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Experiments for 'sodium sulfite'
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Results for 'sodium sulfite':
EXPERIMENT 1 --------------- Vanadium pentoxide hardly dissolves in water. In acid it dissolves slightly better, but even then its solubility is small.
EXPERIMENT 2 --------------- Vanadium pentoxide can be easily dissolved in acid, when a reductor is present. Then it is dissolved and at the same time reduced to vanadyl (vanadium (V) to vanadium (IV)). With very strong reducing compounds, further reduction to vanadium (III) or even vanadium (II) is possible.
EXPERIMENT 3 --------------- Hydrogen peroxide builds complexes with vanadium (IV) and vanadium (V) species. These compounds are not stable and result in dissociation of the complex and formation of vanadium (IV) compounds. The net result of adding hydrogen peroxide to a solution containing vanadium (V) can be reduction to vanadium (IV) with the formation of oxygen.
EXPERIMENT 4 --------------- The vanadyl salt of ferricyanide does not dissolve. The differences between the ferricyanide salt and ferrocyanide salts are not very clear. In alkaline solution apparently ferricyanide and vanadate (IV) can coexist.
EXPERIMENT 5 --------------- Vanadium (V) compounds can coexist with ferricyanide in solution. Reduction of either one of them results in formation of a precipitate.
EXPERIMENT 6 --------------- The result of this experiment is remarkable. Hydroxyl amine, being a strong reductor, appears to oxidize vanadium (IV) to vanadium (V) in alkaline environments. Or is there another compound, which strongly resembles the well-known yellow colour of vanadium (V) in acidic environments and the (almost) colourless appearance of vanadium (V) in alkaline environments?
EXPERIMENT 7 --------------- Vanadyl is oxidized by bromate quickly and completely.
EXPERIMENT 8 --------------- Vanadium (V) is capable of forming many peroxo compounds, whose appearance strongly depends on pH.
EXPERIMENT 9 --------------- 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 10 --------------- Copper (II) reacts with thiocyanate in a complex way.
EXPERIMENT 11 --------------- Hydroquinone is capable of reducing copper (II) to copper (I) in alkaline environments. The copper is not reduced to its metallic form.
EXPERIMENT 12 --------------- Metol is capable of reducing copper (II) to copper (I) in alkaline environments.
EXPERIMENT 13 --------------- Copper builds higher oxides than CuO when strong oxidizing agents are present in alkaline environments. Probably these are not copper (III) compounds, but the oxo-ion probably is replaced by peroxo or superoxo.
EXPERIMENT 14 --------------- 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 15 --------------- Copper (II) salts give a cyan precipitate with bicarbonates. The color of this precipitate is the same as the color of commercially available basic copper carbonate. This precipitate reacts with hydrogen peroxide, forming a dark green/brown compound. With sulfite it also reacts, forming a brownish compound, which on acidification dissolves, forming a light yellow/brown clear liquid.
EXPERIMENT 16 --------------- This is a very nice experiment, involving beautifully coloured compounds, but it is a hazardous experiment as well, due to the use of mercury (II) compounds. Mercury (II) builds a complex with excess iodide, [HgI4]2-, which gives a beautiful bright yellow precipitate with Ag+ and a beautiful bright brick- red precipitate with Cu+.
EXPERIMENT 17 --------------- Platinum (II) can be oxidized to platinum (IV) by strong oxidizing agents. Reduction to metallic platinum cannot be achieved by sulfite nor by stannous chloride.
EXPERIMENT 18 --------------- Platinum (II) gives a highly coloured compound with tin (II), it is not reduced to metallic platinum.
EXPERIMENT 19 --------------- The hexanitrito cobaltate (III) ion can be reduced by SO2 to cobalt (II), but this reduction requires heating. Some brown compound remains, this probably is due to the inertness of many cobalt (III) coordination complexes. With nitrite, a brown complex is formed again. This differs from the gold/yellow hexanitrito cobaltate (III).
EXPERIMENT 20 --------------- Iodide ion and sulphur dioxide form a deep orange/yellow complex at high concentration. At somewhat lower concentration this complex looks deep yellow. The complex formed in this experiment is {I.nSO2]-.
EXPERIMENT 21 --------------- Molybdates and phosphates produce a yellow complex in an anion, containing both molybdenum and phosphorus. This complex is slowly reduced by sulfite.
EXPERIMENT 22 --------------- Molybdate gives rise to all kinds of complexes, when combined with reducing agents. These complexes can be yellow, green or blue. The composition of all these complexes is not very clear.
EXPERIMENT 23 --------------- Molybdenum trioxide dissolves well in strongly alkaline liquids. It does not dissolve (or just a little bit) in plain water. Once dissolved, it can be kept in solution, even when pH is lowered. Molybdates are capable of oxidizing iodide and sulfite.
EXPERIMENT 24 --------------- Hydroquinone is a very strong reductor in alkaline environments. Oxygen from the air is readily absorbed by an alkaline solution of hydroquinone. Sulfite, however, makes an alkaline solution of hydroquinone much more stable, because of formation of special hydroquinone/sulfite compounds.
EXPERIMENT 25 --------------- Hydroquinone is readily oxidized by ferricyanide, even in the presence of sulfite, when in alkaline environments.
EXPERIMENT 26 --------------- Metol is easily oxidized by oxygen from the air, when dissolved in alkaline media. When sulfite is present, however, oxidation does only occur at a low rate.
EXPERIMENT 27 --------------- Silver (I) is reduced to metallic silver by metol. This metallic silver is easily oxidized by peroxosulfate. Insoluble silver (I) compounds dissolve in thiosulfate solutions (principle of photography fixer) while metallic silver is not affected. When a mild oxidizer is added, the metallic silver also dissolves (principle of photography reducer, Farmer's reducer).
EXPERIMENT 28 --------------- Pyrogallol gives rise to many colored products on oxidation and coordination. More investigation is needed in order to get more insight in all these colors and the conditions under which they are formed.
EXPERIMENT 29 --------------- When p-aminophenol is oxidized in an acidic environment, then a compound is formed, with a deep indigo/purple color.
EXPERIMENT 30 --------------- 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 31 --------------- Bromate is reduced by sulfite quickly in acidic environments. When an excess amount of bromate is used, then bromine is formed. When an excess amount of sulfite is used, then the bromine is reduced further to bromide.
EXPERIMENT 32 --------------- 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 33 --------------- 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 34 --------------- A large set of compounds is checked on interaction with concentrated nitric acid. Many reductors react violently with nitric acid.
EXPERIMENT 35 --------------- Nitric acid, mixed with sulphuric acid is a strong oxidizer. It is capable of oxidizing iodine to iodate.
EXPERIMENT 36 --------------- Selenium dissolves in a sulfide solution, forming a deep red/brown solution. Hydrogen peroxide is capable of oxidizing this solution.
EXPERIMENT 37 --------------- Rhenium is oxidized easily by nitric acid. The oxidation product is a color- less compound, soluble in water (according to literature it is perrhenic acid, HReO4). Perrhenic acid is not a really strong oxidizer. It can be reduced by zinc, but addition of sodium sulfite does not result in formation of the same compound. Hydrogen peroxide is capable of oxidizing back to perrhenic acid, but some light yellow compound remains. What is it?
EXPERIMENT 38 --------------- Rhenium can be oxidized to colorless perrhenate [ReO4]-, with nitric acid. With zinc it can be reduced to a yellow/green species in the presence of hydrochloric acid at sufficient concentration. This species apparently is not reduced any further with borohydride in alkaline environments. In acidic environments, a dark brown/black compound can be formed easily, due to reduction of thiosulfate to sulfide by the borohydride. The sulfide forms a dark compound with rhenium. With sulfite, perrhenate nor the yellow/green compound can be reduced to a lower oxidation state.
EXPERIMENT 39 --------------- Chromium (III) has many different colors, depending on coordinated ligands.
EXPERIMENT 40 --------------- Chromium (III) has many different colors, depending on coordinated ligands.
EXPERIMENT 41 --------------- Chromium (III) can have many different colors, depending on how it is created and with which it coordinates.
EXPERIMENT 42 --------------- 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 43 --------------- When chromium (III) is created by reduction from dichromate with acidified sulfite, then a green ion is formed. When acidified sulfite is added to violet chromium (III), then the ions remain violet. Apparently the way of creating chromium (III) determines its color (and hence to what it is coordinated).
EXPERIMENT 44 --------------- When chromium (III) is created from dichromate, its color depends on the reductor used and on the acid which is used for supporting the redox reaction.
EXPERIMENT 45 --------------- 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 46 --------------- Chromium (III) builds a purple complex with EDTA, both when it is created from dichromate and when it already exists and is brought in contact with EDTA. When the pH is too low (or is this due to formation of a complex with sulfate?), the formation of the complex does not occur.
EXPERIMENT 47 --------------- Chromium (III) gives coordination complexes of all kinds of colours, when formed from a redox reaction, starting with dichromate.
EXPERIMENT 48 --------------- Bisulfite and sulfite form coordination complexes with chromium (III). The exact behaviour strongly depends on the pH of the solution. When the pH is raised with sulfite and then decreased again with sulphuric acid, then the color does not revert to the original color of aqueous chromium (III). Probably a new compound is found, which is inert and does not fall apart quickly in acidic environments.
EXPERIMENT 49 --------------- Dichromate is reduced by sulfite in neutral/slightly alkaline enviromments. Under these conditions a jelly-like precipitate is formed, which is fairly stable and does not dissolve immediately in dilute sulphuric acid. This jelly-like precipitate is a chromium (III) compound. The compound, however, does dissolve easily in strongly alkaline liquids. The formation of this compound is not affected by the type of the cation in the chromium-compound.
EXPERIMENT 50 --------------- Persulfate is not capable of oxidizing manganese to the (VII) state in acidic environments.
EXPERIMENT 51 --------------- Manganese (II) ions apparently do not form coordination complexes with EDTA. If they do so, then the coordination complex is (almost) colorless.
EXPERIMENT 52 --------------- Permanganate is capable of oxidizing formic acid quickly, itself being reduced to manganese (IV). Sulfite is needed to bring the manganese to the +2 oxidation state.
EXPERIMENT 53 --------------- 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 54 --------------- Ferric ions form coordination complexes with citrates and oxalates. These coordination complex have completely different properties than free ferric ions.
EXPERIMENT 55 --------------- Ferric ions form a coordination complex with sulfite.
EXPERIMENT 56 --------------- Aluminium (III) does not form colored compounds with ferrocyanide nor with ferricyanide. Manganese (II) reacts with both of them, but a colored compound is formed with ferricyanide only.
EXPERIMENT 57 --------------- Although p-aminophenol and metol are similar compounds (metol is the sulfate salt of p-aminophenol with a H-atom at the amino-group replaced by a methyl group) they show fairly large differences as far as complex- formation is concerned with ferric compounds. Metol reacts more slowly and the color of the compounds differ.
EXPERIMENT 58 --------------- This experiment describes a qualitative method, useful for showing the presence of minute quantities of manganese (II), which cannot be detected by oxidation with H2O2 in alkaline environments anymore. Chloride ions may not be present besides the manganese to be detected.
EXPERIMENT 59 --------------- Sodium selenite dissolves in concentrated hydrobromic acid with a red/brown color. When this solution is shaken with ligroin, then the ligroin layer also turns red/brown. The compound, dissolved in the ligroin layer is a selenium compound, as is demonstrated by the experiment, described in more detail below.
EXPERIMENT 60 --------------- Copper(II) ion and sulfite ion react in aqueous solution. A dirty green/yellow precipitate is formed when solutions with these ions are mixed. When there is excess sulfite, then on slight heating the precipitate redissolves and the liquid becomes colorless.
Apparently a coordination complex is formed with copper(I). This coordination complex is very air-sensitive. It reacts with air, giving a dirty brown/green/yellow precipitate.
EXPERIMENT 61 --------------- Sodium sulfite reacts vigorously with 68% nitric acid.
EXPERIMENT 62 --------------- Iodoform is only moderately stable. On heating, it decomposes to iodine, carbon and hydrogen iodide. This process of decomposition looks quite special.
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 --------------- Dichromate ion oxidizes thiosulfate easily in acidic media, but in neutral media it only is oxidizing incompletely, and a solid compound is formed.
EXPERIMENT 65 --------------- Sodium sulfite is not capable of reducing CrO3, dissolved in acetyl chloride. As soon as water is added, the red color of the hexavalent chromium disappears and green/blue trivalent chromium is formed.
EXPERIMENT 66 --------------- Arsenic in oxidation state +5 is not easily reduced to elemental arsenic, except by tin(II) chloride.
EXPERIMENT 67 --------------- The hexanitritocobaltate (III) ion is quite stable, but at very low pH, it is destroyed either by reducing agents, or by coordinating agents. But the nitrito ligand is MUCH more stable than in the plain nitrite ion.
End of results for 'sodium sulfite'
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