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Sodium sulfate Salt cake Na2SO4 CAS NO.7757-82-6
- FOB Price: USD: /Metric Ton Get Latest Price
- Min.Order: 1 Kilogram
- Payment Terms: T/T,MoneyGram
- Available Specifications:
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- Product Details
Keywords
- Salt cake supplier
- Thenardite
- Na2SO4 suppliers
Quick Details
- ProName: Sodium sulfate Salt cake Na2SO4
- CasNo: 7757-82-6
- Molecular Formula: Na2SO4
- Appearance: White crystalline solid, hygroscopic
- Application: Instrustrial and pharma grade
- DeliveryTime: 5-7 days
- PackAge: Buyer's request
- Port: Odessa
- ProductionCapacity: 10000 Kilogram/Week
- Purity: 99.9999%
- Storage: as per buyer's request
- Transportation: Air, sea freight
- LimitNum: 1 Kilogram
- Grade: Industrial Grade,Pharma Grade
- 1: 2
Superiority
Physical and chemical properties
Na2SO4 is chemically very stable, being unreactive toward most oxidising or reducing agents at normal temperatures. At high temperatures, it can be reduced to sodium sulfide. It is a neutral salt, which forms aqueous solutions with pH of 7. The neutrality such solutions reflects the fact that Na2SO4 is derived, formally speaking, from a strong acid (sulfuric acid) and a strong base (sodium hydroxide). Sodium sulfate reacts with an equivalent amount of sulfuric acid to give an equilibrium concentration o the acid salt sodium hydrogen sulfate:
- Na2SO4( aq) + H2SO4(aq) → 2 NaHSO4(aq)
In fact the equilibrium is very complex and dependent on concentration and temperature, with other acid salts being present.
Na2SO4 is a typical ionic sulfate, containing Na+ ions and SO42− ions. Aqueous solutions can produce precipitates when combined with salts of Ba2+ or Pb2+, which form insoluble sulfates:
Na2SO4(aq) + BaCl2(aq) → 2 NaCl(aq) + BaSO4( s)
Sodium sulfate has unusual solubility characteristics in water, 3 as shown in the graph below. Its solubility rises more than tenfold between 0 °C to 32.4 °C, where it reaches a maximum of 49.7 g Na2SO4 per 100 g water. At this point the solubility curve changes slope, and the solubility becomes almost independent of temperature. In the presence of NaCl, the solubility of Na2SO4 is markedly diminished. Such changes provide the basis for the use of sodium sulfate in passive solar heating systems, as well is in the preparation and purification of sodium sulfate.
This nonconformity can be explained in terms of hydration, since 32.4 °C corresponds with the temperature at which the crystalline decahydrate (Glauber's salt) changes to give a sulfate liquid phase and an anhydrous solid phase.
Details
Physical and chemical properties
Na2SO4 is chemically very stable, being unreactive toward most oxidising or reducing agents at normal temperatures. At high temperatures, it can be reduced to sodium sulfide. It is a neutral salt, which forms aqueous solutions with pH of 7. The neutrality such solutions reflects the fact that Na2SO4 is derived, formally speaking, from a strong acid (sulfuric acid) and a strong base (sodium hydroxide). Sodium sulfate reacts with an equivalent amount of sulfuric acid to give an equilibrium concentration o the acid salt sodium hydrogen sulfate:
- Na2SO4( aq) + H2SO4(aq) → 2 NaHSO4(aq)
In fact the equilibrium is very complex and dependent on concentration and temperature, with other acid salts being present.
Na2SO4 is a typical ionic sulfate, containing Na+ ions and SO42− ions. Aqueous solutions can produce precipitates when combined with salts of Ba2+ or Pb2+, which form insoluble sulfates:
Na2SO4(aq) + BaCl2(aq) → 2 NaCl(aq) + BaSO4( s)
Sodium sulfate has unusual solubility characteristics in water, 3 as shown in the graph below. Its solubility rises more than tenfold between 0 °C to 32.4 °C, where it reaches a maximum of 49.7 g Na2SO4 per 100 g water. At this point the solubility curve changes slope, and the solubility becomes almost independent of temperature. In the presence of NaCl, the solubility of Na2SO4 is markedly diminished. Such changes provide the basis for the use of sodium sulfate in passive solar heating systems, as well is in the preparation and purification of sodium sulfate.
This nonconformity can be explained in terms of hydration, since 32.4 °C corresponds with the temperature at which the crystalline decahydrate (Glauber's salt) changes to give a sulfate liquid phase and an anhydrous solid phase.