Chemical Oxygen Demand (COD) is a measure of the capacity of water to consume oxygen during the chemical decomposition of the organic matter and oxidation of inorganic chemicals such as ammonia and nitrite.
Test Procedure
The COD was determined by the dichromate reflux method. The appropriate amount of sample was introduced into commercially available digestion solution containing potassium dichromate, sulphuric acid and mercuric sulphate and the mixture was then incubated for 120 min at 150º C in a COD reactor (HACH, USA). COD concentration was measured colorimetrically using a spectrophotometer (DR 2010, HACH, USA). Chemical Oxygen Demand (COD) is used as a measure of oxygen requirement of a sample that is susceptible to oxidation by strong
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Add 5 to 7 glass boiling beads.
3. Add 1g of mercuric sulphate, 5 ml of concentrated sulphuric acid solution, and mix until the HgSO4 is in solution. The function of the mercuric sulphate is to bind or complex chlorides. One gram may not be required if the chloride concentration is low (caution: always add acid slowly down the side of the flask while mixing to avoid overheating).
4. Accurately add 25 ml of 0.25 N potassium dichromate (K2Cr2O7) and mix.
5. Add while mixing, 70 ml of concentrated sulphuric acid solution.
6. After through mixing, attach the flask to the reflux condenser, apply heat, and reflux for 2 hours. Refluxing time can be decreased depending on the ease of oxidation of organic materials. This time may be determined by refluxing for periods from 15 minutes to 2 hours and comparing the results.
7. A reagent blank containing 50 ml of distilled water treated with the same reagent as the sample should be refluxed with each set of samples.
8. Cool the apparatus to room temperature after the refluxing period. Wash down the interior of the condenser and flask twice with approximately 25 ml portions of distilled water.
9. Remove flask from the condenser and dilute to a final volume of approximately 350ml with distilled
This is what I will mix with the varying amounts of Strontium nitrate to form the precipitate. • Strontium Nitrate (enough to fill 8 boiling tubes with your varying amounts/36cm³) This is what I will mix with the sodium carbonate in order to form my precipitate. • Test Tube Rack
In the first part of the experiment, Part A, the standard solutions were prepared. As a whole, the experiment was conducted by four people, however, for Part A, the group was split in two to prepare the two different solutions. Calibrations curves were created for the standard solutions of both Red 40 and Blue 1. Each solution was treated with a serial 2-fold dilution to gain different concentrations of each solution.
4. Pour the salt-water solution into the water bottle. 5. Stretch the open end of the balloon around the mouth of the bottle and hold it there. 6.
For this I needed to first obtain deionized water. I cleaned my large graduated cylinder and got 20 + or - 2 mL of deionized water. I then added this water to the beaker that contained the mixture I created from the last step of the experiment. I also gathered 2 boiling stones and added them to the mixture of the last step. I placed the beaker on a hot plate and heated it up to 130 degrees Celsius.
Tyler White CHEM151LL 32658 04/01/2018 Different Types Chemical Reaction Types and Equations Purpose: The purpose of this lab experiment is to examine different types of chemical reactions such as Decomposition reaction, Synthesis reactions, Combustion reactions, and different Chemical equations. The experiments were conducted online using Late Nite Labs. Materials: Because the experiments were conducted online there wasn’t any physical use of materials, only digital ones, for these labs to be performed. Only the registration for the website was needed to perform these online labs, as well as a desktop computer.
Copper/ Red Stuff/ Chemical Reaction The purpose of this experiment was to determine what the red stuff that was produced was. We put aluminum foil in a test tube filled with 100 milliliters of copper chloride. During the experiment, I observed that the aluminum foil was breaking away, the aluminum foil that was breaking away was turning into red stuff. After a while, the once light blue copper chloride was turning into a dull gray, almost clear.
Background Research: Isopods are group of small, cold-blooded, crustaceans also known as pillbugs and sowbugs (pillbugs are commonly known as “roly polies”). Pillbugs are almost exactly like sowbugs, but differ because they can curl up into balls and are thicker than sowbugs (PNNL). Isopods are related to a few water crustaceans including crabs, crayfish, and shrimp, so water is necessary for them to survive. For that reason, they live in damp or wet areas such as forests and meadows. Isopods have seven armour plates, called “pereonites,” that serve as protection from predators and have seven pairs of legs.
Equipment: • Different coloured pens/textas • Filter paper • Scissors • 250ml beaker • Pencil or pop stick • Tape • Water Methylated spirits Ruler • Measuring cylinder Method 1. Cut a 10cm length of filter paper 2.
In the round-bottom flask (100 mL), we placed p-aminobenzoic acid (1.2 g) and ethanol (12 mL). We swirled the mixture until the solid dissolved completely. We used Pasteur pipet to add concentrated sulfuric acid (1.0 mL) to the flask. We added boiling stone and assembled the reflux. Then, we did reflux for 75 minutes.
The decomposition of NaHCO3 is an example of Prevention within Green Chemistry principles because all solid waste in this experiment is collected and used again. The only gaseous wastes generated by the reaction in the experiment are carbon dioxide and water, which are benign (Lab 3). The decomposition reaction of NaHCO3, generates virtually no waste, therefore less hazardous chemical syntheses. The byproducts of the reaction are gaseous CO2 and H2O which possess little or no toxicity to human health and the environment, because of the amounts released in this experiment. (Lab 3).
11) After you have prepared the dilutions, clean the outsides of the cuvettes with a paper towel. 12) Place the blank tube (tube 0) in the spectrophotometer. Since distilled water has no color it will not absorb any light so the absorbance number would be zero and this done to test the absorbance scale on the Spectrophotometer for the purpose of having it calibrated correctly. 13) Set the spectrometer to a wavelength of 530 nanometers. 14) Place the cuvettes (numbers 1-6) with the appropriate substance and record it’s reading in the data table.
Acids are proton donors in chemical reactions which increase the number of hydrogen ions in a solution while bases are proton acceptors in reactions which reduce the number of hydrogen ions in a solution. Therefore, an acidic solution has more hydrogen ions than a basic solution; and basic solution has more hydroxide ions than an acidic solution. Acid substances taste sour. They have a pH lower than 7 and turns blue litmus paper into red. Meanwhile, bases are slippery and taste bitter.
The CO2 gas produced can be used as an indicator for the rate of reaction as the amount of CO2 gas that is collected with in a fixed time is proportional to the rate of reaction. Therefore, the average rate of reaction can be calculated by measuring the amount of CO2 collected for a set period of time. The rate expression of the reaction is written as: rate = k[CaCO3]a[HCl]b 1 http://www.nlm.nih.gov/medlineplus/druginfo/meds/a601032.html 2 http://www.thechemicalblog.co.uk/10-uses-of-hydrochloric-acid/ Page 2 of 7 k represents the rate constant, a and b signify the order of reaction with respect to the reactants. The order of the reaction is the power to which the concentration of that reactant is raised to, for example, doubling the concentration of a reactant that is first order would double the rate of reaction while doubling the concentration of a reactant that is in the second order would quadruple the rate of reaction.
Once dissolved, fill the rest of the volumetric flask up to the line on the neck of the flask. Again mix the solution. Use four, 10mL volumetric flask, and label them from 1-4. Add approximately 2mL of copper sulfate pentahydrate into flask 1, 4mL to flask 2,
Afterwards, have the flask sit on the wire guaze on the iron ring and stand and attach it to the distillation