- "Historical Background - Sodium Acetate." Sodium Acetate. Weebly, n.d. Web. 30 Mar. 2014.
- Tangient LLC, Eric Ablett. "Uses." SodiumAcetate -. Wikispaces, n.d. Web. 30 Mar. 2014.
- "How Do You Get Heat from a Supercooled Solution? Explore the Chemistry Within Hand Warmers." How Do You Get Heat from a Supercooled Solution? Sciencebuddies, n.d. Web. 30 Mar. 2014.
- "Amazing Rust.com - Hot Ice." Amazing Rust.com - Hot Ice. Amazing Rust, n.d. Web. 30 Mar. 2014.
- Helmenstine, Anne Marie. "Hot Ice or Sodium Acetate." About.com Chemistry. NRelate, n.d. Web. 28 Mar. 2014.
- "How to Make Hot Ice." WikiHow. N.p., n.d. Web. 27 Mar. 2014.
Saturday, 21 December 2013
Bibliography
Friday, 20 December 2013
Store bought Sodium Acetate Method V.S. Homemade sodium Acetate Method
The Homemade hot ice produces some pretty bad hot ice but will still usable. If you have already used up all your sodium acetate powder which had been obtained from the pan you can still initiate the freezing process by using baking soda. This method is not recommended as it can contaminate the solution and many reuses it will eventually stop working. The homemade method works but the reaction rate is slow and even if you did not burn it, its still not clear as store bought vinegar has impurities in it.
NaHCH3= Sodium Bicarbonate ( baking soda)
CH3COOH= Acetic acid ( Vinegar)
When a Sodium bicarbonate solution reacts with an Acetic acid, the result would be a Sodium Acetate.
Chemical reaction
NaHCH3+ CH3COOH = NaCH3COO+H2O+ CO2= C2H3NaCO2+H2O+CO2
C2H3NaO2+H2O+CO2= Chemical Formula for Sodium Acetate
Where as Laboratory grade chemicals give out much cleaner and faster reactive hot ice than what home chemistry can give. Instead of making Sodium acetate trihydrate which is slow, it would be preferable to buy it as it is cheaper for large quantities and gives the best quality Hot ice.
CH3COOH= Acetic acid ( Vinegar)
When a Sodium bicarbonate solution reacts with an Acetic acid, the result would be a Sodium Acetate.
Chemical reaction
NaHCH3+ CH3COOH = NaCH3COO+H2O+ CO2= C2H3NaCO2+H2O+CO2
C2H3NaO2+H2O+CO2= Chemical Formula for Sodium Acetate
Where as Laboratory grade chemicals give out much cleaner and faster reactive hot ice than what home chemistry can give. Instead of making Sodium acetate trihydrate which is slow, it would be preferable to buy it as it is cheaper for large quantities and gives the best quality Hot ice.
Cold Fire
There is an exact opposite reaction of Hot ice and it is Cold Fire. In Hot ice the reaction is Exothermic hence the reaction creating heat energy.Where as in Cold Fire the reaction is Endothermic as the absorbs heat.For a fire to be created it must require three components which are fuel, oxygen and heat. This is known as a fire triangle. Most agents extinguish fire by breaking down one 'leg' of the fire triangle, fuel and heat. Cold fire is considered to have 6 times the penetrating capability of water. Cold fire has an extraordinary capability of absorbing heat thus allowing it to penetrate fire more quickly, hence extinguishing it faster than normal rate.
Cold Fire also works to encapsulate the fuel source and its vapor and simultaneously begins to break down the molar structure of the hydrogen fuel source preventing re-ignition.
This is the exact opposite of what Hot ice does. Sodium acetate gives out heat energy making the ice hot. This can be used to give warmth when needed. Cold fire acts as an agent to absorb and extinguish heat. It can be used to put out a fire.
It is a non toxic and non corrosive solution, hence it can even pt out a fire on a booster or fuel tank.
This is just an example of the exact opposite of Hot Ice in case of wanting to switch experiments. Both are equally cool and are enjoyable to perform.
Other Medical Uses
DNA & RNA Isolation
DNA Isolation is the process of purifying DNA using a combination of chemical and physical methods.
DNA is not soluble in ethanol and isopropanol thus precipitation of DNA is improved by increasing the ionic strength generally using sodium acetate.
A modified and optimized method for RNA isolation was developed. It is based on a CTAB method including mercaptoethanol and PVPP with sequential Chloroform, Phenol, isoamyl alcohol extractions to remove protein, and polyhenols followed by two selective purification with LiCL and Sodium acetate in order to eliminate polysaccharedes. Though the introduced modifications are not new their addition resulted to be decisive for success in RNA isolation.
DNA & RNA Extraction
The principle of this single- step technique is that RNA is separated from DNA after extraction with acidic solution consisting chloroform,guanidinium thiocyante, phenol and sodium acetate.
The low pH sodium acetate tends to be used in some DNA extractions.
In acidic conditions, total RNA will remain in the upper aqueous phase of the entire mixture while DNA and proteins remain in the interphase or lower organic phase Recovery of RNA is then done by precipitation with isopropanol.
DNA Isolation is the process of purifying DNA using a combination of chemical and physical methods.DNA is not soluble in ethanol and isopropanol thus precipitation of DNA is improved by increasing the ionic strength generally using sodium acetate.
A modified and optimized method for RNA isolation was developed. It is based on a CTAB method including mercaptoethanol and PVPP with sequential Chloroform, Phenol, isoamyl alcohol extractions to remove protein, and polyhenols followed by two selective purification with LiCL and Sodium acetate in order to eliminate polysaccharedes. Though the introduced modifications are not new their addition resulted to be decisive for success in RNA isolation.
DNA & RNA Extraction
The low pH sodium acetate tends to be used in some DNA extractions.
In acidic conditions, total RNA will remain in the upper aqueous phase of the entire mixture while DNA and proteins remain in the interphase or lower organic phase Recovery of RNA is then done by precipitation with isopropanol.
Uses in the Field of Medicine
Sodium acetate in Clinical Pharmacology
Sodium is a principal cation of extra-cellular fluid. It comprises of more then 90 percent of total cations in its normal plasma concentration of an estimate of 140 mEq/ liter. The ion of sodium plays a major role in controlling the total body water and its distribution.
Acetate (CH3COO) is a hydrogen ion receptor. It also serves as an alternate source of bicarbonate(HCO3) by metabolic alteration in the liver. The conversion has been shown to advance, even in the presence of liver diseases.
Sodium acetate Injection:
USP (2 mEq/ml) is a sterile, nonpyrogenic, concentrated solution of sodium acetate present in water form in
the injection. The solution is administered after dilution by the intravenous route as an electrolyte replenisher.
Each ml contains 164 mg of sodium acetate (anhydrous) which would provide about 2 mEq each of sodium (Na+) and acetate (CH3COO. It may also contain acetic acid for pH adjustment; approximate pH- 6.5. The osmolar concentration is 4mOsmol/ml (calc.). A pharmacy bulk package is a container of sterile preparation for parental use that contains many single doses.
The contents are intended for the use in a pharmacy admixture program and are restricted to the preparation of admixtures for intravenous infusion. The solution is intended as an alternative to sodium chloride in order to provide sodium ion (Na+) for addition to large volume infusion fluids for intravenous use.
Sodium acetate injection USP (2 mEq/ml) is indicated as a source of sodium for addition to large volume intravenous fluids to prevent or correct hyponatremia in patients with restricted or no oral intake. It is also useful as an additive for preparing specific intravenous fluid formulas when the needs of the patient cannot be met by standard electrolyte or nutrient solutions.
Sodium is a principal cation of extra-cellular fluid. It comprises of more then 90 percent of total cations in its normal plasma concentration of an estimate of 140 mEq/ liter. The ion of sodium plays a major role in controlling the total body water and its distribution.
Acetate (CH3COO) is a hydrogen ion receptor. It also serves as an alternate source of bicarbonate(HCO3) by metabolic alteration in the liver. The conversion has been shown to advance, even in the presence of liver diseases.
Sodium acetate Injection:
USP (2 mEq/ml) is a sterile, nonpyrogenic, concentrated solution of sodium acetate present in water form in
the injection. The solution is administered after dilution by the intravenous route as an electrolyte replenisher.
Each ml contains 164 mg of sodium acetate (anhydrous) which would provide about 2 mEq each of sodium (Na+) and acetate (CH3COO. It may also contain acetic acid for pH adjustment; approximate pH- 6.5. The osmolar concentration is 4mOsmol/ml (calc.). A pharmacy bulk package is a container of sterile preparation for parental use that contains many single doses.
The contents are intended for the use in a pharmacy admixture program and are restricted to the preparation of admixtures for intravenous infusion. The solution is intended as an alternative to sodium chloride in order to provide sodium ion (Na+) for addition to large volume infusion fluids for intravenous use.
Sodium acetate injection USP (2 mEq/ml) is indicated as a source of sodium for addition to large volume intravenous fluids to prevent or correct hyponatremia in patients with restricted or no oral intake. It is also useful as an additive for preparing specific intravenous fluid formulas when the needs of the patient cannot be met by standard electrolyte or nutrient solutions.
Other Uses and Applications
Heating Pads:
Hot ice is generally found in heating pads. Small amounts of sodium acetate are positioned inside small pouches which contain a metal disc. When the user is in need of warmth, they will simply need to click on the metal disc inside the pouch which will then trigger the release of a few crystals of sodium acetate.
The sodium acetate liquid will immediately turn to its solid state and since the sodium acetate freezes at 54 degrees Celsius, the solid ice returns to the same temperature giving out heat.
Various types of hand warmers use permanent reactions that produce heat. Sodium acetate pads can be used repeatedly by just simply boiling them in hot water which will return the solid sodium acetate back into a liquid form.
Hand Warmers:
Hot ice is generally found in heating pads. Small amounts of sodium acetate are positioned inside small pouches which contain a metal disc. When the user is in need of warmth, they will simply need to click on the metal disc inside the pouch which will then trigger the release of a few crystals of sodium acetate.The sodium acetate liquid will immediately turn to its solid state and since the sodium acetate freezes at 54 degrees Celsius, the solid ice returns to the same temperature giving out heat.
Various types of hand warmers use permanent reactions that produce heat. Sodium acetate pads can be used repeatedly by just simply boiling them in hot water which will return the solid sodium acetate back into a liquid form.
Hand Warmers:
Hand warmers are small and practically disposable packets which are held by hand. They produce heat on demand and when they are shaken they produce heat energy. Depending on the type and source of heat, hand warmers can last about 30 minutes (re-crystallization) to 24 hours max (platinum catalyst).
They are almost as similar as the heat pads but they cannot be reused and they are air activated meaning that the sodium acetate inside the small bag reacts with the air particles in order to generate heat energy out into the surface.
Applications
Sodium Acetate has many applications in the world today. It is currently being used for Industrial purposes, in food, it is being used as a buffer solution and in Concrete longevity, Heating pads, Hand warmers, in medicine and is being studied for further future uses.
Industrial Uses:
Sodium acetate is being used in the textile industry to neutralize sulfuric acid waste streams and as a photo resistor while using aniline dyes. It also works as a pickling agent in chrome tanning and it helps to retard vulcanization of chloroprene in synthetic rubber production. Sodium acetate is also used to eliminate static electricity buildups in processing cotton for disposable cotton pads. It is used as a buffering agent in leather tanning to create a more even tan and to make the leather more durable. Sodium acetate is as well used in the buffering of petroleum products and even in the production range of cosmetic products. It is generally being used in industrial factories as it is inexpensive and very safe to use.
Food:
This solution is safe to act as a food additive. Sodium diacetate which is sodium acetate and acetic acid is commonly uses as a seasoning in salt and vinegar potato chips in the U.S. It is also used to enhance the flavor of some meat and poultry products.
Buffer Solution:
As a conjugate base of acetic acid, a solution of sodium acetate and acetic acid can act as a buffer in order to keep a relatively constant pH level. This is very useful mostly in the field of biochemical applications in which the reactions are pH dependent in a mildly acidic range such as pH 4-6.
Concrete Longevity:
Sodium acetate is used to reduce the damage water can potentially do to concrete by acting as concrete sealant as well as being environmentally benign and cheaper than the epoxy alternative that is usually in employment for the sealing of concrete against water permeation.
Industrial Uses:
Sodium acetate is being used in the textile industry to neutralize sulfuric acid waste streams and as a photo resistor while using aniline dyes. It also works as a pickling agent in chrome tanning and it helps to retard vulcanization of chloroprene in synthetic rubber production. Sodium acetate is also used to eliminate static electricity buildups in processing cotton for disposable cotton pads. It is used as a buffering agent in leather tanning to create a more even tan and to make the leather more durable. Sodium acetate is as well used in the buffering of petroleum products and even in the production range of cosmetic products. It is generally being used in industrial factories as it is inexpensive and very safe to use.
This solution is safe to act as a food additive. Sodium diacetate which is sodium acetate and acetic acid is commonly uses as a seasoning in salt and vinegar potato chips in the U.S. It is also used to enhance the flavor of some meat and poultry products.
Buffer Solution:
As a conjugate base of acetic acid, a solution of sodium acetate and acetic acid can act as a buffer in order to keep a relatively constant pH level. This is very useful mostly in the field of biochemical applications in which the reactions are pH dependent in a mildly acidic range such as pH 4-6.
Concrete Longevity:
Sodium acetate is used to reduce the damage water can potentially do to concrete by acting as concrete sealant as well as being environmentally benign and cheaper than the epoxy alternative that is usually in employment for the sealing of concrete against water permeation.
Apparatus
Method 1- Homemade Sodium Acetate
1. Cooking pan-x1
2.Glass beaker-150ml x1
3. Baking soda-x1 box
4. White Vinegar-x2 liters
5. Spoon-x1
6. Stove-x1
7. Ice bath-x1 (Glass tray, Ice)
8. Sodium acetate-x1 box
9.Tablespoon-x1
10. Thermometer
Method 2- Store bought Sodium acetate
1. Microwave-x1
2.Glass beaker-150ml x1
3.Store bought Sodium Acetate or Sodium Acetate anhydrous- x1 box
4.Spoon-x1
5.Electric Stove-x1
6.Ice bath-x1 ( Tray, Ice)
7.Thermometer-x1
8. Petridish-x1
9. Cooking pan
The apparatus required for the two types of experiments are almost somewhat similar except for a few chances her and there. You can choose any of the two methods for your experiment and from this you will know the apparatus required from the above.
1. Cooking pan-x1
2.Glass beaker-150ml x13. Baking soda-x1 box
4. White Vinegar-x2 liters
5. Spoon-x1
6. Stove-x1
7. Ice bath-x1 (Glass tray, Ice)
8. Sodium acetate-x1 box
9.Tablespoon-x1
10. Thermometer
Method 2- Store bought Sodium acetate
1. Microwave-x1
2.Glass beaker-150ml x1
3.Store bought Sodium Acetate or Sodium Acetate anhydrous- x1 box
4.Spoon-x1
5.Electric Stove-x1
6.Ice bath-x1 ( Tray, Ice)
7.Thermometer-x1
8. Petridish-x1
9. Cooking pan
The apparatus required for the two types of experiments are almost somewhat similar except for a few chances her and there. You can choose any of the two methods for your experiment and from this you will know the apparatus required from the above.
Method 2 continuation
Step 6- Stir the aqueous solution till all the solid compounds are completely dissolved.
Step 7- Begin to cool the beaker in an ice bath or you can keep the beaker in the refrigerator.
When the solution has finished cooling it becomes 'super-cooled' which means that it went below its temperature of freezing without actually solidifying.
Step 8- Now add a pinch of sodium acetate trihydrate crystals (which you had obtained from the pan earlier) onto the solution.
At first begin with just a pinch then 2 and if there still isn't any effect taking place then you will have to add a larger amount of the crystals into the aqueous
solution.
Step 9- Now that you have added the sodium acetate crystals into the super-cooled solution of sodium acetate you will notice the solution solidifying.
This is as a chain of reaction is set off when the crystals came in contact with the liquid.
Step 10- The crystals are releasing energy when the reaction is taking place thus the solidified solution will radiate heatof an estimate of 130 degrees Celsius or 54 degrees Fahrenheit.
There will be a problem with the solution if the reaction doesn't occur. You could try once again but a better solution would be to do the experiment with Store bought Sodium Acetate.
Step 7- Begin to cool the beaker in an ice bath or you can keep the beaker in the refrigerator.
When the solution has finished cooling it becomes 'super-cooled' which means that it went below its temperature of freezing without actually solidifying.
Step 8- Now add a pinch of sodium acetate trihydrate crystals (which you had obtained from the pan earlier) onto the solution.
At first begin with just a pinch then 2 and if there still isn't any effect taking place then you will have to add a larger amount of the crystals into the aqueous
solution.
Step 9- Now that you have added the sodium acetate crystals into the super-cooled solution of sodium acetate you will notice the solution solidifying.
This is as a chain of reaction is set off when the crystals came in contact with the liquid.
Step 10- The crystals are releasing energy when the reaction is taking place thus the solidified solution will radiate heatof an estimate of 130 degrees Celsius or 54 degrees Fahrenheit.
There will be a problem with the solution if the reaction doesn't occur. You could try once again but a better solution would be to do the experiment with Store bought Sodium Acetate.
Method 2
Homemade Sodium Acetate Method
Step 1- You will need to add baking soda ( not baking powder) onto a pan.
An Approximate of 6 tablespoons would be good.
Step 2- Now you will be required to add White Vinegar onto the baking soda until it stops fizzing.
An estimate of 2 liters of vinegar should do the job.
Step 3- Boil the solution till about an approximate of 90 percent of the water solution has evaporated.
The solution will be ready when you will be able to notice the formation of a crusty film on top of the water solution.
The solution will appear as slight yellow or brown. This indicates that the solution is a more concentrated solution of sodium acetate trihydrate.
Step 4- As the solution finishes boiling down you will be able to notice sodium acetate crystals left sticking onto the bottom of the pan. Pour the solution into a beaker carefully and you must not pour the crystals into the beaker.
Use a spoon to collect the crystals as you will be needing the crystals for later on in the experiment. Do not let the film on the top of your solution get developed or thickened as this indicates that another reaction is occurring stating that your experiment is ruined.
Step 5- After you have moved the solution into a beaker (of your choice) add 2 tablespoons of vinegar into the solution.
The solution will not solidify due to the vinegar keeping the solution in its aqueous form.
Step 1- You will need to add baking soda ( not baking powder) onto a pan.
An Approximate of 6 tablespoons would be good.
Step 2- Now you will be required to add White Vinegar onto the baking soda until it stops fizzing.
An estimate of 2 liters of vinegar should do the job.
Step 3- Boil the solution till about an approximate of 90 percent of the water solution has evaporated.The solution will be ready when you will be able to notice the formation of a crusty film on top of the water solution.
The solution will appear as slight yellow or brown. This indicates that the solution is a more concentrated solution of sodium acetate trihydrate.
Step 4- As the solution finishes boiling down you will be able to notice sodium acetate crystals left sticking onto the bottom of the pan. Pour the solution into a beaker carefully and you must not pour the crystals into the beaker.
Use a spoon to collect the crystals as you will be needing the crystals for later on in the experiment. Do not let the film on the top of your solution get developed or thickened as this indicates that another reaction is occurring stating that your experiment is ruined.
Step 5- After you have moved the solution into a beaker (of your choice) add 2 tablespoons of vinegar into the solution.
The solution will not solidify due to the vinegar keeping the solution in its aqueous form.
Continuation of Method 1
The temperature in which the solution is saturated is brought down.
In general the crystals are supposed to crystallize when brought below this point but as the sodium acetate is in a supersaturated liquid state it super-cools
This indicates that it will not crystallize even when it goes below its normal temperature.
The solution must not be spilled or come in contact with the sodium acetate trihydrate powder.
Step 8- You can either add a pinch of powder onto the solution by hand or you can use a toothpick
The liquid solution will automatically as soon as it come in contact with the sodium acetate powder.
When the 'seed crystal' is introduced into the solution, a nucleation center has been created resulting to solidification being triggered.
Step 9- The solid in the tray will be radiating heat due to the crystals releasing energy in the reaction.
The solid will radiate heat of approximately 54 degrees Celsius or 130 degrees Fahrenheit.
Two Methods of making Hot ice
There are two ways in which hot ice can be created. The two methods in which sodium acetate can be made are either by using the Store bought Sodium Acetate Trihydrate method or by following the Homemade Sodium Acetate Trihydrate method provided below.
Step 1- You will need to obtain sodium acetate Trihydrate.
This material will not be easy to acquire even though it is a nontoxic and inexpensive ingredient.
This material will not be easy to acquire even though it is a nontoxic and inexpensive ingredient.
The best way to get the material is to purchase it online.
Step 2- Scoop the sodium acetate and place it in a pan. It will be in powder form in most cases but at times it will be gel-like as it has just been removed from the pan.
An approximate of a cup of powder would be good and leave some of the powder out of the pan in order that it can be used as a seed crystal later.
Step 3- Add enough water onto the pan so that the sodium acetate will dissolve.
Do not add too much water onto the pan as you will need to supersaturate the sodium acetate water solution.
So the less amount of water added will result to a more dense solution and better crystal formation.
Step 4- Now you will need to dissolve the sodium acetate thirhydrate crystals (as much as possible) in hot (almost boiling) water.
Stir the mixture constantly resulting the powder to dissolve into a liquid.
There should be a bit of the powder left in the end. This is the undissolved powder left at the bottom of the pan.
It is essential and a must that the solution be stirred at this point and you will need to add the powder solution as much as possible.
Step 5- After that you will need to pour out the solution into a glass beaker (of your choice).
It is required that the undissolved powder does not enter the glass beaker and that it remains at the bottom of the pan.
History
Since the discovery of Sodium acetate was probably an accident it would be difficult to pin point the exact date, location, person and time as per its invention. The best guess is that its discovery was made in ancient times by someone who mixed ashes from a fire with vinegar by accident.
The acetic acid or vinegar was what led to the discovery of the first know to be Hot ice. When vinegar mixed with the ashes it helped prepare leather. This solution was know as sodium acetate.
Sodium Acetate Trihydrate
Hot Ice also known as Sodium Acetate Trihydrate is a chemical which can be prepared from substances used in everyday cooking.Vinegar and baking soda are the two components that combine together to form the substance known as Sodium acetate.This substance is know as 'Hot Ice' as it somewhat resembles 'water ice' or solidified water and due to the generation of heat when it crystallize.
It is known as Hot ice as it is in a solid state but like no other this type of ice is generates out heat waves.
Sodium Acetate Thihydrate is a white crystalline at room temperature and melts into a liquid form at 324 degrees Celsius. The boiling point of hot ice is 881.4 degrees Celsius and its density is 1.53g/cm3. Sodium acetate trihydrate has a molar mass of 82.0343g/mol
You can super-cool sodium acetate or hot ice in order for it to remain in a liquid state below its melting point. The crystallization can be activated on command, thus forming sculptures as the liquid solution solidifies.This reaction is exothermic hence heat is generated from the hot ice.
Hot Ice has multiple names. There are various ways of saying it.
The IUPAC name for is Sodium Acetate.
The Systematic name for is Sodium Ethanoate
The Other names are Hot ice or Sodium Acetate Trihydrate
The Chemical Formula for Sodium Acetate Trihydrate is C2H3NaO2.
Sodium Acetate abbreviated as NaOAc, also known as Sodium Ethanoate is the sodium salt of acetic acid.
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