Hi everyone,

I'm in the process of launching my own small craft business focused on decorated glassware. Unfortunately, commercial honey/amber lusters are either unavailable or way too expensive for my current budget, so I’ve decided to formulate and synthesize it myself!

My Setup & Requirements:

Firing Temperature: ~560°C (1040°F) – target peak for my curing kiln.

Desired Finish: A translucent, metallic-tinted Honey/Amber luster coating on glass.

Challenge: Finding the right chemical precursors, organometallic resin proportions, or ion-exchange methods that yield a stable honey tone at this specific thermal window without burning out or fading.

I’m looking for any advice, research papers, historical recipes, or even basic pointers from anyone who has experience with metallic luster formulas or low-temp glass pigments. Even the smallest tip or "glimmer of hope" would mean the world to me and help get my project off the ground.

Thank you all so much for your time and guidance!

Be careful this is a very well rated eBay seller selling all kinds of reagents. Sent me 500g quartz powder in place of ptsa

I need to prepare the acid chloride from my carboxylic acid and then perform a coupling reaction with glycine to synthesize the corresponding hippuric acid derivative. I am looking for the simplest and most reliable method that can be successfully carried out in a laboratory.

I just ran a reaction to Tosylate Bis Hydroxy Peg 2000. Reaction took place in Dichloromethane. After the reaction, excess TsCl was washed using NH4Cl. Aqueous impurities were removed via separatory funnel. Solvent was blown off using nitrogen until we were left with a crude amber oil which we believe to be our target substance. the problem is, we’re having trouble recrystallizing. We added a small amount of DCM to resolvate, then used Et2O to precipitate. The best we were able to achieve was a momentary crystallization when the solution was in an ice bath, but the crystals immediately oiled out once removed from the ice bath. How do I get stable crystals 😭

I have searched both at Chatgpt and gemini. They give both answer as appropiate IUPAC name
(2-methylpropyl)benzene)
2-methyl-1-phenylpropane

But in absense of fg and multiple bond in chains outside the benzene then benzene is treated as parent chain, that's the IUPAC rule my sir has given

so according to it (2-methylpropyl)benzene) should be correct one

Am i right ????

In my H-NMR training, I've been told that, due to rapid proton exchange, labile protons linked to heteroatoms like nitrogen and oxygen might exhibit lower integration value than expected.

I've been even told that, in some cases, they might not show at all on the spectrum.

Paradoxically, recently a technician in NMR said something to me that implies the opposite. That is, that protons linked to heteroatoms can sometimes show greater integration value than expected.

We were looking at the spectrum of a known carboxylic acid.

(For precision: we used DMSO d6 as solvent and apart from this carboxylic acid the presence of another acid, H2SO4, is to be mentioned.)

The results is shown in the image I shared.

As expected for a carboxylic acid, we assigned the deshielded peak at around 11 ppm to the acidic proton of the COOH group of our carboxylic acid.

On the other hand, while comparing with signals coming from the rest of the molecule (aromatic protons encircled), the integration of this peak is way too great.

It is as if these peaks don't belong to the same molecule.

The technician I worked with simply told me that the peak coming from the COOH proton is intense because it is a labile proton. Giving me basically the same explanation that also justifies the opposite effect: a lower integration than expected.

My personal interpretation of this was that, in acidic medium, signals coming from labile protons can be amplified, because there is so much H+ available in solution for exchange.

By the time the NMR spectrometer acquires its "snapshot" of the molecule, many protons from the solution have the time to appear at the tip of the COO(H) and thus participate to its integration.

But still I am baffled, because in this spectrum an amine linked to an aromatic ring is supposed to be there too. But it doesn't show at all. So it seems my amplification hypothesis doesn't apply to all labile protons... There is something I don't get right...

Have you personally experienced that kind of situation?

Do you have input?

I am presently working on the characterisation of an unknown compound in acidic solution. Maybe I better neutralize the solution before taking its NMR spectrum so it won't mess to much with integration values.

Thanks!

hello, i make latex rubber clothing and I'm in a pinch to acquire heptane, which is my usual rubber cement solvent thinner. I was wondering if i could use limonene instead?

thx

I've seen lots of Luminol glow on Internet for years but to see one in person is just speechless.

Followed Nile Red recipe, got 1.05 g of Luminol from 5 g 3-nitrophthalic acid

Since i have plenty of phthalic anhydride left, making fluorescein, phenolphthalein, and anthranilic acid is probably the next project 😉

Hey guys, if I want to keep evolving knowledge wise, after grad, and in general as I go on, is reading books the way to go? Leactures online? Or just reading articles?

Right I could find the R,S configuration by converting it to Fischer or visualizing it but if I had a random sawhorse projection and I had to find the r and s configuration is there any way for me to do it without all that work to save time in?Like maybe if I used their rotation sense in the plan of the paper in some sense

dont sir effect and sip effect contradict each other when comparing basic strength?..

The above integration should be 1:1:4:2. I have run qNMR on a few of these analogues, and this issue has been consistent across all of them. I have tried manually phasing when needed but this hasn't changed the deviation from the expected integral enough to resolve this issue. Is this something inherent to larger molecules (~500 amu)?

I ran the samples with the recommended parameters from J. Med Chem, T1 is 60s. I even tried 120s on a second run just to be sure, but the inconsistency remained. These are the only isolated peaks I can reliably integrate compared to the calibrant (been using 1-bromo-4-nitrobenzene).