Science topics: BiochemistryNitric Acid
Nitric Acid - Science topic
Nitric acid (HNO3). A colorless liquid that is used in the manufacture of inorganic and organic nitrates and nitro compounds for fertilizers, dye intermediates, explosives, and many different organic chemicals. Continued exposure to vapor may cause chronic bronchitis; chemical pneumonitis may occur. (From Merck Index, 11th ed)
Questions related to Nitric Acid
using KOH (10%) and incubation for 48 Hrs. was not enough because the slime of the snails was not degrade and it was effect the filtration process ...Shall i increase the concentration ? or better to have alternatives let us say Nitric Acid ?
please let me know your ideas ..
Nitration of anhydrous Ethanediol is done with Adding 65% Nitric acid with excess 98% sulfuric acid around 100 degrees C (adding one chemical drop by drop on mix of other two, allowing copious fumes of NO2 go out and) and then boiled above 180 C (to remove all yellow-brown color of the liquid to colorless).
The dehydration of ethanediol is likely to produce ethene-1-ol that may be further dehydrated to ethyne (acetylene, and escape from solution) or tautomerized to ethanal (acetaldehyde). Nitrating can produce either 2-nitroethanol or 1.2-dinitroethane, or the nitric acid itself can oxidize acetaldehyde to acetic acid. Or can nitroethene form?
However, I cooled the solution to 4 C and reheated to around 30 C, but fine needle shaped crystals precipitated that didn't dissolve. Is this glacial acetic acid? I cannot separate them due to lack of distillation apparatus or Barium Nitrate.
BTW: I took the supernatent liquid at room temperature, dissolved it 2000 times and drank it a little. It tastes awfully sour, but doesn't taste like vinegar. When I was boiling the solution, upon ceasing of chocking sharp metallic-smelling brown fume evolution, a strong vinegary smell appeared.
As I kept the solution bottled shut for a day or two , some tiny gas bubbles started to appear. What are these bubbles? Acetic anhydride, Acetylene, or something else? they are very low voluminous, so cannot be put to test for gases as per wet-chemical method. And I do not have Gas Chromatography at my hand.
I am starting to learn computational chemistry and would like to look at pdb files of some simple molecules. I know usually xyz files are enough for representing these simple molecules, but I need them more for understanding how the file format works. Does anyone know where can I acquire these files?
9.7 g Bi(NO3)·5H2O and 0.034 g AgNO3 were dissolved in concentrated nitric acid under vigorous stirring at 30°C to form a clear solution. The sample obtained above was labeled as Ag-1.
Which chemical can I use to make 1000mg/L of Magnesium (mg) standard solution in 100ml 5% of nitric acid? I want to make a standard solution for ICP-OES.
Can a particular type of stainless steel be recommended that will not leach magnesium?
Nitric acid is strong oxidizer- no doubt, but the -CH2- groups of citric acid would likely not be oxidized, and the OH group has no alpha-hydrogen nearbly to convert it to ketone. But, would the citric acid crystals put into nitric acid be dissolved overcoming the common-ion effect? would the C-C bonds of citric acid be cleaved by nitric acid? I know nitric acid is not as hygroscopic as concentrated sulfuric acid, but what about concentrated nitric acid?
And when a metal would react with this mix, profuse amount of NO2 gas is supposed to evolve. Would it react with citric acid to convert it into some sort of Explosive?
It is precisely for this risk of explosion i am asking this question before trying it out physically.
Edit: I have mixed around 1 g of Citric acid trihydare crystals in around 1.8 g Conc. nitric acid and evaporated sloyly to dryness. What does the crystals remaining contain? (They seem like small rounder flat spot on bottom of beaker, rosette-like radiating out from a center) I cannot run any sort of FTIR/ UV-VIS/ TA on this sample, so only knowledge of organic chemistry is of help fopr me as of now.
I'm trying to prepare a nitration mixture to nitrate a quinazolin-4-one compound, I did so by adding H2SO4 dropwise to 69% HNO3 through a dropping funnel in ice/salt bath in 1:1 ratio, the first time I did this I saw lots of reddish brown fumes turning to white fumes inside the flask, however I didn't see that on repeating the experiment and the color of the mixture is colorless, on standing I noticed the mixture turning to slightly reddish yellow color.
Is it a must to see reddish brown fumes turning to white fumes as an indication of formation of fuming HNO3 acid in-situ?
Hello please assist,
How can I make a 2% of nitric acid solution in 100ml of water? if you don't mind please show with calculation so I to understand better.
I usually use nitric acid as a washing filter glass.
Sometimes mix with ethanol.
I found some acid like hydrochloric acid and phosphoric acid.
So here is the question.
Does acid like hydrochloric acid and phosphoric acid can be used to wash filter glass?
Reactor for hydrothermal reaction:
Volume = 100 ml
Pmax = 3 MPa
Maximum operating temperature = 200 °C
Nitric acid - 15 ml
Sulfuric acid - 5 ml
Distilled water - 100 ml
I am looking for the pressure to be generated inside the reactor (the equation) to know what volume of solution I can introduce at what temperature without generating the allowed pressure limit.
Putting nitric acid was necessary to increase the carboxylic groups on the nanoparticles surface.
Does the purity of the nitric acid play any role in the acid digestion to determine heavy metals?
If i not study effect of pH what is problem in this case?
Please, in order to be able to analyze the mineral composition of an aqueous extract of plants in ICP , how can we prepare the samples? what are the steps to do the acid dissolution? choose solid acids (citric acid) or liquid acids (nitric acid)?
Commercially produced Activated carbon+ Nitric acid reflux. Is it suitable for better adsorption properties?
Hi I am aiming to replicate an aerosol assisted CVD metod of fabricating BiFeO3, In this method it calls for 18 vol% nitric acid to disolve the Bi precursor in triple distilled water. I was wondering if it would be possible to used citric acid at higher concentration, as I already have this in stock and it is less intense in terms of safety? I appolgise if this is a stupid question, I'm not a chemist.
I have a question. I oxidize a sample of carbon dots by refluxing it with nitric acid (7M, 180 mL). I would like to know how to remove or neutralize the nitric acid and purify the carbon dots.
Thanks in advance!
Looking forward to anyone who can help me with this.
If I dissolve 1 gram Pr6O11 in nitric acid than will it be dissolved? if yes than how much quantity of nitric acid I use to dissolve? If not than How much I use other acid for dissolving the praseodymium?
or else can we use concentrated nitric acid instead of concentrated sulphuric acid in GO synthesis
Reported procedures mainly use fuming nitric acid (concentration >86 %) with or without conc. H2SO4 to nitrate quinazolineones, however the only available concentration for me is 69%, can it nitrate it or it should be fuming?
To functionalize the carbon nanotube, I first mixed it in 3 m nitric acid at 60 °C for 15 min. Then I kept it in an ultrasonic bath for 2 hours. After drying, I repeated the same process using hydrogen peroxide. But But the degradation in the TGA analysis was minimal. What would be the reason. or how can i increase the binding of functional groups. Thank you
Does anyone know how we could reduce the nitric acid content in the catalyst slurry (because of NOx release during drying step) without viscosity increment. Does the acid replacement work? If so, what kind of acids do you suggest?
This tipe of reaction is widely discussed in many articles and books like a Bruice, chapter 20 The Organic Chemistry of Carbohydrates (Organic Chemistry eighth edition 2016)... but I do not find any specific method for oxidate galactose to galactaric acid with diluite nitric acid HNO3.
Does anyone have a tested and effective method of oxidation of galactose to galactaric acid with diluite nitric acid?
How do we prepare 1% 7M HNO3?
I am about to analyze the cation exchange capacity of a soil sample, however I am not sure how to prepare the above solution?
What is the ideal nitric acid purity for this analysis?
I am trying to do ECCI on a sample of 316L steel. In the preparation, I am mechanically polishing 400-600-800-1200 grit paper then to a 0,3um silica polish. I finish with a electropolish of 25% nitric acid/75% methanol at 1Amp, 2 V. When I look at the sample under an optical microscope, I see NO grain boundaries.
My question is, should I expect to see grain boundaries after electropolishing under an optical microscope? Or should I not even be electropolishing. I HAVE ti use the nitric acid, as my lab is not set up for sulphuric or perchloric.
If I am supposed to see grain boundaries, but since I do not, what should I try to change?
Thank you for your help.
There are different methodologies to digest plant material for heavy metal analysis; for example, they use 1) nitric acid, 2) nitric acid + hydrogen peroxide, 3) hydrochloric acid, among others.
Experimentally, 4-aminosalicylic attained an inhibition efficiency of 99.4% at 303K and a concentration of 0.0005 M. Other compounds it was compared with at a much higher concentration are; salicylic acid, 5-chlorosalicylic acid, 5-sulfosalicylic acid, benzaldehyde, and 4-chlorobenzaldehyde.
I would find a safer route to synthetize rhodizonic acid from Inositol, than oxidizing it with nitric acid to avoid nitrogen dioxide.
I am currently working on 3D printed copper using L-PBF. While conducting Light Optical Microscopy (LOM) I couldn't see the melt pools in the cross sections. I tried etching the Cu specimens with two etchants namely: 50% water - 50% nitric acid and Ammonium hydroxide - hydrogen peroxide. Using these two etchants I could see the grain structure but not the melt pools.
Can I use 0.07 g MWCNTs, then how many quantity of HNo3 i will use for my setup?
I nitrated lignin by dissolving it in acetic acid and nitric acid. I am suppose to use extinction coefficient for vanillin as pure lignin and 5-nitro vanillin as nitrated lignin. According to literature the extent of nitratation was estimated from Ratio of 300A/280A where the 'A' stands for absorbance how do the calculation.
It wasn't dissolved in Nitric acid without heating, and also it was evaporated completely with heating. what is problem?
Hi if any one can help I have a standard stock solution that prepared in nitric acid and I want to prepare several concentration for AAS from the stock in which dissolvent should I prepare the concentration? can I used distilled water or 0.1 nitric acid?
ICP-based analytical instruments (Agilent ICP-MS 7900) often have white dot-like deposits on the quartz transmission line. Are these substances salt deposits? We use 10% nitric acid soaking ultrasound over night, however, the effect is not great and white spots (deposited salt) can still be seen after cleaning. Is there a more effective way to clean the salt from the quartz?
I‘m looking forword to your answer, thank you!
a) Cu concentration. In Molarity, mg/L.
b) if I take 10 mL of this solution and dissolve it up to 100 mL. What is the new concentration?
We are looking to incorporate BPOG/USP<665> testing on SUS in the future. I am told the extractions need to go through nitric acid digestion before running on our ICP-MS. Which concentration of HNO3 would be best for this?
The concentration limits we are looking for range from 0.15 - 100ppm (see attached), target LOD is 20ppb, and our instrument works best with TDS < 0.25%.
I am brand new to this, so any and all information would be greatly appreciated.
Most of the reserchers have digested the gill tissue with nitric acid and perchloric acid (4:1 ratio) but rest of the tissues in fish they have used only nitric acid. Is it because of the difference in composition muscle and gill tissue? If yes, what is their composition?
I need to prepare yttrium nitrate by dissolving its oxide into 6M nitric acid.
I would like to know any experimental considerations in this process to get best results.
If we are using this Cd (II) standard 1000 ppm solution (Cd (NO3)2 in 0.1 M HNO3) (Wako Pure Chemical Industries, Ltd., Osaka, Japan)
was diluted with 10 mM sodium citrate buffer (pH 6.0) and used as a one ppm Cd (II) solution.
if we use HCL or NaCl on place of HNO3 (Nitric acid) can we use?
I'm currenting using the Bertsch and bloom method of analysing exchangeable Al in soils. The method says to use nitric acid to buffer the pH filtrates to <3. But Id prefer to avoid using HNO3, would using HCl to acidify the samples be appropriate?
I'd like to prepare a solution of MoCl3. According to the supplier, MoCl3 is soluble in nitric acid and sulfuric acid, and insoluble in water and dilute hydrochloric acid.
Does anyone work with MoCl3? I'd like to prepare a solution of MoCl3 with a concentration between 0.1 and 1 M but not using nitric acid as it will give (MoO4)2- species. I need to obtain the Mo3+ species.
Hello, i am going to analyse the amount of Lead (pb) present in water by atomic absorption spectrometry in the protocol it says that i have to use 120 ml of nitric acid (1+5) , i'm not exactly sure what this ratio means ! do i have to dilute the nitric acid first and than use it for analysis ? please help
When I ran my blank which is 2% nitric acid in ICP-OES, I get negative values of cps which causes the RSD to be higher than 10%. I think it may be due to detector ... Can anyone help me to solve this problem please? Thanks
I use 70% nitric acid to activate the quartz coverslip for silanization. After 1 year storage, the nitric acid turned yellow due to, presumably, dissolved nitrogen dioxide. Can it still be used for my application?
If one is having problems related to contamination of iron in the glassware, what is the best way to clean it? I have tried to clean with nitric acid 10% solution (v/v), but I'm not sure if that's enough. If someone already had the same problem and wants to share the solution, I would be thankful.
It is nitration reaction and using the reagents such as nitric acid, acetic acid or acetic anhydride and sulphuric acid
The two graph attached here show FTIR and XRD of material (ZnO) form the same paper. i can not make out why some the molecules like nitric acid group present in the ZnO as shown by FTIR does not show its presence in XRD graph?
Is it dangerous to heat mixture of sulphuric acid, nitric acid and water above 50C? Furthermore with cellulosic material immersed?
I have a MOS structure- Al/HfO2/Si. I want to remove the aluminium metal contact without harming/etching the underlying hafnium oxide film. Can Nitric acid do that since hafnium is unaffected by all concentrations of nitric acid?
I am analyzing different metals in Nitirc acid and Hydrochloric acid by FAAS AND FAES. I want to know the highest molarity of the acid I can aspirate into the flame directly without damaging the nebulizer. Will the difference in molarity or pH affect the result?
I want to synthesize ammonium nitrate (NH4NO3), based on NH4OH + HNO3 → NH4NO3+H2O For this purpose, the mixture of nitric acid ( 65wt% in water) and ammonium hydroxide solution (NH4OH , 28wt% NH3 in water) should be made. I have some doubts about the calculation of the required amount of Ammonium solution. Should we choose NH4OH or NH3 as a reactant? If we choose NH4OH, we don’t have its concentration in water, because 28wt% is NH3 concentration.
my task is it to create a specific extraction process. There is a mixture containing water, nitric acid and hydrochloric acid. It is known, that tributyl-phosphate is a solvent, which prefers the extraction of nitric acid compared to hydrochloric acid. The problem is how to use Aspen for this case. I tried different ways step by step, using ELECNRTL as the property method and TBP as a solvent but all the results did not confirm these effects. I hope someone could help me with this or can share similar results with Aspen Plus.
With kind regards
I am trying to study the cellular uptake of specific metal inside the cancer cells by measuring the concentration of this metal by ICP-OES using a standard.
So, the first step after incubation of metal with cancer cells and cell harvesting is the cell digestion.
what is the best protocol for cell digestion before applying to ICP-OES measurment?
and why we usually use conc. nitric acid and H2O2 at high temperature(1600C) for for the digestion protocol?
Thanks in advance.
A corrosive electrolysis experiment attacked a slightly exposed Ag wire junction in the reference electrode of our Electrasyn instrument. Afterward, the Pt foil counter electrode (cathode) had raised deposits of a silvery metal when examined under an optical microscope. Naturally, I suspect the metal is silver; the only other possibility would be Pt etched from the working electrode (which I hope isn't happening). The electrode is too large to fit in our SEM without cutting so I can't easily check the surface composition. Assuming it is Ag, what would be the best way to remove it? My first impulse is to strip it off anodically but I don't know what sort of conditions would be appropriate. Hot nitric acid would get most of it, but could some contamination remain? Polishing off a thick deposit might risk damage to the foil.
Given the popularity of Ag reference electrodes, I can't be the first person to encounter this.
We're using a fluorometer (Horiba Aqualog) to analyze fluorescent dissolved organic matter (FDOM) in water samples. The samples are analyzed in quartz cuvettes, which must be bathed in a solution of 50% nitric acid for 24hrs. In theory, the nitric acid bath can be reused between multiple runs.
I'm now trying to find a lidded container that can safely hold 50% H2NO3 at 20 degrees C inside a fumehood for a week or more without damage. Minimum internal dimensions would be approximately 15cm square bottom and 3cm deep. We've considered jars or large beakers, but we need something wide enough to fit a butyl-gloved hand into to handle the delicate cuvettes.
In terms of materials, plastic options exist (https://www.calpaclab.com/chemical-compatibility-bottles-containers/). Teflon would be the "gold star" but I've found no teflon tanks available from suppliers. I'm currently looking at a Nalgene LLDPE rectangular tank with lid. Another idea is a glass bakeware dish with lid (much cheaper and AFAIK 50% nitric won't attack glass).
But I'm curious to know what others are using.
Nitrooxy group (nitrate esters) is used in the preparation of vasodilators.
The use of silver nitrate to convert alkyl halides to nitrate esters is very common.
A. McKillop & M. E. Ford used mercury nitrate in organic media, but not repeated by someone else.
Can other nitrate salts be used to convert halides to nitrate esters?
Emami, Mut orgsynth.student
Does it really work?
I tried to make a standard curve of clodronate solution through measuring the absorbance at mixing clodronate with copper in the presence of nitric acid.
Please, could you help me?
I want to elaborate a presentation to my students of Chemical Reaction Engineering where I can illustrate them reactor design with multiple reactions, including reversible exothermic reactions. I think this classic reaction system conducting to nitric acid synthesis could be useful.
I need the thermodynamic and kinetic information to simulate the system behavior in different contact systems. Could any of you help me to have a comprehensive review about this reaction system?
Using the Equation Cu + 4 HNO3 -> Cu(NO3)2 + 2NO2 + 2Water
If I want to make 1% solution of copper Nitrate in water - how much copper and how HNO3 (55%) do I require?
How much water is produced?
How much water must be added?
Show your calculations, please
In the following tutorial I show how to make white fuming nitric acid from cheap household products.
I believe that my product has a concentration of 95% or more, however it has a yellow tint due to nitrogen dioxide, which usually is not a problem for most applications. I read that the tint can easily be removed by bubbling air into the acid to push the nitrogen dioxide away.
My question is whether this operation would reduce the concentration of my product or not? Since low concentrated nitric acid can be produced by bubbling nitrogen dioxide into water, it seems that it is a good idea to keep the nitrogen dioxide in my product?
I have tried by adding nitric acid and then heated, still it didn't dissolve.
Diazotrophs 'fix' atmospheric nitrogen into biologically available forms. In very general, non-technical terms, an over-abundance of these organic nitrogen forms within a soil beyond what biota in the soil metabolically require has been suggested to result in the increase of nitric acid in the soil. What I would be very interested in is if anyone has done work to help establish a rate of nitric acid production in response to this over abundance of organic nitrogen.
Arsenobetaine is the non toxin organic form of Arsenic commonly found in fish.If muscle of fish samples subject to a acid digestion, will non toxic nature be changed
I have extracted Manganese dioxide from zinc-carbon battery in order to prepare Manganese fertilizer . but it never dissolve , Why ??
maybe someone knows how polyurethane (food packaging adhesive layers) reacts with 2M nitric acid? heating added
i have bismuth(III) nitrate pentahydrate and 2M nitric acid. how much nitric acid in ml used to dissolve 1gram of bismuth nitrate completely
I am writing my Bachelor´s thesis about different methods of quantify the phosphates into fertiliers.
I have experimented the "yellow method" in order to quantify the phosphates (PO43-) amount in form of sodium dihydrogen phosphate dihydrate (NaH2PO4 . 2 H2O) with one UV-VIS spectrometer, in order to make a calibration function. However, I don´t know how the reagent solution reacts with the phosphates and respectively with the sodium dihydrogen phosphate dihydrate (NaH2PO4 . 2 H2O):
I made a reagent solution of:
- Ammoniumvanadat (NH4VO3)
- Ammoniumheptamolybdat (NH4)6Mo7O24 . 4 H20
- nitric acid (HNO3)(65%) diluted in ratio 1: 3
I have just find this reaction :
PO4-3+ 12 MoO2-4 + 3 NH4++ + 24H++ ó (NH4)3(P(Mo3O10)4 (gelb) + 12 H2O
but I would like to know what happens with the Ammoniumvanadat?
Thank you very much in advance for your help,
I am using 70% nitric acid and I saw the white crystal blocking my dispenser. Can somebody help me out with the same?
Also, it seems impossible to see crystals of nitric acid at RT, so can someone suggest to me the possibilities?
I have synthesized zif-8 using a three fold excess of 2-methylimidazole. I would like to purify the excess 2-methylimidazole from uncreated zinc nitrate (very little) and nitrate. What is the nitrate ion paired with after the reaction takes place. It is a weak conjugate base so very little will form nitric acid. Will it be paired with the reacted zinc in zif-8? Any clarification would be helpful.
I am trying to form a bismuth complex using thiosemicarbazones as ligands. Many articles I read describe the bismuth complex as a yellow precipitate orange or red but not black. I am using bismuth nitrate and tried forming the complex under reflux in methanol with the help of nitric acid. I also tried without nitric acid and without heat. Still every time I get a black fine precipitate. At first the mixture turns into a vibrant yellow color and within 20 min its starts to darkened. Can someone help me understand what is going on.
i want to estimate the metal present in our plant sample, for this initial step is sample digestion. many reference paper use nitric acid, is there any other method which can follow. need protocol with reference
We are developing a general method for Q3D elements by ICP-MS, out of all Q3D elements Au shows inconsistency in spike recoveries and bracketing standard recoveries. We are using 2% Nitric acid and 0.5% HCl in water(Trace elemental grade) as diluent. Au was analysed against Y and Tb as internal standards, results remain same. Some times we were getting recoveries with in limit (70% to 150%) with the same conditions the other time recoveries fell short. The reason for this is Au is not stable in HNO3 and HCl? or is there any other reason? and what would be the optimal conditions to get consistent results? (We are not using any glassware for sample preparation, we only use Poly propylene tubes throughout the analysis.)
I need to change the technique I was using to measure heavy metals in plant samples. Until now I was making a wet digestion in an open recipient with concentrated nitric acid and at boiling temperature to obtain an extract and measure by atomic absorption spectroscopy. The problem is the amount of acid fumes that are generated, because I have a large number of samples. I wanted to know if diluted nitric acid can be used to reduce the amount of acid fumes without mayor variations in metal measurements or if they know of any other modification that can be done to the technique.
I need a solvent which it can dissolve PbS (lead II sulfide) well. I can't use nitric acid because it destroy S2- in PbS.