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Experiments for 'Cl'
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Results for 'Cl':
EXPERIMENT 1 --------------- Cobalt (II) ions build pink aqua complexes are intense blue chloro complexes. Heat favors the chloro complex.
EXPERIMENT 2 --------------- Ferric ions form a colorless complex with phosphate ions in acidic environments. In the presence of chloride ions, a yellow coordination complex is formed, which can exist, even in the presence of phosphate.
EXPERIMENT 3 --------------- When solid potassium permanganate is added to concentrated hydrochloric acid, then a gas is evolved, being chlorine. The liquid becomes almost black. When the reaction is driven to an end by heating (almost boiling) the liquid, then the final liquid does not become colorless, but green. The green color is not a bright green, but it is brownish/sepia-like. What is the constitution of this green/sepia compound? A similar observation is done when hydrochloric acid is heated with manganese dioxide. In the cold there is no visible reaction, but when heated, chlorine is produced and a green compound is formed.
EXPERIMENT 4 --------------- Thionyl chloride quickly hydrolyses in the presence of water.
EXPERIMENT 5 --------------- Acetone and chloroform react with each other in strongly alkaline environments, building a compound, called chloretone or chlorbutol. Formal name of the compound is 1,1,1-trichloro 2-methyl 2-propanol, formula CCl3 C(CH3)(OH) CH3. A similar reaction is observed, when MEK is used instead of acetone, but the reaction is much less vigorous.
EXPERIMENT 6 --------------- Trichloro ethene reacts with acetone, forming a brown substance, but only when in a strongly alkaline environment. The exact conditions, under which this brown substance is formed must be further investigated.
EXPERIMENT 7 --------------- Silver (I) forms a precipitate with bromates, while it does not do so with chlorates.
EXPERIMENT 8 --------------- When copper dissolves in aqua regia, then a colorless gas is produced. Oxidation apparently proceeds in a different way, when compared with dissolving copper in nitric acid.
EXPERIMENT 9 --------------- Copper (II) chloride reacts violently with metallic aluminium. When copper sulfate or nitrate is used, then this reaction does not occur. When sodium chloride is used, this reaction also does not occur. Both cupric ions and chloride ions are needed for quick reaction with aluminium, but if they are present, then a very violent reaction occurs.
EXPERIMENT 10 --------------- Cupric chloride forms a coordination complex when a large excess of chloride is present and this chloro cuprate complex easily oxidizes metallic copper. This oxidation causes formation of copper (I), which forms a very dark brown complex in the presence of copper (II) and hydrochloric acid (what is this dark brown compound?).
EXPERIMENT 11 --------------- Cupric chloride dihydrate dissolves in acetone. The solution becomes yellow at low concentrations, green/brown at higher concentrations. When sulphuric acid is added, then a precipitate of anhydrous cupric chloride is formed.
EXPERIMENT 12 --------------- Copper (II) chloride dissolves in fairly concentrated nitric acid, but it does not dissolve easily. Only a small amount can be dissolved. It dissolves with a bright green/cyan color. Aluminum metal is not attacked by this solution. Slight dilution does not make the liquid more active towards aluminum. When a lot of sodium chloride is added, then the aluminum is attacked and it dissolves.
EXPERIMENT 13 --------------- Nitrite forms a dark green coordination complex with copper (II) ions in neutral environments. When acidified, then a new coordination complex (dark blue with a grey hue) is formed in the presence of chloride of very high concentration. This is not formed when chloride is absent.
EXPERIMENT 14 --------------- Copper (II) forms a yellow/brown coordination complex with cyanide in acidic media in the presence of chloride.
EXPERIMENT 15 --------------- Copper (I) oxide, when added to sulphuric acid, disproportionates. Metallic copper is formed and a blue solution of copper (II) sulfate. The copper (I) oxide looses its oxide ion to the acid and that would leave aqueous copper (I) ions. These are not stable and disproportionate at once.
Copper (I) oxide, added to hydrochloric acid dissolves and forms a solution, containing a copper (I) complex, [CuCl2]-. This complex is very easily oxidized by oxygen from the air and then a dark brown mixed valency complex of copper (I) and copper (II) is formed.
EXPERIMENT 16 --------------- Copper(I) iodide dissolves in a concentrated solution of potassium iodide. In such a solution the complex ion CuI2(-) is formed. On dilution, this ion decomposes and a precipitate of CuI is formed again.
Copper(I) iodide does not dissolve in hydrochloric acid, or just a small amount dissolves.
EXPERIMENT 17 --------------- Praseodymium chloride dissolves in water very well and very easily, but it hydrolyses. A solution of this is turbid. When the solution is slightly acidified, then a very pale green and clear solution is obtained. Praseodymium chloride only dissolves slowly in concentrated hydrochloric acid. The solution also has another color than a plain slightly acidified solution. The solution in concentrated hydrochloric acid is yellow and its color is much more intense than the pale green color of aqueous praseodymium ions.
EXPERIMENT 18 --------------- Praseodymium (III) ions form complexes with chloride, bromide and iodide. With fluoride a precipitate is formed.
EXPERIMENT 19 --------------- Vanadyl ions apparently do not form a coordination complex with chloride at extremely high concentration, or the coordination complex has the same color as the vanadyl-aqua complex.
EXPERIMENT 20 --------------- Bleach is capable of oxidizing chromium (III) to its hexavalent state, but this is not accomplished easily and completely.
EXPERIMENT 21 --------------- Potassium chlorate is able to liberate bromine from a bromide. Reaction with sodium sulfide of the bromine shows formation of fumes/smoke.
EXPERIMENT 22 --------------- Potassium chlorate only reacts slowly with iodide at room temperature. When heated, the reaction proceeds much faster. Probably KClO3 oxidizes iodine further, until iodate is formed.
EXPERIMENT 23 --------------- It is possible to make an aqueous solution of bromine, which is so saturated, that the bromine separates from the liquid. In order to do so, a chemical reaction, producing large quantities of bromine must be performed.
EXPERIMENT 24 --------------- Sodium chloride reacts with sulfuric acid to give hydrogen chloride gas. Sodium bromide shows a similar reaction, producing hydrogen bromide, but in a side reaction some bromine is formed.
EXPERIMENT 25 --------------- When potassium chlorate and concentrated sulphuric acid are mixed, a very dangerous and strong oxidizer is created, which reacts explosively with organic matter.
EXPERIMENT 26 --------------- Bromide is oxidized by sulphuric acid, even when diluted with water. Bromine precipitates from water, when it is created in high concentrations.
EXPERIMENT 27 --------------- Chlorine reacts with acetylene gas (C2H2), without the need to ignite it.
EXPERIMENT 28 --------------- Sodium chlorate reacts with chloride in acidic environment, forming chlorine (which can be detected by means of its odour) and a fairly intensely colored yellow gas (chlorine dioxide). The color of this gas is much more intense than the color of chlorine. The yellow compound is destroyed by sulfite and nitrite.
EXPERIMENT 29 --------------- Potassium bromate reacts vigorously with concentrated hydrochloric acid. A green gas is evolved, but this gas has a color, which is fairly intense. The green gas consists of chlorine, but it also contains bromine, probably combined with chlorine in a compound as BrCl, which is slightly darker green than Cl2.
EXPERIMENT 30 --------------- Although the redox potential from bromate to bromine is higher than the potential from perchlorate to chlorate, when chlorate and bromate are mixed, then no reaction occurs. When some hydrochloric acid is added, then a reaction occurs with the chloride ions.
EXPERIMENT 31 --------------- Chlorate and bromate react with hydrochloric acid, but bromate reacts more vigorously. There also is a marked difference between potassium and sodium chlorate. The sodium salt reacts more vigorous with hydrochloric acid, but not as vigorous as potassium bromate. Reactions of bromate are faster than reactions of chlorate, but for sodium and potassium chlorate, the difference can be explained by the speed at which the salt dissolves.
EXPERIMENT 32 --------------- A mixture of chlorine and chlorine dioxide oxidizes bromide quickly to bromine. When an excess amount of nitrite is added, then the bromine is quickly reduced again to bromide. Addition of an acid does not result in formation of bromine again.
EXPERIMENT 33 --------------- Bromates are more reactive than chlorates in dilute aqueous solutions.
EXPERIMENT 34 --------------- Bromate reacts with chlorides, releasing chlorine. Probably some bromine is produced as well or a bromine/chlorine compound is produced.
EXPERIMENT 35 --------------- Bromate oxidizes iodine to iodate, itself being converted to bromine. Chlorate does not oxidize bromine to bromate, itself being converted to chlorine (at least not quickly).
EXPERIMENT 36 --------------- Both iodate and periodate form the tetrachloroiodide ion in a strong solution of hydrochloric acid. A redox reaction occurs, where the iodine is reduced to its +3 oxidation state and chlorine is released.
EXPERIMENT 37 --------------- The tetrachloroiodide ion is not stable in water at high dilution. It tends to disproportionate to iodine, choride and iodate. With sulfite, it is reduced to iodine. With excess sulfite, it is reduced to iodide.
EXPERIMENT 38 --------------- Potassium tetrachloroiodide decomposes on heating. The residue, which remains behind is potassium chloride.
EXPERIMENT 39 --------------- Potassium chlorate and sulphur form a potentially explosive mixture, which is quite sensitive to shock.
EXPERIMENT 40 --------------- TCCA does not react with sulphuric acid, at least not visibly. Even when heated, no reaction seems to occur. On addition of some solid NaCl vigorous evolution of chlorine gas is observed.
EXPERIMENT 41 --------------- TCCA reacts with ammonia. With 5% ammonia the reaction already is very vigorous, producing copious amounts of white smoke. With 15% ammonia the reaction is VERY violent, almost explosive.
EXPERIMENT 42 --------------- Chlorite ion forms complexes with cobalt(II) and copper(II). It forms a precipitate with lead(II). The precipitate with lead(II) forms a highly energetic compound.
EXPERIMENT 43 --------------- Bismuth shows remarkable coordination chemistry with iodide and chloride. In the absence of chloride, a black precipitate of BiI3 is formed. In the presence of chloride, a deep yellow/orange compound is formed, but only if also iodide is present. So this compound must be a complex of bismuth, iodide and chloride.
EXPERIMENT 44 --------------- Bismuth (III) forms a deep-orange iodo-complex and a yellow iodo-chloro complex.
EXPERIMENT 45 --------------- Nickel in nickel (II) hydroxide is oxidized to a higher oxidation state by hypochlorites, but not by chlorates. The oxidation product is reduced by hydrogen peroxide and ammonia. Heating of the oxidation product makes it more resistant to reduction and to breakdown by acids.
EXPERIMENT 46 --------------- When p-aminophenol is oxidized by hypochlorous acid, then an other oxidation product is formed, compared to oxidation by e.g. persulfate, hydrogen peroxide etc. When oxidized by hypochlorous acid a yellow solid compound is formed, otherwise an intense indigo/purple compound is formed, which remains dissolved.
EXPERIMENT 47 --------------- Pyrogallol reacts with chlorine, forming an orange/red compound. When excess chlorine is used, this compound is further oxidized to an almost colorless compound.
EXPERIMENT 48 --------------- P-aminophenol, when oxidized, forms a deeply colored compound. The color of this compound is deep blue/purple, but the environment and the used oxidizer have some influence on the color of the liquid as a whole (other compounds may make the color less pure).
EXPERIMENT 49 --------------- Titanium slowly dissolves in concentrated hydrochloric acid, forming deep blue/violet titanium (III) ions. On addition of hydrogen peroxide these are oxidized to titanium (IV), which in turn forms a deep red coordination complex with hydrogen peroxide. The deep red coordination complex is only stable in acidic to neutral media. It also is easily reduced by nitrite. It is not affected strongly by persulfate. With fluoride, a light yellow compound is formed, but the formation of that may also be due to rise of pH.
EXPERIMENT 50 --------------- When nitric acid is mixed with hydrochloric acid, then so called aqua regia is obtained. This is a colorless liquid, which, however, is not very stable and which decomposes. What are the decomposition products?
EXPERIMENT 51 --------------- Nitrites react with concentrated hydrochloric acid, forming a brown/orange compound, which remains dissolved in the acid. When the acid is diluted with water, then this orange compound is destroyed (probably it hydrolyses, due to lower concentration).
EXPERIMENT 52 --------------- Acetyl chloride is capable of dehydrating copper(II) chloride, and it even is capable of replacing sulfate ion by chloride, itself being converted to acetyl sulfate.
EXPERIMENT 53 --------------- Niobium pentachloride reacts with acetic acid, giving a colorless fuming gas (most likely HCl) and a fuming liquid (most likely acetyl chloride).
EXPERIMENT 54 --------------- Magnesium perchlorate dissolves in acetone very well. The mix of acetone and magnesium perchlorate does burn like normal acetone. No spectacular reaction occurs when the solution is ignited.
EXPERIMENT 55 --------------- Acetyl chloride can be used to make several esters, but with some alcohols, the reaction is EXCEEDINGLY violent and some dilution is needed to make the experiment safe.
EXPERIMENT 56 --------------- Ferric chloride anhydrous easily melts and when it melts, it also nearly boils and a dark yellow/brown vapor is formed, which condenses to beautiful crystals in cooler areas.
A small part of the ferric chloride reacts either with oxygen from the air, or with water vapor in the air. Insoluble oxide-species are formed.
EXPERIMENT 57 --------------- Antimony trioxide dissolves in hydrochloric acid, giving a colorless solution. When hydrogen sulfide is passed through such a solution, then a small amount of a yellow precipitate is formed and the liquid becomes very pale yellow. On dilution, much more precipitate is formed and the surprisingly, the color shifts from pale yellow to orange. The orange solid must be hydrous Sb2S3.
EXPERIMENT 58 --------------- Antimony trioxide does not dissolve in concentrated nitric acid, not even when the liquid is heated to boiling. When some hydrochloric acid is added as well, then it quickly dissolves, producing a colorless gas as well. It is oxidized to the +5 oxidation state. When this solution is diluted, then a white precipitate is formed. This white precipitate must be hydrous Sb2O5. When a dilute solution of sodium sulfide is added to this still strongly acidic solution, then H2S bubbles out of solution, but also a lot of precipitate is formed, which has a beautiful bright orange/red color.
EXPERIMENT 59 --------------- A mix of potassium perchlorate and sulphur cannot easily be ignited. When just a tiny pinch of red phosphorus is mixed in, then the mix is ignited very easily and it burns very fast with a bright flash.
EXPERIMENT 60 --------------- Formation of hypochlorite esters is very easy. With many alcohols, it is possible to make hypochlorite esters. These esters are very unstable and easily explode or burn very fiercely when ignited. All experiments, described here are quite dangerous, use good protection of the eyes and keep test tubes wrapped in a thichk layer of towels. Do not scale up!
EXPERIMENT 61 --------------- Ascorbic acid and sodium chlorite react violently and the dry mix can even inflame.
EXPERIMENT 62 --------------- Potassium perchlorate is only marginally soluble in cold water, while being much more soluble in hot water. From perchloric acid solutions, one can easily precipitate KClO4, almost quantitatively. It is funny to see how a potassium salt precipitates so quickly and densely.
EXPERIMENT 63 --------------- When a solution of manganese(II)chloride in moderately concentrated hydrochloric acid is electrolysed, then at the anode a remarkable very dark compound is formed. The liquid remains clear, but it becomes very dark. This must be a compound of manganese in higher than +2 oxidation state.
When a similar experiment is performed with manganese(II)sulfate in a 20% solution of sulphuric acid, then a drk brown precipitate is formed at the anode.
EXPERIMENT 64 --------------- Tert-butanol is very easily converted to tert-butyl chloride. Simply adding tert-butanol to concentrated hydrochloric acid allows the formation of this compound.
EXPERIMENT 65 --------------- Formic acid acts as a reductor, while acetic acid does not do so. Formic acid, however, is not that easily reduced. Reduction requires elevated temperature and strong oxidizers.
EXPERIMENT 66 --------------- Iodoform reacts exothermically with chlorine, one of the reaction products being iodine. The other products must be substitution products, with iodine completely or partly replaced by chlorine.
When excess chlorine is used, then iodine monochloride and iodine trichloride are formed as well. These products react with iodoform as well, resulting in formation of iodine.
EXPERIMENT 67 --------------- Ethylene glycol does not easily form a hypochlorite ester like ethanol or other mono-alcohol.
EXPERIMENT 68 --------------- Triethylamine frequently is used in reactions, where thionyl chloride is used, in order to capture any HCl formed in the reaction. However, when the only reactive compounds are thionyl chloride and triethylamine, then these two compounds react by themselves, giving rise to formation of black material, which sticks to the glass and is difficult to remove.
EXPERIMENT 69 --------------- Niobium pentachloride does react with methanol, but not nearly as violently as phosphorus pentachloride.
EXPERIMENT 70 --------------- Titanium metal slowly dissolves in concentrated hydrochloric acid and then forms a very dark solution of a titanium/chloride complex. This solution is much darker than an aqueous solution of titanium(III) in which the ions are present as aqua complex. With thiocyanate an even more intensely colored complex is formed. This complex has the same color, but it is very dark.
EXPERIMENT 71 --------------- When phosphorus pentachloride is added to chromium trioxide, then a fairly vigorous reaction occurs and exchange of oxygen and chlorine atoms occurs. The two solids react with each other, forming liquid CrO2Cl2 and liquid POCl3.
EXPERIMENT 72 --------------- Chromium trioxide (CrO3) dissolves in concentrated hydrochloric acid, giving a dark brown liquid. When this liquid is heated, then some orange/brown chromyl chloride is formed, which can easily be observed as a vapor above the liquid. On further heating the hydrochloric acid is oxidized and the hexavalent chromium is converted to green trivalent chromium.
EXPERIMENT 73 --------------- Vanadium pentoxide does not dissolve in thionyl chloride, but when a small amount of water is added, then it reacts. Vanadium pentoxide dissolves in acetyl chloride, giving a dark red/brown solution.
EXPERIMENT 74 --------------- Hydrogen chloride does not dissolve very well in concentrated perchloric acid.
EXPERIMENT 75 --------------- Thionyl chloride and copper nitrate react with each other, giving gaseous products and solid anhydrous copper(II) chloride remains behind.
EXPERIMENT 76 --------------- Copper(II) can be reduced to the very peculiar compound CuH by hypophosphorous acid, but only under very specific conditions. The compound CuH is quite unstable and easily looses hydrogen. In the presence of chloride ions, no CuH is formed, but CuCl is formed instead.
EXPERIMENT 77 --------------- This is a spectacular experiment. A mix of sodium chlorite and red phosphorus can be ignited by bringing it in contact with hydrochloric acid.
EXPERIMENT 78 --------------- When trichloroisocyanuric acid and sodium nitrite are mixed then no reaction occurs. As soon as some water is added a fairly vigorous reaction starts. A brown gas mix is produced, and the material starts foaming. The gas inside the foam bubbles is colorless and only when bubbles pop, a brown gas is observed.
EXPERIMENT 79 --------------- Anhydrous magnesium perchlorate dissolves in acetone easily, giving a colorless solution. Some heat is produced when the magnesium perchlorate dissolves, but it is not much. The resulting solution does not conduct electricity. When just a few drops of water are added to the solution, then it becomes conducting.
EXPERIMENT 80 --------------- Anhydrous copper (II) chloride, when added to acetone, dissolves with a yellow/brown color. If more copper (II) chloride is added, than can be dissolved in acetone, then the remaining solid becomes red/brown, like iron rust. When the red/brown solid is added to water, then at once it becomes green and then it dissolves, just as normal copper (II) chloride. The dilute solution becomes light blue.
EXPERIMENT 81 --------------- Chlorite ion and chlorine dioxide are sluggish oxidizers when in aqueous solution, even in the presence of quite some acid. Bromide ion only is oxiduzed very slowly and only partially.
EXPERIMENT 82 --------------- The combination of acetyl and sulfate, either directly, or derived from other compounds reacts extremely energetically with water. It is remarkable that it is this specific combination of three entities which gives extremely violent reactions. This effect is demonstrated with different chemicals in different combinations.
EXPERIMENT 83 --------------- Hydrofluoric acid (48% by weight) dissolves potassium chlorate and potassium bromate much more easily than water. The bromate also slowly decomposes in a peculiar way, which is not observed in other acidic solutions (like sulphuric or nitric acids).
EXPERIMENT 84 --------------- Azide ion reacts with hypochlorite, giving a yellow compound, which is colorless in the gaseous state. This compound can easily be ignited and explodes with a really loud report, even when very small quantities are used.
EXPERIMENT 85 --------------- Methylene chloride is capable of extracting nitric acid from its aqueous solution.
EXPERIMENT 86 --------------- When sodium chlorite solution is acidified with acetic acid, then a brown solution is obtained, which on addition of more acetic acid becomes lighter and which on addition of hydrochloric acid becomes bright yellow.
EXPERIMENT 87 --------------- Sodium hypophosphite is remarkably flammable. A mix with potassium chlorate is dangerously explosive and can easily be ignited.
EXPERIMENT 88 --------------- Cesium forms a solid red/brown chloro complex of copper(II). This complex is very remarkable, due to its rust-like color, which is very uncommon for copper(II) salts.
EXPERIMENT 89 --------------- Magnesium and potassium tetrachloro iodide do not react when dry, but when a drop of water is added, then a violent reaction starts, with production of purple clouds of iodine.
EXPERIMENT 90 --------------- Chlorosulfonic acid is an extremely reactive compound. It reacts violently with many salts of oxoacids.
EXPERIMENT 91 --------------- When concentrated hydrochloric acid is added to solid NaClO2, then a lot of intense yellow ClO2 is produced, but normally the gas does not explode. When concentrated hydrochloric acid is added to a mix of solid NaClO2 and solid NaBrO3, then a yellow gas is produced and within a few seconds at most, the gas explodes, the explosion starting at/near the liquid surface.
EXPERIMENT 92 --------------- Silver chlorite is stable, but only light heating is required for its decomposition.
EXPERIMENT 93 --------------- Perchloric acid is very reluctant to reacting with many chemicals. This is different from what many sites are telling. Perchloric acid only is extremely reactive when it is anhydrous, the hydrous acid (60 ... 70%) is not that reactive.
EXPERIMENT 94 --------------- Chlorite ion and nitrite ion react with each other in acidic medium, giving off quite some heat, while this does not occur with chlorate and nitrite.
EXPERIMENT 95 --------------- Hypochlorite ion forms esters very easily with alcohols. The esters simply are formed from aqueous solutions. The methyl ester is a colorless gas, which gives extremely powerful explosions when ignited. The ethyl ester is a very volatile yellow/green oil, which burns with a WHOOSH sound and which is quite unstable (it easily decomposes). The t-butyl ester is quite stable and can be kept around for a somewhat longer time. This burns quickly with a sooty flame.
EXPERIMENT 96 --------------- When compounds of manganese(IV) or manganese(VII) are added to hydrochloric acid, then chlorine gas is produced and the solution becomes very dark brown/green. Only after a long time of heating, all dark brown/green material is gone and what remains is a pale solution, containing manganese(II) ions.
In this series of experiments it was attempted to go the other way around. Is it possible to go from almost colorless manganese(II) to the dark colored compounds of manganese(III) or manganese(IV). This was done by adding chlorine to solutions of manganese(II) salts in concentrated hydrochloric acid.
While doing so, an interesting observation was made. The dark colored compound indeed can be made from manganese(II) in concentrated hydrochloric acid, but only from hypochlorite and not from chlorine.
When calciumhypochlorite is added to hydrochloric acid, then chlorine is formed vigorously, and the solution becomes green and clear.
It seems, however, that even in concentrated hydrochloric acid some of the hypochlorite is not decomposed at once, but remains in solution as yellow/green hypochlorous acid.
A freshly prepared solution, made from a pinch of calcium hypochlorite and concentrated hydrochloric acid, reacts differently than a saturated solution of chlorine in concentrated hydrochloric acid. This is shown with manganese(II) ions in hydrochloric acid.
EXPERIMENT 97 --------------- Lead(II) ion and chlorite ion produce a pale yellow precipitate. This solid, when dried, explodes when heated in a test tube, it deflagrates when heated in an open flame.
EXPERIMENT 98 --------------- Sodium chlorite and sodium nitrite do not react with each other in neutral solution, but when acid is added, they react extremely violently, possibly explosively.
End of results for 'Cl'
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