Sodium chloride (chemical formula NaCl), known as table salt , rock salt, sea salt and the mineral halite, is an ionic compound consisting of cube-shaped crystals composed of the elements sodium and chlorine . This salt has been of importance since ancient times and has a large and diverse range of uses.

The most common compound of sodium is sodium chloride (common salt). It is added to food and used to de-ice roads in winter. It is also used as a feedstock for the chemical industry. Sodium carbonate (washing soda) is also a useful sodium salt. It is used as a water softener.

Not combustible, but substance is a strong oxidizer and its heat of reaction with reducing agents or combustibles may cause ignition. Explosion: Explosive with shock, heat or friction. Sodium Nitrate decomposes explosively when heated > 538C (1000F).

Sodium nitrate

Acute Potenial Health Effects: Skin: It may cause mild skin irritation. Eyes: Can cause mechanical eye irritation. Inhalation: May cause upper respiratory tract and mucous membrane irritation. Ingestion: Sodium Thiosulfate is an agent with a low order of toxicity.

7.0 – 9.0

Sodium thiosulfate crystallin from TIB Chemicals makes an important contribution to health and can be dissolved in water or tea and used as a drink once a day. The external application is also possible, for example as a foot bath together with baking powder or for massages.

Most important symptoms and effects, both acute and delayed Inhalation May cause respiratory irritation. Ingestion May cause discomfort or nausea. Skin contact Not available Eye contact May cause eye irritation and redness.

Adding chlorine and chloramines to our drinking water is very important to keep people healthy. But the same chemicals which keep us safe can be very toxic to fish. They both include sodium thiosulfate, which reacts with the chlorine (or the chlorine portion of the chloramine) to form harmless chloride ions.

Flammability of the Product: Non-flammable. Auto-Ignition Temperature: Not applicable.

When sodium thiosulphate is added to a solution of hydrochloric acid, an insoluble precipitate of sulphur (S) is formed. This transforms the solution from being colourless to being milky and entirely opaque.

Hydrochloric acid solution is corrosive to eyes and skin. It is moderately toxic by ingestion and inhalation. Sodium thiosulfate solution is a body tissue irritant. The reaction of sodium thiosulfate and hydrochloric acid generates sulfur dioxide gas, which is a skin and eye irritant.

The Rate of Reaction in the Reaction Between Hydrochloric Acid and Sodium Thiosulphate. the reaction between hydrochloric acid and sodium thiosulphate. the reaction between hydrochloric acid and sodium thiosulphate. exothermic reaction will increase to give out more heat.

This application as a photographic fixer was discovered by John Herschel. It is used for both film and photographic paper processing; the sodium thiosulfate is known as a photographic fixer, and is often referred to as ‘hypo’, from the original chemical name, hyposulphite of soda.

Thiosulfuric acid (as sodium thiosulfate) has the chemical name thiosulfuric acid, disodium salt, pentahydrate. The chemical formula is Na2S2O3•5H2O and the molecular weight is 248.17.

) (IUPAC-recommended spelling; sometimes thiosulphate in British English) is an oxyanion of sulfur. The prefix thio- indicates that the thiosulfate ion is a sulfate ion with one oxygen replaced by sulfur. Thiosulfate occurs naturally and is produced by certain biochemical processes.

As nouns the difference between thiosulphate and sulfate is that thiosulphate is a salt of thiosulphuric acid while sulfate is (organic chemistry) any ester of sulfuric acid.

Sodium thiosulfate (sodium thiosulphate) is an inorganic compound with the formula Na2S2O3. xH2O. Typically it is available as the white or colorless pentahydrate, Na2S2O3·5H2O. The solid is an efflorescent (loses water readily) crystalline substance that dissolves well in water.

In an iodometric titration, a starch solution is used as an indicator since it can absorb the I2 that is released. This absorption will cause the solution to change its colour from deep blue to light yellow when titrated with standardised thiosulfate solution. This indicates the end point of the titration.