Lab Report on Volumetric Determination of Iron with Potassium Permanganate Principle: This experiment consists of titrating the ferrous ion with permanganate ion to study the oxidation-reduction reaction. The ions react in acidic solution to give ferric ion and a reduced ionic form of manganese. All the reactants and products except permanganate ion are weakly colored, whereas permanganate is a very intensely colored ion. Then a solution of permanganate is removed as long as there is a ferrous ion present to react with it. But as soon as the entire ferrous ion has been oxidized, the next small portion of added permanganate colors the solution. The first appearance of a permanent pink color indicates the endpoint of the experiment. From the titration it will be able to calculate the percentage of iron in the sample from the data. Experimental Procedure: Add 15mL of 6N sulfuric acid to a 125mL Erlenmeyer flask containing 105mL of deionized water (preparing approximately 0.75N sulfuric acid). Obtain a sample of the unknown. Weight the vial and contents accurately on an analytical balance. Handle the vial with a small strip of paper to reduce the risk of error (due to added weight). Pour about half of the sample into a clean dry 200mL Erlenmeyer flask and weight again. Use the remaining half of the sample to get a second weight of around 0.6g-0.7g. Make sure the vial is capped on every weight taken. Rinse a 25mL buret with three 5mL portions of standard permanganate solution. Fill the buret with the standard permanganate solution and record initial and final readings. To the first Erlenmeyer flask with the ferrous salt add about 1/3 of the 0.75N sulfuric acid. Dissolve the salt by gently swirling it in the dilute acid. Add about 5mL of the Zimmerman-Reinhardt Reagent (this reagent contains phosphoric acid which complexes yellow ferrous ions into colorless compounds which do not obscure the endpoint; it also contains manganous ions which inhibit the oxidation of any chloride ions in the sample). The use of a white background underneath the flask aids in the detecting of the endpoint. Repeat with second sample. Raw Data: 1st weighing, vial and sample 6.
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).
Each subsequent trial will use one gram more. 2.Put baking soda into reaction vessel. 3.Measure 40 mL vinegar. 4.Completely fill 1000 mL graduated cylinder with water.
The purpose of this experiment was to examine how the stoichiometry, “the quantitative relationships between substances involved in a chemical reaction”, can be applied to determine the quantity of sodium hypochlorite found in a bleach product. This experiment allowed it to determine how much oxidizing agent is in a cleaner by using a redox reaction, which is a reaction involving the transfer of electrons from the compound being oxidized to the compound being reduced. To determine the amount of oxidizing agent, it is necessary to accurately measure out known amounts of redox reactants, know the stoichiometry
We used the pipette filler and filled the glucose rinsed pipette to add 10ml of 10% of glucose in test tube 0.
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:
First, you obtain a sample of saliva and do so by putting a couple of ounces of water in your mouth, swishing it around, and then spitting it into a small cup. Then, you label the two test tubes with your initials on them and labeling them by number one and number two. Then, you add ten drops of starch solution and ten drops of water to the first test tube. For the second test tube you do the same as well. After this is done, you then place both test tubes in the water bath for thirty minutes. When you place the test tubes in there label the two wells of the spot place one and two with the wax pencil provided. Finally, add one drop of the iodine solution to each well. Once this is all done, you can then record and analyze your
An elements¡¦ reaction to certain substances may be predicted by its placement on the Periodic Table of Elements. Across a period, an element on the left will react with more vigor than one on the right, of the same period. Vertically, as elements are sectioned into groups, the reaction of each element increases as you move down in the same group. With this in mind, the reactions of the substances involved in this experiment may be hypothesized, observed, and validated.
Summary and procedures: the use of the different types of apparatus to get the correct results is always knowing it functionality and the correct significant digits. We always must make sure the balance should be 0.000 g when it is completely empty. In the case of the electric balance, the tray must to be clean and free of water or dirt, this machine is very accurate and precise. In the use of the flask and beaker, those should be cleaned before and after the use, that is how we avoid and create accidents for unknow chemicals or substances that were used before in the containers. Starting with the procedure, first is determine the mass for each balance in use, then record all the necessary data of that.
3.) Divide your 30g of white substance into the 4 test tubes evenly. You should put 7.5g into each test tube along with the water.
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
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.
Create wells: put a comb template in the middle of the tray; wait until the mixture becomes solid. After, remove the comb standing straight. 4. Remove rubber ends: transfer the gel tray into the horizontal electrophoresis and fill it with the concentrated electrophoresis buffer. 5. Materials and methods: Experiment: 1st, prepared milk samples should be already done by the teacher.
Remove the extra solvent on a steam bath under a hood while flushing the flask with N2 gas, leaving the crude extract. Weigh extract.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and