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jsatan

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Posts posted by jsatan

  1. Hi guys, Its been a while and my brain has gne soft, (blows the dust off the chess set).

     

    Right,

    I've got a LED it is a 2.5V at 11mA

    I've got a battery at 1.5V 1800mA

    How long would the battery last if the led worked at this low voltage.

    worked it out and I got some silly number, something like 43 sec's.

     

    Can someone show me the way this would be worked out so I know for the future.

    My cals were:

    (1.5 * 1.8)/(2.5 * 0.011)

    That says my led would only last 108s, my maths has gone!!!

     

    Jon.

  2. aha from what I've read (a few years back) you can boil it then heat it like you say but I'm not sure on any numbers at all. lol.

    But I've got a shed load of it, from my home made air filter.

    If you find a fish shop (pet fish, not dinner) they sell it for filters. There is an online Co that sell it very cheep but for small amount wilkos sells it.

    I'll try and find my link tonight about cleaning A, carcoal and let you know.

    :)

  3. another nice one like that is Cobalt Chloride' date=' it`ll go from dark blue to bright pink with temp change, It looks even more impressive if you dissolve it in alcohol, put it in a test tube with a stopper. the color change from taking it out of the fridge or into a glass of hot water from room temp is quite dramatic.

    Sodium Sulphide soln also changes color on heating, from a light yellow to a deep red/brown.

    there are others, but these are probably the most simple examples anyone could do :)[/quote']

    lol.I did this with out know what I was doing when I was young,:D

    I think I was about 11 or so, I just added water and put it on some paper, lol.

    I'll have to try the ethanol.

  4. yeah, don`t store it as conc, the acid can be a little unpredictable with at those levels, battery conc is fine in those sorts of plastics, AND you have the added advantage that most bleach bottles have a sucurity cap on them too, but I`de still label it clearly to avoid mistakes, you don`t want someone adding it to the Final Rinse in your washing machine beleiving it was Bleach! :)

     

    Points finger at mum and GF.

    lol.

    Yeah I always lable my things.

    :D

  5. positive' date=' I have a bottle in my shed that`s been there for over 2 years now, I actualy had to get some out of it on Saturday to re-fill my glass bottle that`s kept in the lab, I also have 3 litres of it in a plastic soda bottle too, that`s nearly 5 years old now, no decay at all, the acid conc is 35%.

     

    I stock anything above this in glass though, never in plastic.[/quote']

    lol that sound just like what I'm wanting to do.

    When I was in coventry I had trouble finding any S-acid with out buying in bulk so I just left it for the time being.

    I put the feelers out for old car batts and before 2 weeks is up I've got 4.

    :D

    I'll be keeping the % low I'll boil it up when I need to, :D

  6. well the sulphate batch I made doesn`t' date=' nor does the carbonate with the sulphide imputities in it (I`ve tried it) and even tried UV exposure too, Nada.

     

    I think it`ll be like the Zinc Sulphide I made, it`s too pure, and requires an impurity to "Activate" it, I think Copper is used in ZnS to make it "work".

    I tried that too, but didn`t know the method and it`s also not exactly Googleable (my new word) either :([/quote']

    lol, yeah I read something about copper as well.

    I'll see if I can find any info,

    sounds fun to me, :)

    BTW will a bleach (house) bottle hold sulphuric acid?

    I'm going to go to the pharmacists down my street and ask for some of their old lotions bottle they keep in the cellar, I worked there a while back.

  7. actualy that`s the same method I used a year or so back to make the precursor for Zinc Sulphide' date=' I got my Zinc Sulphide perfectly, but it did NOT Glow-in-the-dark as hoped :(

     

    another interesting action of Sodium Sulphide is that it changes color with temperature, from a light yellow to a deep red/brown :)[/quote']

     

    hummm I think Barium sulphate (or sulphide) is meant to glow in the darks as well, but I think its something to do with the phosphorus in with it.

    :D

  8. well yeah' date=' if you`de like to part with some of it, I know of a good home where it WILL be used in a little less hap-hazzard way :)

     

    if you can get any Strontium salts also, that would be worth me putting you on my X-Mas card list too :)

    I don`t have a lot time to do much "Shopping around" anymore (domestic duties).

     

     

    btw, have you had a look at the last few posts here, the chloride and subsequent conversions of this are well worth doing, it`s a most excellent Green! :)[/quote']

    I'll have a look out for you, I'm wanting some Strontium salts.

    I'm sure I can find some and send some your way. lol.

  9. The first part of this is absolutly right. Next you say that warming your mixture turns it into Copper Hydroxide? This obviously can't be true since you said already that heating copper hydroxide yeilds Copper oxide. This isn't a reversable reaction with heat or lack of alone.

    lol. Nah I dont mean heating I mean letting it warm to room temp, :D

    Not that it matters now,

    Yeah I had the copper probes in the water all the time.

    I did get to a point with one sample of black crap plating out, lol.

    Thats whne I knew the soln was full. :)

  10. aha, I'm getting there slowly but its fun on its way, :D

    Yeah the blue/white precipitate with room temp water did make me think.

    I was using 12V (I know its too much but its all I've got atm).

    Now I know What I'm getting that will help. :D

    I think I remember That there is something good about copper hydroxide but I'm not sure what it was.

     

    I'll be back with more later in the week, :D

    Even tho it didnt do anything that I thought I've still learned something, and thats the best bit, :D

  11. well I`ve finaly finished my electrolysis of the barium chloride to make the Chlorate' date=' it`s been running since friday evening until about 2 hours ago, the soln after filtering was perfectly clear and crystalised beautifuly :)

    the filter paper was also kept as a test, and burned well with more green around the edges and gets washed out by the sodium in the paper, but non the less, the crystaline product is practicaly free of all sodium ions :)))

     

    I`ve also found an interesting read here: http://www.geocities.com/CapeCanaveral/Campus/5361/chlorate/barium.html

     

    now that this process is "tried and tested" I`ll scale it up a little and hopefully get about 25 grams (a container full) for later/future use.

     

    Also, I`m now drying my Barium Nitrate crystals, Start with a near saturated soln of Barium Chloride and add that a near saturated soln of Ammonium Nitrate, making sure the AN is slightly in excess, you`ll see the soln go cloudy almost instantly, stir well and leave it in a warm place to evaporate the water off slowly, you`ll start to see crystals form, that`ll be your Barium Nitrate :)

     

    I could of sent you some Barium nitrate,I had 250g or so of it, wasted most of it as I put it on a fire ( the only way it would do anything).

    I've about 100g left of so, :)

  12. So Now I've got a better power suplly I didnt the age old thing.

    Salty water and copper electrode.

     

    You know the story,

    You get (blue) copper hydroxide and (brown) copper oxide.

    The copper hydroxide will decomposses if over a certain temperature.

     

    So I thought lets cool it and try and make just copper hydroxide.

    So I Let the salty water sit in the freezer until nice and cool and then placed in a ice bath just to make sure.

     

    But I didnt get copper hydroxide.

    I got a green/brown precipitate.

     

    I'm sure I made copper chloride.

    I tested this by taking a sample of the sludge and adding Sodium hydroxide.

    I got copper oxide precipitate and copper hydroxide soln

    I did the same with my sample of copper oxide as a control test, No reaction.

    I also notice if I dont descent a sample it will (as it warms) turn into copper hydroxide(which is should anyway).

     

    There is one thing I did notice with all this, is that the salty water and sodium hydroxide will form different layers.

    This can be used to change what is made.

     

    If I've missed any information out let me know as I've had to type this 2x as the library computers are.....(fill in blank).

  13. The penny has finally dropped from a great height...

    I've made nitric acid later I'm going to make HCl acid.

    I wasnt thinking along the right lines at first.

    Iwas thinking I would mix the chems and heat to give off the gas, BUT not because of boiling away the water.

    So now I know why it seemed as if I didnt have a clue.

    :D

  14. *BUMP*

     

    Update and Possible Hypothesis' date=' Could the copper be having an effect on the Sodium/Potassium pumps in the cells, maybe even calcium?

     

    the reason I ask is that I`ve found that Barium salts have a similar effect, and they are Toxic because of this effect of interfering with these cellular ion pumps, the effects of barium salts last alot longer too.

     

    Could this be what`s going on here?[/quote']

     

    You didnt put Barium salts in your mouth, you crasy!!

    lol

    Does it taste nice?

    :P

  15. For obvious reasons - its not stable! You'd have a bit of a problem if someone accidentally hit a huge vat of this stuff.... BOOOOM! And as for making this stuff a higher concentration i think that would be dangerous past a certain point?

     

    @YT2095: A Hydrogen Peroxide and liver rocket... it could be the new craze... or maybe not. Low concentration was quite fun too - it works with just about anything.

     

    Off topic the enzyme is called catalase and it has one of the fastest turnover rates of any enzyme :eek: (Its probably because of the importance of stopping Hydrogen peroxide build-up)!

     

    Cheers' date='

     

    Ryan Jones[/quote']

     

    Now that does bring back memories, I too was a bio lover..... grrr

    lol.

  16. in that case you were doing the HCl synth then' date=' and as stated in post #28 for HCl NaCl and conc H2SO4 will make a yellowish mixture, and the Brown gas is from Na or KNO3 salts for the Nitric synth :)

     

    it sounds like you didn`t have enough acid and let it boil too dry, naturaly as soon as you lose heat, you lose presure, and that will force any product you`ve made back up the distilation tube, you`re lucky it didn`t go back into the boiling flask! it would have likely caused a steam explosion! (I`ve seen it done in basic chem with newbies, remove the bunsen, sucks the product up into the reaction vessel and BANG!).

    often blowing appart the quikfit glass joints appart too and utterly ruining the reaction vessel (quite expensive to replase also!).[/quote']

     

    Quick fit is what I'm using.

     

    Anyway problem solved.

    I didnt (dont know why) check the ph of the acid.

    Well it was....6 wow.

    So I boiled some up then added the KNO3 and it worked a treat.

    I've now charged the bat (slow very slow old bat) and its ph is about 3 (about 1hr ago) so thats working. lol

    I'm all set.

    such a silly over sight.

  17. HCl is colorless' date=' brown gas can be seen if you make nitric acid and even then most of gas is colorless. Suckback is a problem when dissolving gas in water. I usually leave gas tube slightly above the liquid - all gas will dissolve almost as well. Of course you need fume hood for this. As rogh estimate you need equal weights of sulfuric acid and salt.

     

    It seems that you have not enough experience with labwork to do this process succesfully. Its good idea to spend some days disitilling just water or boiling out table salt from solution. This may seem useles but in fact will give you a lot of invaluable experience.[/quote']

     

    Well thanks for the advice but I've done distilling more times that I can count.

    I normal use a condenser as water or ethanol is a liquid and will turn back into a liquid.

    I've always had the bumping going on in my tubing but with water or ethanol pvc tubing is fine.

  18. well' date=' a little more than just Boiling, you need to distill it, and then collect the vapors in another vessel (Idealy a Cold one).

     

    we have threads on here about making the stuff, but I cannot stress enough, that when making Nitric Acid the apparatus must NOT EVER have any organic mater exposed, ideal an all glass distilation kit is what you need, but there ARE ways to "Cheat"!

    Investing in a roll of PTFE tape would be a wise move :)[/quote']

     

    Yeah My stuff is all glass, (ebay and friends).

    I tried last night, I got the mix down to a powder which was bubbling but looked dry.

    It didnt give any brown gass off, :(

    Then my flask cracked, lol.

    So I turned off the heat and it cooled FAST, making a vacuum and sucking in water at a speed.

    So that messed it up, but the water I was collecting the gas into didnt even change that much (ph).

    I had my ph tester in it on all the time watching it.

    Maybe I wasnt using enough acid. :(

  19. Should not nbe too hard to do if you do as Lance said and use patience (I really don't have muc but thats just me ;))

     

    I actually baught it - had to pay a £20 hazard shipping expence because the concentration was about 30%. I only ordered a small bottle of this stuff and' date=' unfortunatly that was the only concentration they supplied :D

     

    Have some good experimentation,

     

    Ryan Jones![/quote']

    You can buy 17.5% from most hydroponic stores as well as nitric acid (28% I think)

    Thats what I was using before, but I ran out, lol.

    That was £3.50 ish for 1li but cheeper for 5li.

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