hermanntrude

but then you'd only know the total amount of copper in the solution, not the amount of copper (I) and copper (II)

no no, I can have both. I work at a college, not a school, and that's why.

bummer. I forgot about the HCl CuCl is insoluble? really? I googled it and you're right... one of the exceptions to the solubility rules LINK OK so how about this: neutralise the solution with NaOH, recording the amount you use, then filter it and weigh the dreid solid obtained. Then evaporate the neutral filtrate to dryness and calculate how much of it is copper (II) chloride either by subtraction, using the amount of NaCl you know you formed, or by titration for Cu(II), if there is such a thing, or by both methods to prove some level of accuracy.

here in newfoundland the schools aren't allowed sodium or potassium on site. colleges are, though I could have rubidium and cesium if i wanted

Be extremely careful with thermite-type reactions. It's a reaction hotter than almost any other you can do, and can very easily run out of control, setting fire or melting things you didn't know could catch fire or melt. If you put sand under the reaction it'll be turned into glass, for instance...

thread moved to homework help. When diagrams are given in this format, finding the enantiomer is easy, just look for the one where the wedges and dotted lines are swapped.

what you need here is nor raoult's law or the ideal gas law, what you need is the clausius clapeyron equation. Look it up in your textbook.

the stuff in electronics stores is in solution. Probably not what you want for a moisture sensitive experiment...

Advice to anyone who wants to make halogens or group I metals: Look up the MSDS of all the relevant materials BEFORE you start. MSDS are easily found by googling. They are very revealing documents. example: MSDS for chlorine

excellent idea YT, assuming the reaction goes to completion, it'd give you a simple method, without even titrating. Gravimetric rather than volumetric. I was just about to suggest it myself

while it's true that CO is often man made, it is also created by incomplete combustion, which happens without man's intervention sometimes. Interesting demonstration. Lawlord, to answer your original question, there are VAST amounts of different "chemicals" which can be extracted with ease. I recently saw a demonstration of someone extracting DNA from strawberries, which was pretty impressive. I expect it's online somewhere

interesting speculation lawlord. let me know when you've decided which experiments to do, and i'll let you know if they're suicidal, and give you some tips and hints.

I think you mistyped your post, hs. I corrected the mistake

that's a toughie. You can't titrate for the Chloride ions because of the HCl. I guess you'll have to find something which a) reacts only with cupric or cuprous ions b) either changes pH upon reaction or changes colour good luck!

with conc nitric, I always stick to glass. I wouldnt advise making it at all, but if you do, good luck and please dont hurt yourself MSDS for nitric acid-PLEASE READ

you can tell by looking at the colours. Copper (I) and copper (II) look very different

ha. probably, but you never know who else will be reading the thread.

I suspect the distillation your friend did was the distillation of salt water, which would result in salt and water, separated. You can't really distil sodium chloride, but like some of the members suggest here, you can electrolyse it, which is a hazardous process and not for someone who is new to chemistry

dr P i have three pounds of sodium in my laboratory! and 5 g of potassium! also a large tin of red phosphorus. I'm a little scared of that room.

or electrolysis of a concentrated solution of KI will give iodine. Halogens are very highly dangerous, though. Inhalation can cause a delayed pulmonary oedema

weird exam, but if you study organic chemistry you ought to know the stuff on there... assuming you also know the language in which the naming is being done

chemistry is very hazardous. Be very careful. To be honest i'd reccomend you take a degree-level course before messing about at home. Another thing to become very familiar with is MSDS (material safety data sheets), they'll tell u the hazards you're dealing with. Having said that, a home laboratory is a difficult thing to run, especially in a place like the USA (i assume that's where you are), since many of the normal chemicals are only available to commercial buyers. Perhaps get a chemistry set for children? They come with instructions for some interesting experiments. There might even be a book you can find for your particular interests, but it'd probably be old. sorry I couldnt be of more help but i can't suggest particular chemicals or apparatus because i dont know which experiments you want to do or whether you'd be allowed to make the purchase.

by the way, if you electrolyse a very concentrated solution of sodium chloride with a 9V battery, you will get some chlorine at one electrode. I did it once, thinking I'd get oxygen but once i saw the yellow bubbles i rushed outside so as not to give my family pulmonary oedemae (sp?)

thread moved to homework help. Please do not post in the general forum when you are seeking help with homework. Please also do not give out answers to questions like these, especially when the orginal poster writes "please can you help me with". This phrase implies the poster wants assistance in understanding the concept, not just answers. Unfortunately, nomenclature is a fairly difficult subject to summarize, since there are so many functional groups and rules for the process, BUT it IS all written down by IUPAC. The first one is a real toughie, since it involves a fairly uncommon functional group, the substituted hydrazine. Once you've recognised the hydrazine you can write down the two substituents in alphabetical order, followed by the word "hydrazine". i think TJames got it right. The second one is much easier, since it is a common functional group with only one attachment point. All we have to do is find the longest possible parent chain, in this case there are two, both with seven carbons, so we know it is a type of heptane. Then we look to see the other substituents, which are ethanyl and the alcohol group. The chain containing the alcohol group will be a heptanol chain so all we have to do is put in the ethyl group, giving them both numbers. The rule is we put the numbering system in such a way as to make sure the numbers are as low as possible, so instead of 5-ethyl-heptan-4-ol, it's written 3-ethyl-heptan-4-ol. THIS site has the IUPAC nomenclature rules on it THIS site, from wikipedia, is a bit simpler to understand and is where i tend to go if i have problems. There are computer programs which can do the naming process too, but they're a bit unreliable and usually fairly expensive.

I think in that case they're saying "supercooled" meaning below the normal freezing point of [salt] water, but under the ice is a very different environment, very cold, very high pressure. It probably means not that it is "supercooled" in the sense that it might go crinch any minute and turn into an arctic slushie, but that it's colder than you might expect, given the normal conditions under which water is liquid.