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Sodium Carbonate-1

Characteristics of Sodium Carbonate

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Sodium Carbonate-1

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  1. PRESENTATION TOPIC: 1. Sodium Carbonate 2. Sodium Nitrite 3. Magnesium Carbonate Presented to: prof. Dr. Jawad Ahmed Khan Presented By: Muhammad Mubashir-024 Rabel Hussain-029 Wali Muhammad-048

  2. Sequence of Presentation

  3. CCURRENCE Sodium carbonate • Sodium carbonate Na2CO3.10H20 ( also known as washing soda, soda ash and soda crystals) is the inorganic compound with the formula Na2CO3 and its various hydrate. • Occurrence: • Sodium carbonate occurs naturally in minerals form as its hydrate salts( such as trona, natron, thermonatrite etc) • These are several of its mineral deposits found in dry and arid regions around the world.

  4. Propertiesof Sodium Carbonate 1. Physical Properties: • Sodium Carbonate is a white crystalline powder. • Sodium Carbonate is odorless, water soluble salts that yield moderately alkaline solutions in water. • Sodium carbonate has density 2.54 g/ml. • Sodium carbonate has melting point 851 C. • Sodium carbonate boiling point is 1600 C.

  5. 2. Chemical Properties • Sodium carbonate is stable but hygroscopic solid( absorbs water from air) and readily dissolves in water to form weakly acidic carbonic acid and the strong base, sodium hydroxide. • The aqueous solution of Na2CO3is overall a strong base. It react violently with many acids . • When Na2CO3heated to high temperature, it decomposes to emit toxic fumes of Disodium oxide (Na2O). • Sodium carbonate is the disodium salt of carbonic acid with alkalinizing property.

  6. PREPARATION • Sodium carbonate is prepared from sodium chloride (NaCl) by “ammonia Solvay process”. • The raw materials used are sodium chloride, limestone and ammonia gas. The process involve three important steps. Step-I: Ammoniationof Brine In this step a saturated solution of sodium chloride ( about 28% by mass) or brine is allowed to flow down an ammoniating tower. The tower consists mushrooms shaped baffles at short intervals which control the flow of brine and ensures proper saturation with ammonia passing up the tower.

  7. Step-II: Carbonation of Ammoniated Brine • In this step ammoniated brine is allowed to trickle down a carbonated tower, called SOLVAY TOWER fitted with baffle-plates and meets an upward current of carbon dioxide gas obtained by heating limestone. The baffle-plates check the flow of liquid and break up the carbon dioxide into small bubbles to ensure good conditions for the reaction. The carbon dioxide and ammonia react to give NH4+ and HCO3- ions. 2NH3(g)+ CO2(g) + H2O(l)2NH4(aq) + CO3-2(aq)

  8. CO32- (aq)+CO2 (g)+H2O(l)2HCO3- (aq) • Hydrogen Carbonate ion (Bicabonate ion) • i.e. • I- 2NH3+CO2+H2O (NH4)2+1 CO3-2(aq) • II- (NH4)2+1CO3-2(aq)+CO2(g) + H2O (l) 2NH4+1HCO3-1(aq)

  9. Step-III: Conversion to Sodium Carbonate • The Sodium hydrogen carbonate is heated to give anhydrous sodium carbonate (Soda ash) 2NaHCO3 (g) Na2CO3 (g)+ H2O (l)+CO2 (g) Sources of Materials • Brine is obtained from natural sources of common salt • Carbon dioxide is obtained by heating lime stone • Ammonia is recover from the solution of ammonium chloride left after the removal of NaHCO3by vacuum filtration.

  10. Applications • Sodium carbonate (washing soda) is used as a cleansing agent for domestic purpose like washing cloths. • Sodium carbonate is used for removing temporary and permanent hardness of water. • Sodium carbonate is used in the manufacturing of glass and water glass. • Sodium carbonate is used in the making of soap, paper, detergents and chemicals such as NaOH. • Sodium carbonate is used in the manufacture of sodium compounds like borax. • Sodium carbonate is used in toothpaste where it acts as foaming agent. • Sodium carbonate is used as laboratory reagent . • Sodium carbonate is used as food additive as anticaking agent, as raising agent and as stabilizer, etc. • Sodium carbonate is used in the production of rayon polymers. • Sodium carbonate is used in the brick industry.

  11. Sodium Nitrite Sodium nitrite is an inorganic compound with the chemical formula NaNO2.Sodium nitrite is a chemical compound. It contains sodium and sodium and Nitrate ions. Occurrence : It is found in some vegetables. It is also found in some merit in small amounts. Otherwise, it is man made.

  12. Properties Physical properties : • Sodium nitrate is white or white yellowish hygroscopic solid, soluble in water and slightly soluble in primary alcohols. While insoluble in alkanes and chlorocarbons it has a density of 2.168 g/cm3. It melts when heated to 271 °c and will also decompose with significant decomposition starting above 320°c. • It is a white or yellowish crystalline compound. It is a strong oxidizing agent, being reduced to nitrogen. It is also a weak reducing agent being oxidized to nitrate.it contains nitrogen in its +3 oxidation state it is toxic in large amounts. Chemical properties : • Sodium nitrite will react with sodium chloroacetate in aqueous solution to give nitro methane : NaNo2 + ClCH2 COONa+ H20 CH3 NO2 + NaCl+NaHCO3

  13. Preparations: • There are many ways to prepare sodium nitrite. A known process involves the reduction of sodium nitrate with metallic lead about 8.5 g of powdered NaNo3 is mixed with 21g of lead and heated until it melts. The mixture is kept liquid and stirred / agitated for 30-45 minutes until all the lead is oxidized to lead (ll) oxide forming sodium nitrate. NaNO3 +Pb NaNO2+PbO • The resulting 5kg is grounded and the sodium nitrite is purified by recrystallizing it form water. This procedure has the disadvantage of contaminating the product with lead oxide, making it less safe to handle without proper protection .It is also temperature sensitive. The thermal reduction of sodium nitrate with calcium sulfite will also yield sodium nitrite. NaNo3 + CaS03 NaN02 +CaSO4. • Calcium sulfamate can also be used. Another method involves heating sodium nitrite with carbon in the presence of Sodium hydroxide or Calcium hydroxide. 2NaN03+2NaOH+C 2NaNO2+Na2CO3+H20 2NaN03+Ca(0H)2+C 2NaN02+CaC03+H20 .

  14. The later method is preferred as calcium carbonate is insoluble in water and can be easily removed from the 5kg. A mixture of aluminum powder and sodium nitrite heated for 40 minutes will yield sodium nitrite. • The industrial route involves treating aqueous solution of sodium hydroxide with a mixture of nitrogen dioxide and nitric oxide: 2NaOH+NO2+NO 2NaNO2+H2O • This reaction is air sensitive and traces of oxygen will lead to sodium nitrite • Very pure sodium nitrite can be obtained by reacting nitrous acid (which can be obtained by adding Dinitrogentrioxide to pure water)with sodium hydroxide.

  15. Applications • The main use of sodium nitrite is for the industrial production of organonitrogen compounds. • Sodium nitrite is used to speed up the coming of meat and also impart an attractive pink color. • It means sodium nitrite is used as food additive. • Sodium nitrite is also used as bleaching agent and dye. • Sodium nitrite used in the production of herbicides organic pesticides. • Sodium nitrite is used as polymer inhibitors and as lubricant. • Sodium nitrite is used as antimicrobial agent.

  16. Magnesium Carbonate. Magnesium Carbonate is an inorganic compound with the Chemical Formula MgCO3. Occurrence: • Magnesium Carbonate is largely found in nature. • It is found in a diverse range of minerals such as the magnesite, artinite and dypingite. • Magnesium Carbonate MgCO3 also occur in nature as the mineral magnesite and is an important source of elemental magnesium.

  17. Properties Physical properties: • Magnesium Carbonate is a white, hygroscopic, odourless,solid. • The density of this salt 2.95g/ml for the anhydrous salt, however the density decreases with the degree of hydration, being 1.73g/ml in the Pentahydrate salt. • The Melting point is 350°c for the anhydrous and above the Melting point, the salt decompose. Magnesium Carbonate is almost insoluble in water and acetone. It is soluble in acid solutions. Chemical properties: • Magnesium Carbonate is able to react with acids to form a binary salt that depends on the anion formed from the acid used for the reaction. Similarly to the behavior expected for Carbonate (Calcination reaction),when magnesium carbonate is heated, it decomposed to form an oxide and CO2 : MgCO3 MgO+CO2.

  18. Preparation: • Magnesium Carbonate is ordinarily obtained by mining the mineral magnesite. Seventy percent of the world's Supply is mined and prepared in China. • Magnesium Carbonate can be prepared in laboratory by reaction between any soluble magnesium salt and sodium bicarbonate: • MgCl2 (aq)+2NaHCO3 (aq)MgCO3 (s+2 Nacl(aq)+H20 (I)+CO2 (g) • If Magnesium Chloride (or sulfate)is treated with aqueous sodium carbonate, a precipitate of basic magnesium carbonate- a hydrated complex of magnesium carbonate and magnesium hydroxide rather than Magnesium carbonate itself is formed: 5MgCl2 (aq) + 5 Na2C03(aq) + 5 H20 (I)Mg (OH)2.3 MgCO3.3 H20 (s) + Mg (HC03)2(aq) + 10 Nacl(aq) • High purity industrial routes include a path through Magnesium bicarbonate ,which can be formed by combining a slurry of Magnesium hydroxide and Carbon dioxide at high pressure and moderate temperature . The bicarbonate is the than vacuum dried, causing it to lose carbon dioxide and a molecule of water: Mg(OH)2+2CO2 Mg(HCO3)2 Mg(HCO3)2 MgCO3+CO2+H2O

  19. Applications • The primary use of magnesium carbonate in the production of magnesium Oxide by Calcining. • Magnesium Carbonate MgC03 is also used in flooring, Fireproofing, Fire extinguishing compositions, cosmetic, dusting powder, and toothpaste. • Other applications are as filler material, smoke suppressant in plastics, a reinforcing agent in neoprene rubber, a drying agent, a laxative to loosen the bowels and color retention in foods. • Magnesium Carbonate is used as a food additive. • Magnesium Carbonate is used in taxidermy for whitening skulls. • Magnesium Carbonate is used as antacid and fertilizer.

  20. Reference of Sodium Carbonate • https://en.m.Wikipedia.org • https://www.scienecedirect.com • https://www.softschools.com • https://www.vedantu.com • Chemistry Sindh Text Book Board Class XII Page No. 32- 34

  21. References of Sodium Nitrite • https: //www science direct.com • https:// en.m.wikipedia.org. • https://Simple in wikipedia.org References of Magnesium Carbonate • https://en.m.wikipedia.org. • https://www.soft schools.com. • https:// knowledge Ulprospector.com

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