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Structure of sodium nitroprusside in the solid state, obtained by neutron diffraction Space filling model of sodium nitroprusside Nitroprusside is an inorganic compound with the chemical formula Na 2 [Fe(CN) 5 NO], usually encountered as the dihydrate , Na 2 [Fe(CN) 5 NO]·2H 2 O. [ 47 ] This red-colored sodium salt dissolves in water or ...
Nitrosation is typically performed with nitrous acid, formed from acidification of a sodium nitrite solution. Nitrous acid is unstable, and high yields require a rapid reaction rate. NO + synthon transfer is catalyzed by a strong nucleophile, such as (in order of increasing efficacy) chloride, bromide, thiocyanate, or thiourea.
The anion in this species has the formula [Fe 4 (NO) 7 S 3] −. It has C 3v symmetry. It consists of a tetrahedron of iron atoms with sulfide ions on three faces of the tetrahedron. Three iron atoms are bonded to two nitrosyl groups. The iron atom on the threefold symmetry axis has a single nitrosyl group which also lies on that axis.
A solution of 2% sodium carbonate in water (solution B) [4] Separate storage of the aldehyde and base are necessary to prevent aldol polymerisation of the aldehyde. When exposed to an amine, reaction with acetaldehyde produces the enamine , which subsequently reacts with sodium nitroprusside to the imine .
The reagent used can be any substance that gives S 2− ions in such solutions; most commonly used are hydrogen sulfide (at 0.2-0.3 M), thioacetamide (at 0.3-0.6 M), addition of hydrogen sulfide can often prove to be a lumbersome process and therefore sodium sulfide can also serve the purpose. The test with the sulfide ion must be conducted in ...
Nitromethane can be produced in the laboratory by treating sodium chloroacetate with sodium nitrite. [7] Oxidation of oximes [8] or primary amines. [9] Reduction of β-nitro alcohols [10] or nitroalkenes. [11] By decarboxylation of α-nitro carboxylic acids formed from nitriles and ethyl nitrate. [12] [13]
The combination of drinking lots of water while taking in a high amount of fiber could lead to unpleasant side effects, like bloating, gas, and constipation, according to the Cleveland Clinic.
In the laboratory, sodium nitrite can be used to destroy excess sodium azide. [86] [87] 2 NaN 3 + 2 NaNO 2 + 4 H + → 3 N 2 + 2 NO + 4 Na + + 2 H 2 O. Above 330 °C sodium nitrite decomposes (in air) to sodium oxide, nitric oxide and nitrogen dioxide. [88] 2 NaNO 2 → Na 2 O + NO + NO 2. Sodium nitrite can also be used in the production of ...