Difference between revisions of "Sodium acetate"
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| − | '''Sodium acetate''' is the sodium salt of [[acetic acid]], with the chemical formula CH<sub>3</sub>COONa. It forms a white or translucent powder or crystals that have a variety of uses in the home lab. | + | | Name = Sodium acetate |
| + | | Reference = | ||
| + | | IUPACName = Sodium acetate | ||
| + | | PIN = | ||
| + | | SystematicName = Sodium ethanoate | ||
| + | | OtherNames = Hot ice (Sodium acetate trihydrate) | ||
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| + | | ImageFile = Sodium acetate by No Tears Only Dreams Now.jpg | ||
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| + | | ImageCaption = Crystals of sodium acetate trihydrate. | ||
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| + | <!-- Sections --> | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | 3DMet = | ||
| + | | Abbreviations = | ||
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| + | | Section2 = {{Chembox Properties | ||
| + | | AtmosphericOHRateConstant = | ||
| + | | Appearance = Hygroscopic solid | ||
| + | | BoilingPt = | ||
| + | | BoilingPtC = | ||
| + | | BoilingPt_ref = | ||
| + | | BoilingPt_notes = ''Anhydrous:''<br>881.4 °C (1,618.5 °F; 1,154.5 K) (decomposes)<hr>''Trihydrate:''122 °C (252 °F; 395 K) (decomposes) | ||
| + | | Density = 1.528 g/cm<sup>3</sup> (20 °C, anhydrous)<br>1.45 g/cm<sup>3</sup> (20 °C, trihydrate) | ||
| + | | Formula = C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>Na<br>CH<sub>3</sub>COONa (anhydrous)<br>CH<sub>3</sub>COONa·3 H<sub>2</sub>O (trihydrate) | ||
| + | | HenryConstant = | ||
| + | | LogP = | ||
| + | | MolarMass = 82.03 g/mol (anhydrous)<br>136.08 g/mol (trihydrate) | ||
| + | | MeltingPt = | ||
| + | | MeltingPtC = | ||
| + | | MeltingPt_ref = | ||
| + | | MeltingPt_notes = ''Anhydrous:''<br>324 °C (615 °F; 597 K)<hr>''Trihydrate:''<br>58 °C (136 °F; 331 K) | ||
| + | | Odor = Odorless<br>Acetic (at high temp.) | ||
| + | | pKa = 24 (20 °C)<br>4.76 CH<sub>3</sub>COOH | ||
| + | | pKb = 9.25 | ||
| + | | Solubility = ''Anhydrous:''<br>119 g/100 ml (0 °C)<br>123.3 g/100 ml (20 °C)<br>125.5 g/100 ml (30 °C)<br>137.2 g/100 ml (60 °C)<br>162.9 g/100 ml (100 °C)<hr>''Trihydrate:''<br>32.9 g/100 ml (-10 °C)<br>36.2 g/100 ml (0 °C)<br>46.4 g/100 ml (20 °C)<br>82 g/100 ml (50 °C) | ||
| + | | SolubleOther = Soluble in [[ethanol]], [[hydrazine]], liq. [[sulfur dioxide|SO<sub>2</sub>]] | ||
| + | | Solubility1 = 0.05 g/100 g (15 °C) | ||
| + | | Solvent1 = acetone | ||
| + | | Solubility2 = ''Trihydrate:''<br> 5.3 g/100 ml | ||
| + | | Solvent2 = ethanol | ||
| + | | Solubility3 = 16 g/100 g (15 °C)<br> 16.55 g/100 g (67.7 °C) | ||
| + | | Solvent3 = methanol | ||
| + | | VaporPressure = | ||
| + | }} | ||
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| + | | Coordination = | ||
| + | | CrystalStruct = Monoclinic | ||
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| + | | Section4 = {{Chembox Thermochemistry | ||
| + | | DeltaGf = −607.7 kJ/mol (anhydrous) | ||
| + | | DeltaHc = | ||
| + | | DeltaHf = −709.32 kJ/mol (anhydrous)<br>−1,604 kJ/mol (trihydrate) | ||
| + | | Entropy = 138.1 J·mol<sup>-1</sup>·K<sup>-1</sup> (anhydrous)<br>262 J·mol<sup>-1</sup>·K<sup>-1</sup> (trihydrate) | ||
| + | | HeatCapacity = 100.83 J·mol<sup>-1</sup>·K<sup>-1</sup> (anhydrous)<br>229 J·mol<sup>-1</sup>·K<sup>-1</sup> (trihydrate) | ||
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| + | | Section6 = {{Chembox Hazards | ||
| + | | AutoignitionPt = 600 °C (1,112 °F; 873 K) | ||
| + | | ExploLimits = None | ||
| + | | ExternalMSDS = [https://www.docdroid.net/MHLNv3x/sodium-acetate-anhydrous-sa.pdf.html Sigma-Aldrich] (anhydrous)<br>[https://www.docdroid.net/VEtQXD9/sodium-acetate-trihydrate-sa.pdf.html Sigma-Aldrich] (trihydrate) | ||
| + | | FlashPt = 250 °C (482 °F; 523 K) | ||
| + | | LD50 = 3,530 mg/kg (rat, oral) | ||
| + | | LC50 = | ||
| + | | MainHazards = Irritant | ||
| + | | NFPA-F = | ||
| + | | NFPA-H = | ||
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| + | }} | ||
| + | | Section7 = {{Chembox Related | ||
| + | | OtherAnions = | ||
| + | | OtherCations = | ||
| + | | OtherFunction = | ||
| + | | OtherFunction_label = | ||
| + | | OtherCompounds = [[Acetic acid]]<br>[[Calcium acetate]] | ||
| + | }} | ||
| + | }} | ||
| + | '''Sodium acetate''' is the sodium salt of [[acetic acid]], with the chemical formula '''CH<sub>3</sub>COONa'''. It forms a white or translucent powder or crystals that have a variety of uses in the home lab. | ||
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Sodium acetate is most commonly seen as a buffering agent for acetic acid solutions. Pure, anhydrous sodium acetate and other acetates may be [[dry-distilled]] to yield [[acetone]], though this may not be economical. Though [[calcium acetate]] is more often considered, sodium acetate may potentially be combined with concentrated [[sulfuric acid]] and then distilled to yield nearly glacial acetic acid, a highly sought-after chemical. Finally, sodium acetate can be reacted with primary [[haloalkanes]], such as [[chloromethane]], to yield an alkyl acetate [[ester]] and a sodium salt containing the respective halogen. That esterification is catalyzed by [[ | + | Sodium acetate is most commonly seen as a buffering agent for acetic acid solutions. Pure, anhydrous sodium acetate and other acetates may be [[dry-distilled]] to yield [[acetone]], though this may not be economical. Though [[calcium acetate]] is more often considered, sodium acetate may potentially be combined with concentrated [[sulfuric acid]] and then distilled to yield nearly glacial acetic acid, a highly sought-after chemical. Finally, sodium acetate can be reacted with primary [[haloalkanes]], such as [[chloromethane]], to yield an alkyl acetate [[ester]] and a sodium salt containing the respective halogen. That esterification is catalyzed by [[caesium]] salts. |
===Physical=== | ===Physical=== | ||
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==Availability== | ==Availability== | ||
Though not commonly found in stores, sodium acetate is easily produced from two common household chemicals: vinegar and baking soda. | Though not commonly found in stores, sodium acetate is easily produced from two common household chemicals: vinegar and baking soda. | ||
| + | |||
| + | Some if not most type of heat pads contain a supersaturated solution of sodium acetate. | ||
==Preparation== | ==Preparation== | ||
Sodium acetate can be crystallized from a solution in which [[sodium bicarbonate]], [[sodium carbonate|carbonate]], or [[sodium hydroxide|hydroxide]] was combined with an equal or excess of acetic acid (distilled white vinegar will work if high purity is not vital). This is the very same reaction behind the common "baking soda volcano" science experiments that produce a voluminous foam of sodium acetate and [[carbon dioxide]]. | Sodium acetate can be crystallized from a solution in which [[sodium bicarbonate]], [[sodium carbonate|carbonate]], or [[sodium hydroxide|hydroxide]] was combined with an equal or excess of acetic acid (distilled white vinegar will work if high purity is not vital). This is the very same reaction behind the common "baking soda volcano" science experiments that produce a voluminous foam of sodium acetate and [[carbon dioxide]]. | ||
| − | The main problem with using even the purest vinegar is that distilled vinegar is not pure acetic acid, as there are plenty of extra organics. Distilling the vinegar beforehand produces pure acetic acid. | + | The main problem with using even the purest vinegar is that distilled vinegar is not pure acetic acid, as there are plenty of extra organics. Distilling the vinegar beforehand produces pure acetic acid. However, obtaining concentrated acetic acid from vinegar via distillation is not easy and requires several distillations to remove the water that also distills due to their close boiling points. |
==Projects== | ==Projects== | ||
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===Disposal=== | ===Disposal=== | ||
Sodium acetate has very little toxicity and doesn't require any special disposal. However, because is a sodium salt it's recommended to avoid dumping it on grass or other plants, as it will kill it. It can however be used as a (weak) weedkiller. | Sodium acetate has very little toxicity and doesn't require any special disposal. However, because is a sodium salt it's recommended to avoid dumping it on grass or other plants, as it will kill it. It can however be used as a (weak) weedkiller. | ||
| + | |||
| + | ==Gallery== | ||
| + | <gallery widths="200" position="center" columns="4" orientation="none"> | ||
| + | Sodium_acetate_trihydrate.jpg|Sodium acetate trihydrate | ||
| + | Sodium_acetate_iron_iii_chloride.jpg|Deep red complex between iron(III) and acetate ions.<ref>http://www.chemieunterricht.de/dc2/essig/hac-06.htm</ref> | ||
| + | </gallery> | ||
==References== | ==References== | ||
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[[Category:Buffering agents]] | [[Category:Buffering agents]] | ||
[[Category:Easily prepared chemicals]] | [[Category:Easily prepared chemicals]] | ||
| + | [[Category:Readily available chemicals]] | ||
[[Category:Edible chemicals]] | [[Category:Edible chemicals]] | ||
[[Category:Chemicals for crystal growing]] | [[Category:Chemicals for crystal growing]] | ||
Latest revision as of 10:08, 7 May 2021
 Crystals of sodium acetate trihydrate.
| |
| Names | |
|---|---|
| IUPAC name
Sodium acetate
| |
| Systematic IUPAC name
Sodium ethanoate | |
| Other names
Hot ice (Sodium acetate trihydrate)
| |
| Properties | |
| C2H3O2Na CH3COONa (anhydrous) CH3COONa·3 H2O (trihydrate) | |
| Molar mass | 82.03 g/mol (anhydrous) 136.08 g/mol (trihydrate) |
| Appearance | Hygroscopic solid |
| Odor | Odorless Acetic (at high temp.) |
| Density | 1.528 g/cm3 (20 °C, anhydrous) 1.45 g/cm3 (20 °C, trihydrate) |
| Melting point | Anhydrous: 324 °C (615 °F; 597 K) Trihydrate: 58 °C (136 °F; 331 K) |
| Boiling point | Anhydrous: 881.4 °C (1,618.5 °F; 1,154.5 K) (decomposes) Trihydrate:122 °C (252 °F; 395 K) (decomposes) |
| Anhydrous: 119 g/100 ml (0 °C) 123.3 g/100 ml (20 °C) 125.5 g/100 ml (30 °C) 137.2 g/100 ml (60 °C) 162.9 g/100 ml (100 °C) Trihydrate: 32.9 g/100 ml (-10 °C) 36.2 g/100 ml (0 °C) 46.4 g/100 ml (20 °C) 82 g/100 ml (50 °C) | |
| Solubility | Soluble in ethanol, hydrazine, liq. SO2 |
| Solubility in acetone | 0.05 g/100 g (15 °C) |
| Solubility in ethanol | Trihydrate: 5.3 g/100 ml |
| Solubility in methanol | 16 g/100 g (15 °C) 16.55 g/100 g (67.7 °C) |
| Acidity (pKa) | 24 (20 °C) 4.76 CH3COOH |
| Thermochemistry | |
| Std molar
entropy (S |
138.1 J·mol-1·K-1 (anhydrous) 262 J·mol-1·K-1 (trihydrate) |
| Std enthalpy of
formation (ΔfH |
−709.32 kJ/mol (anhydrous) −1,604 kJ/mol (trihydrate) |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (anhydrous) Sigma-Aldrich (trihydrate) |
| Flash point | 250 °C (482 °F; 523 K) |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
3,530 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Acetic acid Calcium acetate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium acetate is the sodium salt of acetic acid, with the chemical formula CH3COONa. It forms a white or translucent powder or crystals that have a variety of uses in the home lab.
Contents
Properties
Chemical
Sodium acetate is most commonly seen as a buffering agent for acetic acid solutions. Pure, anhydrous sodium acetate and other acetates may be dry-distilled to yield acetone, though this may not be economical. Though calcium acetate is more often considered, sodium acetate may potentially be combined with concentrated sulfuric acid and then distilled to yield nearly glacial acetic acid, a highly sought-after chemical. Finally, sodium acetate can be reacted with primary haloalkanes, such as chloromethane, to yield an alkyl acetate ester and a sodium salt containing the respective halogen. That esterification is catalyzed by caesium salts.
Physical
Sodium acetate typically exists as an anhydrous white crystalline powder or as thin, transparent crystals of the trihydrate. When produced using household vinegar, solutions and crystals of sodium acetate may appear golden or amber in color. Sodium acetate has an odor resembling that of vinegar, though slightly more fruity and pleasant. The taste and low toxicity of this compound allow it to be used as a salt-and-vinegar-type flavoring agent in some foods.
Sodium acetate trihydrate supercools easily and will crystallize on contact with a sufficient nucleation site, such as another crystal of sodium acetate or sodium bicarbonate.
Availability
Though not commonly found in stores, sodium acetate is easily produced from two common household chemicals: vinegar and baking soda.
Some if not most type of heat pads contain a supersaturated solution of sodium acetate.
Preparation
Sodium acetate can be crystallized from a solution in which sodium bicarbonate, carbonate, or hydroxide was combined with an equal or excess of acetic acid (distilled white vinegar will work if high purity is not vital). This is the very same reaction behind the common "baking soda volcano" science experiments that produce a voluminous foam of sodium acetate and carbon dioxide.
The main problem with using even the purest vinegar is that distilled vinegar is not pure acetic acid, as there are plenty of extra organics. Distilling the vinegar beforehand produces pure acetic acid. However, obtaining concentrated acetic acid from vinegar via distillation is not easy and requires several distillations to remove the water that also distills due to their close boiling points.
Projects
- Make hot ice
- Production of acetone by dry-distillation
- Highly concentrated acetic acid (possibly glacial)
- Make acetic anhydride
Handling
Safety
Pure sodium acetate, as well as sodium acetate produced in a sterile environment from vinegar, is of very low toxicity and is even safe to season food with in reasonable quantities (though this usage is not recommended with lab grade chemicals).
Storage
Sodium acetate should be stored in closed bottles. The anhydrous form should be stored in sealed bottles.
Disposal
Sodium acetate has very little toxicity and doesn't require any special disposal. However, because is a sodium salt it's recommended to avoid dumping it on grass or other plants, as it will kill it. It can however be used as a (weak) weedkiller.
Gallery
Sodium acetate trihydrate
Deep red complex between iron(III) and acetate ions.[1]
