Organic chemistry question on acid/base extraction?
A solvent such as ether, dichloromethane or chloroform will dissolve both components. The addition of 3M HCl will protonate the aniline nitrogen, making it highly charged and thus more water soluble. Naphthalene is not water-soluble, and will stay in the organic layer. Separate the layers. The organic layer has naphthalene in it, and the aqueous layer has 4-nitroaniline ydrochloride. To isolate the aniline, you would add base. The free amine may precipitate; if not, it will be soluble in the organic solvent you used before. You can then separate the layers again, and 4-nitroaniline will be in the organic layer. The only reaction taking place is an acid-base reaction, which doesn't have any intermediates. Perhaps by intermediate you mean aniline + HCl --> anilineH+ Cl- + NaOH --> aniline + NaCl + H2O. AnilineH+ Cl- is intermediate in the sense that it is formed in the course of the experiment, then consumed in a later workup step.
What are the uses of "NaNO2/HCl" in organic chemistry?
The reagent NaNO2/HCl is used in preparation of Nitrous Acid in the laboratory. The nitrous acid (HNO2) is a very unstable acid, therefore cannot be preserved, and thus it has to be prepared at the time of the reaction.Using Nitrous Acid, we can perform a diazotization reaction with primary amines. Primary aromatic amines, like aniline react with HNO2 to form Benzene Diazonium Chloride, which if reacted with other aromatic compounds such as Phenol, or beta Naphthol can form orange-yellow coloured dyes, commonly known as “azo dyes”.Besides this, there are many other purposes of HNO2, which includeIdentification of aromatic compounds, or primary amines.Synthesis of various compounds, mostly aromatic compounds.It forms the best route of conversion if we want to remove an amino(-NH2) group.It should be noted that a diazotization reaction is carried out at low temperatures, typically in an ice bath (in lab) since the diazo group is quite unstable and readily decomposes into nitrogen gas at higher temperatures.Structure of the Benzenediazonium ion.Links:-Diazonium Compound
Organic chem question?
This should work. What will make it work is taking advantage of the acidity of the aniline hydrogens due to the presence of the nitro group in the para position. 1. p-nitroaniline + p-dichlorophenol mixture dissolve in diethyl ether 2. add 1N aqueous NaOH 3. separate layers 4. remove the solvent from the organic layer to give p-dichlorophenol 5. acidify the aqueous layer 6. extract this with diethyl ether 7. remove the solvent from the organic layer to give p-nitroaniline. Hope this helps
ORGANIC CHEMISTRY question regarding separation of anthracene and aniline?
"Construct a complete and detailed flow scheme for the separation of anthracene and aniline. You can use H2O, HCl(aq), NaOH(aq), and dichloromethane (CH2Cl2) as the reagents/solvents for answering the question. Remember, an extraction requires two solvents to be present. Also, note that aniline is a liquid at all temperatures that you can access in the teaching laboratory."
How I would separate a mixture of benzoic, aniline, and phenol dissolved in chloroform and the solution treated with NaoH, HCL and NaHCO3?
If I understand the question, you have a mix of benzoic acid, aniline and phenol in chloroform?And then you have, at your disposal, NaOH, HCl and NaHCO3? I assume you also have water at your disposal?The first thing to note is that these three compounds are similar, but they differ. So obviously, we will need to use the parts where they differ.The parts that differ are three different functional groups. A carboxylic acid, an amine and an alcohol group.The second part is to think about how you can manipulate these, with the chemicals you have available. Here, you need to know about Brønsted acids and bases. You also need to know about solubility and polarity. So if you are unfamiliar with any of these concepts (you shouldn’t be if you are expected to be able to solve this problem), go ahead and google those.…If not, let’s continue.You want to utilize the fact that ions are more soluble in polar (hydrophilic) solvents, and less so in apolar (hydrophobic) solvents. Then you want ionize one compound at a time, which will then become much less soluble in chloroform (and if you mix if with water, will then be dissolved in the aqueous phase, which you can separate mechanically).This is of course easiest to do with the compounds that have pKa and pKb values closer to 7. And you would probably want to look up the pKa and pKb values of each of these. Again, google (or even better for these things; wolframalpha) is your friend. You need to know these values, so you can avoid ionizing more than one of the three at any given time (which again would be the one with pKa or pKb closest to 7).But after you do this for the two easily ionizable compounds, you are left with the last one in your hydrophobic solvent, and the two others in two separate fractions of water.I’ll let you figure out which compound separates with which treatment, but this is the general principle. You use the different chemical properties of the functional groups (specifically, how you can make them ionic), and the polarity (which gives rise to solubility differences).
TLC chromatography question for organic lab@?
This is essentially the same as your column chromatography question, except here the samples that would elute first on a column will travel the farthest and therefore have the highest Rf value. Silica is a polar solid phase and cyclohexane is a nonpolar mobile phase. Therefore, the polar compounds on the column will interact more with the solid phase and will not travel as far (lower Rf). Rf will increase with decreasing polarity and the order will likely be polar compounds with the lowest Rf and nonpolar compounds with the highest Rf. Benzoic acid will have the lowest Rf (polar carboxyl group), followed by benzyl alcohol (slightly polar), and biphenyl (nonpolar) with the highest Rf.
Organic Chemistry Problem?
Your para-nitroaniline is not water soluble. Therefore when exposed to water, it will crash out. You can then collect it by centrifuge and deal with the phenol and benzoic acid which should still be in your solution. Adding bicarbonate will cause the phenol to precipitate, and that may be separated as well. Summary Add water →Collect solid p-nitroanaline Add NaHCO3 →Collect solid phenol Remaining solution contains only benzoic acid Done.
Extraction method to separate 50: 50 mixture?
Rather trivial. Consider what you have. An amine (basic) and a hydrocarbon, which is neutral. Dilute it with an organic solvent, and then wash the solution with dilute HCl soln. The aniline compound will go into the aqueous layer. You separate the layers, and the anthracene is in the organic phase. You take the aqueous phase, and make it basic, and the aniline compound will be insoluble. Since the aniline compound will be a solid, slowly making the solution basic should give crystals that can be filtered off.
What is the reaction of benzene with a mixture of concentrated HNO3 and concentrated H2SO4?
This mixture produces the strong electrophile “the nitronium ion”.The nironium ion is produced from sulphuric acid and the concentrated nitric acid:Nitronium ion is attacked by benzene to produce the product Nitrobenzene. Diagrams were taken from the article cited below; which is an excellent read!Nitration and Sulfonation of BenzeneHere is something for you to look up!What is the purpose of the sulphuric acid? Also what is the protonated form of nitric acid (which forms the nitronium ion) known as?Lastly if you increase the reaction temperature does it affect the reaction products?Why should I do all the work lol!Good luck with your studies, all the best to you!