|
Experiments for 'ammonia'
Below follows a summary of all experiments, matching your
search. Click one of the EXPERIMENT hyperlinks for a complete description of the
experiment.
Results for 'ammonia':
EXPERIMENT 1 --------------- Thiocyanate is oxidized by nitrate very violently under the right conditions.
EXPERIMENT 2 --------------- Vanadyl (vanadium (IV)) does not give a coordination complex with ammonia. It does not dissolve in ammonia. With stronger bases, a brown vanadate (IV) compound dissolves (a poly-vanadate (IV) compound??).
EXPERIMENT 3 --------------- Sulfide reacts with metavanadates, resulting in the formation of a dark brown/greenish compound.
EXPERIMENT 4 --------------- Vanadium pentoxide dissolves in ammonia and when heated a white solid is formed, probably this is ammonium meta vanadate.
EXPERIMENT 5 --------------- Vanadium pentoxide reacts with ammonia, producing a strong hissing noise. A white compound is created. This probably is ammonium metavanadate, NH4VO3.
EXPERIMENT 6 --------------- Vanadium in its +4 oxidation state forms a blue compound, vanadyl, in acidic environments. In near neutral to alkaline environments, the situation is less clear. Reduction of neutral or alkaline vanadium (V) compounds yields a dark and turbid liquid. Vanadium in its +5 oxidation state gives light yellow compounds in mildly alkaline environments. Al lowering the pH, the color becomes more intense, until a maximum is reached. When the pH is lowered even more, then lighter yellow compounds are formed again. Vanadium (IV) cannot coexist with hydrogen peroxide. In alkaline media it is oxidized to vanadium (V), which with excess peroxide gives a yellow peroxo complex. In acidic media, vanadium (IV) is oxidized to vanadium (V) which gives a deep brown/red peroxo complex with excess poroxide.
EXPERIMENT 7 --------------- Copper (II) reacts with thiocyanate in a complex way.
EXPERIMENT 8 --------------- Copper (II) reacts with thiocyanate in a complex way.
EXPERIMENT 9 --------------- Copper (II) reacts with ferrocyanide and builds a fairly stable compound.
EXPERIMENT 10 --------------- Vitamin C is a strong reductor in alkaline environments. Copper (II) is reduced to copper (I).
EXPERIMENT 11 --------------- Copper (I) iodide dissolves in dilute ammonia, resulting in a colorless liquid. Copper (I) builds a coordination complex with ammonia. This complex is oxidized by oxygen from the air exceedingly easily.
EXPERIMENT 12 --------------- Copper builds a complex with urea, which has a pale purple color (or is this due to contamination of the urea with traces of biuret?). The copper, bound to urea, does not build the intense blue cuprammine complex with ammonia.
EXPERIMENT 13 --------------- When tetraammine-copper (II) is reduced by dithionite in excess ammonia, then a colorless copper (I) complex is formed, which remains dissolved.
EXPERIMENT 14 --------------- Decomposition of hydrogen peroxide is catalyzed by cuprammine complex.
EXPERIMENT 15 --------------- In alkaline environments, copper (II) shows remarkable behavior, when brought in contact with strong oxidizers or reductors.
EXPERIMENT 16 --------------- Hydroxyl amine sulfate (containing protonated hydroxyl amine) is not capable of reducing copper (II). When the liquid becomes basic (releasing free hydroxyl amine), then the copper (II) is reduced to copper (I).
EXPERIMENT 17 --------------- Copper builds a remarkable complex with ascorbic acid and is easily reduced by ascorbic acid in alkaline environments. Copper (II) builds a brown compound with hydrogen peroxide in alkaline environments.
EXPERIMENT 18 --------------- Copper and nickel carbonates (basic), which do not dissolve in water, do dissolve in ammonia, due to formation of a complex with ammonia. Cobalt carbonate also dissolves, but now an additional reaction occurs, taking up oxygen from the air.
EXPERIMENT 19 --------------- Copper (II) is reduced by sulfite. With chloride the resulting copper (I) can be kept in solution. The copper (I) compound is very susceptible to oxidation by oxygen from the air.
EXPERIMENT 20 --------------- Copper (II) amine complex is reduced to a colorless copper (I) amine complex by hydroxyl amine. The copper (I) complex is oxidized by oxygen from the air very easily.
EXPERIMENT 21 --------------- When copper (II) is present in hydrochloric acid, then it does not react immediately with hydroxyl ammonium, some heating is required to have a reaction, resulting in formation of a dark green/brown compound. When the liquid is made alkaline with excess ammonia, then it quickly becomes colorless, due to reduction of copper (II) to copper (I), which forms a colorless complex with ammonia. A very peculiar reaction occurs on oxidation by oxygen from air. The liquid is covered by a very thin shiny layer, looking like a strongly coloured oil on water. It is not clear what it is, more research is needed.
EXPERIMENT 22 --------------- Copper (II) chloride is reduced by hydroxyl amine, when dissolved in ethanol. First, the solution becomes much darker and apparently, a mixed oxidation state complex of copper (I) and copper (II) is formed. Finally, all copper (II) is reduced to copper (I). This experiment is another example, which shows that copper (I) and copper (II), when in solution at the same time, form a highly colored complex.
EXPERIMENT 23 --------------- Mercury (II) salts give an oxide/hydroxide, which does not dissolve in large excess amounts of alkaline solutions. Ammonia does not dissolve the precipitate of mercury (II) oxide/hydroxide.
EXPERIMENT 24 --------------- 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 25 --------------- Cobalt (II) appears to react with ammonia, but only when an oxidizer is available. The resulting compound has an intense color.
EXPERIMENT 26 --------------- Cobalt (II) is stable in acidic environments, but in alkaline environments in the presence of ammonia it reacts with oxygen from the air, resulting in the formation of a dark red/brown coordination complex.
EXPERIMENT 27 --------------- Cobalt carbonate does not dissolve completely in dilute mineral acids. With some heating, however, it does dissolve completely. With nitrite a yellow/orange complex is formed, which forms a precipitate when treated with alkalies. The precipitate is resistant to treatment with acid and bases.
EXPERIMENT 28 --------------- Cobalt forms many complexes with ammonia and it forms these complexes easily, but when cobaltosic oxide (Co3O4, black oxide) is used, then no such reactions can be observed. Co3O4 appears to be very inert.
EXPERIMENT 29 --------------- Cobalt (II) salts give a blue/green precipitate when dilute ammonia is added. This precpitate is fairly stable towards air. When more concentrated ammonia is used, then a dark brown compound is formed, but this compound is formed by contact with air. On addition of hydrogen peroxide also a very dark brown compound is formed. When the pH is increased strongly, then the blue precipitate is not stable anymore, instead a dark bright blue compound is formed, which, however, quickly turns pink. When a large amount of ammonia is replaced by ammonium, then the blue precipitate is not formed anymore, but a coordination complex is formed, which is very easily oxidized by oxygen from the air.
EXPERIMENT 30 --------------- In this experiment, some of Werner's experiments are repeated. Here it is shown that cobalt forms beautifully colored carbonato complexes. The exact complex formed, depends on the experimental conditions. It is remarkable what kinds of reactions are shown by cobalt in its complexes and it is really difficult to precisely determine what is happening and it even is difficult already to get the same results without precisely specifying the exact experimental conditions (e.g. using HCl instead of H2SO4 already results in a different outcome).
EXPERIMENT 31 --------------- Diverse phenol-derivatives, can be oxidized easily by bromine, yielding intensely colored oxidation products.
EXPERIMENT 32 --------------- Ammonia reacts with iodine, giving nitrogen iodide, coordinated to ammonia. When acetone is present, however, then a so called haloform reaction occurs, resulting in formation of CHI3.
EXPERIMENT 33 --------------- 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 34 --------------- When bromate, manganese (II), citric acid and sulphuric acid are mixed at certain propertions, then an oscillating reaction occurs, finally resulting in an oily compound, which separates from the aqueous liquid.
EXPERIMENT 35 --------------- When Cr3+ is added to an aqueous solution of ammonia, then a precipitate is created, which does not dissolve on addition of much more ammonia.
EXPERIMENT 36 --------------- Chromium (III) does not quickly build a coordination complex with ammonia, such as is the case with copper (II) and nickel (II). Even in a slightly alkaline environment of dilute ammonia, chromium (III) can be oxidized to chromium (VI) by the action of hydrogen peroxide. Reduction, back to chromium (III) is not easily accomplished in alkaline environment.
EXPERIMENT 37 --------------- The color of chromium (III) depends on how it is part of coordination complexes.
EXPERIMENT 38 --------------- Chromium (III) apparently builds a coordination complex with hydroxyl amine, but this complex does not simply form from chromium (III) salts and hydroxyl amine. If chromium (III) is formed by means of reduction of chromium (VI) in the presence of hydroxyl amine, then the complex is formed. If hydroxyl amine is added to chromium (III) without redox reaction, then another complex is created.
EXPERIMENT 39 --------------- Hydroxyl amine gives a brown coordination complex when it reduces hexavalent chromium to trivalent chromium in alkaline environments. This coordination complex is really due to the hydroxyl amine. When other reducing agents are used in the presence of ammonia in alkaline environments, then no similar reaction product can be obtained.
EXPERIMENT 40 --------------- Aniline, combined with acidified dichromate gives intensely colored compounds.
EXPERIMENT 41 --------------- Aniline gives colored compounds with chromium. The colors are remarkably intense.
EXPERIMENT 42 --------------- When aqueous ammoniacal silver is reduced by glucose, a nice silver mirror is produced. Peroxosulfate is capable of oxidizing silver to a higher oxidation state (+2 or +3), even in acidic environments.
EXPERIMENT 43 --------------- Silver is coordinated by thiosulfate. The silver-thiosulfate complex does not show any of the reactions of free aqueous silver (I).
EXPERIMENT 44 --------------- Silver (I) is not reduced by hydroxyl amine in neutral environments. When made alkaline, it is reduced to metallic silver immediately.
EXPERIMENT 45 --------------- Silver (I) gives a white precipitate with thiocyanate, which does not dissolve in excess ammonia. Hydroxyl amine does not affect this precipitate.
EXPERIMENT 46 --------------- Silver (I) does not give a precipitate with hydroxyl amine sulfate (if concentrations are not too high), but ammonia causes formation of a precipitate, which does not dissolve in excess ammonia.
EXPERIMENT 47 --------------- This experiment is performed in order to determine, whether iodoform (CHI3) shows a reaction, similar to chloroform, when treated with acetone in a strongly alkaline environment. The result of this experiments suggests that indeed a similar reaction occurs, resulting in the formation of a compound with a sweetish mint-like odour.
EXPERIMENT 48 --------------- Tetraethyl ammonium ion does not form a sparingly soluble salt with bromate ion. The tetraethyl ammonium ion forms an oily compound, when treated with bromate and hydrochloric acid. The halogen, released in that reaction apparently forms a liquid organic, insoluble in water, or is a liquid ionic compound formed, some tetraethyl ammonium polyhalogenide compound??? There is evidence for the latter (see experiment detailed description).
EXPERIMENT 49 --------------- Iron (III) builds a coordination complex with phosphates.
EXPERIMENT 50 --------------- Ferrocyanide reacts with hydrogen peroxide, forming a fairly intensely colored yellow compound (probably ferricyanide), but this reaction was expected to make the liquid more alkaline, but this cannot be observed.
EXPERIMENT 51 --------------- Analysis of the composition of the dutch coin 'dubbeltje' shows that it does not contain any copper or just a very small quantity of it.
EXPERIMENT 52 --------------- Adding ammonia to a Ni2+ solution results in formation of a purple/blue coordination complex.
EXPERIMENT 53 --------------- 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 54 --------------- Dichromate/chromic acid is reduced by malic acid and in this reaction an intensely colored purple complex of chromium(III) is formed. If the reaction is performed in the presence of an excess amount of strong non-coordinating acid, then the reaction proceeds faster, and also a purple complex is formed, but the color is much less intense. Without the extra acid, there really is a new complex with chromium(III). This complex reacts with ammonia, giving a nice green solution.
EXPERIMENT 55 --------------- Hydrazine seems to be able to reduce copper(II) to copper(I) in mildly acidic environments. In alkaline environments the reaction is fast and most likely elemental copper is produced in the reaction.
EXPERIMENT 56 --------------- Ammonium iodate can very easily be prepared by adding a slight excess of ammonia to a solution of iodic acid in water. The dry compound is stable, but when it is heated, it violently decomposes, but it does not explode.
Ammonium periode can be prepared in a similar way. When ammonium periodate is heated, then it explodes, giving a cloud of iodine.
EXPERIMENT 57 --------------- Mercurous ions are stable in aqueous solution at room temperature. They do not hydrolyse, nor disproportionate. However, when a compound is added, with which a stable mercury(II) complex is formed, or with which a stable mercury(II) precipitate is formed, then the mercury(I) disproportionates to the metal and mercury(II).
EXPERIMENT 58 --------------- When antimony is added to liquid bromine, then a violent reaction occurs, even with appearance of sparks.
EXPERIMENT 59 --------------- Thallium(I) ion is fairly easily oxidized to thallium(III). In neutral aqueous solutions, this ion hydrolyzes to a dark hydrous oxide, which forms a compact precipitate. The dark oxide easily can be dissolved in nitric acid, such that a colorless solution of thallium(III) nitrate is formed in nitric acid.
Thallium(III) ion forms an ochre/yellow color with ferricyanide ion, which is stable at low pH, but at high pH this decomposes, giving a yellow solution of ferricyanide and a dark brown suspension of hydrous thallic oxide.
EXPERIMENT 60 --------------- Titanium(III) ions are fairly stable in acidic media, but in alkaline solution, these become so strongly reducing that hydrogen gas is formed and water is reduced!
End of results for 'ammonia'
|