acetic acid sodium hydroxide equation

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From Wikipedia

Sodium acetate

Sodium acetate, NaOAc, also sodium ethanoate, is the sodiumsalt of acetic acid. This colourless salt has a wide range of uses.



Sodium acetate is used in the textile industry to neutralize sulfuric acid waste streams, and as a photoresist while using aniline dyes. It is also a pickling agent in chrome tanning, and it helps to retard vulcanization of chloroprene in synthetic rubber production.


Sodium acetate may be added to foods as a seasoning. It may be used in the form of sodium diacetate— a 1:1 complex of sodium acetate and acetic acid, given the E-numberE262. A frequent use of this form is in salt and vinegar chips in the United States. Many US brands, including national manufacturer Frito-Lay, sell "salt and vinegar flavoured" chips that use this chemical, with lactose and smaller percentages of other chemicals, in lieu of a real salt and vinegar preparation.

Buffer solution

As the conjugate base of a weak acid, a solution of sodium acetate and acetic acid can act as a buffer to keep a relatively constant pH. This is useful especially in biochemical applications where reactions are pH dependent.

Heating pad

Sodium acetate is also used in consumer heating pads or hand warmers and is also used in hot ice. Sodium acetate trihydrate crystals melt at 58°C, dissolving in their water of crystallization. When they are heated to around 100°C, and subsequently allowed to cool, the aqueous solution becomes supersaturated. This solution is capable of cooling to room temperature without forming crystals. By clicking on a metal disc in the heating pad, a nucleation centre is formed which causes the solution to crystallize into solid sodium acetate trihydrate again. The bond-forming process of crystallization is exothermic, hence heat is emitted. The latent heat of fusion is about 264–289 kJ/kg. Unlike some other types of heat packs that depend on irreversible chemical reactions, sodium acetate heat packs can be easily recharged by boiling until all crystals are dissolved; they can be reused indefinitely.


For laboratory use, sodium acetate is inexpensive, and is usually purchased instead of being synthesized. It is sometimes produced in a laboratory experiment by the reaction of acetic acid with sodium carbonate, sodium bicarbonate, or sodium hydroxide. These reactions produce aqueous sodium acetate and water. Carbon dioxide is produced in the reaction with sodium carbonate and bicarbonate, and it leaves the reaction vessel as a gas (unless the reaction vessel is pressurized). This is the well-known "volcano" reaction between baking soda and vinegar.


Industrially, sodium acetate is prepared from glacial acetic acid and sodium hydroxide.

C2H4O2 + NaOH → NaO2CCH3 + H2O


Sodium acetate can be used to form an ester with an alkyl halide such as bromoethane:

NaO2CCH3 + BrCH2CH3→ C2H5O2CCH3 + NaBr

Caesium salts catalyze this reaction.

From Yahoo Answers

Question:Hi, Just a quick and simple chemistry question for you: May you please create a chemical equation for reacting acetic acid with sodium hydroxide? Please label states and balance it as well. Thank you for your time.

Answers:HC2H3O2(aq) + NaOH(s) ------> H2O(l) + NaC2H3O2(s)

Question:ionisation equilibrium equation for acetic acid and sodium hydroxide

Answers:CH3COOH + NaOH = CH3COONa + H2O CH3COOH + OH- = CH3COO- + H2O K = [CH3COO-]/[CH3COOH][OH-] ie K = [salt]/[acid][base] Not that [H2O] is considered to be 1.

Question:It starts off as HCH3COO + NaOH ---> H20 + NaCH3COO Correct? And furthermore, What about Calcium Hydroxide and Acetic Acid? Ca(OH)2(aq) + HCH3COO(aq) --> CaCH3COO(aq) + H2O(l) is the balanced right??

Answers:I'm using + for positive charged ions and & for the plus in reactions. It's CH3COO- & H+ & Na+ & OH- -> CH3COO- & Na+ & H+ & OH- Ca2+ & 2 OH- & 2 CH3COO- & 2 H+ -> 2 H+ & 2 OH- & 2 CH3COO- & Ca2+ So, the balanced form is: Ca(OH)2 + 2 CH3COOH -> 2 H2O + Ca(CH3COO)2


Answers:Ethanoic (Acetic) acid is CH3COOH CH3COOH +NaOH > Na (CH3COO) + H2O