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Sodium Thiosulphate

Sodium Thiosulphate

The chemical formula Na2S2O3 represents Sodium Thiosulfate, a crystalline compound composed of sodium (Na), sulfur (S), and oxygen (O). Let’s understand its properties and applications in detail

1.0What is Sodium Thiosulfate

Sodium thiosulfate (Na2S2O3) is a salt composed of sodium (Na+), sulfur (S), and oxygen (O). It is a white, crystalline substance that dissolves readily in water. The compound consists of two sodium ions and one thiosulfate ion (S2O32-). The thiosulfate ion is an interesting structure with a sulfur atom at the center, bonded to three oxygen atoms and another sulfur atom. The overall charge on the thiosulfate ion is -2.Sodium thiosulphate molecular weight  is 158.11 grams per mole. The more commonly available pentahydrate form, Na2S2O3·5H2O, has a molar mass of 248.18 g/mol.

Here is a representation of the Crystals of Sodium Thiosulphate

Crystals of Sodium thiosulphate

Sodium thiosulfate is prepared by neutralizing sulfur dioxide with sodium hydroxide and is often encountered as the pentahydrate Na2S2O3·5H2O, a colorless, monoclinic crystalline substance that is readily soluble in water.

The name "thiosulfate" is derived from the presence of sulfur and oxygen in the molecule. In chemical reactions, sodium thiosulfate can undergo various transformations, including redox reactions where it can either gain or lose electrons. Understanding its chemical structure and reactivity is crucial for its diverse applications in photography, medicine, water treatment, and analytical chemistry.

2.0Structure of Sodium Thiosulphate

Structure of Sodium Thiosulphate

3.0Physical Properties of Sodium Thiosulphate 

Sodium thiosulfate (Na2S2O3) has several notable physical properties:

State

Solid, white, crystalline powder

Solubility

highly soluble in water

Molar Mass

158.11 g/mol.

Melting Point

48 °C

Hydrate Form

Pentahydrate (Na2S2O3·5H2O)

Density

1.667 g/cm³

4.0Chemical Properties of Sodium Thiosulfate

Sodium thiosulfate (Na2S2O3) exhibits various chemical properties due to its composition and the nature of the thiosulfate ion. Here are some key chemical properties:

  • Redox Properties: Sodium thiosulfate is involved in redox reactions. It can act as both an oxidizing agent and a reducing agent. In the presence of strong acids, it can be oxidized to form sulfur or sulfur dioxide. In other reactions, it can undergo reduction.
  • Reaction with Acids: Sodium thiosulfate reacts with acids, such as hydrochloric acid (HCl), to produce sulfur dioxide, sulfur, and water. The reaction is commonly used in analytical chemistry to generate a standardized solution of iodine for titrations.

                       Na2S2O3    +  2 HCl     →    2 NaCl  +  S  +  SO2  +  H2O

  • Complex Formation: Thiosulfate ions can form complexes with metal ions. In the presence of certain metal ions, thiosulfate can act as a ligand, forming coordination complexes.
  • Tetrathionate Formation: In alkaline conditions, sodium thiosulfate can undergo further reactions to form tetrathionate ions (S4O62-). This property is sometimes utilized in analytical chemistry for specific reactions.
  • Dechlorination: Sodium thiosulfate is known for its ability to dechlorinate water. It reacts with chlorine to form sodium chloride and sulfate:

                      2Na2S2O3   +      4Cl2      →    4NaCl    +    2Na2SO4

  • Photographic Fixing: In photography, sodium thiosulfate is used to fix developed silver halide crystals by converting them into a water-soluble complex, preventing further exposure to light.

5.0Applications of Sodium Thiosulphate 

Sodium thiosulphate ( Na2S2O3 ) finds applications in various industries and scientific fields due to its unique properties. Some notable applications include:

1. Photography: Sodium thiosulphate solution is a key component in photographic fixing solutions. It is used to remove unexposed silver halide from developed photographic emulsions, stabilizing the final image.

2. Medical Use: Sodium thiosulfate is employed as an antidote for cyanide poisoning. It forms a complex with cyanide ions, reducing their toxicity. This application is critical in emergency medicine.

3. Water Treatment: Sodium thiosulphate solution is used to dechlorinate water. It reacts with chlorine, neutralizing its presence in tap water, swimming pools, and wastewater before discharge.

4. Analytical Chemistry: Sodium thiosulfate is widely used in analytical chemistry for titrations, particularly in the determination of iodine concentration. It is also used to standardize solutions of other substances.

5. Gold Extraction: In certain gold extraction processes, sodium thiosulfate is used as an alternative to traditional cyanide-based methods. This is especially relevant in environmentally conscious mining practices.

6. Chemical Reduction Reactions: Sodium thiosulfate is involved in redox reactions, serving as both an oxidizing and reducing agent. This versatility makes it useful in various chemical processes and experiments.

7. Hair Care Products: In the cosmetic industry, sodium thiosulfate is used in hair care products to neutralize or remove residual hair dyes, preventing discoloration.

8. Wastewater Treatment: It is utilized to neutralize excess chlorine in wastewater before discharge, contributing to environmental protection.

6.0 Preparation of Sodium Thiosulphate

(i)

Preparation of Sodium Thiosulphate


(ii)     2Na2S + Na2CO3 + 4SO2       →     3Na2S2O3 + CO2

(iii)    6NaOH + 4S               →    Na2S2O3 + 2Na2S + 3H2O

         3Ca(OH)2 + 12 S        →    CaS2O3 + 2CaS5 + 3H2O

(iv)    Na2SO3 + Na2S + I2    →     Na2S2O3 + 2NaI (spring reaction)

(v)     2Na2S + 2O2 + H2O    →     Na2S2O3 + 2NaOH

[Na2S is readily oxidised in air giving rise to Na2S2O3]

7.0Reactions of Sodium Thiosulphate

  1. Reaction with Iodine (I2): In this reaction, sodium thiosulfate reacts with iodine to form sodium iodide and sodium tetrathionate.

           Na2S2O3    +   I2               →   Na2S4O6    + 2NaI 

  1. Reaction with Chlorine Water (Cl2 in water): In the presence of water, chlorine reacts with sodium thiosulfate to form sodium bisulfate, hydrochloric acid, and sulfuric acid.

Na2S2O3       +  Cl2 – water     →    NaHSO4  + S + 2HCl

  1. Reaction with Bromine Water (Br2 in water): Similar to chlorine water, bromine water reacts with sodium thiosulfate in the presence of water to produce sodium bisulfate and sodium bromide.

Na2S2O3       +  Br2 – water     →   NaHSO4   + S + 2HBr

  1. Reaction with Chlorine (Cl2):Chlorine reacts with sodium thiosulfate to produce sodium chloride and sodium tetrathionate.

Na2S2O3       +  4Cl2 + 5H2O     →  Na2SO4 + H2SO4 + 8HCl

↓

2NaHSO4

Table of Contents


  • 1.0What is Sodium Thiosulfate
  • 2.0Structure of Sodium Thiosulphate
  • 3.0Physical Properties of Sodium Thiosulphate 
  • 4.0Chemical Properties of Sodium Thiosulfate
  • 5.0Applications of Sodium Thiosulphate 
  • 6.0 Preparation of Sodium Thiosulphate
  • 7.0Reactions of Sodium Thiosulphate

Frequently Asked Questions

The uses of sodium thiosulphate are involved in various applications, including photographic fixing, as an antidote for cyanide poisoning, in water treatment to dechlorinate water, and in analytical chemistry for titrations.

In photography, sodium thiosulfate is used as a fixing agent. It reacts with unexposed silver halide crystals, converting them into a water-soluble complex, which prevents further exposure to light and stabilizes the final image.

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