOH

2 NaCl(solution) (on Hg-cathode)→Electrolysis→ 2Na (cathode) + Сl2↑(anode).


 

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