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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.

Applications

Industrial

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.

Food

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.

Preparation

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.

CH3COOH + NaHCO3→ CH3COONa + H2O + CO2

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

C2H4O2 + NaOH → NaO2CCH3 + H2O

Reactions

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 Encyclopedia

sodium hydrogen carbonate

sodium hydrogen carbonate see sodium bicarbonate .


From Yahoo Answers

Question:answer gets a best answer thingy!

Answers:CH3COOH + NaHCO3 >> CH3COONa + H2O + CO2

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Answers:C2H4O2 + NaHCO3 -> NaC2H3O2 + H2CO3 and as far as I can see it is balanced.

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Question:Sodium carbonate reacts with acetic acid to produce carbon dioxide gas, aqueous sodium acetate and water. if 75mL of .30M acetic acid is allowed to react with excess sodium carbonate, then how many mL of dry carbon dioxide gas are produced at 22*C and 745 mm Hg? Zinc metal reacts with aqueous hydrochloric acid to produce aqueous zinc chloride and hydrogen gas. if 20 grams of zinc is allowed to react with excess hydrochloric acid, then what is the volume in liters of dry hydrogen gas collected at 35*C and 733 mm Hg? What are the steps to solve these questions? Thank you for the help.

Answers:Question: Sodium carbonate reacts with acetic acid to produce carbon dioxide gas, aqueous sodium acetate and water. if 75mL of .30M acetic acid is allowed to react with excess sodium carbonate, then how many mL of dry carbon dioxide gas are produced at 22*C and 745 mm Hg? To work this one, first write down the chemical reaction. Then you want to balance it with stochemetry. Next, you want to figure out the limit reagent, so you can figure out how many moles of product are produced. Finally, you want to figure out how much volume the number of moles of CO2 would have. The second question is similar.

From Youtube

1-23-2 :Which of the following is an ionic compound? A. ethyl acetate, B. sulfuric acid, C. sodium hydrogen carbonate, D. hydrazine

acid poured on sodium acetate :enjoy if you dont like this vidd i wil take again