Winkler Method for Dissolve Oxygen
I. INTRODUCTION
They are two ways of determining dissolve oxygen in water the titrimetric by Winkler and electrometric. Winkler method is a technique used to measure dissolved oxygen in freshwater systems. Dissolved oxygen is used as an indicator of the health of a water body, where higher dissolved oxygen concentrations are correlated with high productivity and little pollution. This test is performed on-site, as delays between sample collection and testing may result in an alteration in oxygen content. The process includes divalent manganese salt precipitation by strong alkali to divalent manganese hydroxide. Next is the addition of potassium iodide or potassium hydroxide to create a pinkish brown precipitate.
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The sodium thiosulfate was standardized by titration with potassium dichromate dissolved into 50ml that has 1ml H2SO4 and 0.2g Na2CO3 and 0.5g potassium iodide that was allow to stand a while. The solution was titrated until the yellowish color was completely disappeared. Then 1ml of starch solution is added it became dark blue. The titration with thiosulfate was then continue until the dark blue color was disappear making the solution colorless. In the preparation of 2.4M manganese(II)sulfate solution 20.5g of MnSO4 ▪ H2O was dissolved in 50ml distilled water then it was transferred to amber bottle. On the preparation of alkaline iodide solution 7.5g of potassium iodide and 21g of potassium hydroxide was dissolved into 50ml distilled water then it was stored in amber bottle. Before the titration of water sample, all the solution and reagent was prepared, the groups collected water sample using BOD bottles. The bottles were submerged for about 30seconds avoiding introduction of air bubbles and turbulence. After that, the water sample was fixed using 2ml manganous sulfate and alkaline iodide. The bottle was shook then allow the brown precipitate to settled after all brown precipitate settled 2ml of sulfuric acid was added. The stopper was replaced then the bottle was shook again until all precipitate was completely dissolved. As the water
After 28 minutes, the mixture stopped boiling, and approximately 4.5 ml of bromobenzene was added drop by drop in the mixture, and color of the mixture was turned light brown orange. Then, the phenylmagnesium bromide was cooled in ice bath for a few minutes, and 10 ml of anhydrous diethyl ether was added in the mixture by using the syringe. After that, approximately 2.3 ml of methyl benzoate was added to the reaction, and it was added slowly slowly because the reaction was exothermic which needed to be cool in order to maintain a gentle reflux. Once all the methyl benzoate solution was added, the heating mantle was removed from the reaction flask and was cooled to the room temperature. During the reaction, a milky white salt began to precipitate, and the reaction flask was swirled for ten minutes until most of the reaction became visibly subdivided.
While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.
Put the foil into a 250 mL beaker. Get 25 mL of 3M KOH solution, add 5 mL KOH solution into the beaker and stir the beaker. Keep the reaction proceeding until all of the foil is dissolved and use ice bath to make it cool down. Pour the reaction mixture through Buchner funnel and filter flask setup, rinse the filter paper with a small amount of distilled water. Wash the beaker with distilled water and run the rinse solution through the Buchner funnel.
Goals The primary goal of this experiment was to identify an unknown compound by running various tests to determine the qualitative solubility, conductivity, and pH value of the compound. Tests were also performed for the presence of specific cations and anions in the compound. The second goal was to discover the reactivity of the unknown compound by reacting it with different types of substances. The third goal of this project was to calculate the quantitative solubility of the unknown compound in water.
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
Sulfuric acid was added to the distilled water, drop by drop until the solution had a pH of about 4.0. The bottle was labeled “Acid Rain” with a sharpie. Container 3: Alka-seltzer 650mL of water was added to the container 6 alka-seltzer tablets were dissolved into the water.
All of their data was combined and compared to the water quality standards. The maximum range for turbidity was around 0.18- 0.33, while the turbidity for the groups sample and unknown water sample was around 30- 60 ppm. The part F of the lab was a huge discrepancy. The Cu (copper) test was also a huge difference to the given chart. While the conductors of this procedure and the other scientists samples were around 0.1 or 0.2 ppm, the chart showed that the test was actually around 50 ppm .
In this reaction NaOH was added to the Cu(NO3)2. The solution developed a precipitate which made the clear solution become cloudy and uniform in color (blue). The physical color change was demonstrated through the formation of the precipitate. The third step was the formation of CuO. In this reaction, the Cu(OH)2 product was heated on a hot plate and stirred continuously until the solution became colorless and a dark precipitate formed.
Malachite was synthesized using the following reaction (1): 2CuSO4*5H2O(aq) + 2Na2CO3(aq) CuCO3Cu(OH)2(s) + 2Na2SO4(aq) + CO2(g) + 9H2O(l) Based on this chemical equation, two moles of aqueous hydrated copper (II) sulfate reacted with aqueous sodium carbonate, a precipitate of copper (II) carbonate hydroxide was formed along with aqueous sodium sulfate, gaseous carbon dioxide, and liquid water. The copper (II) carbonate hydroxide precipitate is also the malachite that was obtained from the solution. It was known that a chemical reaction was occurring when the copper (II) sulfate solution was mixed in with the sodium carbonate based on the fact that the color of the solution changed from blue to light blue and the solution frothed. The malachite
These color changes indicate a chemical change, which show that a reaction had occurred. In the first step when o-vanillin and p-toludine, imine was formed. The color change from green to orange suggests that imine appears as orange colored. In the second step, the addition of sodium borohydride reduced the imine into another derivative, which was yellowish lime color. The solution turned clear when acids and anhydrides was added, which indicated the precipitate were dissolved.
Next, a 100 mL graduated cylinder was used to measure 60 mL of distilled water. The water was added to the compound and stirred with a glass-stirring rod until dissolved. Next, The flame test required the solution made during the solubility test. The experiment needed a metal wire that was dipped into the solution
Problem: How does the temperature of water used to dissolve an Alka-Seltzer tablet affect the amount of time it would take for the tablet to completely dissolve? An Alka-Seltzer tablet is a medicine tablet made with baking soda used as a pain reliever for “headaches, body aches, pain, heartburn, acid indigestion, and sour stomach” (Alka-Seltzer Tablets). It is put into water, left to dissolve and then consumed. When an Alka-Seltzer tablet is dropped into h20, a chemical reaction immediately takes place and produces bubbles made out of carbon dioxide as a product of the collision (Olson 2). When in its original powder (dry) form, the Alka-Seltzer’s two main ingredients: citric acid and sodium bicarbonate are just there and not reacting to each
In this experiment, Analysis of Gaseous Products, a comparison between the elimination reactions created in the presence of an acidic and basic conditions was observed to be further analyzed through gas-liquid chromatography. These conditions were achieved by acid-catalyzed dehydration of a secondary and primary alcohol and based-induced dehydration of a secondary and primary bromide. As a result of these changing eliminations, gas-liquid chromatography makes it possible to separate and isolate volatile organic compounds to analyze the stereochemistry and regiochemistry of these compounds without decomposing them. Overall, gas-liquid chromatography of these compounds in acidic or basic conditions contributed in the identification and analysis
Empirical Formula of Magnesium Oxide - Lab Report Background Information/Introduction: The aim of this lab is to determine the empirical formula of magnesium oxide by converting magnesium to magnesium oxide. As an alkali earth metal, magnesium reacts violently when heated with oxygen to produce magnesium oxide and magnesium nitride as a byproduct. In order to obtain only magnesium oxide, distilled water was added so that magnesium nitride will react and convert to magnesium hydroxide. Further heating then oxidizes all of the magnesium into magnesium oxide.
The chemical equation for this experiment is hydrochloric acid + sodium thiosulphate + deionised water (ranging from 25ml to 0ml in 5ml intervals) sodium chloride + deionised water (ranging from 25ml to 0ml in 5ml intervals) + sulphur dioxide + sulphur. As a scientific equation, this would be written out as, NA2S2O3 + 2HCL + H2O (ranging from 25ml to 0ml in