Vijainagar, Ajmer and Sodium ferrioxalate

Contents 1 Demographics 2 Geography 3 Transportation 4 Economy 5 Temples 6 Education 7 References

Demographics

As of 2001 India census, Bijainagar had a population of 27,688. Males constitute 52% of the population and females 48%. Bijainagar has an average literacy rate of 69%, higher than the national average of 59.5%: male literacy is 78%, and female literacy is 60%. In Bijainagar, 14% of the population is under 6 years of age. Most of the population is Jain's. Geography

The town is famous for its high living standard and high property rates. Bijainagar's "Krishi Mandi" is second largest in terms of input of Cotton in the state of Rajasthan. Bijainagar has direct Rail connectivity with 4 metros cities i.e. Mumbai, Delhi, Hyderabad and Kolkata.

The main water source is Bisalpur Dam. Rajasthan's largest water treatment plant is connected with Bisalpur Dam. A dam in Para called Para 1 Dam is among the major irrigation dams in Ajmer District. Transportation

As it is situated between Railway track(Ajmer - Bhilwara) and National Highway 79(Dehli-Mumbai) so availability of public transportation is much better. Easily available long distance train and bus for Delhi, Mumbai, Hyderabad, Puna, Agra etc. Economy

It is mainly an industrial area, including the Agricultural Mandi (Market Yard),Cattle feed plants, Oil Mills, Woolen yarn mill, Flour Mills, Ceramic Industries, cotton & synthetic waste recycling plants and some other industries. Temples

Bijainagar has a large number of temples. The list is as follows:

1. Ganesh Mandir 2. Chamatkari Hanuman Mandir (Station wale Balaji) 3. Laxmi Narayan Mandir (Bada Mandir) 4. Shiv Mandir (Peepli Chouraha) 5. Shiv Mandir (Bapu Baazar) 6. Balaji Mandir (Sabji Mandi) 7. Shri Harshiddhi Ganesh Mandir (Chosla) 8. Mosque (Rajnagar) 9. Shwetamber Jain Mandir (Mahavir Bazar) 10. Shani Dev Mandir 11. Tejaji Mandir 12. Vishwakarma Temple 13. Gurudwara 14. Church 15. Digamber Jain Mandir (Sathana Baazar) 16. Nakoda Jain Temple (Rajdarbar colony) 17. Sitla mata mandir

Also famous Lord Ram Mandir is located in nearby town of Gulabpura. Famous temple of Badi Mataji is located in the nearby village Badi. Education

Government Senior Secondary Schools (separate for boys and girls),Shree Pragya College (PG College) and St. Paul School, Shree Pragya Public School (Achiveing High standards of scooling in the surrounding area, conducted by jain samaj of bijainagar) other English and Hindi medium private colleges and schools are present. Famous Vivekananda Kendra Vidhyalaya is also located in nearby to the town. Standard of education in the town are very high.

Sodium ferrioxalate and Vijainagar, Ajmer

Contents 1 Bonding 2 Solubility 3 Preparation 4 Isomerism 5 Photoreduction 6 Uses 7 See also 8 References

Bonding

The bonds to the iron atom are dative covalent bonds where the ligands, (oxalate ions, blue), donate a lone pair into the empty p and d orbitals of the transition metal (iron, red), atom. The three oxalate ions donate 12 electrons in all and Fe-III has three electrons in the d orbitals leaving 13 empty places in the remaining d and p orbitals. Solubility

This compound is very soluble in hot water, (182 parts per 100 parts solvent by mass), but a lot less soluble in cold water, (32 parts per 100 parts solvent), about the solubility of sodium chloride. It is not appreciably soluble in ethanol or ethanol water mixtures which are more than 50% ethanol by mass. It is somewhat more soluble in water than the corresponding potassium salt. Preparation Sodium trisoxalatoferrate crystals

The crystals pictured were synthesised by mixing solutions of sodium oxalate and ferric oxalate and waiting a few hours for the brown colour of the ferric oxalate to be replaced with the green colour of the complex anion. This complex is relatively inert and the equilibrium is attained only slowly at room temperature. The ferric oxalate was made by dissolving rust in oxalic acid and filtering off any residual insolubles. The solution was evaporated at just below boiling until small crystals appeared on the bottom indicating the solution was then hot and saturated. The solution was allowed to cool in a beaker sitting on a large aluminium block. The thermal mass of the block allowed sufficiently slow cooling over night to produce crystals a few millimetres long. These larger crystals are pictured at the upper left.

Fe2(C2O4)3 + 3 Na2(C2O4) → 2 Na3

Stoichiometry was not worried about and an excess of sodium oxalate was added, this is a lot less soluble in hot water than the ferrioxalate and crystallizes out first. The intensity of the green colour was used as a guide to concentration of the solution with respect to the complex. A few drops of 100 vol hydrogen peroxide were periodically added during the evaporation to maintain the iron in the III oxidation state and any insoluble ferrous oxalate was removed if it precipitated out.

The smaller crystals were recovered from the solution by placing it in the freezer after the large crystals had been removed. The smallest crystals, pictured at the lower right were precipitated from the cold solution by addition of methylated spirit. Isomerism

The ferrioxalate complex demonstrates optical activity since there are two non-superimposable stereoisomers of the complex. This is described in more detail under potassium ferrioxalate. Theoretically the two stereoisomers could be separated by crystallization of a diastereomeric salt of the optically inactive racemic mixture of ferrioxalate ions with an optically active cation, such as methylethylpropylammonium ion which is one pure enantomer. Thus methylethylpropylammonium ferrioxalate should crystallize out to produce crystals which are non superimposable mirror images. These would be Λ-methylethylpropylammonium Λ-ferrioxalate and Λ-methylethylpropylammonium Δ-ferrioxalate. Photoreduction

In solution the ferrioxalate complex is decomposed by light. This is described in more detail under potassium ferrioxalate. Some samples of the crystals were exposed to direct sunlight for a few hours, the larger crystals did not appear to be affected, however solutions and small crystals so exposed did change colour to a different shade of green.

If a solution containing both green ferrioxalate ions and colourless free oxalate ions is exposed to strong light, such as direct sunlight, the light allows the Iron-III to oxidize one of the oxalate ligands to carbon dioxide and gives the orange-brown ferrooxalate complex ion which is coordinated around an Iron-II centre, however, when placed in the dark the Iron-II is re-oxidized to Iron-III by the oxygen in the atmosphere and the green ferrioxalate complex ion re-forms. The orange-brown Iron-II complex starts to appear after around ten minutes exposure and after the passage of a few hours in direct sunlight more than half of the green Iron-III complex had been reduced. The re-oxidation in the dark is equally slow and observable under ambient electric lighting. If this process is allowed to repeat over many months, such as leaving a container outside where it is exposed to the sun each day, eventually almost all of the oxalate ions present are oxidized to carbonate and the iron remains as Ferric Hydroxide, Fe(OH)3.

This indicates that when exposed to the environment, particularly if that environment is damp the ferrioxalate ion is quite unstable and gradually decomposes via the above redox processes into much more stable and common compounds.

This light catalyzed redox reaction once formed the basis of some photographic processes, however due to their insensitivity and the ready availability of digital photography these processes have become obsolete and all but forgotten. Uses

In contemporary times ferrioxalate salts, usually the potassium salt, are used as examples of a transition metal ligand complexes which can be easily synthesized by high school, college or undergraduate university students to introduce them to transition metal ligand chemistry, as well as to redox chemistry in now-obsolete photographic processes.

The process of blueprint making, now also nearly obsolete, makes use of Iron-cyanide ligand complexes such as Ferricyanide and Ferrocyanide and redox reactions related to them. The presence of free Iron-II ions and cyanide ions gives rise to a whole family of Iron centered ligand complexes exhibiting intense blue colours. The best known of these is Prussian blue, Potassium Ferrous Ferrocyanide. See also

A number of other iron oxalates are known Iron(II) oxalate Iron(III) oxalate Potassium ferrioxalate
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