Is it possible to dissolve sodium silicate in water and then somehow precipitate the sodium ion without removing the silicate ion from solution or accelerating its polymerization?
I was thinking I could add bismuth trioxide and it would react with the sodium and form insoluble sodium bismuthate, but considering bismuth silicon oxide exists, this likely wouldn’t work the way I want it to. Plus the reaction needs an oxidizer and I assume that would rapidly precipitate the silicate into silica gel if it didn’t already incorporate with the bismuth.
I’m a biologist, not necessarily a chemist, so any advice is appreciated
LAB S. ACIDS AND BASES: TITRATIONS Within the divisions of chemistry there are several distinct types. The subject of study within this report are acid-bas.
When doing an ethanol extraction of THC, my understanding is that THC and many other organic compounds dissolve in the alcohol. So now these are all random O, C, N etc. ions floating around. Lets say hypothetically 100% of the THC was extracted and there was 1 mole of THC in the plant extracted. Once the ethanol is evaporated, my understanding is that there would be 1 mol of solid THC left behind once all the alcohol is gone (unless this is wrong then idk). How do these random ions know to reform THC in the same quantity vs forming other random molecules? I am sure there are plenty of molecules that require less energy to form than THC using these same ions, do the ions not fully separate?
Formula: Ca + 2 HF -->CaF2 + H2
18mL of HF of 6M . Find theoretical yield of hydrogen.
-I converted mL to liters. multiplied by molarity and then multiplied it by moles of hydrogen by atomic weight of H2. I am thinking we have to use density in order to find grams of HF but I am stuck at how to proceed with 6 Molarity in relation to moles HF and H2.
Are there any nitrogen compounds that have high volumetric energy densities comparable to kerosene? I realized that methane like ammonia have low boiling points but methane has compounds with high boiling points like kerosene. Are there aqueous solutions of nitrogenous compounds that have a high boiling and freezing points like kerosene and could replace fossil fuels in our airlines?
Wanting to know if I can add a sulfate anion to an aqueous zinc salt solution by adding a sulphate salt of another type. I'm using this for zinc electroplating and want to know if I need to synthesise zinc sulphate or if it's fine just to add another zinc salt + sulphate salt together for the same effect (to save time, energy and money).
In theory this should work fine as long as the other cation (ammonium in this case) doesn't affect the electroplating process, but I wanted to double check.
Getting some 2-cb but I don't have a mg accurate scale. if I measure out my entire stash (500mg) on a less accurate scale can I dissolve it all in water then take it in doses over time by measuring out the amount of liquid? (so like I could dissolve all 500mg in 500ml, creating a solution of 1mg per ml and then drink 15ml every time I wanna dose). I wouldn't use this all up quickly, so could it have problems like crystallizing or settling or anything like that? I don't want it to end up all going to waste. if any one has done the please lmk.
thank you!
I know that kp is the concentration of solute in organic phase/concentration of solute in aqueous, but wouldn't we need to know the concentration in terms of moles per liter (which we cant do since we don't know what the solute is)? If not, how would I go about solving this?
Anyone have any suggestions for crystals made from solvents other than water? I’m interested in making some crystals that aren’t water soluble. Perhaps crystals grown from saturated solutions of acetone, xylene, ethylene glycol, propylene glycol, glycerine, or methylated spirits?
As an example: One I have done before/am working on is a sulphur crystal formed in a saturated solution of xylene.
Also substances that are liquid only above room temperature (up to 300C) would be cool to try!
I’ve already made metal crystals so I’m moreso interested in non-metallic crystals.
Please leave a comment with any thoughts you have!
I am reading through this extraction protocol. At the step where they have the mescaline in the xylene and are ready to salt it using an aqueous solution of HCl, they write the following:
>You want to add approximately 4-8 drops of HCL acid to 250-350ml of water. Slowly add this acid water to the xylene while gently swirling the liquids around in the jar. Add just enough to make a half inch or so layer beneath the xylene.
>
>Don't worry that you won't get all of the goods because the xylene is going back into the extraction bottle and you'll get another shot at what you missed before. Put the lid on the jar and shake it all up. Wait a few minutes and shake again.
>
>Once it has returned completely to a separated state loosen the lid on the jar and place it in the freezer. You want the bottom layer(the acid water) to now freeze solid. The xylene will not freeze. Once the water is frozen, work quickly and pour the xylene back into the extraction bottle.
>
>With the water still frozen solid, pour in a little warm water and swirl around and discard quickly. This helps get rid of a little more residual xylene. The rest will evaporate later.
>
>Repeat the extraction and salting steps 4 to 6 times to get all of the goodies. You can reuse the xylene over and over again.
Is there any actual advantage to freezing the layered aqueous mescaline HCl + xylene, other than facilitating separating the two layers? I haven't come across another protocol that freezes at this step. It seems like using a sep funnel would be less troublesome.
Thanks!
Hi just starting out and was wondering how much of this solution to use with 250g of MHRB.
And do I need to mix it with water if it's already in liquid form?
Hi all. I have a project where I am quite concerned with balancing what ions cross a membrane and the conductivity of the solution. As a result, I need to use fairly dilute solutions. It seems remarkably difficult to find actual data for the conductivity of, e.g. 10 mM H3PO4 solution, but I know it must be out there. Do any of you know where I could find such a reference???
Hey guys, this is my first post here. I love MDMA as well as MDA and am a responsible user. I have an intriguing idea as to how I can sneak MDMA into concerts when they return though I can’t determine a proper solvent. I would like to make a concentrated solution of MDMA that I can store and transport in a small, leak-proof, 5mL glass vial. Before I begin, I have searched tirelessly across much literature to find my answer and I cannot. I also cannot conduct any tests for fear of wasting precious material.
I cannot concentrate it enough in water so I need a different solvent. I know that a strong ethanol solution (maybe >150 proof) will effectively dissolve it, but does anyone know the literature solubility? Considering that it can H-bond and ethanol is significantly less polar than water, I think it may be my most viable option all things considered. My goal is 100mg/5mL.
Please consider these factors: I must be able to ingest this solvent orally, it must be a solvent that I have access to, and it cannot chemically react with the mdma!
Any ideas, input, or constructive criticism of my current understanding is welcome and appreciated! Thanks for taking the time to read!❤️
Journal of the American Chemical SocietyDOI: 10.1021/jacs.1c05301
Narjes Ansari, Valerio Rizzi, Paolo Carloni, and Michele Parrinello
https://ift.tt/3k3FPAc
Thanks for any replys.. So question is; If on my first attempt I didnt get the PH levels right, is it possible to add more LYE to the MHRB/water/Lye mixture or is it too late to add more Lye if I've already added the MHRB to it?
I'm pretty confident I have the mixture right but I'm just asking in case I need to go back and fix it..I read to save the mixture cause it can always be salvaged I'm curious if that's true.
Amateur chemist here - I am formulating an antioxidant serum and want to use sodium salicyate as a principle stabilizer of organic phenolic compounds (to mitigate their oxidation over time).
It is a biphasic solution containing an oil and aqueous phase. I plan to obtain the salt form of salicyclic acid by reacting with sodium bicarbonate. Two questions however
- What is the ratio of sodium bicarbonate to salicylic acid to properly dissolve salicyclic acid in the aqueous phase?
- Will sodium salicylate precipitate out of solution if I lower the pH to less than 3.5? I am trying to achieve a pH of 2.4. My understanding is that this would happen if salicyclic acid was present in the acid form
Any help would be greatly appreciated
Little confused on the phrasing of this question and just wondering if I did it right:
- What would you expect the van’t Hoff factor to be for an aqueous solution of each of the following: a) NaOH? B) CH3OH? C) K2CO3?
I said :
a) 2 for NaOH
b) 1 for CH3OH
c) 3 For K2CO3
I’m looking to do spectrophotometry in determining the amount of formaldehyde in conditioner and it has to be done BY May 18. I know chromotropic acid detects formaldehyde but I don’t know where to find it and it’s too expensive online and won’t ship until after my deadline. Is there an easily accessible alternative that will result in a color change?
For example, in this precipitation reaction:
Mg(NO3)2(aq) + 2NaOH(aq) -> Mg(OH)2(s) + 2NaNO3(aq)
I understand that when ionic compounds dissolve they separate into ions and surrounded by water molecules. When the solutions are mixed together they react and the ions switch partners, so Mg ends up with OH and Na ands up with NO3. Why do the ions switch partners instead of just staying with their original partners? Is it because Mg(OH)2 is a solid, and if so, do exchange reactions only happen when a precipitate is formed?
LAB S. ACIDS AND BASES: TITRATIONS Within the divisions of chemistry there are several distinct types. The subject of study within this report are acid-bas.
Formula: Ca + 2 HF -->CaF2 + H2
18mL of HF of 6M . Find theoretical yield of hydrogen.
-Using dimensional analysis: I converted mL to liters. multiplied by 6 molarity and then divided it by moles of hydrogen then multiply by atomic weight of H2.
I am thinking we have to use density in order to find grams of HF but I am stuck at how to proceed with 6 Molarity in relation to moles HF and H2.
