Can Scandium be dissolved in anyhting?
371456
It can be dissolved in acid.\n\nhttp://www.lenntech.com/Periodic-chart-elements/Sc-en.htm
829643
Not without a reducing agent that will turn iodine into iodide, and then you will have to get rid of that reducing agent.\n\nI guess if KI is unavailable you'd better look for another titrable reducing agent to react with the bleach, e.g. Fe2SO4 solution.
957199
If you are doing it in a laboratory setting, you can mix it with carbon and reduce it to the metal. You will need high temperatures, though.
842976
20 grams\ndissolving compounds and then driving of the solvent is a common way to purify a compound. You will not lose any of the compound unless it is reactive with the solvent you dissolve it in. In the case of water and salt they are not reactive so when you drive off the water you will be left with the same amount of salt that you started with.
600262
They both dissociate completely in water, but sulfuric is technically the stronger acid.  I think that that's what they use for metal etching as a matter of fact, but I could be wrong.  Anyway, metal would be more adversely affected by sulfuric, as would flesh (although they both hurt pretty freaking bad).  I'm sure it's the same with plastic.  A better way to dissolve plastic, though, is organic solvents such as THF.
430333
it is hard to say as some of these compounds have never been made, but if you stick to your classic organometallic 18 electron rule then i presume they would be.  I know you can make a carbonyl with uranium, but if it is stable i don't know.\n\nEDIT: i've just looked at my organometallic textbook and it states that presently (1988) no lanthanide carbonyl has been made that is stable at room temprature.  You can make them but they hyrolyse straight away.
64690
NA2SO4,KOH,AGCL,CA(NO3)2 ARE SOLUBLE.AND HG2BR2 AND CDS IS INSOLUBLE.
838558
Of course. Take any compound that is not very soluble in water.\nThe saturated solution will have a very low concentration of this compound. E.g a saturated solution of CaCO3 is approximately 5.8*10^-5 M
139382
First, you dissolve your compound in the solvent in which is is most soluable (perhaps THF or methylene chloride).  Then you very carefully use a pipette to layer the solvent in which it is not soluable on top (perhaps diethyl ether or pentane).  You need to add the second solvent slowly and carefully.  Let the solvent run down the side of the container.  Obviously the top solvent needs to be less dense than the bottom one.  You then let the container sit undisturbed on the bench or in the freezer away from any vibrations until crystals form.  As the upper solvent diffuses into the lower solvent, you compound will become less soluable until it falls out.  The first solution should be as close to saturated as possible.
712818
more soluble in what solution?
693880
The answer is NO for both of your questions.\n\nFirst human can't take metals in their free form. Our body can only absorb/utilize metals in ionic form, such as Fe2+ (not Fe3+), Ca2+, Zn2+.\n\nThe metal ions, however, DOESN'T have to be in organic form. For example, you can consume Ferrous sulfate (FeSO4), which is pure inorganic compound or Zinc sulfate (another inorganic compound), although, obviously you can also consume oragnic salt as well, such as calcium citrate or iron fumarate.
508324
First off... dihydrogen monoxide is ....WATER!!!!!!!!!\n\nThe smaller the salt crystals you are trying to dissolve, the more rapidly they will dissolve... due to increased surface area.
822936
Look here:\n\nhttp://jewelrymaking.about.com/od/solderinginformation/a/032806.htm\n\nand here:\n\nhttp://alchemy.chem.uwm.edu/amalgamator/NCW/ncw2001/results.html\n\nto get the following:\n\nThe pickle, used in the soldering metal process is a sodium bisulfate based solution. This pickle is particularly good for gold. Other metals use different pickles. For example, "Copper and copper alloys can be pickled in sulfuric acid solutions with the addition of an oxidizing agent (for heavy scales) such as chromic acid, nitric acid, ferric sulfate or sodium dichromate. NOTE: Chromic acid and dichromate require treatment for hexavalent chromium. Chromic acid or dichromate solutions tend to passivate the substrate and require activation prior to plating. Activation is commonly carried out in 5-10% sulfuric acid solution or 10-20% hydrochloric acid solution. If the latter is used to interchangeably pickle steel parts and copper parts, the dissolved copper must be closely controlled to avoid a typical problem. The dissolved copper will eventually plate out on the steel parts and cause adhesion problems."\n\nI hope this helps.  Be careful.
661226
It doesn't matter how much iron you happen to dissolve as long as you have the exact mass you dissolved for the later calculations. Use just enough sulphuric acid to dissolve all of the iron, then transfer the solution into a measuring bulb and fill up to the mark - the theoretical concentration of iron is the mass you used divided by the volume. \n\nTheoretically you need 1 mol of acid for each mol of iron, but you will want some excess acid to keep the ions in solution. Make sure that oxygen has no chance to react with your solution during dissolving and titration.\n\nTitration with potassium permanganate in acid solution will require 1 mol permanganate for each 5 moles of iron. Usual lab concentrations are 0.02 mol/l (1 ml of that solution detects 0.1 mmol iron). You will want to use roughly 20 ml permanganate solution per titration for a volume error <1%.\n\nNow we start calculating (using SI units). Iron has a molar mass of 55.8... g/mol. If you want to use about 20 ml, you will need about 0.002 mol of iron. \n\nYour iron solution will have a concentration of \n\nC = m / (M * V)\n\nm : mass of (impure) iron you dissolved, in grams\nM : molar mass of iron, in gram/mol\nV : volume of the volumetric bottle you filled your solution up with, in ml (for convenience)\n\nC : concentration of impure iron, in mol/ml\n\nDivide 0.002 by C to see (roughly) how many ml of your iron solution you want for your first titration. Take an appropriate full pipette which fits the order of magniture, or else dilute your original solution in a volumetric bottle so that you can use a full pipette you have at hand.\n\n\nNow to get percentage purity.\n\nI'll assume you can calculate a concentration from titration.\n\nWith your titration you will determine the measured concentration of iron (in small numbers of mol/ml). Divide that result by C (calculated above), and multiply by 100 to get percentiles.\n\nHave fun!
795210
When choosing a recrystallizing solvent you want a liquid that:\n\n1. Does Not React with what your trying to recrystallize.\n\n2. A solvent that the compound is barely soluble in. \n\n3. A solvent that quickly evaporates.\n\n    After you determine your solvent you can dissolve your compound without changing it. You can add just enough solvent to dissolve the compoud. Wait for the solvent to evaporate causing the ppt of your purified compound.\n\nMark
229659
Yes you can.  Some, like radioactive elements, are controlled by law or very difficult to get, but you can buy almost anything if you look around enough.\n\nThis guy has put together an excellent collection of elements:\n\nhttp://www.theodoregray.com/PeriodicTable/\n\nSome he purchased, some were gifts from people who heard he was trying to collect them all, some he isolated from common chemicals himself, and so on.  It's a very interesting collection.
436959
Say goodbye to matter, I suppose.\n\nWithout electrons (which are negative), all chemical bonds would collapse - so definitley say goodbye to any and all compounds. There goes most materials.  Ditto for chemistry.