What is chloroform like when its made out of NaClO and Acetone???
96642
First of all, chloroform will react with sunlight (UV) and air to form phosgene gas, which forms hydrochloric acid and carbon monoxide in your lungs, so no it is not safe to make your own. This gas was used during several wars to kill soldiers en masse.\n\nDEPENDING ON WHAT STATE YOU LIVE IN, CHLOROFORM MAY BE CONSIDERED A CONTROLLED SUBSTANCE AND BE ILLEGAL TO POSSESS AND MANUFACTURE. \n\nIt is also known as trichloromethane. Here's the information from an MSDS sheet:\n********************************************************************\nAppearance: clear colourless liquid with a sweet odour\nMelting point: -63 C\nBoiling point: 61 C\nVapour density: 4.1\nVapour pressure: 159 mm Hg at 20 C\nSpecific gravity: 1.48 g/cm3 \nStability\n May decompose on exposure to light. Incompatible with a wide variety of materials, including peroxy compounds, alkali amides, strong bases, alkali metals, magnesium, aluminium, strong oxidizing agents.\n\nToxicology\nThis material causes cancer in laboratory animals, and is IARC listed as a probable human carcinogen. Inhalation and ingestion are harmful and may be fatal. May cause reproductive damage.  Irritant. Exposure to alcohol may increase toxic effects. Prolonged or repeated skin contact may cause dermatitis. Typical TLV 50 ppm.\n***********************************************\nhttp://ptcl.chem.ox.ac.uk/MSDS/CH/chloroform.html\n\nFurther, approximately 10% of the population is seriously allergic to chloroform. \n\nThe reaction you are proposing is strongly exothermic and is likely to cause the  chloroform to evaporate before the reaction even finishes. This of course will endanger you if you are present and do not have proper ventilation and safety equipment.  Phosgene can also be produced if the reaction proceeds too quickly and this can be fatal. This is NOT a reaction you would want to experiment with outside of a good laboratory with ventilation hoods, fire equipment, etc. \n\nDepending on what other chemicals you may have around, and what else you are doing, it could also get you ARRESTED simply for having the chloroform. The US Drug Enforcement Agency considers this a dangerous drug, for good reason.
838918
Its a decomposition equation. In essence Sodium Chloride (salt) breaks down into the Sodium ion and the Chlorine Ion. Chances are it's talking about NaCl when it's an aqueous solution (a solution who's solvent is water)
561048
Some oxide of chlorine. No idea about which one would be stable at those conditions, though.
949292
NaCl - sodium chloride
235031
those ans r right but I just want add whats not listed.\n\n4 the 2nd ans for explosion just ad pure Rb(37),Cs 55, or Fr 87 (in their pure metal alloy form) mix it with water. then BOOM. Cs and Fr is extremely reactive with H20\nso biggest bang will be Fr. \n\nthe reaction 2Fr(solid) + H20(gas or liquid) = Fr2O(oxide) + H2 (gas)\nthe reaction is very rapid, so it realeases a big ammount of H2 quickly in a very short time ( BOOM)\n\nanyway mixing H20 with NaCl do not create NaOH and HCl in their pure form. they only form ions of H+ and OH- and Cl- and Na+ these things moves arround in liquid, so u cant say that it is a stable NaOH and HCl
929369
I sure hope you have more information than you're giving us.  Typically profs will narrow the choices to one example of each major class of organic compound.  If you have the whole universe of canidates to choose from, you will need a lot more than these simple test.\n\nTLC:  In one of your textbooks or handouts, you should have a short list of organic candidates vs their Rfs.  Assuming you are using silica gel or alumina plates, ethyl acetate is about twice a strong a chromatographic mobile phase as dichloromethane (DCM) (see linked pdf, p. 15).  The fact that your unknown moved at all in ethyl acetate but hardly at all with DCM lets you know that your compound is fairly polar.  This is not an alkane or a fatty acid/ester.\n\nSolubility:  Not soluble in water?  It's not a saccharide, short-chain acid, alcohol or phenol.  Not soluble in base means it's definitely not a carboxylic acid or a phenol.  Soluble in acetone means it's not a fat or long-chain fatty acid.\n\nSo, what are we left with?  Ethers, ketones, esters and aldehydes.  I suggest you look in the chromatographic tables you have for one of these compounds that has the same Rf values and melting point you've quoted us.\n\nGood luck.
13266
There's a lot of something very much like glycerine! It's soapy, and if you get it in the carpet, it makes suds forever!\n\nOf course, I'm just guessing about that. Just don't DROP it!\n\n(and I wouldn't drink it either...no matter how much you might want to...)
140226
ethanol and oil\nwater and chloroform
327225
The elements Chlorine and Nitrogen are found in their natural, elemental forms of Chlorine gas (Cl2) and Nitrogen gas (N2) in nature, not as atomic Chlorine or atomic Nitrogen.\n \nNitrogen gas makes up the majority of Earth's atmosphere (AKA "air").\n\nChlorine gas is faily easy to produce with electrochemical reactions, or even through standard (non electrolytic) reactions.\n\n\nClorox does NOT contain Chlorine gas.  Amongst other things, the active ingredient in clorox bleach is Sodium Hypochlorite (NaOCl), not "Chlorine".
1088379
For over 50 years, chlorofluorocarbons (CFCs) were thought of as miracle substances. They are stable, nonflammable, low in toxicity, and inexpensive to produce. Over time, CFCs found uses as refrigerants, solvents, foam blowing agents, and in other smaller applications. Other chlorine-containing compounds include methyl chloroform, a solvent, and carbon tetrachloride, an industrial chemical. Halons, extremely effective fire extinguishing agents, and methyl bromide, an effective produce and soil fumigant, contain bromine. All of these compounds have atmospheric lifetimes long enough to allow them to be transported by winds into the stratosphere. Because they release chlorine or bromine when they break down, they damage the protective ozone layer. The discussion of the ozone depletion process below focuses on CFCs, but the basic concepts apply to all of the ozone-depleting substances (ODS). \n\nIn the early 1970s, researchers began to investigate the effects of various chemicals on the ozone layer, particularly CFCs, which contain chlorine. They also examined the potential impacts of other chlorine sources. Chlorine from swimming pools, industrial plants, sea salt, and volcanoes does not reach the stratosphere. Chlorine compounds from these sources readily combine with water and repeated measurements show that they rain out of the troposphere very quickly. In contrast, CFCs are very stable and do not dissolve in rain. Thus, there are no natural processes that remove the CFCs from the lower atmosphere. Over time, winds drive the CFCs into the stratosphere. \n\nThe CFCs are so stable that only exposure to strong UV radiation breaks them down. When that happens, the CFC molecule releases atomic chlorine. One chlorine atom can destroy over 100,000 ozone molecules. The net effect is to destroy ozone faster than it is naturally created. To return to the analogy comparing ozone levels to a stream's depth, CFCs act as a siphon, removing water faster than normal and reducing the depth of the stream. \n\nLarge fires and certain types of marine life produce one stable form of chlorine that does reach the stratosphere. However, numerous experiments have shown that CFCs and other widely-used chemicals produce roughly 84% of the chlorine in the stratosphere, while natural sources contribute only 16%. \n\nLarge volcanic eruptions can have an indirect effect on ozone levels. Although Mt. Pinatubo's 1991 eruption did not increase stratospheric chlorine concentrations, it did produce large amounts of tiny particles called aerosols (different from consumer products also known as aerosols). These aerosols increase chlorine's effectiveness at destroying ozone. The aerosols only increased depletion because of the presence of CFC - based chlorine. In effect, the aerosols increased the efficiency of the CFC siphon, lowering ozone levels even more than would have otherwise occurred. Unlike long-term ozone depletion, however, this effect is short-lived. The aerosols from Mt. Pinatubo have already disappeared, but satellite, ground-based, and balloon data still show ozone depletion occurring closer to the historic trend. \n\nOne example of ozone depletion is the annual ozone "hole" over Antarctica that has occurred during the Antarctic Spring since the early 1980s. Rather than being a literal hole through the layer, the ozone hole is a large area of the stratosphere with extremely low amounts of ozone. Ozone levels fall by over 60% during the worst years. \n\nIn addition, research has shown that ozone depletion occurs over the latitudes that include North America, Europe, Asia, and much of Africa, Australia, and South America. Over the U.S., ozone levels have fallen 5-10%, depending on the season. Thus, ozone depletion is a global issue and not just a problem at the South Pole. \n\nReductions in ozone levels will lead to higher levels of UVB reaching the Earth's surface. The sun's output of UVB does not change; rather, less o
735542
This a  difficult question to answer since the solubilty of these three liquids changes with changing temperature.  Water and acetic acid and miscible at all tempertures and chloroform and acetic acid are miscible at all tempertatures.  However, water and chloroform are only partially soluble in each other and their solubilty changes with changing temperatures.  \n\nPlease also refer to the reference that I have indicated below.  It discussed a point in the ternary system diagram called the Plait Point.  It is an example of a critical point, where the composition of the two phases is equal. At this point, the relative volumes of the two phases are equal and the boundary vanishes as the system becomes homogeneous.\n\nPlease refer to this document for more answers, sorry I could not have been more help.
1056970
some basic experiments in chem r making of common salt ,mixing hcl with various chemicals 2 produce gases
835846
probably ether or chloroform
132557
Acetone is a polar molecule (i.e. the centers of positive and negative charges in its molecule do not exactly coincide). It infact is more polar than the water molecule (2.91 D > 1.85 D). Due to this (and of course other reasons I donot know) acetone has a very good solvent action and finds use in industry primarily as a solvent - including its use as a nail polish (which contains nitrocellulose; acetone probably breaks this down) remover.
650250
Styrofoam is made of (drumroll, please) polystyrene. For about as much information as you could possibly want on polystyrene, check out the Polystyrene Packaging Council. There, you'll find general facts, production information, tips on recycling, and articles trumpeting polystyrene's low impact on the environment. \n\nPolystyrene Packaging Council:\nhttp://www.polystyrene.org/\n\n\nStyrofoam ® is a  Dow Chemical Co. trademarked form of  polystyrene foam insulation, introduced in the U.S. in 1954. Styrofoam® is a trademarked name, the real name of the product is foamed polystyrene. \n\nRay McIntire invented Styrofoam for the Dow Chemical Co.. McIntire said his invention of foamed polystyrene was accidental. His invention came as he was trying to find a flexible electrical insulator around the time of World War II. Polystyrene, which already had been invented, was a good insulator but too brittle. McIntire tried to make a new rubber-like polymer by combining styrene with isobutylene, a volatile liquid, under pressure. The result was a foam polystyrene with bubble, 30 times lighter than regular polystyrene. source The Detroit News \n\nhttp://inventors.about.com/library/inventors/blpolystyrene.htm
317693
why....are you trying to take over the world with chloroform by making everyone unconcious?  well dont think that will work!
892054
Is Hydrorogen chloride a solid? I've only ever thought of it as Hydrochloric Acid (get it out of a bottle!) which, of course, liberates See-oh-2 from See-ay-2-see-oh-3.\n\nPS. I asked about the solid 'cos on a practical level be careful of Toluene - it's nasty stuff. It's not used to make HCl, but I can't remember how you do make it. Sorry.