Purpose: The purpose of this experiment is to determine the molarity of a permanganate solution through the use of redox titration. Theory: The following are the reactions that take place in the experiment: Unbalanced: H2C2 O4 (aq) + MnO4- (aq) CO2 (g) + Mn2+(aq) H2C2 O4 Half-Reaction: H2C2 O4 (aq) 2CO2 (g) + 2e- + 2H+(aq) MnO4- Half-Reaction: 8H+ + 2MnO4-(aq) + 5e- Mn2+(aq) + 4H20 (l) Net Reaction: 5H2C2 O4 (aq) + 6H+ + 2MnO4- (aq) 10CO2 (g) + 2 Mn2+(aq) +8H20 (l) The solution was heated in order to reach better reaction rates, since the reaction occurs slowly at room temperature. Unlike many other titrations no indicator is necessary to tell the experimenter when the endpoint of the reaction is. In this case, the experimenter knows when all the oxalate has been consumed because the excess of permanganate will show up as a pink color. Thus, the permanganate ion acts as an indicator itself. The reaction produces its own catalyst in the form of Mn2+ that promotes oxidation. The sulfuric acid added to the titration flask acts as a proton donor for the solution readily giving up protons. Since the oxalic acid is not a strong acid and does not dissociate well, but is still needed in the reaction to form carbon dioxide, the addition of a strong acid, sulfuric acid, supplies the protons needed for the reaction. Procedure: Obtain and zero two burets, one containing .0500M oxalic acid and the other containing the permanganate solution. Next, add 25.00mL of the oxalic acid into a 250mL Erlenmeyer flask (using the bottom of the meniscus for measurements). Then proceed to measure and add 15mL of 3M sulfuric acid to the titration flask with a graduated cylinder. Heat the titration flask to a temperature of 80C. Titrate the contents of the flask with the permanganate solution. Swirl the contents of the flask after adding the permanganate and if the solution drops below 80C heat the flask back up to 80C. Use the top of the permanganate solution to take measurements rather than the bottom of the meniscus. Add just enough permanganate to turn the contents of the flask a light pink color. At this point record the volume of the permanganate solution used. Rinse the titration flask with distilled water and run the experiment one more time. Data: Quantitative: (Trial One): 1. Volume of .0500M Oxalic Acid (H2C2 O4 (aq)) 25.00mL 2. Volume of Permanganate Solution (MnO4- (aq)) 24.55mL 3.
This yellow species can then be measured using UV absorbance (max abs = 420 nm), and thus the concentration of the can species determined.1 Horseradish peroxidase in important in the glucose assay because it catalyzes a reaction that includes one of the products from the glucose oxidase reaction, H2O2. There will be one H2O2 produced for every oxidized B-D-glucose, which will then be used to oxidize one ferrocyanide into the one measurable ferricyanide. Therefore, using the enzymes glucose oxidase and horseradish peroxidase in a consecutive manner, users can determine the concentration of glucose present in solution by simply measuring the amount of ferricyanide produced because of it (this is a one to one ratio).
Record the volume of the sodium thiosulfate solution used in the titration, and repeat the procedure in a duplicate titration.
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
Planning Firstly here is a list of equipment I used. Boiling tubes Weighing scales Knife Paper towels 100% solution 0% solution (distilled water) measuring beakers potato chips Cork borer. We planned to start our experiment by doing some preliminary work. We planned to set up our experiment in the following way.
Objective: The objective of the experiment is to determine what factors cause a change in speed of a reaction. It is also to decide if the change is correlated with the balanced equation of the reaction and, therefore, predictable. To obtain a reaction, permanganate, MnO_4^(1-), must be reduced by oxalic acid, C_2 O_4 H_2. The balanced equation for the reaction is:
Measure the mass of calcium hypochlorite before freshly inserting it into the pool of water using a weight balance Concentration of sodium thiosulfate (0.01 M) If the concentration of sodium thiosulfate differs for each trial, the different concentrations may manipulate how much volume of the solution is used up to produce the change in color when it is titrated with hypochlorite and potassium iodate. Use the right sodium thiosulfate with the intended concentration and do not dilute or mix up the solution with other solutions during the experiment Concentration of potassium iodate (1 M) If the concentration of potassium iodate differs for each trial, the different concentrations may manipulate how fast the change in color would appear in Erlenmeyer flask when it is titrated against sodium thiosulfate Use the right potassium iodate with the intended concentration and do not dilute the solution with other chemical solutions during the
Plan 1. Collect 4 different sized beakers 2. Boil some water in the kettle 3. Pour 50ml into each beaker 4. After 1 minute check temperature 5.
The burette and pipette I’m going to be using should be rinsed out with the solutions they are going to contain. After filling the titrant solution, I have to check the tip of the burette for any air bubbles, if it contains air bubbles the volume readings will be incorrect. Always rinse out the conical flask with distilled water because normal tap water contains ions, this will affect my results. Tap water have chemicals while distilled water is deionized, this simply means there will be no ions.
Na2S203 (aq) + 2HCl (aq) -> 2NaCl (aq) + H20 (l) + SO2 (g) + S (s)
In a 250ml beaker place 100mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved. After 1 minute measure the temperature and record it, do this for a further 2 minutes (3 minutes in total). Repeat this process for a total of 10 teaspoons.
All things, living or nonliving, consist of atoms and molecules. These particles are constantly in motion, and this continuous motion allows for the disbursement of molecules, or diffusion. The overall net movement of these molecules will go from areas of higher concentration, to areas of lower concentration. Therefore, following a concentration gradient (Martini). The rate of diffusion of these molecules, in accordance with Fick’s law of diffusion, is directly proportional to the concentration gradient present. However, the concentration gradient is not static and will change over time and with distance, therefore changing the rate of diffusion. It is hypothesized that the two solutions being tested, Methylene Blue and Potassium Permanganate, will begin their initial diffusion in the agar gel at a quick rate, and then progressively regress over the allotted time of 1 hour. Another factors other that will have an effect on rate of diffusion is molecular size. There is a substantial difference in molecular weight between Methylene Blue (320 g/mol) and Potassium Permanganate (158 g/mol). The combined molecules present in Potassium Permanganate are lighter than those in Methylene Blue, and therefore should allow it to diffuse more rapidly.
Aim: The aim of this experiment was to determine the empirical formula of magnesium oxide.
Complexometric Titrations [homepage on the internet]. No date. [ cited 2014 Mar 20]. Available from: http://www.ciens.ucv.ve:8080/generador/sites/martinezma/archivos/EDTA.pdf
0.1M HCl, 10 mL of 0.1N KMnO4, 0.2 g. KI, 5 mL of alcohol, and 5 mL of
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).