Sodium carbonate decahydrate

Another mining process involves the recovery of sodium carbonate decahydrate from alkaline ponds. EMC mines this material from its solar evaporation pond using a bucket wheel dredge. The decahydrate slurry is dewatered, melted, and processed to soda ash. 

Bromophenol blue Potassium permanganate Sodium carbonate decahydrate Ethanol... 

Sodium carbonate decahydrate, Na2CO3-10H2O, was once widely used as washing soda. It is still sometimes added to water to precipitate Mg2+ and Ca2+ ions as carbonates, as in... 

Solution IV Dissolve 10 g sodium carbonate decahydrate in 100 ml water. Method ... 

Dissolve 173 g /n-sodium citrate dihydrate and 270 g sodium carbonate decahydrate in 600 ml water. 

Copper(II) sulfate pentahydrate tn-Sodium citrate dihydrate Sodium carbonate decahydrate... 

Sodium carbonate decahydrate Sodium carbonate anhydrous Methanol... 

The addition must be regulated so as to prevent the formation of large chunks of sodium carbonate decahydrate. 

Substances (hat are ordinarily efflorescent are sodium sulfate decahy-drate. sodium carbonate decahydrate. magnesium sulfate hcpiahydrate. and ferrous sulfate hepiahydrale. When the saturated solution of a substance in water has a water vapor pressure greater than that of the surrounding atmosphere, evaporation of the water from solution takes place. 

Some crystal hydrates effloresce, that is they lose some or all of their water of crystallisation to the atmosphere. For example, when colourless sodium carbonate decahydrate crystals are left out in the air they become coated with a white powder, which is the monohydrate (Figure 8.22). The process is called efflorescence. 

Figure 8.22 A white powder forms on the surface of sodium carbonate decahydrate when it is left in the air.

Sodium carbonate decahydrate effloresces quite readily. With some substances, such as solid sodium hydroxide, the reverse of efflorescence occurs - they deliquesce. There are some substances, such as concentrated sulfuric acid, which when left open to the atmosphere are diluted - they are hygroscopic. 

A solution of 219 g (1 mol) of a-(p-chlorophenyl)-2-pyridinemethanol in one liter of dry toluene is heated to 100°C with stirring. Twenty-three grams (1 g-atom) of sodium are then added in portions. After all the sodium has reacted, a dried solution of 2-dimethylaminoethyl chloride in benzene is added. This benzene solution is prepared by dissolving 173 g (1.2 mols) of 2-dimethylaminoethyl chloride hydrochloride in the minimum amount of water, adding 500 cc of benzene followed by 300 g of sodium carbonate decahydrate, stirring, separating the benzene layer and drying. 

If you wish, you can remove some of these ions (mainly Ca2+(aq), Mg2+(aq), and Fe2+(aq)) yourself. For relatively small volumes of water (such as enough to fill a bathtub or a washing machine), you can add sodium carbonate decahydrate, Na2CO3-10H2O. This compound is commonly called washing soda. It is an inexpensive way to add carbonate ion to the water. The carbonate ions precipitate the unwanted ions. 

Pour the mixture slowly onto crushed ice (50 g) in a beaker (250 mL) and stir the mixture while adding solid sodium carbonate decahydrate (100 g). Filter off the precipitated product using a sintered glass funnel and wash it with ice-cold water (5 mL). 

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