Purpose:
By doing this experiment, students will properly complete a redox titration well also determining the amount of hypochlorite ions present in the commercial bleach given.
Introduction:
Commercial Bleach and other commercial products like hair colouring agents, contain oxidizing agents. Oxidizing agents are substances that remove electrons from one or more reactants and thereby oxidizes it, whereas reducing agents are substance that give electrons to other reactant. There is some reaction that are called oxidation-reduction reaction, theses reactions are commonly seen in our day to day lives. One example of an oxidization-reduction reaction is the production of iron oxide or what we know as rusting.
〖Fe〗_((s))+O_(2(g)) □(→┬ ) 〖Fe〗_2 O_(3(g))
In the rusting reaction iron is being reduced, and the oxygen is being oxidized. The most common oxidizing agent in bleaches from our experiment is sodium hypochlorite. The bleach that was used in this experiment was made by bubbling chlorine into the hydroxide solution. Some of the chlorine is converted to the hypochlorite ion but there is also some that turns from gas to aqueous. The chemical equation for this processes is as follows: 〖Cl〗_2(g) …show more content…
Dilute the 5mL of bleach by added DI water (deionized water) till the indicated mark. Make sure to invert the volumetric flask at least ten times this will insure that the solution is fully mixed. Weight out approximately 1g solid KI. Use a pipet to obtain and transfer 25mL of diluted bleach into an Erlenmeyer Flask, also add the solid KI and about 25 mL of DI water. Swirl the flask to make sure the KI is dissolved. Take your flask to the fume hood and add approximately 2mL of the 3M HCl, the solution should turn a red-brown colour. Now titrate with a standard 0.100M sodium thiosulfate solution until the colour becomes a
By doing this experiment, students will properly complete a redox titration well also determining the amount of hypochlorite ions present in the commercial bleach given.
Introduction:
Commercial Bleach and other commercial products like hair colouring agents, contain oxidizing agents. Oxidizing agents are substances that remove electrons from one or more reactants and thereby oxidizes it, whereas reducing agents are substance that give electrons to other reactant. There is some reaction that are called oxidation-reduction reaction, theses reactions are commonly seen in our day to day lives. One example of an oxidization-reduction reaction is the production of iron oxide or what we know as rusting.
〖Fe〗_((s))+O_(2(g)) □(→┬ ) 〖Fe〗_2 O_(3(g))
In the rusting reaction iron is being reduced, and the oxygen is being oxidized. The most common oxidizing agent in bleaches from our experiment is sodium hypochlorite. The bleach that was used in this experiment was made by bubbling chlorine into the hydroxide solution. Some of the chlorine is converted to the hypochlorite ion but there is also some that turns from gas to aqueous. The chemical equation for this processes is as follows: 〖Cl〗_2(g) …show more content…
Dilute the 5mL of bleach by added DI water (deionized water) till the indicated mark. Make sure to invert the volumetric flask at least ten times this will insure that the solution is fully mixed. Weight out approximately 1g solid KI. Use a pipet to obtain and transfer 25mL of diluted bleach into an Erlenmeyer Flask, also add the solid KI and about 25 mL of DI water. Swirl the flask to make sure the KI is dissolved. Take your flask to the fume hood and add approximately 2mL of the 3M HCl, the solution should turn a red-brown colour. Now titrate with a standard 0.100M sodium thiosulfate solution until the colour becomes a