کل واکنشهای عنصر سدیم
NATRIUM (SODIUM) - Na
Propertiesof sodium Na:
An alkali metal. A silvery-white (in a thin layer - with a purple tint), lightweight, very soft, low melting. Dark red sodium vapor is composed of atoms Na (predominant) and molecules Na2. Under special conditions is formed a violet-blue colloidal solution of sodium in ether. Chemically dissolves in liquid NH3 (blue solution), molten NaOH. Very reactive, air-covered oxide film (tarnish), ignited at a moderate heat. Stable in an atmosphere of argon and nitrogen. A strong reducing agent, reacts vigorously with water, acids, non-metals. With nitrogen only reacts when heated (as opposed to Li). With the mercury forms an amalgam, amalgam - a strong reducing agent, but (in contrast to the pure sodium), the reaction with water flowing quietly.
Does not react with air, is well preserved under a layer of gasoline or kerosene, is easily suspended in boiling inert solvents (toluene, xylene, heptane, octane, etc.). In an inert atmosphere, the molten sodium is rapidly distributed over the surface of certain solids (NaCl, Na2CO3, coal, iron, Al2O3, SiC, ZrO2), forming a gray-black monatomic coverage. Сolors the flame of a gas burner in yellow. The most widespread metal in seawater.
| Molar mass | g/mol | 22.99 |
| Density in solid state | g/cm3 | 0.968 |
| Melting point | °C | 97.83 |
| Boiling point | °C | 886 |
Obtaining sodium Na:
4 NaOH (liquid) →Electrolysis 4Na (cathode) + O2↑ (anode) + 2H2O.
Na2CO3 + 2C(coke) = 2Na + 3CO (900-1000°C).
2NaCl (liquid) →Electrolysis 2Na (cathode) + Сl2↑ (anode).
2NaCl + 2H2O →Electrolysis→ H2↑ (cathode) + Сl2↑ (anode) + 2NaOH.
2NaCl (melt) (on Hg-cathode)→Electrolysis 2Na (cathode) + Сl2↑ (anode).
Reactions with sodium Na:
2Na + 2 H2O = 2 NaOH + H2↑.
2Na + 2 HСl (diluted) = 2 NaCl + H2↑.
2Na + 2 NaOH = 2 Na2O + H2 (600°C).
2Na + H2 = 2 NaH (250-400°C, pressure).
2Na + O2 (air) = Na2O2 (burning, impurity Na2O)
2Na + O2 = Na2O2 (250-400°C).
4Na + O2 + 2 H2O = 4 NaOH.
2Na + E2 = 2 NaE (normal temp., E = F, Cl; 150-250°C, E = Вr, I).
2Na + E = Na2E (t>130° С, E = S, Se, Те),
2Na + nS = Na2(Sn) [-40° С, in the liquid NH3, n = 1, 2, 4, 5].
6Na + N2 = 2 Na3N (100° С, electric discharge),
3Na + P (red) = Na3P (green) [200°C, in the atmosphere of Аr].
2Na + 2C (graphite) = Na2C2 (150-200°C).
2Na + 2H2S (saturated) = 2NaHS↓ + H2↑ (in benzene).
Na + 4NH3(liquid) = [Na(NH3)4] (blue) (at - 40°C),
[Na(NH3)4] + nNH3(liquid) ↔ [Na(NH3)4]+ + e- - nNH3.
2Na + 2NH3(gas) = 2NaNH2 + H2 (350°C).
2Na + B2O3 + 7H2 = 2Na[BH4] + 3H2O (250-300°C).
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).
SODIUM BIFLUORIDE NaHF2
Properties of sodium bifluoride NaHF2:
White, decomposes when heated. Stable in dry air. Moderately soluble in water, the anion is partially decomposed, and due to protolysis of HF creates an acidic environment. Crystalline hydrates do not form. Decomposed by concentrated acids, neutralized by alkalis.
Obtaining sodium bifluoride NaHF2:
NaOH + HF (diluted) = NaF + H2O
NaOH + 2 HF (conc.) = NaHF2 + H2O.
Na2CO3 + 2 HF (diluted) = 2 NaF + H2O + CO2↑
Na2CO3 + 4 HF(conc.) = 2 NaHF2 + CO2↑ + H2O.
NaF + HF (conc.) = NaHF2
NaF + nHF(liquid) = NaF·nHF↓, or Na[F(HF)n] (n = 1 / 4).
Reactions with sodium bifluoride NaNF2:
NaHF2 = NaF + HF (270—400° C).
NaHF2 (diluted) + 4H2O = [Na(H2O)4](+) + HF2(-)
HF2(-) ↔ HF + F(-)
HF + H2O ↔ F(-) + H3O(+); pKк = 3,18.
2 NaHF2 + H2SO4 (conc.) = Na2SO4 + 4HF↑ (boiling)
NaHF2 + NаOH (conc.) = 2 NaF + H2O
NaHF2 + Ca(ОН)2 (saturated) = NaOH + H2O + CaF2↓.
SODIUM HYDROGEN SULFATE NaHSO4
Properties of sodium hydrogen sulfate NaHSO4:
White. Melts without decomposition, on further heating decomposes. Readily soluble in water, creates an acidic environment due to the complete protolysis of the ion HSO4-. Crystalline NaHSO4-H2O has the structure of Na + H3O + SO42-. Neutralized by the alkali. Participates in the exchange reactions.
| Molar mass | g/mol | 120.06 |
| Density | g/cm3 | 2.742 |
| Melting point | °C | 186 |
| Solubility in water at 0°C | g/100g water | 28.6 |
Obtaining sodium hydrogen sulfate NaHSO4:
2NaOH + H2SO4 (diluted) = Na2SO4 + H2O.
NaOH + H2SO4 (conc., cold) = NaHSO4 + H2O.
Na2SO4 (solid) + H2SO4 (conc.) = 2NaHSO4 (solution).
NaCl (solid) + H2SO4 (conc.) = NaHSO4 + HCl↑ (50°C)
2NaCl (solid) + H2SO4 (conc.) = Na2SO4 + 2HCl↑ (boiling).
H2SO4 (conc., cold) + NaOH = NaHSO4 + H2O
H2SO4 (diluted) + 2NaOH = Na2SO4 + 2 H2O.
H2SO4 (conc.) + NaCl (solid) = NaHSO4 + HCl↑ (30-50°C)
H2SO4 (conc.) + 2NaCl (solid) = Na2SO4 + 2HCl↑ (boiling).
H2SO4 (conc.) + Na2SO4 = 2NaHSO4 (40°C).
Reactions with sodium hydrogen sulfate NaHSO4:
2NaHSO4 = Na2S2O7 + H2O (250-320°C, vacuum).
NaHSO4-H2O = NaHSO4 + H2O (120°C, vacuum)
2(NaHSO4-H2O) = Na2S2O7 + 3H2O (250°C).
NaHSO4 (conc.) + 4H2O = [Na(H2O)4](+) + HSO4(-).
HSO4(-) + H2O = SO4(2-) + H3O(+) (dilution).
NaHSO4 + NаOH (conc.) = Na2SO4 + H2O.
NaHSO4 + NaCl = Na2SO4 + HCl (450-800°C.
SODIUM SULFIDE Na2S
Properties of sodium sulfide Na2S:
White, melts without decomposition, heat-resistant. Anhydrous Na2S powder is pyrophoric in dry air. Readily soluble in water (strong hydrolysis on the anion). High reactivity, in moist state oxidized by oxygen of air, attaches sulfur. Decomposes by acids. Typical reductant.
| Molar mass | g/mol | 78.05 |
| Density | g/cm3 | 1.86 |
| Melting point | °C | 1180 |
Obtaining sodium sulfide Na2S:
2 Na + E = Na2E (t>130° С, E = S, Se, Те)
2 Na + nS = Na2(Sn) (-40° С, in the liquid NH3, n = 1, 2, 4, 5).
Na2SO4 + 4H2 = Na2S + 4H2O (550-600°C, catalyst Fe2O3).
H2S + NaOH (diluted) = NaHS + H2O
H2S + 2NaOH (diluted) = Na2S + 2H2O.
Reactions with sodium sulfide Na2S:
Na2S·9H2O = Na2S + 9H2O (15-35°C; conc. H2SO4, P4O10).
Na2S (diluted) + 8H2O = 2[Na(H2O)4](+) + S(2-).
S(2-) + H2O ↔ HS(-) + OH(-).
Na2S + 2HCl (diluted) = 2NaCl + H2S↑.
Na2S + 3H2SO4 (diluted) = 2NaHSO4 + SO2↑ + S↓ + 2H2O
Na2S + 4HNO3 (diluted) = 2NaNO3 + 2NO2↑ + S↓ + 2H2O.
Na2S (solution) + NaOH → O2(air), solid S(colloid), Na2Sn.
Na2SO3S + Na2S (solid) + 2O2 = Na2SO4 (t>400°C)
Na2S + H2S (saturated.) = 2NaHS.
Na2S (solution) + (n - 1)S = Na2(S4) [boiling].
Na2S + S = Na2(S2) (600°C).
Na2S + 3S = Na2(S4) (400°C).
Na2S + 4S = Na2(S5) (200°C).
Na2S + CaCO3 = Na2CO3 + CaS (1200°C).
Na2S (diluted) + Na2SO3 (diluted) + I2 = Na2SO3S + 2 NaI.
Na2S + 4H2O2 (conc.) = Na2SO4 + 4H2O.
SODIUM BROMIDE NaBr
Properties of sodium bromide NaBr:
White. It melts without decomposition. Readily soluble in water (no hydrolysis). Reducer.
Obtaining sodium bromide NaBr:
2 Na + E2 = 2NaE (normal temp., Е = F, Cl, Вr, I).
6 NaOH + 3 Br2 + 2(NH3-H2O) →(time) 6 NaBr + N2↑ + 8H2O (normal temp.).
2 NaI (cold) + E2 = 2NaE + I2↓ (E = Cl, Br)
NaI (hot) + 3 H2O + 3Cl2 = NaIO3 + 6HCl.
Reactions with sodium bromide NaBr:
NaBr-2H2O = NaBr + 2H2O (t> 51° C, vacuum).
NaBr (diluted) + 4 H2O = [Na(H2O)4](+) + Br(-) (pH 7).
2 NaBr (solid) + H2SO4 (conc. 10-50%, cold) = Na2SO4 + 2HBr
2 NaBr (solid) + 3 H2SO4 (conc.>50%, hot) = 2 NaHSO4 + Br2 + SO2 + 2H2O.
2 NaBr (hot) + Cl2 = 2 NaCl + Br2↑.
5 NaBr + 3 H2SO4(diluted) + NaBrO3 = 3Br2 + 3Na2SO4 + 3H2O
2 NaBr + 2 H2SO4 (conc.) + MnO2 = Br2 + Na2SO4 + MnSO4 + 2H2O (boiling).
NaBr + 3 H2O →Electrolysis→ 3H2↑ (cathode) + NaBrO3 (anode).
SODIUM IODIDE NaI
Properties of sodium iodide NaI:
White, when stored in the light turn yellow due to oxidation. It melts without decomposition, on further heating decomposes. Readily soluble in water (no hydrolysis). Typical reductant.
Obtaining sodium iodide NaI:
2 Na + E2 = 2 NaE (normal temp., E = F, Cl; Вr, I).
2 NaOH (hot) + I2 + H2O2 =2 NaI + O2↑ + 2H2O
2 NaOH (cold) + I2 + H2S(gas) = 2 NaI + S↓ + 2H2O.
2 NaOH (diluted) + FeI2 = 2NaI + Fe(OH)2↓ (in the atm. N2)
2 NaOH (diluted) + 2AgNO3 = Ag2O ↓ + H2O + 2NaNO3.
NaIO3 + H2O + 2 Fe = NaI + 2 FeO(OH)↓ (boiling, on air).
Reactions with sodium iodide NaI:
2 NaI = 2Na + I2 (t > 1400° С).
NaI·2H2O = NaI + 2H2O (t > 68,9° С, vacuum).
NaI (diluted) + 4 H2O = [Na(H2O)4]+ + I- (pH = 7).
8NaI (solid) + 9 H2SO4 (conc.) = 4 I2↓ + H2S↑ + 4H2O + 8 NaHSO4 (30-50° С)
2NaI (solid) + 4 HNO3 (conc.) = I2↓ + 2NO2↑ + 2H2O + 2NaNO3 (boiling, impurity of HIO3).
6NaI + 2H2O + O2 → time → 4NaOH + 2Na[I(I)2] (normal temp.,on the light)
4NaI + 4 НСl (diluted.) + O2 = 2I2↓ + 4 NaCl + 2H2O (normal temp.,on the light).
2NaI (cold) + E2 = 2NaE + I2↓ (E = Cl, Br)
Nal (hot) + 3 H2O + 3Cl2 = NaIO3 + 6HCl.
NaI + 4 NH3 (liquid) = [Na(NH3)4]I↓ ↔ [Na(NH3)4]+ + I-
2 NaI + 3 H2SO4 (conc.) + MnO2 = 2NaHSO4 + I2↓ + 2H2O.
NaI + 4 NaOH + 4 NaNO3 = Na5IO6 + 4NaNO2 + 2H2O (300-330° C).
NaI + 3H2O → Electrolysis → 3H2↑(on cathode) + NaIO3 (on anode).
SODIUM HYDROSULFIDE NaHS
Properties of sodium hydrosulfide NaHS:
White, in the liquid state - black. It melts without decomposition, on further heating decomposes. Readily soluble in cold water (hydrolysis on the anion). Decomposed in the boiling solution. Neutralized by the alkali (as opposed to NH4HS). Attaches sulfur. A typical reducing agent, is oxidized by atmospheric oxygen.
Obtaining sodium hydrosulfide NaHS:
2Na + 2H2S (saturated) = 2NaHS↓ + H2↑ (in benzene).
Na2S + H2S (saturated) = 2NaHS.
H2S + NaOH (diluted) = NaHS + H2O.
H2S + 2 NaOH(conc.) = Na2S + 2H2O.
2H2S + 2Na = 2NaHS + H2 (150°C).
H2S + M(C2H5O) = MHS↓ + C2H5OH (M = Li, Na, K; in ether)
Reactions with sodium hydrosulfide NaHS:
NaHS = Na2S + H2S (450-500°C).
NaHS·nH2O↓ ↔ NaHS (saturated) + nH2O (normal temp., n >= 3).
NaHS (diluted) + 4 H2O (cold) = [Na(H2O)4](+) + HS(-).
HS- + H2O ↔ H2S + OH-.
2NaHS (solution) = Na2S + H2S↑ (boiling).
NaHS + НСl (diluted) = NaCl + H2S↑,
NaHS + 3HNO3 (conc.) = S↓ + 2 NO2↑ + NaNO3 + 2H2O.
NaHS + NaОН (conc.) = Na2S + H2O.
2n NaHS (solid) + (n - 1)O2 = 2 H2O + (2n - 4) NaOH + 2 Na2(Sn) (100-250°C).
NaHS (saturated, hot) + NaOH + (n - 1)S = Na2(Sn) + H2O
SODIUM SULFATE Na2SO4
Properties of sodium sulfate Na2SO4:
Thenardite, Glauber's salt or mirabilite (hydrated). White. Melts and boils without decomposition. Readily soluble in water (without hydrolysis). Participates in the exchange reactions. Reduced with hydrogen, carbon.
| Molar mass | g/mol | 142.04 |
| Density | g/cm3 | 2.66 |
| Melting point | °C | 884 |
| Boiling point | °C | 1430 |
| Solubility in water at 20°C | g/100g water | 19.2 |
Obtaining sodium sulfate Na2SO4:
2 NaOH + H2SO4 (diluted) = Na2SO4 + H2O
NaOH + H2SO4 (conc., cold) = NaHSO4 + H2O.
NaHSO4 + NaCl = Na2SO4 + HCl (450-800°C).
NaCl (solid) + H2SO4 (conc.) = NaHSO4 + HCl↑ (to 50°C)
2 NaCl (solid) + H2SO4 (conc.) = Na2SO4 + 2HCl↑ (boiling).
Na2S (solid) + 2O2 = Na2SO4 (t> 400°C).
Na2S + 4 H2O2 (conc.) = Na2SO4 + 4H2O.
Reactions with sodium sulfate Na2SO4:
2 (Na2SO4-10H2O) (liquid) = Na2SO4↓ + Na2SO4(saturated) + 20 H2O (at 32,384°C).
Na2SO4 (diluted) + 8H2O = 2 [Na(H2O)4]+ + SO42- (pH = 7).
Na2SO4 (solid) + H2SO4(conc.) = 2 NaHSO4(solution).
Na2SO4 + SO3 = Na2S2O7.
Na2SO4 + 4 H2 = Na2S + 4H2O (550-600°C, catalyst Fe2O3).
Na2SO4 + 2 F2 = 2NaF + SO2F2 + O2 (100-150°C).
Na2SO4 + 2C (coke) + CaCO3 = Na2CO3 + CaS + CO2 (1000°C).
Na2SO4 + BaE2 = BaSO4↓ + 2NaE (E = Cl-, OH-).
SODIUM NITRATE NaNO3
Properties of sodium nitrate NaNO3:
Soda (Chilean) nitrate, nitratin. White, hygroscopic. Melts without decomposition, on further heating decomposes. Readily soluble in water with high endo-effect (without hydrolysis). Crystalline hydrates do not form. Practically insoluble in concentrated nitric acid. Strong oxidizing agent at sintering. In solution recovered only by atomic hydrogen.
| Molar mass | g/mol | 84.99 |
| Density | g/cm3 | 2.266 |
| Melting point | °C | 306.5 |
| Solubility in water at 20°C | g/100g water | 87.6 |
Obtaining sodium nitrate NaNO3:
NaOH + HNO3(diluted) = NaNO3 + H2O.
2 NaOH (cold) + NO + NO2 = 2 NaNO2 + H2O
4 NaOH (hot) + 4NO2 + O2 = 4 NaNO3 + 2H2O.
4 NO2 + O2 + H2O = 4 HNO3
4 NO2 + O2 + 4NaOH(hot) = 4 NaNO2 + 2H2O.
2 NO2 (liquid) + Na = NO↑ + NaNO2
NaNO2 + H2O2 (hot) = NaNO3 + H2O.
Reactions with sodium nitrate NaNO3:
2 NaNO3 = 2 NaNO2 + O2 (380-500° С; impurity Na2O, NO2).
NaNO3 (diluted) + 4 H2O = [Na(H2O)4](+) + NO3(-) (pH 7).
NaNO3 + 2H0 (Zn, diluted НСl) = NaNO2 + H2O (normal temp.)
NaNO3 + 8H0 (Zn, conc. NaOH) = NH3↑ + 2H2O + NaOH (boiling).
2 NaNO3 + (NH4)2SO4 = Na2SO4 + 2 N2O + 4H2O (230-300° С).
8 NaNO3 + 10Na = N2 + 6 Na3NO4 (250° С, vacuum)
NaNO3 + Na2O = Na3NO4 (310-320° С)
NaNO3 + Pb = PbO + NaNO2 (t>350° С).
3 NaNO3 + 4 NaOH + Cr2O3 = 2 Na2CrO4 + 3 NaNO2 + 2H2O (350-400° С).
SODIUM BICARBONATE NaHCO3
Properties of Sodium bicarbonate NaHCO3:
Baking soda, salt Bulriha, nahkolit. White, at low heat decomposes. In the wet state begins to decompose at room temperature. Moderately soluble in water (weak hydrolysis on the anion). Crystalline hydrates do not form. Decomposes by acids, neutralized by alkalis. Participates in the exchange reactions.
| Molar mass | g/mol | 84.01 |
| Density | g/cm3 | 2.24 |
| Solubility in water at 20°C | g/100g water | 9.59 |
Obtaining Sodium bicarbonate NaHCO3:
NaOH (diluted) + EO2 = NaHEO3 (E = С, S)
2 NaOH (conc.) + EO2 = Na2EO3 + H2O.
Na2CO3 (saturated) + H2O + CO2 = 2 NaHCO3↓ (30-40° С).
NaCl (saturated) + H2O + NH3 + CO2 = NaHCO3↓ + NH4Cl
Reactions with Sodium bicarbonate NaHCO3:
2 NaHCO3 = Na2CO3 + CO2 + H2O (250-300° С).
NaHCO3 (diluted) + 4H2O = [Na(H2O)4](+) + НСO3(-)
НСO3(-) + H2O ↔ H2CO3 + ОН(-).
NaHCO3 + НСl (diluted) = NaCl + CO2↑ + H2O.
NaHCO3 + NaOH (conc.) = Na2CO3 + H2O.
6 NaHCO3 (conc.) + 3Cl2 = NaClO3 + 5 NaCl + 6CO2↑ + 3H2O (boiling).
NaHCO3 + SO2 (gas) = NaHSO3 + CO2↑.
NaHCO3 + NaH2PO4 = Na2HPO4 + CO2↑ + H2O.
4 NaHCO3 + 2CuSO4 = Cu2CO3(ОН)2 ↓ + 2 Na2SO4 + 3 CO2 ↑ + H2O (boiling).
SODIUM CARBONATE Na2CO3
Properties of Sodium carbonate Na2CO3:
Soda (hydrate), soda ash, or washing (anhydrous). White, melts without decomposition, decomposes on further heating. Readily soluble in water (strong hydrolysis on the anion), creates a highly alkaline solution. Reacts with acids, non-metals and their oxides. Reduced by carbon.
| Molar mass | g/mol | 105.99 |
| Density | g/cm3 | 2.539 |
| Melting point | °C | 851 |
| Solubility in water at 20°C | g/100g water | 21.8 |
Obtaining Sodium carbonate Na2CO3:
2 Na2O2 + 2CO2 = 2Na2CO3 + O2
Na2O2 + CO = Na2CO3 (normal temp.).
NaOH (diluted) + EO2 = NaHEO3 (E = С, S)
2 NaOH (conc.) + EO2 = Na2EO3 + H2O.
2 NaHCO3 = Na2CO3 + CO2 + H2O (250-300°С).
NaHCO3 + NaOH (conc.) = Na2CO3 + H2O.
Na2SO4 + 2C(coke) + CaCO3 = Na2CO3 + CaS + CO2 (1000°С).
Reactions with Sodium carbonate Na2CO3:
Na2CO3 = Na2O + CO2 (1000° С).
Na2CO3-10H2O = Na2CO3 + 10H2O (100-120° С, vacuum).
Na2CO3 (diluted) + 8 H2O = 2 [Na(H2O)4]+ + CO32-
CO32- + H2O ↔ HCO3- + ОН-.
Na2CO3 + 2 НСl (diluted) = 2NaCl + CO2↑ + H2O.
Na2CO3 (saturated) + H2O + CO2 = 2 NaHCO3↓ (30-40° С).
Na2CO3 + 2 HF (diluted) = 2 NaF + H2O + CO2↑
Na2CO3 + 4 HF (conc.) = 2Na(HF2) + CO2↑ + H2O.
3Na2CO3 (conc.) + 2H3PO4(diluted) = 2Na3PO4 + 3H2O + 3CO2↑ (boiling).
Na2CO3 + M(ОН)2 (saturated) = MCO3↓ + 2 NaOH (M = Ca, Sr, Ba).
3Na2CO3 + 3H2O(hot) + 2AlCl3 = 2 Al(OH)3↓ + 3 CO2↑ + 6NaCl.
Na2CO3 (conc.,hot) + 3E2 = 5NaE + NaEO3 + 3CO2↑ (E = Cl, Br, I).
Na2CO3 + 2C(coke) = 2Na + 3CO (900-1000° C).
Na2CO3 + C(coke) + CaCN2 = 2 NaCN + CaCO3 (600-700° C).
Na2CO3 (conc.) + SO2 = Na2SO3 + CO2↑.
SODIUM SUPEROXIDE NaO2
Properties of sodium superoxide NaO2:
The orange-yellow, when heated decomposes without melting. Ion has the structure of the (Na +) (O2-). Reacts with water, acids, mono and dioxide of carbon. A strong oxidizer.
Obtaining sodium superoxide:
Na2O2 + O2 = 2NaO2 (450—500° C, pressure).
O2 + 2Na = Na2O2 (burning in air, the impurity of Na2O)
O2 + Na2O2 = 2 Na2O (400° C, pressure).
Reactions with sodium superoxide:
Na2O (-O2, 100-270°C) → Na2O2( -O2, 400-675°) C, vacuum
2 Na2O + H2O (cold) = NaOH + NaHO2(solution) + O2↑
2 NaHO2 (solution) →(time) 2 NaOH + O2↑ (normal temp.).
4 Na2O + 2 H2O (hot) = 4 NaOH + 302↑.
2 Na2O + 2 HCl (diluted, cold) = 2NaCl + H2O2 + O2↑.
4 Na2O + 2CO2 = 2Na2CO3 + 3O2 (normal temp.).
2 Na2O + CO = Na2CO3 + O2 (100° С).
4 Na2O + З С (graphite) = 2 Na2CO3 + CO2 (100° С).
Na2O + Аl (powder) = NaAlO2 (100° С).
SODIUM HYDROXIDE NaOH
Properties of sodium hydroxide NaOH:
Caustic soda, caustic. White, hygroscopic, melts and boils without decomposition. Readily soluble in water (with a high exo-effect), creates in the solution a highly alkaline environment. Greatly reduces the solubility of many salts of sodium in the water. Does not dissolve in liquid ammonia. Exhibits the properties of basic oxides (refers to alkali), neutralized by acid, reacts with acidic oxides. Absorbs CO2 from the air. Reacts with nonmetals, metals, amphoteric oxides and hydroxides.
| Molar mass | g/mol | 40.00 |
| Density | g/cm3 | 2.13 |
| Melting point | °C | 321 |
| Boiling point | °C | 1390 |
| Solubility in water at 20°C | g/100g water | 108.7 |
Obtaining sodium hydroxide NaOH:
2 Na + 2H2O = 2 NaOH + H2↑.
4 Na + O2 + 2H2O = 4 NaOH.
Na2O + H2O = 2 NaOH.
Na2CO3 + MCO3 (saturated) = MCO3↓ + 2 NaOH (M = Ca, Sr, Ba).
2 NaCl + 2H2O →Electrolysis H2↑(cathode) + Cl2↑(anode) + 2 NaOH
2 NaCl (melt) (on Hg-cathode)→Electrolysis→ 2Na(cathode) + Cl2↑(anode).
Reactions with sodium hydroxide NaOH:
NaOH-H2O = NaOH + H2O (100-400°C, vacuum).
NaOH (diluted) + 4H2O = [Na(H2O)4](+) + ОН(-).
NaOH + НСl (diluted) = NaCl + H2O.
2 NaOH + H2SO4 (diluted) = Na2SO4 + H2O
NaOH + H2SO4 (conc.,cold) = NaHSO4 + H2O.
NaOH + HNO3 (diluted) = NaNO3 + H2O.
NaOH (diluted) + H3PO4 (conc.) = NaH2PO4 + H2O
2 NaOH (diluted.) + H3PO4 (diluted) = Na2HPO4 + 2H2O
3 NaOH (conc.) + H3PO4 (diluted) = Na3PO4 + 3H2O.
NaOH + HF(diluted) = NaF + H2O
NaOH + 2HF (conc.) = Na(HF2) + H2O.
NaOH (conc.) + HCN = NaCN + H2O.
6 NaOH (diluted) + 4 F2= OF2↑ + 6 NaF + O2↑ + 3H2O.
2 NaOH (conc., cold) + E2 = NaEO + NaE + H2O (E = Cl, Br, I)
6 NaOH (conc.,hot) + 3E2 = NaEO3 + 5NaE + 3H2O. (E = Cl, Br, I)
12 NaOH (conc.,hot) + 5Cl2 + Br2 = 2NaBrO3 + 10NaCl + 6H2O.
20 NaOH (conc.,hot) + 7Cl2 + I2 = 2Na3H2IO6↓ +14NaCl + 8H2O
24 NaOH (conc.,cold) + 7Cl2 + I2 = 2Na5IO6↓ +14NaCl + 12H2O.
6 NaOH + 3 Br2 + 2(NH3-H2O) →time→ 6NaBr + N2↑ + 8H2O (normal temp.).
2 NaOH(hot) + I2 + H2O2 =2 NaI + O2↑ + 2H2O
2 NaOH(cold) + I2 + H2S(gas) = 2 NaI + S↓ + 2 H2O.
2 NaOH + 2Na = 2 Na2O + H2 (600°C).
4 NaOH + 3Ca = 3 CaO + Na2O + 2 Na + 2H2 (600°C).
2 (NaOH-H2O) + 2Al = 2 NaAlO2 + 3H2 (400-500°C)
2 NaOH (conc.) + 6 H2O(hot) + 2Al = 2 Na[Al(OH)4] + 3H2↑.
2 NaOH (conc.) + 2 H2O + Zn = Na2[Zn(OH)4] + H2↑.
NaOH (diluted) + EO2 = NaHEO3 (E = С, S)
2 NaOH (conc.) + EO2 = Na2EO3 + H2O.
4 NaOH (conc.) + SiO2 →time→ Na4SiO4 + 2H2O
2 NaOH + SiO2 = Na2SiO3 + H2O (900-1000°C).
4 NaOH + 6NO = 4 NaNO2 + N2 + 2H2O (300-400°C).
2 NaOH (cold) + NO + NO2 = 2NaNO2 + H2O
4 NaOH (hot) + 4 NO2 + O2 = 4NaNO3 + 2H2O.
2 NaOH + Al2O3 = 2 NaAlO2 + H2O (900-1100°C)
NaOH + Al(OH)3 = NaAlO2 + 2H2O (1000°C).
2 NaOH (conc., hot) + 3 H2O + Al2O3 = 2 Na[Al(OH)4]
NaOH (conc.) + Al(OH)3 = Na[Al(OH)4].
2 NaOH (conc. 60%) + H2O + ZnO = Na2[Zn(OH)4] (90°C)
2 NaOH (conc.) + Zn(OH)2 = Na2[Zn(OH)4] (normal temp.).
NaOH (conc.) + NH4Cl(conc.) = NaCl + NH3↑ + H2O (boiling).
2 NaOH (diluted) + FeI2 = 2 NaI + Fe(OH)2↓ (in the atmosphere of N2)
2 NaOH (diluted) + 2 AgNO3 = Ag2O↓ + H2O + 2 NaNO3.
3 NaOH (diluted) + AlCl3 = Al(OH)3↓ + 3 NaCl
4 NaOH (conc.) + AlCl3 = Na[Al(OH)4] + 3 NaCl.
2 NaOH (conc.) + ZnCl2 = Zn(OH)2↓ + 2NaCl
4 NaOH (conc.) + ZnCl2 = Na2[Zn(OH)4] + 2 NaCl.
2 NaOH (diluted, conc.) + Zn + 2 SO2 = Na2S2O4 + Zn(OH)2↓.
2 NaOH + 2 H2O + 3H2O2(conc.) = Na2O2-2H2O2-4H2O↓ (0°C)
Na2O2-2H2O2-4H2O = Na2O2 + 2 H2O2 + 4 H2O (normal temp., over conc. H2SO4).
4 NaOH (melt) →Electrolysis→ 4Na(cathode) + O2↑(anode) + 2H2O.
SODIUM HYDRIDE NaH
Properties of Sodium hydride NaH:
White. Decomposes when heated, under hydrogen pressure melts without decomposition. A strong reducing agent, reacts with water, acids, ammonia and oxygen.
Obtaining Sodium hydride:
2Na + H2 = 2 NaH (250-400°C, pressure).
2Na2[ReH9] = 4 NaH + 2 Re + 7H2 (245°C).
Reactions with Sodium hydride:
2NaH = 2Na + H2 (430-500°C, vacuum).
NaH + H2O = NaOH + H2↑.
NaH + HCl (diluted) = NaCl + H2↑.
2NaH + O2 = 2 NaOH (t>230°C).
NaH + Cl2 = NaCl + НСl (450-500°C)
2NaH + 2 S = Na2S + H2S (350-400°C).
2NaH + 4C (graphite) = Na2C2 + C2H2 (350°C).
NaH + CO2 = Na(HCOO) (until 200°C, pressure).
2NaH + 2 SO2 = Na2SO4 + H2S (200-250°C).
4NaH + AlCl3= Na[AlH4] + 3NaCl (in ether).
2NaH + (FeIIFe2III)O4 = 4NaOH + 3Fe (350-420°C).
2NaH + TiCl4 = Ti + 2NaCl + 2HCl.
NaH + NH3 (gas) = NaNH2 + H2 (350°C).
SODIUM OXIDE Na2O
Properties of Sodium oxide Na2O:
White, heat-resistant, refractory. Shows strong basic properties, reacts vigorously with water (forms an alkaline solution), acids, acidic and amphoteric oxides, liquid ammonia.
| Molar mass | g/mol | 61.98 |
| Density | g/cm3 | 2.36 |
| Melting point | °C | 1132 |
Obtaining sodium oxide:
2 Na + 2 NaOH = 2 Na2O + H2 (600°C).
2 Na + O2 (air) = Na2O2 (burning, impurity Na2O)
2 Na + O2 = Na2O2 (250-400°C).
2 Na2O2 = 2 Na2O + O2 (400-675°C, vacuum).
Na2O2H + 2Na = 2 Na2O (130-200°C, in the atmosphere of Аrgon).
2 NaOH + 2Na = 2 Na2O + H2 (600°C).
Na2CO3 = Na2O + CO2 (t>1000°C).
5 NaN3 + NaNO3 = 8N2 + 3Na2O (350-400°C, vacuum).
2 NaNO2 + 6 Na = 4 Na2O +N2 (350-400°C).
Reactions with sodium oxide:
2 Na2O = Na2O2 + 2Na (t>700°C).
Na2O + H2O = 2NaOH.
Na2O + 2HCl (diluted) = 2NaCl + H2O.
Na2O + CO2 = Na2CO3 (450-550°C).
Na2O + NO + NO2 = 2 NaNO2 (250°C).
Na2O + Al2O3 = 2 NaAlO2 (1200°C).
2 Na2O + O2 = 2 Na2O2 (250-350°C, pressure).
Na2O + NH3 (liquid) → time → NaNH2 + NaOH (- 50°C).
SODIUM PEROXIDE Na2O2
Properties of Sodium peroxide Na2O2:
White (sometimes yellow because of the impurities NaO2). When heated in air turn yellow and decomposes, melts at a pressure of O2. Has an ionic structure of the (Na +) 2 (O2 2-). Absorbs CO2 from the air. Completely decomposed by water, acids. Reacts vigorously with oxygen, sulfur, sodium, mono and carbon dioxide. Exhibits redox properties.
Obtaining sodium peroxide Na2O2:
2Na + O2 (air) = Na2O2 (burning, impurity Na2O)
2Na + O2 = Na2O2 (250-400°C).
2Na2O = Na2O2 + 2Na (t>700°C).
2Na2O + O2 = 2Na2O2 (250-350°C, pressure).
2NaOH + 2H2O + 3H2O2 (conc.) = Na2O2-2H2O2-4H2O↓ (0°C)
Na2O2-2H2O2-4H2O = Na2O2 + 2H2O2 + 4H2O (normal temp., over conc. H2SO4).
Reactions with sodium peroxide Na2O2:
2Na2O2 = 2 Na2O + O2 (400-675°C, vacuum).
Na2O2 + 8H2O(moisture) = Na2O2 - 8H2O (0° С).
Na2O2 + 2H2O(cold) = H2O2 + 2NaOH
2Na2O2 + 2H2O(hot) = O2↑ + 4NaOH.
Na2O2 + 2HCl(diluted, cold) = 2NaCl + H2O2.
2Na2O2 + 2H2SO4 (diluted, hot) = 2Na2SO4 + 2H2O + O2↑.
Na2O2 + O2 = 2NaO2 (450-500°C, pressure).
2Na2O2 + S = Na2SO3 + Na2O (100° C)
2Na2O2 + С(graphite) = Na2CO3 + Na2O (100°C)
3Na2O2 + 2Al (powder) = 2NaAlO2 + 2Na2O (70-120°C).
2Na2O2 + 2 CO2 = 2Na2CO3 + O2
Na2O2 + CO = Na2CO3 (normal temp.).
Na2O2 + MnO2 = Na2MnO4 (400-500°C).
Na2O2 + 2Na = 2Na2O (130-200°C, in the atmosphere of Ar).
5Na2O2 + 8H2SO4(diluted) + 2KMnO4 = 5O2↑ + 2MnSO4 + 8H2O + 5Na2SO4 + K2SO4.
Na2O2 + 2H2SO4(diluted) + 2NaI = I2↓ + 2Na2SO4 + 2H2O.
3Na2O2 + 2Na3[Cr(OH)6] (hot) = 2 Na2CrO4 + 8NaOH + 2H2O.
Na2O2 + 2H2SO4 (diluted) + 2FeSO4 = Fe2(SO4)3 + Na2SO4 + 2H2O
Na2O2 + 2Fe(ОН)2(suspension) = 2FeO(OH)↓ + 2NaOH.
SODIUM POLYSULFIDES Na2Sn
Properties of Sodium polysulfides Na2Sn:
A mixture of Na2Sn (n = 2, 4, 5) has a yellow-brown color, Na2S2 - yellow. All Na2Sn - a very hard, melt without decomposition, melts - brown mobile liquid. Thermal stability decreases with increasing n. Readily soluble in water, hydrolyzed (on anion) is significantly weaker than Na2S. The aqueous solution is yellow. Oxidized in air. Reacts with acids and strong reducing agents.
Obtaining sodium polysulfides Na2(Sn):
2Na + E = Na2E (t>130° С, E = S, Se, Те)
2Na + nS = Na2(Sn) [-40° С, in the liquid NH3, n = 1, 2, 4, 5].
Na2S (solution) + (n-1)S = Na2(Sn) [boiling]
Na2S + S = Na2(S2).
Na2S + 3S = Na2(S4).
Na2S + 4S = Na2(S5).
Reactions with sodium polysulfides Na2(Sn):
Na2(Sn) = Na2S + (n-1)S (t>600° С).
Na2(Sn)[diluted] + 8H2O = 2[Na(H2O)2](+) + S2(2-)
Sn(2-) + H2O ↔ HSn(-) + OH(-).
Na2Sn + 2 НСl (diluted) = 2 NaCl + H2S↑ + (n - 1)S↓ (normal temp.)
Na2Sn + 2 НСl (conc) = 2 NaCl + H2Sn (- 15° С).
2 Na2Sn + 2H2O(cold) + O2 = nS(colloid) + 4NaOH (on the light)
2 Na2(Sn)(saturated, hot) + 3O2 = 2Na2SO3S + (2n - 4)S↓.
Na2(Sn) + H2O + SO2 = Na2SO3S + H2S↑ + (n - 2)S↓ (normal temp.).
Na2(Sn) + SnS2 = Na2[SnS3] + (n - 1)s↓
3 Na2(Sn) + As2S3 = 2Na3[AsS4] + (3n - 5)S↓.
Na2(Sn)+(n-1)Na[Sn(OH)3]+3(n - 1)NaOH = nNa2S+(n-1)Na2[Sn(OH)6].
SODIUM AMIDE NaNH2
Properties of Sodium amide NaNH2:
White. Melts without decomposition, sublimes readily, on further heating decomposes. Oxidized in air, and turn yellow (the products are unknown). Poorly soluble in liquid ammonia. Completely hydrolyzed in water, reacts with acids.
Obtaining sodium amide:
2Na + 2 NH3 (gas) = 2NaNH2 + H2 (350°C).
NaH + NH3 (gas) = NaNH2 + H2 (350°C).
NaN3 + H2 = NaNH2 + N2 (200°C, impurity NH3, catalyst Pt).
Reactions with sodium amide:
6 NaNH2 = 6Na + 4NH3 + N2 (500-600°C).
NaNH2 + 2H2O(cold) = NaOH + NH3-H2O
NaNH2 + H2O(hot) = NaOH + NH3↑.
NaNH2 + 2HСl (diluted) = NaCl + NH4Cl.
NaNH2 + 2 HNO3 = NaN3 + NaNO3 + 3H2O (boiling).
NaNH2 + C (coke) = NaCN + H2 (500-600°C).
NaNH2 + NH4Cl = 2NH3 + NaCl (at -40°C, in the liquid NH3).
SODIUM FLUORIDE NaF
Properties of Sodium fluoride NaF:
Villiaumite. White, melts without decomposition. Moderately soluble in water (hydrolysis on the anion), the solubility is only slightly dependent on temperature. Crystalline hydrates do not form. Decomposed by concentrated acids. Participates in the exchange reactions.
Obtaining sodium fluoride NaF:
2 Na + E2 = 2NaE (normal temp., E = F, Cl, Вr, I).
NaOH + HF(diluted) = NaF + H2O
NaOH + 2HF(conc.) = NaHF2 + H2O.
NaOH (conc.) + NH4F (conc.) = NaF + NH3↑ + H2O (boiling)
Na2SiF6 + NaOH (conc., cold) = 6 NaF + Na4SiO4 + 4H2O.
Na2SiF6 + 2Na2CO3 (conc.) = 6 NaF +SiO2↓ + 2CO2↑ (boiling).
Reactions with sodium fluoride NaF:
NaF (diluted) + 4H2O = [Na(H2O)4]+ + F-
F(-) + H2O ↔ HF + ОН(-).
NaF + HF(conc.) = Na(HF2)
NaF + nHF(liquid) = NaF·nHF↓, or Na[F(HF)n] (n = 1 / 4).
2 NaF + H2SO4(conc.) = Na2SO4 + 2 HF↑ (bolilig).
NaF + LiOH (saturated) = NaOH + LiF↓.
2NaF(conc.) + H2[SiF6] = Na2[SiF6]↓ + 2HF.
3NaF(conc.) + AlF3 = Na3[AlF6]↓.
NaF(melt) → Electrolysis 2Na↓(cathode) + F2↑(anode).
