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When conducted in warm water, Na 2 SO 3 initially precipitates as a white solid. With more SO 2, the solid dissolves to give the disulfite, which crystallizes upon cooling. [2] SO 2 + 2 NaOH → Na 2 SO 3 + H 2 O. Sodium sulfite is made industrially by treating sulfur dioxide with a solution of sodium carbonate. [3] The overall reaction is:
SO 2 + NaOH → NaHSO 3 SO 2 + NaHCO 3 → NaHSO 3 + CO 2. Attempts to crystallize the product yield sodium metabisulfite (also called sodium disulfite), Na 2 S 2 O 5. [6] Upon dissolution of the metabisulfite in water, bisulfite is regenerated: Na 2 S 2 O 5 + H 2 O → 2 Na + + 2 HSO 3 −. Sodium bisulfite is formed during the Wellman-Lord ...
Sodium metabisulfite can be prepared by treating a solution of sodium hydroxide with sulfur dioxide. [3] When conducted in warm water, Na 2 SO 3 initially precipitates as a yellow solid. With more SO 2, the solid dissolves to give the disulfite, which crystallises upon cooling. [4] SO 2 + 2 NaOH → Na 2 SO 3 + H 2 O SO 2 + Na 2 SO 3 → Na 2 S ...
C 6 H 6 + H 2 SO 4 → C 6 H 5 SO 3 H + H 2 O. Sulfur trioxide or its protonated derivative is the actual electrophile in this electrophilic aromatic substitution. To drive the equilibrium, dehydrating agents such as thionyl chloride can be added: [2] C 6 H 6 + H 2 SO 4 + SOCl 2 → C 6 H 5 SO 3 H + SO 2 + 2 HCl. Historically, mercurous sulfate ...
Solutions of bisulfite are typically prepared by treatment of sulfur dioxide with aqueous base: [3] SO 2 + OH − → HSO − 3. HSO − 3 is the conjugate base of sulfurous acid, (H 2 SO 3). HSO − 3 is a weak acidic species with a pK a of 6.97. Its conjugate base is sulfite, SO 2− 3: HSO − 3 ⇌ SO 2− 3 + H +
Sodium bisulfate, also known as sodium hydrogen sulfate, [a] is the sodium salt of the bisulfate anion, with the molecular formula NaHSO 4.Sodium bisulfate is an acid salt formed by partial neutralization of sulfuric acid by an equivalent of sodium base, typically in the form of either sodium hydroxide (lye) or sodium chloride (table salt).
For example, in ammonium chloride solution, NH + 4 is the main influence for acidic solution. It has greater K a value compared to that of water molecules; K a of NH + 4 is 5.6 × 10 −10, and K w of H 2 O is 1.0 × 10 −14. This ensures its deprotonation when reacting with water, and is responsible for the pH below 7 at room temperature.
Sodium aluminate is an inorganic chemical that is used as an effective source of aluminium hydroxide for many industrial and technical applications. Pure sodium aluminate is a white crystalline solid having a formula variously given as NaAlO 2, NaAl(OH) 4 (), [3] Na 2 O·Al 2 O 3, or Na 2 Al 2 O 4.