Pretty Pictures (2)

I also have a good stones, gemstones and fossiles collection
Also some other not yet exposed in my glass shelf...

And a few close up of my bismuth cristals:

Quote: Originally posted by crystal grower

Wow that's gorgeous. Do you buy minerals or you dig the them yourself ? And also what purity bismuth do you use?

I made an ampoule with IBr. Very weird crystals are formed in the inside of the ampoule:

This is the ampoule:



You can see some solid IBr at the bottom of the ampoule, the brown/pink vapor above it, and beautiful crystals at the bottom half of the ampoule.


Here follow some closeups of the crystals:

Crystals on the far side of the ampoule:





Crystals on the near side of the ampoule:





Crystals all around the ampoule:





One week later, the crystals disappeared at one side of the ampoule, but they are still present on one side:

Quote: Originally posted by woelen

I made an ampoule with IBr. Very weird crystals are formed in the inside of the ampoule: This is the ampoule: You can see some solid IBr at the bottom of the ampoule, the brown/pink vapor above it, and beautiful crystals at the bottom half of the ampoule. Here follow some closeups of the crystals: Crystals on the far side of the ampoule: Crystals on the near side of the ampoule: Crystals all around the ampoule: One week later, the crystals disappeared at one side of the ampoule, but they are still present on one side:

Wow, that's really weirdo .
What melting point does it have?

I want to try growing some iodine crystals, too bad that I can't find any iodine for a reasonable price (local eshops offers only big quantities so I can't afford it) and I won't probably get enough from povidone .

Quote: Originally posted by crystal grower

Quote: Originally posted by woelen   I made an ampoule with IBr. Very weird crystals are formed in the inside of the ampoule: This is the ampoule: You can see some solid IBr at the bottom of the ampoule, the brown/pink vapor above it, and beautiful crystals at the bottom half of the ampoule. Here follow some closeups of the crystals: Crystals on the far side of the ampoule: Crystals on the near side of the ampoule: Crystals all around the ampoule: One week later, the crystals disappeared at one side of the ampoule, but they are still present on one side: Wow, that's really weirdo . What melting point does it have? I want to try growing some iodine crystals, too bad that I can't find any iodine for a reasonable price (local eshops offers only big quantities so I can't afford it) and I won't probably get enough from povidone .

Quote: Originally posted by Velzee

http://www.ebay.com/itm/25-grams-0-88oz-pure-elemental-iodin... Pretty high purity; this is the time in which products from China should be considered. I ordered a smaller amount before, which came out to be legitimate, but I should note that they do tend to lie to the customs(as in my case, they labeled the iodine as "clothing accessories" ).

Well....that didn't really work out as expected. So this was supposed to be Hexamminecobalt(III)oxohexacarbonatotetraberyllate but I just recently found the description of how to actually prepare it and I should have had used a Carbonate...so from the fact that even the so called insoliuble Co(III)ammine-Complex didnt really precipitate and that stuff is still full of Ammonia its probably just some Be(OH)₂ that has formed.

I just read that even that complex mentioned above is supposed to be white when clean...so no colored Be compound again which is really sad. I'd really like to show you that Be Chemistry can be interesting, too but there is just no good inorganic complex which would be colored. s-Orbitals don't split so there is no transition unfortunately.

I think the only way to make it a bit more colorful would be to bind it to a pi-System that is already colored like in Chlorophyll for Magnesium.

So I will try to prepare the complex mentioned above again in a pure form and hopefully give you a real picture of it. Does anyone know about a good inorganic perhaps colored Be Compound ?

A slight break from the preceding, but...
I hope nobody objects to explicit images of naked flames?




Candle in microgravity



Direct photographs of sooting n-C₄H₁₀ non-premixed gas-jet flames at 1 µg at Reš42, jet diameter 10 mm, showing evidence of thermophoresis-induced agglomeration at µg.



"CH₄/Air premixed flame attached to a carbon-coated brass matrix cooled with water. Fuel rich to fuel lean from left to right and top to bottom by increasing air flow rate and decreasing CH₄ flow rate. Small flames dance around and a butterfly appears. When the butterfly flies away, flame is gone."


Last not least:


Why you don't extinguish Mg fires with a carbon dioxide extinguisher - even on a space station

Quote: Originally posted by Theoretic

A slight break from the preceding, but... I hope nobody objects to explicit images of naked flames? Candle in microgravity Direct photographs of sooting n-C4H10 non-premixed gas-jet flames at 1 µg at Reš42, jet diameter 10 mm, showing evidence of thermophoresis-induced agglomeration at µg. "CH4/Air premixed flame attached to a carbon-coated brass matrix cooled with water. Fuel rich to fuel lean from left to right and top to bottom by increasing air flow rate and decreasing CH4 flow rate. Small flames dance around and a butterfly appears. When the butterfly flies away, flame is gone." Last not least: Why you don't extinguish Mg fires with a carbon dioxide extinguisher - even on a space station

So did another attempt to make a colored Beryllium Compound. This time I used an organic ligand. It took me quite a while and a few tries to get a useful result but it looks quite cool right now.

According to literature there is a Curcumin complex with Beryllium in an alkali solution. Literature suggests using Ammonia but I found that the results are so dark if you use too much indicator that you wont be able to see anything. So I switched to KOH as base.

What you see here are two test tubes filled with the same amount of KOH solution, made from one spatula of KOH in about 30 ml of water.
To one I added a Berylliumsulfate soltuion, made from 2 small spatulas of pure BeSO4 in about 25 ml of water. I took about 3-4 ml of this solution and added it to one of the test tubes and to the other one the same amount of water.

Literature often talks about the precipiate formed (BeOH₂) but I did a run with quite much precipitate and it didn't really change that much. The one you see here is only a little cloudy and its really hard to even see the Hydroxide formed. So this can be done in a quite low concentration as well. I then added a few drops of curcumine in Ethanol to both of them.

The one without Beryllium stayed in solution and became brown-orane the other one precipitated and changed to a red color (hard to see on the photo).

In the pictures on the bottom I added a lot of indicator to the left test tube without beryllium and some solid BeSO4 to the other one as you can see as long as they are diluted even higher conc. of indicator and Be althought the both form a red layer where they meet differ in color if you diluted them long enough.

So I know Quinalizarin looks better but that is too expensive for me to buy it so I stay with curcumin but will try something interesting, soo.

Copper(II) acetylacetone

Copper(II) acetylacetonate recrystallized from chloroform... Check out article about preparation - COPPER ACETYLACETONATE PREPARATION



[Edited on 23-3-2016 by Hegi]

Quote: Originally posted by Zephyr

Those look like amazing crystals! I'm interested in viewing the prep but it seems your link doesn't work? Sadly my acetylacetone synthesis failed, maybe I'll try again in a few weeks...

Wonderful, thanks DraconicAcid. I look forward to more great projects from pieceofscience!

Here's a pic of the drying rack I built for some substance:

Quote: Originally posted by Zephyr

Those look like amazing crystals! I'm interested in viewing the prep but it seems your link doesn't work? Sadly my acetylacetone synthesis failed, maybe I'll try again in a few weeks...

Here is the synthesis I attempted. As you can see moisture leads to issues, and I suspect it was the culprit... A bit of



Insight on how it could be done better or issues with this route are appreciated.

Quote: Originally posted by Hegi

Quote: Originally posted by zts16   Nice! I'm actually currently working on an indigo synthesis too, however I'm actually synthesizing my own 2-nitrobenzaldehyde, so it's a more lengthy procedure. I have 2-nitrotoluene now, and I'm currently awaiting the arrival of the solvent that I need for the oxidation step. Then it should be smooth sailing from there. A writeup will be posted once I am finished. Oh man, such a long way. The last step is really smooth sailing besides making your own 2-nitrobenzaldehyde. Did you prepare 2-nitrotoluene?

Quote: Originally posted by Zephyr

Here is the synthesis I attempted. As you can see moisture leads to issues, and I suspect it was the culprit... A bit of Insight on how it could be done better or issues with this route are appreciated.

I think your scheme is wrong because it looks like you work with an alcoolate of 4-hydroxy-pentan-2-one.

2,4-Pentandione (CH3-CO-CH2-CO-CH3 equal to CH3-C(=O)-CH2-C(=O)-CH3 ) can make a stabler enol because of the resonance between the C=C double link and the C=O double link...such systems are acidic see phenol.

CH3-C(-OH)=CH-C(=O)-CH3 <==> CH3-C(=O)-CH2-C(=O)-CH3 <==> CH3-C(=O)-CH=C(-OH)-CH3

So it looks like you simply have forgotten the C=C double link in your scheme and that the resonance hybrid includes the C atom between the two C=O groups.




[Edited on 25-3-2016 by PHILOU Zrealone]

Some Thallium Nitrate on an Iron nail in the flame, a beautiful green although its pretty hard to get on cam, nothing like Barium or Copper would emit.

@TheVolatileChemist:

Thanks. Take it if you need it for the wiki. As our Cyanide Chemist I should probably do some pages on transition metal cyanides for our Wiki but I'm too busy doing other stuff and I don't like writing articles .

Also if anyone knows a cool colored complex with Thallium I'd be interested. I have an Ebook on Thallium Chemistry but I won't buy special reagents just for that single experiment. So no complicated organic ligands. I found 2 interesting, one with Chromium and Thallium(III)Chloride where Thallium is really in a [TlCl6]-complex so not just a precipitate and one with Cobalt. Problem the fist one requires Hexamminechromium(III)chloride which is either done using cold Sodium Amide or cold temperatures and quite a lot of Ammonia and Cr(II). So nothing I have time for at the moment. And for the Cobalt one...well that was kinda my bad to accientally use Potassium Nitrite instead of Sodium Nitrite and I now have the precipitated Potassium salt -.- . So if anyone has a good suggestion, I don't want to waste it since I'll be needing it soon but for one or two cool compounds I'd gladly sacrifice some of it.



[Edited on 2-4-2016 by fluorescence]

Nothing fancy, just some urea needle-shaped crystals I made a few days ago. Longest crystals are about 5 cm long.
Too bad they broke when I tried to get them out of the beaker (they are very fragile)

Quote: Originally posted by Mabus

Nothing fancy, just some urea needle-shaped crystals I made a few days ago. Longest crystals are about 5 cm long. Too bad they broke when I tried to get them out of the beaker (they are very fragile)

They look really amazing Nice one Mabus! How fast did they grow?

Quote: Originally posted by Hegi

Quote: Originally posted by Mabus   Nothing fancy, just some urea needle-shaped crystals I made a few days ago. Longest crystals are about 5 cm long. Too bad they broke when I tried to get them out of the beaker (they are very fragile) They look really amazing Nice one Mabus! How fast did they grow?

Quote: Originally posted by Mabus

Quote: Originally posted by Hegi   Quote: Originally posted by Mabus   Nothing fancy, just some urea needle-shaped crystals I made a few days ago. Longest crystals are about 5 cm long. Too bad they broke when I tried to get them out of the beaker (they are very fragile) They look really amazing Nice one Mabus! How fast did they grow? I left them to grow overnight, between 12-18 hours. I think it also helped that the temperature slowly went down from 20 °C in the noon to 5 °C during the night. I didn't intend to grow such large crystals, I merely wanted to purify some urea I got for free.

Quote: Originally posted by Theoretic

A slight break from the preceding, but... I hope nobody objects to explicit images of naked flames?

So....I have no idea what I just did.

Some time ago a friend gave me a bag full of natural Arsenic, he purchsed that somewhere, I dunno. Some black chunks, some have impurities some are quite pure. I did some experiments with them like dissolving them, there is a pictrue in this thread. So I decided to try to make some Oxide from it by heating it. I took some small chunks into the test tube and heated them with the burner till the glass became quite soft, dunno where the melting point of my glass is. The chuncks started to smoke producing a dense brown smoke. I stopped and the thing you see on the picture formed. I than took the test tube and turned it upside down. The Arsenic fell out and started smoking brown again. You can see a dark brown trail on the upper part of the test tube where they touched the glass when falling out.

That is not what I expected. I tried this before, back then with a heat gun so it was much slower and back then only white stuff had formed. Ehm...well it looks like an Arsenic mirror, its fully reflective, as you can see there is my reflection in it its silvery on the outside and on the inside it has a quite rough black surface.
It really reminds me of the Arsenic you make using the Marsh test. Also I noticed a familiar smell comiing from the test tube after it cooled down. It reminds me of the smell that Phosphorus has when you burn it. It wil alwys leave behind a white, waxy rest when its burned and that usually smells like the stuff coming from the test tube....

Anny suggestions ? Maybe Sulfide or something that fell apart under the hot temperatures forming elemental Arsenic ?

I read about a suboxide of Arsenic that can form and that smells like phosphorus and is brown as well.

I mean I could have distilled Arsenic as well although I'm not sure if the temperatures really reached 600°C and maybe the fine powdered arsenic when cooled down got coated with this suboxide that appearently smells like garlic. That could be an explanation.

Hard to admit for me as an Inorganic Chemist but I have no idea what this could really be.




Edit:

I took one of the small grains and heated it directly with the bunsen burner on a metal surface. It immediately formed the same black stuff behind the metal. So I guess that by heating it wih the burner in the test tube it got the sublimation point of Arsenic faster than Arsenic reacts at these temperatures with the oxygen to form the Oxide. So I guess the black stuff it just Arsenic and some small amounts of Oxides which give the smell.


[Edited on 9-4-2016 by fluorescence]

Tin crystals

Here is some Thallium Chemistry. I wasn't that creative this time simply because I didn't have too much time. Still I like the results. Those are only very small amounts due to the fact that pure Thallium Salts are really expensive and I need them for some other experiments soon and they are not that well soluble as you might expect at least if you dont boil the solution. So I stayed with small samples and still enough compounds formed. Note that all of these compounds are insoluble and seperated pretty fast I just shook them before I took the photos so you could see them better.

I really like how the colors vary with Potassium Ferrocyanide and Chromate both being yellow and many other prec. Ferrocyanides being brownish as well it surprises how the Thallium sample can form a white compound and a yellow one. Usually I check these reactions before I post them here but I didnt have time so if there is any mistake like a side reaction I didnt think of just tell me.
To the Selenide. I suppose this is the Selenide. I tried a new method to make transition metal chalcogenides. There will be a post on it soon i am still drying the Cadmium Sulfide I made for test and then I have to test if its really the Sulfide and not something else. After that I will make a post on how I made this Selenide.

OH YEAH!!! Sassafras Albidum (it IS chemistry related, mua-ha-ha)

Arkoma, binomial names have the species part written in all lowercase!

Barium chloride crystallising out of solution!
Largest crystal was about 15cm long, smaller crystals around 3cm ish. It happened by accident as I was evaporating down a solution of barium chloride I had just made with HCl and barium carbonate. I managed to keep most of them intact when getting them out of the dish.

This is why I love copper salts: Easy to make and beautiful.

It's Copper II chloride in excess HCl

Wow looks really cool, I like green compounds ^^.
Did you even put some hazard labels on the bottle ?


So here are two other Thallium compounds. As promised I made some Tl(III) Oxide from Ferricyanide(III), KOH and Tl-Nitrate.

And on the right is some Thallium(I)-Iodide. I tried some Tl(III)Iodide as well but it wouldt form. I love how the color changes from the fine powdered orange iodide to the bigger yellow chunks after standing for 5 min. or so.

Patterns in a flame reminiscent of the patterns on the cathode of a low pressure discharge tube.

@Fluorescence , Yes, I made them with a label printer. The glue on it is too weak to hold the hazard signs in place, so I had to put some tape...

Here's my whole "collection" of componds (including a some elements).
A lot is "homemade".

Chlorine

Another poster requested I upload a photo of my sample of pressurized chlorine. Just a little ampule cast inside a much larger cube of high quality resin.



I'm setting a goal of photographing each of the elements in case anyone has any requests :-)

Rasiel

Wooops, I meant for this to show up on the pretty pictures thread. What'i do wrong??

Quote: Originally posted by rasiel

Wooops, I meant for this to show up on the pretty pictures thread. What'i do wrong??

Quote: Originally posted by fluorescence

Looks really well done. Some guys I knew tried that as well but after some time they tend to get all brown and cloudy. I hope your resin will stay as it is at the moment. Looks really nice.

Beatiful green-blue crystals of a-modification of NiSO4.6H2O.
Im still growing them, the biggest is about 1cm in diameter .

EDIT: I didnt notice that hegi has already posted this picture in another thread, should I delete this post?


[Edited on 11-5-2016 by crystal grower]

Quote: Originally posted by rasiel

Oh wow, they look like breath mints! :-) Rasiel

Lol, they remind me sapphires .

Quote: Originally posted by rasiel

Another poster requested I upload a photo of my sample of pressurized chlorine. Just a little ampule cast inside a much larger cube of high quality resin. I'm setting a goal of photographing each of the elements in case anyone has any requests :-) Rasiel

Today I took a pic of calcium... the way few people get to see it!

Some Se₈²⁺ cations forming. The first run was too concentrated and appeared almost black this one here is really dilute and still it has a quite strong green color.

For those who actually read my bio ^^, I do a lot of Selenium Chemisry for my Thesis. Certainly not an element I would work with if nobody had asked me to do it. I love toxic compounds but Selenium is just really nasty. And most of my Selenides at work fall apart on air producing some H₂Se and it's really terrible to work with that.

I think that Selenium chemistry is something most people have no clues about. If wanted I could do a small article on the forum on actual selenium chemistry and behaviour in comparison to sulfur for example.


Also has anyone made some NaHSe before. I tried yesterday via the Se + NaBH₄ in Ethanol method and it didn't really work.

I'd love to hear more about selenium chemistry. It will save me actually doing it.

Just discovered while drying my product that Thallium(I)Chromate seems to be thermochromic. Tried it 3 times in a row and it would quickly turn orange-red while heated even slightly and quickly turn yellow again afterwards. Not sure if this is already in the literature I didn't check yet but Tl-Chemistry just surprises me everytime I try it.

Quote: Originally posted by fluorescence

Just discovered while drying my product that Thallium(I)Chromate seems to be thermochromic. Tried it 3 times in a row and it would quickly turn orange-red while heated even slightly and quickly turn yellow again afterwards. Not sure if this is already in the literature I didn't check yet but Tl-Chemistry just surprises me everytime I try it.

Wow that is really amazing! I had never chance to work with Tl and its compounds. I heard about a few mercury compounds that are thermochromic. If you find more about, please share info. Thanks.

Just got a sep funnel! Also, one of those actinic Erlenmeyer flasks and some small volumetric flasks, all of which my AP teacher had decided she didn't need. *Score*

Edit: At least I think it's a pretty picture...it's the most sophisticated piece of glassware in my lab...Also, it was formerly a piece used at OSU, our local university...


[Edited on 5-24-2016 by The Volatile Chemist]

Nice I got mine in a similar way. Went to a pharmacy when they closed and sold all their stuff and bought a lot of glassware. I think the seperating funnel was really cheap or even a gift like yours. Cant' really remember

TVC-it IS pretty. Both of mine are only 250ml

Quote: Originally posted by The Volatile Chemist

Just got a sep funnel! Also, one of those actinic Erlenmeyer flasks and some small volumetric flasks, all of which my AP teacher had decided she didn't need. *Score* Edit: At least I think it's a pretty picture...it's the most sophisticated piece of glassware in my lab...Also, it was formerly a piece used at OSU, our local university... [Edited on 5-24-2016 by The Volatile Chemist]

Quote: Originally posted by mr.crow

Quote: Originally posted by The Volatile Chemist   Just got a sep funnel! Also, one of those actinic Erlenmeyer flasks and some small volumetric flasks, all of which my AP teacher had decided she didn't need. *Score* Edit: At least I think it's a pretty picture...it's the most sophisticated piece of glassware in my lab...Also, it was formerly a piece used at OSU, our local university... [Edited on 5-24-2016 by The Volatile Chemist] That's a nice sep funnel. Its always nice to save old junk from the university.

Recently, I've been really interested in crystals of pure metals, mostly for my element collection. After being inspired by The Backyard Scientist's video (see his post on page 23 of this thread), I decided to grow some of my own copper crystals. Over a period of six weeks, I used a 40g/L solution of copper sulfate and two copper electrodes with a current of always less than 10mA to grow some truly amazing copper crystal clusters. Unlike nearly all the other experiments I saw online, these crystals are very large and sharply defined - they are not nodules or rounded growths. I think that the extremely low current and the very long growth time contributes to the crystalline nature of this growth.

I made a YouTube video about how I grew this, and I also included a 360° rotation to show the entire crystal. https://www.youtube.com/watch?v=zZniOJ7swic

Also, for those who might like to repeat this experiment (the crystal is truly stunning), I wrote an extensive post on my website with details on the experiment. http://sciencewithscreens.blogspot.com/2016/06/experiment-53-growing-large-copper.html This post also has a link to my experimental data and observations I recorded during the six-week period.

Finally, I also included the less-impressive picture of my first attempt. This used currents of around 20mA over two weeks, and I accidentally broke the crystal. It's still pretty neat, though.

In the future, I will be trying other metals. Does anyone have experience with growing crystals of other metals? Thank you!

Quote: Originally posted by The Plutonium Bunny

In the future, I will be trying other metals. Does anyone have experience with growing crystals of other metals? Thank you!

First pic: Te metal, Se metal, copper nanoparticles and a copper acetate solution. Te and Se metal was a souvenir during my internship hahahaha . Copper nanoparticles were synthesized from ascorbic acid and copper acetate solution.


Second pic: A potassium ferrioxalate crystal. Around 1.5 inches in size.
Grown around 4 weeks, and grows cleanly and fast as well.
Made from dissolving iron with HCl, forming FeCl2 then precipitated into FeC2O4 using oxalic acid, washed away the chlorides with water, then oxidized into Fe(OH)3 with H2O2 made basic with K2C2O4. The resulting precipitate (Do not decant away the solution!) is then dissolved with oxalic acid again forming apple green solution.

The brown stain is the reacted solution with light, meaning it is light sensitive.



[Edited on 28-6-2016 by CrystalCage]

Quote: Originally posted by The Plutonium Bunny

Recently, I've been really interested in crystals of pure metals, mostly for my element collection. After being inspired by The Backyard Scientist's video (see his post on page 23 of this thread), I decided to grow some of my own copper crystals. Over a period of six weeks, I used a 40g/L solution of copper sulfate and two copper electrodes with a current of always less than 10mA to grow some truly amazing copper crystal clusters. Unlike nearly all the other experiments I saw online, these crystals are very large and sharply defined - they are not nodules or rounded growths. I think that the extremely low current and the very long growth time contributes to the crystalline nature of this growth.

Hi man,

very nice work! I decided to set up the same experiment and grow my own crystals. I used LM317 as well with 2x120 ohm resistor and potentiometer on adjustement pin of LM317. This resulted in 0.30V between cathode and anode but I could not measure current flowing through the circuit. Display stayed at 0.00 mA. Something must have gone wrong. Would you mind posting your LM317 circuit scheme and how did you measure volatge and current?

Thanks a lot!

Quote: Originally posted by Hegi

Hi man, very nice work! I decided to set up the same experiment and grow my own crystals. I used LM317 as well with 2x120 ohm resistor and potentiometer on adjustement pin of LM317. This resulted in 0.30V between cathode and anode but I could not measure current flowing through the circuit. Display stayed at 0.00 mA. Something must have gone wrong. Would you mind posting your LM317 circuit scheme and how did you measure volatge and current? Thanks a lot!

Certainly! Here is a schematic I drew in Paint of my setup. The five 1N4007 diodes drop the output voltage a little bit so that I can get lower output voltages with the LM317. Also, the resistors and potentiometers don't have to be exact- adjustments will still give you a wide range of voltages.

Also, something I learned a while back is that to measure current with a multimeter, the electricity must flow through the multimeter. This is different from measuring voltage, where the multimeter connects to two opposite points. Measuring current requires breaking the circuit and connecting the multimeter to either end of the break. It took me a while to learn this.

Good luck, and keep trying! It will be worth it in the end!

It's always a good idea to decouple the ADJ input and have at least a bit of smoothing on the output, thusly :



If not, there is a risk of oscillation which is hard to see on a digital multimeter.

Thanks guys, my scheme is the same (except i did not use capacitors)... After 24 hours dendritic copper crystals about 0.3-0.4 mm size can be observed. I did measurement of current in the way it is supossed to be measured but NOTHING happened - value stays at 0.00 mA. Voltage is in range 0,27-0,30V and the resistance of the solution is approximately 220 ohm.

Did you observe forming small dendrites at the begining? .. or should I start again?

Woah, the copper crystals are amazing, I must try that one day.

A colorful reaction to make a new compound and its crystals during my internship.

[Edited on 9-7-2016 by alexleyenda]

The effect of 8bar water on the seat of my sink water tap.
Its soft water but it may have been caused by inclusions in the poor quality brass or cracks.

Quote: Originally posted by wg48

The effect of 8bar water on the seat of my sink water tap. Its soft water but it may have been caused by inclusions in the poor quality brass or cracks.

Soft water is better/gentle for resistance into warming systems but it is also more corrosive to plumbing and piping than hard water.
No pain, no gain ...no universal curing agent

[Edited on 14-7-2016 by PHILOU Zrealone]

This compound I made (at the research lab where I'm working this summer) shows drastically different fluorescence in solution (30 mg/mL in CDCl₃) vs. as a solid.



[Edited on 7-20-2016 by Metacelsus]