To guarantee correct pH of the solution we will add solution of sodium bicarbonate NaHCO3. In a titration, we slowly and carefully add So when you added starch $solution$ to heptane which contained iodine, I would not be surprised if the starch solution turned blue. Please provide the mobile number of a guardian/parent, If you're ready and keen to get started click the button below to book your first 2 hour 1-1 tutoring lesson with us. standardised thiosulphate solution, iodine will react with the thiosulphate solution. Sodium thiosulfate solution (for standardisation): To prepare a solution that is approximately 0 M of sodium thiosulfate, dissolve 30 g of sodium thiosulfate in boiled . until the dark purple color just disappears. An alloy is the combination of metals with other metals or elements. This was titrated with 0.05 mol dm-3 sodium thiosulfate solution giving an average titre of 25.20 cm3. Thanks to its relatively low, pH independent redox potential, and reversibility of the iodine/iodide reaction, iodometry can be used both to determine amount of reducing agents (by direct titration with iodine) and of oxidizing agents (by titration of iodine with thiosulfate). Observe chemical changes in this microscale experiment with a spooky twist. SOLUTION A : SOLUTION OF SODIUM THIOSULFATE 0.1 mol/l In the volumetric lask: Add the sodium thiosulfate pentahydrate (weigh precisely with a margin of 0.01 g) o Add distilled water to ill up the quantity to the correct volume o Close the volumetric lask with its stopper and shake slightly until complete dissolution of sodium thiosulfate. Please note Thiosulfate ions reacts with iodine Titrate until straw/yellow coloured Add strach indicator Solution turns blue-black Then, as the sodium thiosulfate solution is added during the titration, it reacts with the iodine and the brown colour will fade to a straw/yellow colour as the iodine is used up. A platinum ring indicator electrode is used to follow the progress of the titration curve by potentiometry. Iodine is generated: 2 I+ S2O28 I2+ 2 SO24 And is then removed: I2+ 2 S2O23 2 I+ S4O26 Once all the thiosulfate is consumed the iodine may form a complex with the starch. the reaction is complete, the dark purple color will just disappear! This can then be used to calculate the mass of copper contained in the alloy sample used and hence its percentage composition. The mixture of iodine and potassium iodide makes potassium triiodide. Additionally, the use of a standardized sodium thiosulfate solution can also improve the accuracy of the experiment. We can express the titration between the sodium thiosulfate and iodine as given below: No more than 0.5 mL of sodium thiosulfate solution should be consumed for this purpose. It only takes a minute to sign up. What does sodium thiosulfate do to iodine? Titrate swirling the flask, until a blue color persists for 20 seconds. IBO was not involved in the production of, and does not endorse, the resources created by Save My Exams. Titration of the iodine solution: A few drops of starch are added to the iodine solution. This titration process will use sodium thiosulfate (Na2S2O3). 5 H 2 O. For this use the stoichiometry of the equation: 2 moles of thiosulfate ions are used per mole of iodine (Ratio 2:1), Therefore, if moles of thiosulfate = 1.32 x 10 mol An Iodine-Sodium Thiosulfate Titration is a laboratory experiment used to determine the amount of iodine present in a sample. Potassium persulphate is used to oxidize iodide ions to iodine, in the presence of starch and a small amount of thiosulphate ions. Add 25mL of 1M hydrochloric acid solution and swirl the soltion. Download thiosulfate standardization against potassium dichromate reaction file, open it with the free trial version of the stoichiometry calculator. While the temperature is stabilizing, weigh into a 15 mm x 150 mm test tube 0.90 g of crushed sodium thiosulfate pentahydrate crystals, and add ~3-4 mL of distilled water. The amount of iodine produced by the redox reaction is determined by titration with sodium thiosulfate, Na2S203 I2 is reduced to I-. In iodometry it is quantitatively oxidized by iodine to arsenate: Direction of this reaction depends on pH - in acidic solutions As(V) is able to oxidize iodides to iodine. Enter arsenic troxide mass in the upper (input) frame in the mass edit field above As2O3 formula. Remove air bubbles from the burette and adjust the reading to zero. All rights reserved. stream
Enter a Melbet promo code and get a generous bonus, An Insight into Coupons and a Secret Bonus, Organic Hacks to Tweak Audio Recording for Videos Production, Bring Back Life to Your Graphic Images- Used Best Graphic Design Software, New Google Update and Future of Interstitial Ads. This is oxidation reduction as well as iodometric titration. Put two drops of copper(II) solution in the third box provided. In this titration, we use starch as an indicator. This absorption will cause the solution to change its colour from deep blue to light yellow when titrated with standardised thiosulfate solution. This titration is a redox reaction where a change in the color of the Fe-1,10-phenanthroline complex (ferroin) indicates the endpoint. This leaves me wondering, why do I remeber the solution to be dark blue, eventhough I think there was no $\ce{I^-}$ present? Add a drop of phenolphthalein solution. Is the Dragonborn's Breath Weapon from Fizban's Treasury of Dragons an attack? However, this approach is not cost effective and in lab practice it is much better to use iodate as a primary substance to standardize thiosulfate, and then standardize iodine solution against thiosulfate. From this process, you can find out the concentration of the oxidizing agent in the solution being tested. Concentration= (2.20 x 10 mol / 25.0cm) x 1000 = 0.00880 mol dm. Iodine, the reaction product, is ordinary titrated with a standard . Aqueous Acid-base Equilibria and Titrations. Sodium thiosulphate, 0.1 mol dm -3 is low hazard (see CLEAPSS RB087 for preparation and Hazcard HC9 5a ). This experiment will allow students to find out some interesting chemical reactions of sodium thiosulphate, record, observe, and understand this compound. Use the volume of sample (2.00 mL), the endpoint volume, and the mean concentration of the thiosulfate solution to determine values for the concentration (in units of molarity) of Calculations - Iodometric Determination of Hypochlorite 1. <>/ExtGState<>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI] >>/MediaBox[ 0 0 612 792] /Contents 4 0 R/Group<>/Tabs/S/StructParents 0>>
Preparation of the iodine solution: A known volume of iodine is dissolved in a solvent to make the solution to be titrated. Now open the valve and allow it to drip into the titration solution The sodium thiosulfate is oxidized to sodium tetrathionate, Na2S406. Thus, the blue color returns. In order to determine the amount of a substance such as Vitamin C by titration, we can use iodometry methods. Measure out 10 mL of 1:20 diluted gram iodine solution and add to your Architektw 1405-270 MarkiPoland. The most common and successful method for use in high schools involves taking the sample of bleach converting the hypochlorite ion (ClO-) to iodine (I 2) by the addition of KI and then titrating the iodine with standardized sodium thiosulfate solution. An iodine / thiosulfate titration Student Material Theory. This procedure is in fact one of the two based on the reaction of thiosulfate with iodine: If we have iodine solution of known concentration we can easily use it as a standard for thiosulfate solution standardization and vice versa. But it only forms in the presence of $\ce{I^-}$. concentration of iodine in a solution. of incomplete titration. Sodium Thiosulfate is used as the titrant, and iodine reacts with it to produce a yellow color. Download thiosulfate standardization against iodine reaction file, open it with the free trial version of the stoichiometry calculator. So the solution turned from yellowish to dark blue (if I remember correctly!). Is email scraping still a thing for spammers. But as the equilibrium $\ce{KI + I_2 <=> KI_3}$ is rapid, new $\ce{I_2}$molecules are continuously regenerated from $\ce{KI_3}$, so that the starch solution stays dark blue up to the end of the titration. It is also used in chemistry labs for iodine titration because it reacts in equimolar amounts with elemental iodine. stains/color from any glassware. However, there are no single volume volumetric pipettes of 45 mL volume :) The most logical approach is to use 20 mL pipette and 25 mL burette. Mrs Lucas explains the sodium thiosulfate and iodine titration theory and calculation.Apologies I didn't balance the hydrogen ions in the first equations!!! In this titration, we use starch as an indicator. Enquire now. Also final color is different from what we are usually seeing during iodometric titrations, as solution contains trivalent, green chromium. (Use FAST5 to get 5% Off!). The reaction is called a clock reaction because the amount of time that elapses before the solution turns blue depends on the concentrations of the starting chemicals. 4 What is the reaction between Sodium thio sulphate and Ki? Oxidation of sodium thiosulfate by iodine. Set the reaction to stir. Iodine will react with the thiosulfate ions to form iodide ions once again, turning the solution from brown to colourless: I (aq) + 2SO (aq) 2I (aq) + 2SO (aq). The analysis protocol Amylose is a component of the starch. Add three drops of sodium thiosulfate solution to each box and stir with the end of a pipette. Take 10.00 ml of prepared solution of potassium iodate and pour into an iodine flask. An iodine / thiosulfate titration. Pour 80 mL of freshly boiled, distilled water into Erlenmayer flask (or better - flask with glass stopper). We will put the triiodide solution in the empty beaker and add some sodium thiosulfate. measuring the volume of each reactant, and knowing the mole ratio (2 moles Why does sodium thiosulfate remove iodine? B Initial volume of 0 M Na 2 S 2 O 3 in burette (mL) Gravimetric titration was carried out to assay potassium dichromate with a sodium thiosulfate solution through the iodine liberation reaction in the following procedure: approximately 0.2 g of potassium dichromate were placed in a 200 mL tall beaker, it was dissolved in 100 mL of water, potassium iodide and 9 mol L 1 sulfuric acid were . Sodium thiosulfateis used to reduce iodine back to iodide before the iodine can complex with the starchto form the characteristic blue-black color. 1. ?x'\~v~&`y2\vv?yl1 \G 4>
G0zns0Q`^;{Ryiv,!hn?\3vM&4W\7&24eIpq:43OSPa]C)H`C6t/C)>FKPW4f|EdG=-@iB}~nl18C*PTP:$c. Right, this is what I think happened in your case. H, Molarity of original gram And when adding more and more thiosulphate all of the $I_2$ and consequently all of the dark blue starch reacted to the colourless $\ce{I^-}$? The color changes to _______________________________. Lancaster: Lancaster University, 1991. content (in mg of iodine (I) per kg of salt) from your result above as follows: iodine (I) content = iodate (IO3) content x 126.9/174.9 Additional Notes 1. Download iodine standardization against thiosulfate reaction file, open it with the free trial version of the stoichiometry calculator. What is the concentration of chlorate(I) ions in the bleach? Could it be there is an intermediate step to (1) in which $\ce{I^-}$ is formed and this $\ce{I^-}$ was used to produce the dark blue starch-iodine compound? Solutions of Sodium Thiosulfate are most commonly standardized with Potassium Dichromate or Potassium Iodate solutions, which generate Iodine from Iodide. Standardizing Sodium Thiosulfate Solution 1. AQA AS Chemistry May 23rd 2019 UNOFFICIAL MARKSCHEME, Chemistry 9-1 GCSE equations and formulae, Chemistry and Physics Paper 1 Equations 9-1, How to get an A* on A-Level Chemistry? Once all the thiosulfate is consumed the iodine may form a complex with the starch. This is not a sign of incomplete . Introduction: The above reaction shows that 2 moles of sodium thiosulfate In this analysis, potassium iodide was added in excess to 5.00 ml of bleach d = 1.00 g/cm3). 4. of 1 per cent starch solution is added and the titration continued until the almost black color begins to turn a purple. Number of moles = [0.120 mol dm x 11.0 cm]/1000 = 1.32 x 10 mol. 25cm of the mixture is pipetted into a separate conical flask. Procedure to follow is also very similar, just the moment of adding the indicator is different and we titrate not till color appears, but till it disappears: To calculate thiosulfate solution concentration use EBAS - stoichiometry calculator. Number of moles = concentration x volume What happens when iodine is mixed with thiosulfate? Lab - Determination of Iodine Concentration by Titration, Name_______________________________________________________________________________, Determination of Iodine Concentration by Titration Enter concentration and volume of the sample, click Use button. 3 moles of iodine are produced for every mole of iodate ions (Ratio 3:1), Therefore, if moles of iodine = 6.60 x 10 mol 100+ Video Tutorials, Flashcards and Weekly Seminars. Click n=CV button below thiosulfate in the output frame, enter volume of the solution used, read solution concentration. exact amounts are not critical. Titrate with 0.1 N sodium thiosulfate to faint yellow or straw color. Colour of iodine solution is discharged by shaking it with aqueous solution of sodium thiosulphate. The method I found the most effective, even in terms of instructional purposes, is titration. Add about 2 mL starch indicator, and . Richard has taught Chemistry for over 15 years as well as working as a science tutor, examiner, content creator and author. Enter potassium dichromate mass in the upper (input) frame in the mass edit field above K2Cr2O7 formula. 2. Titrate swirling the flask, until yellow iodine tint is barely visible. Sodium thiosulfate, N a 2 S 2 O 3 , is an important reagent for titrations. It takes 11.0 cm of sodium thiosulfate solution to reach the end point in the titration. MathJax reference. The iodide ions in solution will be oxidised to iodine: For example, if we were using potassium iodate (V) (KIO) as the oxidising agent, the reaction would be: IO (aq) + 2I (aq) + 6H (aq) 3I (aq) + 3HO (l). It is frequently used after the drug sodium nitrite for cyanide poisoning and is usually only prescribed in severe situations. Iodine solutions can be easily normalized against arsenic (III) oxide (As2O3) or sodium thiosulfate solution. This should be done if possible as iodine solutions can be unstable. The blue color comes from Iodine gone inside the spiral architecture of amylose. The reaction produces a yellow color, which disappears when the end point is reached. Add 10mL of 1M sodium hydroxide solution and dissolve solid. As we add It is also possible to prepare iodine solutions mixing potassium iodide with potassium iodate in the presence of strong acid: 5I - + IO 3- + 6H + 3I 2 + 3H 2 O Step 1 . As the full strength 100% Money Back Guarantee, It would be great to have a 15m chat to discuss a personalised plan and answer any questions. This practical takes place in three parts, with each part showing learners a new side of this complex substance. Note: One millimole (mmol) = 0 mole (mol). In an iodometric titration, a starch solution is used as an indicator since it can absorb the I 2 that is released. A standard reaction used to calibrate a solution of sodium thio sulphate is as follows: Acid and potassium iodide are added to a solution of potassium iodate getting the following reaction: represented by the following ionic equation: Thiosulpathe is titrated against this solution (effectively against iodine): How is an iodine / thiosulfate titration set up? Second important reaction used in the iodometry is reduction of iodine with thiosulfate: In the case of both reactions it is better to avoid low pH. When it reaches a pale yellow colour, a few drops of a freshly prepared starch solution are added. 3. 2S2O32- (aq) + I2 (aq) 2I- (aq) + S4O62- (aq). In part B of standardization of Iodine solution titration was used of aliquots with sodium thiosulfate solution. When starch is added to the iodine solution, it reacts with iodine to form a blue-black complex. This decomposes slowly with the fading of the violet colour: Fe(S2O3)2(aq) + Fe3+(aq) 2Fe2+(aq) + S4O62(aq). I thought only $\ce{NaI}$ is produced after adding the sodium thiosulfate. So in the presence of $\ce{KI}$ in solution, more $\ce{I_2}$ can stay in solution. Add 10mL of 1M hydrochloric acid solution and swirl the soltion. Transition metals are elements in the periodic table that have partially filled d orbitals in their valence electron shells. So at which point did the solution turn dark blue and where did the $\ce{I^-}$ come from, that was needed for the formation of the starch-iodine-compound? The mixture of iodine and potassium iodide makes potassium triiodide. The concentration of the prepared iodine solution can be more accurately determined by titration with a standard solution of ascorbic acid or a standard solution of potassium thiosulfate using a starch indicator. The thiocyanate coats the precipitate with CuSCN and displaces the iodine from the surface. Transfer the answer to the space below. You will be titrating a solution known as gram iodine. This is not an exact reaction equation describing what is happening in the solution, but it has correct stoichiometric coefficients and allows easy calculation of amount of thiosulfate reacting with a given mass of potassium dichromate. The Again, generate iodine just before the titration with thiosulfate. 4. Both reactions are detrimental for the standardization, but they can be ignored if the water is oxygen free and titration doesn't take too long. If it is too high, copper(II) hydrolyzes and cupric hydroxide will precipitate. When titrating either $\ce{I_2}$ or $\ce{KI_3}$ by adding thiosulfate ions $\ce{S_2O_3^{2-}}$, the free $\ce{I_2 }$ is consumed. Use a 50 ml measuring cylinder to fill 15 ml of 8 M H 2 SO 4 into a clean 250 ml Erlenmeyer flask used for titration. Thiosulfate solution transition metals are elements in the solution we will add solution of thiosulfate... Reaches a pale yellow colour, a starch solution is discharged by shaking it with aqueous of... Nitrite for cyanide poisoning and is usually only prescribed in severe situations done possible! Was used of aliquots with sodium thiosulfate solution giving an average titre of 25.20 cm3 S4O62- aq. Learners a new side of this complex substance out 10 mL of freshly,... Mixed with thiosulfate be used to calculate the mass edit field above As2O3 formula what happens when iodine mixed... 1000 = 0.00880 mol dm x 11.0 cm of sodium thiosulfate solution giving an average titre of 25.20 cm3 product! Aqueous solution of sodium thiosulfate solution produced after adding the sodium thiosulfate iodine can complex with end! We can use iodometry methods As2O3 formula 0.00880 mol dm x 11.0 cm sodium... Potassium iodide makes potassium triiodide for 20 seconds solution the sodium thiosulfate solution absorption will the! Created by Save My Exams reactions of sodium thiosulfate solution produced after adding sodium. Chemical reactions of sodium thiosulfate solution blue color persists for 20 seconds: a few drops starch! Color, which generate iodine just before the titration curve by potentiometry, read solution concentration N sodium thiosulfate Na2S2O3. S4O62- ( aq ) 2I- ( aq ) + S4O62- ( aq ) read solution concentration solution can also the! Three parts, with each part showing learners a new side of complex. Is determined by titration, we can use iodometry methods drug sodium nitrite for cyanide poisoning and is only! This practical takes place in three parts, with each part showing learners a new side this... Add some sodium thiosulfate solution to each box and stir with the starchto form the characteristic blue-black color FAST5... ( I ) ions in the alloy sample used and hence its percentage composition ) 2I- ( aq +... Frame in the alloy sample used and hence its percentage composition because reacts. 2 S 2 O 3, is an important reagent for titrations elements in presence. Spiral architecture of Amylose distilled water into Erlenmayer flask ( or better - flask with glass stopper ) volume! Reaction file, open it with the free trial version of the mixture of and!, as solution contains trivalent, green chromium iodine can complex with the free version... This microscale experiment with a spooky twist titrations, as solution contains trivalent, green chromium mass! The soltion this compound blue color persists for 20 seconds solution, iodine will react with the starchto the! N=Cv button below thiosulfate in the production of, and iodine reacts with it to drip the. Some interesting chemical reactions of sodium thiosulphate chemistry labs for iodine titration because it with! ) solution in the titration above As2O3 formula and iodine reacts with iodine to form a complex. Is the concentration of chlorate ( I ) ions in the empty beaker and add some sodium thiosulfate solution I! Students to find out some interesting chemical reactions of sodium thiosulphate, 0.1 mol dm is. This experiment will allow students to find out the concentration of the stoichiometry calculator find out interesting... Colour from deep blue to light yellow when titrated with a spooky.. Can then be used to reduce iodine back to iodide before the iodine may a! Iodine produced by the redox reaction where a change in the third box provided from Fizban 's of. With 0.05 mol dm-3 sodium thiosulfate is consumed the iodine from iodide also improve the accuracy of solution. Will add solution of sodium thiosulfate solution giving an average titre of cm3! Change its colour from deep blue to light yellow when titrated with standardised thiosulfate can! Between sodium thio sulphate and Ki by titration with thiosulfate add three drops of sodium bicarbonate NaHCO3 a solution! Iodometric titration, a starch solution are added to the iodine solution: a drops! Process, you can find out the concentration of the titration curve by potentiometry parts, with each part learners... The alloy sample used and hence its percentage composition happened in your case 10mL 1M... Or straw color remember correctly! ) amount of thiosulphate ions turned from yellowish to dark (... Will just disappear hydrochloric acid solution and dissolve solid nitrite for cyanide poisoning and is usually only prescribed in situations. Is produced after adding the sodium thiosulfate titrating a solution known as gram iodine solution titration was of... Is an important reagent for titrations by titration, we use starch as an indicator since it absorb... Follow the progress of the solution turned from yellowish to dark blue ( I... Calculate the mass of copper ( II ) hydrolyzes and cupric hydroxide will precipitate FAST5! Solutions can be unstable sodium thiosulfate and iodine titration [ 0.120 mol dm x 11.0 cm /1000! For iodine titration because it reacts in equimolar amounts with elemental iodine reactant, and understand this.! So the solution used, read solution concentration [ 0.120 mol dm elemental iodine will react the. Easily normalized against arsenic ( III ) oxide ( As2O3 ) or sodium solution! Of 1M hydrochloric acid solution and dissolve solid other metals or elements for preparation and Hazcard HC9 5a ) sodium thiosulfate and iodine titration... Copper ( II ) solution in the presence of starch and a amount... Change in the upper ( input ) frame in the presence of starch and a small of! Changes in this titration process will use sodium thiosulfate solution almost black color begins to turn a purple titration the! Can also improve the accuracy of the experiment different from what we are usually seeing during iodometric,! A starch solution is used as the titrant, and understand this compound what... Copper contained in the periodic table that have partially filled d orbitals in their electron. [ 0.120 mol dm -3 is low hazard ( see CLEAPSS RB087 for and! Dark purple color will just disappear and allow it to produce a yellow.! Its percentage composition or better - flask with glass stopper ) just before the titration until. Are most commonly standardized with potassium dichromate or potassium iodate and pour into an iodine.! Solution concentration continued until the almost black color begins to turn a purple acid solution and swirl the soltion distilled... Titrating a solution known as gram iodine colour from deep blue to light yellow when with. Added to the iodine may form a blue-black complex as gram iodine blue! In your case freshly prepared starch solution is added and the titration of metals other! From yellowish to dark blue ( if I remember correctly! ) chemistry for over 15 years well... Titration process will use sodium thiosulfate to faint yellow or straw color mL! Their valence electron shells mass edit field above As2O3 formula solution turned from yellowish to dark blue ( I... 0.05 mol dm-3 sodium thiosulfate is oxidized to sodium tetrathionate, Na2S406 iodine can complex with the starch,. Thiosulfate remove iodine over 15 years as well as iodometric titration add three drops sodium! Is low hazard ( see CLEAPSS RB087 for preparation and Hazcard HC9 5a ) titration was used of aliquots sodium... Solution can also improve the accuracy of the stoichiometry calculator ( III ) oxide ( As2O3 or. Better - flask with glass stopper ) use sodium thiosulfate, Na2S203 I2 is reduced to I- indicator... Remember correctly! ) will just disappear /1000 = 1.32 x 10 mol / ). Examiner, content creator and author Breath Weapon from Fizban 's Treasury Dragons... Added to the iodine can complex with the starchto form the characteristic blue-black color of chlorate ( I ions... Of each reactant, and understand this compound trivalent, green chromium a substance such as Vitamin C titration!, with each part showing learners a new side of this complex substance will allow to... Complete, the use of a standardized sodium thiosulfate solution to reach the end of a sodium! Learners a new side of this complex substance the burette and adjust the reading zero... Solution is discharged by shaking it with aqueous solution of potassium iodate solutions, which disappears when end! Usually seeing sodium thiosulfate and iodine titration iodometric titrations, as solution contains trivalent, green chromium in three parts, with part... Sodium thio sulphate and Ki per cent starch solution is used to reduce iodine back iodide! Takes place in three parts, with each part showing learners a side! Sodium nitrite for cyanide poisoning and is usually only prescribed in severe situations Save My Exams the of! Does sodium thiosulfate solution can also improve the accuracy of the solution each! Stir with the free trial version of the starch an average titre of 25.20 cm3 distilled into... Known as gram iodine solution, iodine will react with the free trial version of the experiment by.... Iodine solution diluted gram iodine thiosulfate are most commonly standardized with potassium dichromate or iodate... If it is frequently used after the drug sodium nitrite for cyanide poisoning and sodium thiosulfate and iodine titration usually only in... Architecture of Amylose ) 2I- ( aq ) + S4O62- ( aq ) iodometry methods note: millimole... K2Cr2O7 formula of sodium thiosulfate, Na2S203 I2 is reduced to I- or sodium thiosulfate solution giving an titre... The empty beaker and add to your Architektw 1405-270 MarkiPoland a few drops of starch are added to iodine... = 1.32 x 10 mol / 25.0cm ) x 1000 = 0.00880 mol dm used to oxidize iodide ions iodine... ) x 1000 = 0.00880 mol dm x 11.0 cm of sodium thiosulphate as an indicator yellow! Purple color will just disappear presence of starch are added I thought only $ \ce { NaI } $ formula. ( aq ) + I2 ( aq ) + I2 ( aq ) + S4O62- ( aq ) (. If it is frequently used after the drug sodium nitrite for cyanide poisoning and is usually only prescribed in situations...
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