Synthesis of bromine using only standard chemicals

Bromine is a chemical which is considered very cool by many home chemists. Due to its toxic and corrosive nature, however, this is a hard to obtain chemical and no chemical supply house is willing to sell this to private persons.

    

Bromine can be made fairly easily. Many synthesis methods have been presented already and most of these work well. But all of these syntheses require the use of large quantities of non-OTC chemicals. Even chemicals like sulphuric acid may be hard to obtain in some countries. The synthesis in this webpage only requires very easy to obtain chemicals. The only special chemical needed in this synthesis is potassium dichromate or potassium chromate, but this only is required in very small quantities.

The method, presented here, allows one to make approximately 20 ml of bromine from 100 grams of sodium bromide. No strong acid like sulphuric acid is needed and no strong oxidizer is needed. Oxidation is done by means of electrolysis.

 

Required chemicals:

  • sodium bromide (brominator for swimming pools)

  • sodium bisulfate (pH-minus for swimming pools)

  • any soluble chromate, dichromate or chromic acid a few 100's of mg

The chromium compound is needed to increase the efficiency of the electrolysis process. Without the chromium compound it also works, but a lot of time is needed for the electrolysis. The presence of a small amount of chromate or dichromate prevents the back-reduction of bromine and/or bromate at the cathode.

Required equipment:

  • power supply (12 V ... 15 V, capable of delivering a few ampere)

  • graphite rods (from big battery or welding rods)

  • simple glass jars and bottles

  • glass funnel (plastic is corroded by bromine)

  • pipette for sucking bromine from bottle, or a separating funnel

  • a good bottle for storing the final product

Safety:

  • bromine is very toxic and very corrosive.

Disposal:

  • Besides the 20 ml of bromine, approximately 600 ml of bromine water is produced, which contains another 15 grams of bromine. By means of distillation it is possible to recover this bromine as well, but this is a lot of work. The bromine water is impure, contains a small quantity of chromium(VI) and fine particles of graphite. Easiest way to get rid of it is adding 20 grams of potassium metabisulfite or sodium metabisulfite (used for disinfecting wine bottles and available OTC as well). The bromine and the hexavalent chromium are reduced by this. The final liquid can be flushed through the toilet. It should have a gray or green color.

 

 

 

 

 

Preparation of cell

No special apparatus is needed for the cell. A 500 ml glass food jar with a plastic cap is perfectly suitable. These are present as waste in most households (e.g. from sauces, marmalade, or pickled gherkins).

Take approximately 100 grams of sodium bromide and add 300 warm water. The water can be plain tap water. Dissolve all of the sodium bromide. The result is a little bit more than 300 ml of colorless liquid.

Drill or cut two holes in the cap of the jar, such that two graphite rods can be pushed through these holes. No tight fit is needed, the cell will be operated such that hardly any fumes are produced.

 

    

The cell as displayed can be used, but the result is far from optimal. After an initial nice start the efficiency of the cell drops sharply and at the end its efficiency almost drops to 0. Bromine is produced at the anode and in the cell liquor this is converted to bromate, but at the cathode a large part of the bromate is reduced back to bromide. If a few 100's of mg of hexavalent chromium is added, then the cell works much better.

Dissolve half a gram of potassium chromate or dichromate in a few ml of water and add this to the cell liquid (sodium (di)chromate can also be used). This is the only non-OTC compound, which may be hard to obtain. Making a few 100's of mg of this in an impure state is not that difficult though (e.g. from pottery grade green chromium oxide, or from chrome alum and hydrogen peroxide).

Wrap the graphite rods above the cap of the jar in paper or plastic and fix them, such that the cell becomes mechanically stable and no accidental short circuit can occur when the jar is carefully moved around. How this is done is not really important. In this setup some toilet paper was wrapped around the rods and some paper was wrapped around the total of rods and paper and crocodile clamps were used to fix the whole construction (see further below on pictures of the cell).

 

 

Preparation of circuit

The cell should not be connected directly to a constant voltage power supply. Using such a supply leads to fairly strong variation in the cell current during operation of the cell. For this experiment it is important that the cell current is fairly constant. A nice value for the current is somewhere between 1 and 2 A. With such a current the cell needs to be operated for one or two days. In order to achieve a fairly constant current, a series resistor must be used and the following circuit must be created.

     

The DC power supply can be anything from 12 to 15 volts. The resistor R can be anything from 5Ω to 10Ω. The resistor must be a big power resistor, it becomes VERY hot. Use 25 Watt power resistors and if a single resistor becomes too hot, then use a series connection of multiple resistors, such that the heat is divided over multiple resistors.

The practical implementation of this circuit is shown below:

   

The power supply is a 13.8 V power supply and the resistors are two pieces of 3.9Ω switched in series, so the total resistance is 7.8Ω. There is nothing special about this value of 7.8Ω. These two 3.9Ω resistors just happened to be available in my home lab. If resistors must be purchased for this experiment, then it is suggested to buy 8 pieces of 1Ω/10W and connect all of these in series. Such ceramic power resistors are cheap and will not cost more than a few tens of cents per piece.

Keep in mind that during operation of the cell these resistors will become VERY hot, even if 8 resistors are put in series!

 

 

Operation of circuit

Now, the cell must be operated for a certain amount of time. Switch on the cell and allow it to run for an hour or so, such that it stabilizes. After that hour measure the voltage across the resistor or series connection of resistors. Compute the current from the measured voltage and the total resistance. In my particular case, the measured voltage was 9.5 volts and the total resistance was 7.8Ω. This means that the cell runs at 1.2 A.

The cell must operate for a certain amount of time, but not for too long. In theory, the total running time of the cell should be as follows:

     T = F*M/I

Here F is Faraday's constant which is 96485 C/mol

M is the number of moles of sodium bromide. When exactly 100 grams of NaBr were used, then M is 100/(22.99+79.90) = 0.972.

I is the cell current. In my particular cell this is 1.2 A.

So, the total running time for my cell should be 96485*0.972/1.2 = 78153 seconds. This is almost 22 hours.

In practice, the cell efficiency is not 100%, due to back reduction at the cathode. Without added hexavalent chromium the cell efficiency is very low (maybe just a few percents), but with added hexavalent chromium the cell efficiency usually is better than ⅔.

Overrunning the cell leads to losses, but underrunning the cell leads to much larger losses. If the cell is overrun for 50%, then still 90% of bromide is converted to bromine. Even if the cell is overrun for 100% (twice as much oxidation as optimal) still 80% of bromide is converted to bromine. Even small underrunning leads to catastrophic losses. So, just to be sure that the cell is not underrun, the cell is allowed to run for 1.5 times the theoretically computed time. So, for any practical purpose use the following formula for the cell running time:

     T = 1.5 * F * M / I

In my particular setup, the cell running time was 33 hours.

After a few hours of running, the cell liquor becomes turbid and black crud collects at the bottom, due to loss of graphite from the anode.

   

 

At the end of the running time, the liquid has become very dark and a lot of black particles are floating around in the liquid.

   

 

During the running time of the cell the liquid only becomes luke warm and hardly any bad fumes are produced. This cell can be operated inside without any problem as long as the cell current is not much more than 1 A.

 

 

Creation of bromine

After running the cell for sufficient time (see above) the liquid ideally contains 1 bromate ion for each 5 bromide ions. As indicated above, the cell is allowed to run for a longer time than theory predicts and usually it contains a little more bromate than the ideal ratio of 1 : 5. This, however, is not a real issue, it only leads to marginal losses.

Bromine now can be created, simply by adding acid. An acid, which is available OTC and which is sufficiently strong is so-called pH-minus for swimming pools. This is technical grade sodium bisulfate.

For each gram of sodium bromide take 1.5 grams of sodium bisulfate. In my particular experiment with 100 gram of sodium bromide, 150 grams of sodium bisulfate was used. This material was put in another jar.

     

Dissolve the sodium bisulfate in as little as possible of tap water. In my particular experiment, almost 300 ml of solution was obtained.

Filter the contents of the cell, such that most of the graphite crud is left behind in the filter. The resulting liquid is fairly clear.

             

 

Pour the solution of sodium bisulfate in the bottle with the filtered cell liquid. Do this outside! Lots of vapor of bromine will be produced in this step. Do not pour the solution of sodium bisulfate in the liquid at once but do this in three steps of appr. 100 ml. After each addition swirl the bottle with liquid, such that there is good mixing. The liquid heats up in this reaction, but if the addition is not done too fast, then the liquid will not become hot. After adding all solution of sodium bisulfate the liquid has become very dark and turbid, and there also is very dark vapor of bromine above the liquid. Do not open the bottle at this stage!

   

 

Allow this bottle with liquid and vapor to stand in a cool place. A good option is to put it in a bucket full of cold tap water for one hour. Lots of bromine droplets will collect at the glass above the liquid and a layer of bromine will settle at the bottom. After the hour of cooling, carefully swirl the liquid such that all droplets of bromine, which collect at the glass in the upper part of the bottle also are immersed in the liquid.

       

The pictures above show the bromine, settled at the bottom and the much lighter liquid above the bromine.

 

Finally, using a glass funnel, pour the liquid from the bottle, but keep the last 100 ml (which also holds the bromine). Pour the last 100 ml of liquid in a small bottle of 100 ml and use a pipette to extract the bromine from the bottom. Alternatively, pour the last 100 ml into a separating funnel and use that to separate the bromine from the other liquid. This final step must be done outside!

The final product is appr. 20 ml of bromine. This is displayed at the top of this webpage.

The bromine can be bottled like this, but it is better if it is dried and further purified. Drying and further purification, however, requires concentrated sulphuric acid and a distillation setup. For most experiments and many syntheses this crude bromine is perfectly suitable.

Total yield in this experiment is appr. 70% of all bromine. The remaining part is in the 600 ml of liquid and in the vapor above that.

 

 

Discussion of results

This synthesis of bromine is based on a very simple principle. Ideally for each bromide ion one electron is taken from the system, such that all bromide is converted to bromine. In practice, this is done through an intermediate step of formation of bromate.

In the electrolysis cell the following reactions occur:

At anode: 2Br 2e Br2

At cathode: 2H2O + 2e  2OH + H2

The hydrogen escapes as gas. The bromine dissolves in the liquid and reacts with the hydroxide, formed at the cathode as well:

   3Br2 +  6OH  5Br +  BrO3 + 3H2O

The reaction uses up exactly all bromine and hydroxide and the liquid does not become alkaline, nor does hardly any bromine vapor escape from the liquid.

For each 6 electrons, produced at the cathode (and absorbed at the same time at the anode), one bromate ion is produced. Ideally, after the electrolysis, 1/6 of all bromide is converted to bromate and the number of electrons needed for that is exactly the number of bromide ions in the cell when it is started. So, if 1 mole of NaBr is used initially, then 1 mole of electrons must be passed through the cell to convert 1/6 of all bromide to bromate.

 

Current efficiency

In an ideal cell, the above reactions are the only ones which occur. The net effect of these reactions is that for each mole of electrons supplied by the power supply 1/6 mole of bromate ion is produced and three molecules of hydrogen. If only these reactions occur, the cell efficiency is said to be 100%.

In a practical cell, there is back reduction of bromate at the cathode. Bromate again is converted to bromide and hydroxide is produced as well. This side reaction occurs instead of production of hydrogen gas and hydroxide ions. When this occurs, then the cell efficiency becomes lower. A lower cell efficiency means that less bromate is produced than what is expected on the basis of theory.

 

Production of bromine, effect of overrunning and underrunning the cell

The step of making bromine is based on the reaction between bromide and bromate in acidic solution:

     5Br +  BrO3 + 6H+  3Br2 + 3H2O

If exactly 1/6 of all bromide is converted to bromate, then all bromine in the liquid will end up as elemental Br2 when sufficient acid is added. Now suppose that there is a deviation from the ideal amount of bromate and that the total part of bromate is (1+ε)/6.

For positive ε the cell is overrun (too much bromate is formed). A cell, which is overrun for 50% has ε equal to . An overrun cell is not really bad, even very strong overrunning like 50% or even 100% only leads to moderate loss of bromine. The total amount of bromide is 1(1+ε)/6 = 5/6(1-ε/5). The bromide is the limiting reactant for positive ε and the ideal amount is 5/6 part. With positive ε the percentage of loss of bromine is only ε/5. So, for a cell which is overrun by 50% the loss only is 10% and for a cell which is overrun for 100% still the loss only is 20%.

If on the other hand the value of ε is negative, then the bromate is the limiting reactant. In that case, the relative loss is equal to ε. I.e. for a cell, which is only underrun for 10% there also is 10% loss of bromine and for a cell, which is underrun for 50% half of the bromine is lost. There also is another undesirable side effect when the cell is underrun. If not all bromide is used up, then the bromine is kept in solution and does not precipitate. Bromine dissolves quite well in a solution, which is rich in bromide:

     Br2 + Br  Br3

This equilibrium is quite strongly to the right. Bromine really dissolves quite well when bromide is present as well. In a cell, which is underrun by a factor ε, there is a relative loss of ε in terms of bromine production, but all non-converted bromine is present as bromide, holding back another 2ε of bromine molecules. So, in practice nearly 3ε is lost when precipitated bromine is isolated and bromine, dissolved in the large amount of water is not recovered. Only by means of leading air through the solution and condensing the bromine, taken with the air the 2ε part of the bromine can be taken out of the solution. So, underrunning the cell is very bad in terms of yield. Underrunning only 10% may lead to up to 30% additional loss, while overrunning 10% only leads to 2% additional loss. So, for this reason it is really important to assure that the cell is not underrun and take the slight loss of overrunning the cell for granted.

 

   

 

   

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