Determining the final concentration of calcium hypochlorite in pool water sample after manipulating the different time intervals of the pool water sample being exposed to sunlight
Aim:
To investigate to what extent the concentration of calcium hypochlorite in pool water sample would degrade, depending upon the different time intervals of the water sample being exposed to the sunlight
Introduction:
The idea for this investigation was inspired by my childhood experience. As a toddler, I grew up in an environment near the pools of water. Naturally, I swam a lot and was frequently exposed to hypochlorite in swimming pools, as every time I swam in my swimming pool with my swimming goggles on, I would see a white circular object, which was calcium
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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
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Use a measuring cylinder to properly measure the volume of potassium iodate at 10 mL to be used before each trial
Volume of starch indicator per trial
(10 mL) If the volume of the starch indicator is different, the time it takes for the color to change to occur as a starch indicator is used to allow a color change to occur. Hence, different volumes of starch indicator may influence how fast the color change to occur. Use a measuring cylinder to properly measure the volume of starch indicator at 10 mL to be used before each trial.
Temperature of the calcium hypochlorite water sample stays within maintained band
(35-38°Celsius) Different temperatures of the water sample may affect the chlorination level of the pool and the rate of reaction ongoing between water, calcium hypochlorite and other chemical and biological organisms. Use a thermometer to measure the temperature of the calcium hypochlorite water sample and to only take the samples if the temperature that day was roughly between 35-38°
First, 100 mL of regular deionized water was measured using a 100 mL graduated cylinder. This water was then poured into the styrofoam cup that will be used to gather the hot water later. The water level was then marked using a pen on the inside of the cup. The water was then dumped out, and the cup was dried. Next, 100 mL of regular deionized water was measured using a 100 mL graduated cylinder, and the fish tank thermometer was placed in the water. Once the temperature was stabilizing in the graduated cylinder, the marked styrofoam cup was filled to the mark with hot water. Quickly, the temperature of the regular water was recorded immediately before it was poured into the styrofoam cup. The regular/hot water was mixed for a couple seconds, and the fish tank thermometer was then submerged into the water. After approximately 30 seconds, the temperature of the mixture leveled out, and was recorded. This was repeated three
2-ethyl-1,3-hexanediol. The molecular weight of this compound is 146.2g/mol. It is converted into 2-ethyl-1-hydroxyhexan-3-one. This compounds molecular weight is 144.2g/mol. This gives a theoretical yield of .63 grams. My actual yield was .42 grams. Therefore, my percent yield was 67%. This was one of my highest yields yet. I felt that this was a good yield because part of this experiment is an equilibrium reaction. Hypochlorite must be used in excess to push the reaction to the right. Also, there were better ways to do this experiment where higher yields could have been produced. For example PCC could have been used. However, because of its toxic properties, its use is restricted. The purpose of this experiment was to determine which of the 3 compounds was formed from the starting material. The third compound was the oxidation of both alcohols. This could not have been my product because of the results of my IR. I had a broad large absorption is the range of 3200 to 3500 wavenumbers. This indicates the presence of an alcohol. If my compound had been fully oxidized then there would be no such alcohol present. Also, because of my IR, I know that my compound was one of the other 2 compounds because of the strong sharp absorption at 1705 wavenumbers. This indicates the presence of a carbonyl. Also, my 2,4-DNP test was positive. Therefore I had to prove which of the two compounds my final product was. The first was the oxidation of the primary alcohol, forming an aldehyde and a secondary alcohol. This could not have been my product because the Tollen’s test. My test was negative indicating no such aldehyde. Also, the textbook states that aldehydes show 2 characteristic absorption’s in the range of 2720-2820 wavenumbers. No such absorption’s were present in my sample. Therefore my final product was the oxidation of the secondary alcohol. My final product had a primary alcohol and a secondary ketone
Using the calorimeter, we firstly needed to calibrate the machine; to do this we took a tube of distilled water and tested it; we knew that this should measure 0 because distilled water is completely transparent. We could have done this with any known reference sample. Once we had calibrated the machine we could then test the real samples for their transparency, we tested all five of these samples a total of three times each. Between each different concentration of solution sample we had to re calibrate the machine using the distilled water again, so in total we did 20 colourimetry tests. We gained three results for each concentration of sample and then calculated an average from these three results; these are shown in the table below.
Apparatus: * 1 measuring cylinder * 1 test tube * 1 stop clock * A large gelatine cube containing indicator and NaOH * Hydrochloric acid ranging from 1-3 molars * A scalpel Diagram: Method: * Take the large gelatine cube and cut into 15 equal pieces * Place on piece of the cube into the test tube * Measure out 10mls of HCl in the measuring cylinder * Pour the HCl into the test tube with the gelatine cube and start the clock * Time how long it takes for the pink colour inside the gelatine cube to completely disappear * You will also notice that the cube dissolves slightly * Record your results and repeat this same process 3 times for each molar of acid: § 1 molar § 1.5 molar § 2 molar
Investigating How the Concentration of Hydrochloric Acid Affects the Rate of Reaction with Calcium Carbonate
Investigating the Rate of Reaction Between Marble Chips and Hydrochloric Acid I am investigating the rate of reaction between marble chips (calcium
The Effect of Temperature on The Rate Of Reaction Between Magnesium And Hydrochloric Acid Planning I'm planning on investigating how temperature effects the reaction between magnesium and hydrochloric acid, the experiment will show whether the reaction will speed up or slow down with the change in temperature. Temperatures will range from room temp up until 70 degrees. The investigation will be a fair test because all quantities will remain the same for each test, each test will use the same amounts of hydrochloric acid and same size of magnesium, also the concentration of the acid will also not be changed. APPERATUS; · Conical flask · Bunsen Burner · Thermometer · Tri-pod · Protective matt · Stopwatch · Gauze · Measuring jug · Goggles
Put 1mL of 0.1M cobalt (II) chloride hexahydrate dissolved in 95% ethanol into a test tube. Then add 1mL of deionized water. Tap the end of the test tube to mix the solution and record the pertinent data in section 2 of the Data Table. Discard the solution in the appropriate container as directed to you by your lab instructor.
the water baths I think were accurate enough but having two thermometers in each bath maybe would have helped to hold the temperature readings more accurately. We were not given any instructions either to shake or not to shake the test tubes with the coloured solutions before inserting them in the spectrophotometer to read the absorbance. By shaking each test tube a certain number of times before putting it in the spectrophotometer could have improved the accuracy of the absorbance of the solutions.
Then, repeat steps 7-11 another 4 times but with the room temperature water. For the room temperature water just leave it in the room but try not to change the room’s temperature. 15. Try to put all your recorded data into a table for organization 16. Repeat the entire experiment for more reliable data.
Also, the temperature of the bath water should be recorded. For the next 15 minutes, the location of the dye should be recorded. Also, the temperature of the bath water should be recorded every other minute. All the data should be recorded in table one and used for analysis.
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
After the addition of HCL, test tubes A and B turned blue. With the addition of AgNO3, a white precipitate formed, and the solution returned to its original pink. Model 3 After 3 minutes in hot water, the resulting color was blue. After 3 minutes in cold water, the resulting water was pink.
The aim is to find out if changing the concentration of the hydrochloric acid solution has an effect on the time taken for the reaction. The reaction that will take place is: Hydrochloric acid + Calcium Carbonate + Calcium Chloride + Water + Carbon dioxide 2HCl (aq) + CaCo3 (s) CaCL2 (aq) + H2O + CO2 (g). Collision theory - Collisions between reactant particles are needed. for the reaction to take place in order to form a product.
the chances of collisions increase thus giving a faster rate of reaction. Then the s Apparatus:. Beaker Hydrochloric acid Distilled water Measuring cylinder Pipette Test tubes Test tube rack Diagram:.. [ IMAGE] Method: The.. Measure out 10cm3 of hydrochloric acid, as the concentration requires. for each concentration its composition is.