What is the best Distillation process to recover pure acid from used acetic acid in a rubber industry?
341747
first vapour it all if there is no rubber monomer vaporize then try a distilation tower with hysys if u want i can simulate it for u?
884674
Distill it.\n\nIn cooking, supposedly you can put a piece of raw potato (sometimes, the hint says a piece of lettuce) in food that's too salty and it takes the salt out.  But I don't know if that works.  I'd go with distillation.  \n\nDistillation is where you boil a liquid and then catch the vapor and condense it.  In the case of salt water, the vapor would be plain water with nothing dissolved in it (the salt gets left behind in whatever you use to boil the liquid in.)  Distillation is also used to make an alcoholic liquid more alcoholic.  I guess the alcohol gets vaporized and condensed.
431802
You are not going to be able to buy nitric acid above 70% pure.  Nitric acid pretty much dissolves anything it comes in contact with which causes for its low purity.  I would not suggest heating concentrated acid since the fumes it will produce are very dangerous.  The fumes at room temperature will even cause burns. Depending on what you are trying to do, the acid will need some oxygen to dissolve metals.  With stainless steel, a small scratch on the surface will be enough.
99880
Glacial Acetic Acid freezes/melts at slightly under room temperature (62.1F,16.7C).
721022
Well, I do not know that syllabus.  You will need to sift useful answers.\n\nI would use:\n\ndifferent solubility in solvents\ndifferent boiling points\nrecrystallise one out of a mixed solution\n\nYou might be at too junior a level to know about ion exchange resins, and other chromatography techniques.
498348
LIQUID-VAPOR EQUILIBRIUM IN BINARY SYSTEMS\nApparatus\nBoiling apparatus with heating mantle and variac (S), 1/100o thermometer (S),\nrefractometer (L), glass beads or boiling chips (S), weighing bottles (D), small\nstoppered vials (D), 250 ml n-hexane (S) and 250 ml absolute ethanol (S).\nOther binary systems which may be investigated are (1) cyclohexane (S)-\nethanol (S); (2) ethyl acetate (S)-ethanol (S); (3) Methanol (S)-ethyl acetate (S);\n(4) isopropanol (S)-n-hexane (S); (5) isopropanol (S)-cyclohexane (S); (6)\nisopropanol (S)-ethylacetate (S); (7) Acetone (S)-cyclohexane (S); (8) Acetone\n(S)- hexane (S); and (9) cyclohexane (S)-2-propanol (S), (10) 1 Propanol-water.\nCONSULT YOUR LAB INSTRUCTOR TO FIND OUT WHICH SYSTEM YOU\nARE TO INVESTIGATE.\nCAUTION: The ORGANIC LIQUIDS are TOXIC and FLAMMABLE! Use all\nnecessary precautions to avoid accidents!\nCAUTION: DISPOSE OF THESE ORGANIC LIQUIDS by placing in the\nWaste Containers provided. DO NOT POUR DOWN THE DRAIN!\n\nAssemble the apparatus with care; consult instructor if you are at\nall doubtful how to put the pieces together. A 3-way stopcock (shown in Figure\n2) is provided as a means of withdrawing samples of distillate and residue at the\nappropriate time. Best procedure is to withdraw distillate first, then the residue.\n\nProcedure\nClean the apparatus by rinsing with a few milliliters of pure n-hexane. Make sure\nvials are clean and DRY and have labels for marking. Add glass beads to flask\n(carefully).\nThere are three particularly important requirements in this experiment.\n• Make sure that the condensed distillate and the liquid residue samples are\ncollected under equilibrium conditions\n• Read the equilibrium temperature accurately\n• Analyze the compositions accurately\nPlace the thermometer in a position near the top and center of the three legs of\nthe first insert as seen in Figure 3. The hole in the second insert should be\nplaced pointed towards the condenser\nPlace 50 ml n-hexane in a flask. Adjust the variac (not more than 100 -110 volts)\nso that liquid boils "reversibly" (very moderate boiling with only very tiny bubbles\nformed) and so that distillate comes over at a rate which will fill the sample tube\nonce every two or three minutes.\nDraw off the first fraction (containing impurities) which comes over and discard\n(use waste container). When a constant boiling mixture is obtained, record the\nboiling point and withdraw samples from distillate and residue into marked vials.\nAdd 1 ml ethanol to the distillate in the flask, obtain equilibrium-boiling, record the\nboiling point, and again withdraw samples of distillate and residue for analysis.\nBoiling points and refractive indices of the distillate and residue are then\ndetermined after successive additions of 0.2, 0.5, 1, 2, 5 and 5 ml of ethanol. The\nrefractive indices are used to obtain the mole fractions of ethanol in these\nsolutions.\nClean the apparatus by rinsing with a few milliliters of ethanol, and repeat the\nprocess starting with 50 ml of ethanol in the flask. Now, however, boiling points\nare to be determined after successive additions of 0.5, 1, 2, 5, 15 and 20 ml of nhexane\nto the flask.\nIn order to construct a plot of refractive index versus mole percent ethanol, the\nrefractive indices are determined for the pure hexane and ethanol and for a\nseries of solutions containing accurately known weights of hexane and ethanol.\nMixtures about 5 ml in volume containing approximately 1 volume of ethanol to 1,\n3, and 6 volumes of hexane are convenient. To obtain a decent standardization\ncurve of refractive index versus mole fraction, a series of 6 to 8 solutions\ncontaining accurately known weights of n-hexane and ethanol must be prepared\nand their refractive indices measured. Only a few milliliters of each of these\nsolutions are required, so do not waste chemicals when preparing them. The\nrequired data for the vapor pressures of the organic liquids are availab
986526
Sulfuric acid has a higher dissociation constant than acetic acid.  This means that more of it will dissociate in solution.\nAlso, sulfuric acid has 2 hydrogen atoms  that it can give up to solution vs. 1 from acetic acid.
197519
acetic acid is vinegar.  used for cooking, cleaning, stripping of other chemicals.  You name it
653092
A 30% Acetic Acid solution has a density of 1.05 g/mL.  Water has a density of 1.0 g/mL.  So it is reasonable to assume that Acetic acid ("vinegar") is more dense than water, but the two are very, very close indeed.\n\nWhen you dissolve Acetic acid in water, the two mix to form a solution.  It is not easy to distill away the acetic acid from the water.\n\nJust because something is more/less dense than water does not necesarily mean it has a lower/higher boiling point.
653331
As said before you can do the classic baking soda and vinagar, but a more dramatic reaction between sulfuric acid and sugar. Mix concentrated sulfuric acid and sugar in a well ventilated glass beaker or container and the acid will dehydrate the sugar leaving a stack of pure carbon
666889
Part of pharmaceutical manufacture involves solvents such as isopropyl alcohol which are driven off during the process. Typically, the volatile solvents are incinerated because letting them just go to the atmosphere is considered pollution.  An attractive option to VOC incineration is solvent recovery. This is a process whereby the process hydrocarbon is sent not to an incinerator but to a bed of activated carbon or zeolite. This material has the unique property by which hydrocarbons are highly attracted and adsorb to it. This functionally filters the hydrocarbon from the process stream effectively removing the pollutant.  The hydrocarbon on the carbon may then be de-sorbed and processed such that the hydrocarbon is recovered. The recovered hydrocarbon may then be re-processed, saving the manufacturer the cost for more solvent. This amounts to a huge cost savings in manufacturing the product, as upwards of 95% or more of the solvent is driven off the product and upwards of 98% of the solvent is filtered from the stream. That means that more than 93% of the solvent may be recovered and reused. Solvent recovery systems, when properly applied will actually pay for themselfs in recovered solvent within 2 years.
1166443
It is not possible to obtain absolute alcohol by simple fractional distillation, because a mixture containing around 95.5% alcohol and 4.5% water becomes an azeotropic mixture. In one common industrial method to obtain 100% pure alcohol, a small quantity of benzene is added to rectified spirit and the mixture is then distilled. Because a small amount of the benzene used remains , the solution is carcinogenic. So production of absolute alcohol is done by desiccation using glycerol. Alcohol produced by this method is known as spectroscopic alcohol.
905536
react ... water gas that is carbon monoxide and hydrogen gas in presence of zinc oxide and Cr 2 O 3 under 200 atm pressure and 450 degree celcius temperature result will be  methanol .. this process is done on industrial scale as well first the purification and then the compression takes place and into the reaction chamber condensed and got the result ... ok wish u best of luck
1033934
Nitric acid is made by mixing nitrogen dioxide (NO2) with water. Creating a very pure nitric acid usually involves distillation with sulfuric acid, as nitric acid forms an azeotrope with water with a composition of 68% nitric acid and 32% water. Commercial grade nitric acid solutions are usually between 52% and 68% nitric acid. Commercial production of nitric acid is via the Ostwald process after Wilhelm Ostwald.\n\nNitric acid can be made from Copper(II) nitrate or by reacting 200 g of potassium nitrate (KNO3) in 106 ml of 96% sulfuric acid (H2SO4), and distilling this mixture at nitric acid's boiling point of 83 °C until only a white crystalline mass, potassium hydrogen sulfate (KHSO4), remains in the reaction vessel. The obtained red fuming nitric acid may be converted to the white nitric acid. Note that in a laboratory setting, it is necessary to use all-glass equipment, ideally a one-piece retort, because nitric acid attacks cork and rubber, and leaks can be extremely dangerous.\n\nThe dissolved NOx are readily removed using reduced pressure at room temperature (10-30 min at 200 mmHg or 27 kPa). Obtained white fuming nitric acid has density 1.51 g/cm³. This procedure can also be performed under reduced pressure and temperature in one step in order to produce less nitrogen dioxide gas.\n\nThe acid can also be synthesized by oxidizing ammonia, but the product is diluted by the water also formed as part of the reaction. However, this synthesization method is important in producing ammonium nitrate from ammonia derived from the Haber process, because the final product can be produced from nitrogen, hydrogen, and oxygen as the sole feedstocks.\n\nWhite fuming nitric acid, also called 100% nitric acid or WFNA, is very close to the anhydrous nitric acid product. One specification for white fuming nitric acid is that it has a maximum of 2 % water and a maximum of 0.5 % dissolved NO2. Red fuming nitric acid, or RFNA, contains substantial quantities of dissolved nitrogen dioxide (NO2) leaving the solution with a reddish-brown color. One formulation of RFNA specifies a minimum of 17% NO2, another specifies 13% NO2. In either event, an inhibited fuming nitric acid (either IWFNA, or IRFNA) can be made by the addition of 0.6 to 0.7% hydrogen fluoride, HF. This fluoride is added for corrosion resistance in metal tanks (the fluoride creates a metal fluoride layer that protects the metal)
842422
Yes, it is true that the density of a solution is different of solvant but tjis difference is small ; So , i propose to dissove 40g of amyl acetate in a liter of water if that acetate is a solid. If that acetate is aliquid the total volume will be 1.04 l and you must use 47 cc tp water
784896
fractional distillation
861653
treat the mixture with sodium carbonate solution and then filter it to separate iron. the filtrate contains sodium benzoate. Liberate benzoic acid by just adding any mineral acid like sulfuric acid. Then u will get the crystals of benzoic acid. This can be filtered off