Lab Letter Detailing Report on Analgesics
CheMystery Labs, Inc 52 Fulton Street Springfield, VA 22150 April 30, 2007 Zachary May 8/27/01 5th Dear Marissa Bellinghausen, We recently analyzed a sample of an unknown analgesic and found its identity. To start off, we were given a crushed tabled of an unknown analgesic in a vial. We then put 20mL of distilled water into a beaker. Next, we added the unknown analgesic to the water and dissolved. Next, we took the pH of it and recorded. We then added 1mL of NaOH to the solution, testing the pH afterwards. We continued this process until we had added 5mL of the NaOH. After all pH measurements had taken place, we rinsed the beaker of its contents. Our analysis was to figure out what the unknown analgesic was. We had three different analgesic from which to choose. They were aspirin, buffered aspirin, and acetaminophen. Previous tests of the pH levels of each were taken in a previous experiment, and each one had a distinct pH change when sodium hydroxide was added. Our conclusion is that the unknown analgesic was certainly aspirin. In previous tests, the pH readings (before and after NaOH additions) stayed the same for aspirin, as it did in this experiment. For the other two analgesics, the pH measurements varied distinctly for each one. Here is a simple chart showing the obvious consistency of the pH levels: As you can clearly see, the pH remained
Huddling sheep In this experiment I plan to do 10 different tests, to discover the effects of huddling.
Huddling sheep In this experiment I plan to do 10 different tests, to discover the effects of huddling. The way I will set up each test is, * Place the test tube(s) on some blue tack (blue tack is used to reduce conduction through the base of the test tube). * If more than 1 test tube is used place an elastic band round them (to reduce the chance of the test falling over) * Fill each test tube with boiling water, placing a thermometer in the centre tube (when water has been added). * When the temperature of this tube drops to 50?c, start timing, and then every two minutes take the temperature, for ten minutes. (Originally I planned to see how long it would take for the temperature to drop from 50?c to room temperature, 23?c, but preliminary work showed this would take far to long). * After I've taken all the results, I shall do the exact same test again to get a more accurate and reliable results, after calculating an average result. Making sure I do the exact same, with all ten experiments, I believe this will make a very consistant and reliable experiment. If the experiments go well I predict that the more 'sheep' are added the longer it shall take for the temperature to drop, within the ten minutes. I have predicted this because, with one 'sheep' the heat will conduct through the sides of it, and heat will be lost. Whereas the more 'sheep' that are added the heat
To find out how temperature will effect the rate of reaction between sodium thiosulphateand hydrochloric acid.
Lewis Brend Friday. 28 September 2001 Rates of Reaction Aim: To find out how temperature will effect the rate of reaction between sodium thiosulphate and hydrochloric acid. Apparatus: Stop-clock Conical flask Thermometer Beaker Tripod Gauze Bunsen Burner Paper with a cross on it Safety Specs Heat Mat Measuring Cylinders Sodium Thiosulphate Hydrochloric Acid Prediction: My prediction is that the higher the temperature the less time it will take to go a cloudy colour because particles 2cxv5 Diagram: Method: Collect all the apparatus and set them all up as it is shown in the diagram above. Light the Bunsen burner and fill a beaker with 100ml of water, then measure 20ml in a measuring cylinder and put into a conical flask. Put the conical flask in with the beaker. Keep checking the temperature by using a thermometer. When it gets to the wanted temperature, take the conical flask out and put it on the piece of paper with the cross on it. Add 20ml of Hydrochloric acid then start the sop-clock. You then wait for the mixture is the flask to go a cloudy colour. Once it has gone this colour stop the sop-clock and take note of the time. Then do this for the rest of the temperatures. This will be made a fair test by not stirring the acids and by doing the exact same procedure to the other tests. Doing this will make it a fair test. Results:
Alcohol Energy Output
Chemistry investigation. In this experiment we will be investigating how the different alcohols heat the water, with their different energy's. Method. We will heat 50ml of water using various different alcohol burners. The alcohols we will be using are: butanol, methanol, ethanol, and propanol. We will heat the set amount of water in a metal beaker. The water will be heated from room temperature, to 50 degrees Celsius. The height of the beaker will also remain The same height, which for us was 15cm, we found this the best height, as the flames tip just touched the beaker, which reduced heat loss which would result in less reliable figures. The diagram shows the set up of the apparatus used, which again remains the same throughout the investigation. All of these variables that are kept the same will ensure a fair test, and more reliable results. The alcohol burner will be weighed before the heating of the water, and after. These figures will be recorded so we can work out the amount of alcohol used in the heating of the water. Various safety measures will be taken, i.e. wearing goggles. Making sure the apparatus is set up correctly and safely. Not carrying the alcohol burners around when lit. Predictions I predict that the different alcohols will heat the water, losing different amounts of weight, due to the different energy properties. The different bonds that need
To find out how much dilute hydrochloric acid (HCI) is needed to neutralise 25mls of sodium hydroxide solution (NaOH).
Aim: To find out how much dilute hydrochloric acid (HCI) is needed to neutralise 25mls of sodium hydroxide solution (NaOH). Equipment: ? Beakers ? Burette ? Stand and clamps ? Conical flask ? Eye protection ? Pipette ? Hydrochloric acid ? Sodium hydroxide Solution ? Measuring cylinder ? pH chart ? Small funnel ? Universal Indicator liquid ? Thermometer Diagram of Apparatus: Method: . Set up apparatus as shown in the diagram. 2. Dispense some hydrochloric acid in a beaker and then pour it into the burette, using a small funnel. (Making sure you pour it up to exactly 0) 3. Get 25ml of Sodium hydroxide and pour it into the conical flask. 4. Add a few drops of Universal Indicator liquid to the sodium hydroxide. 5. Place the thermometer into the conical flask. 6. Now your ready to start the experiment. Open the burette so 2cms of the liquid pours into the conical flask. Shake the conical flask to mix the solution record it's colour, pH and temperature. 7. Keep doing this process in steps of 2cm until you reach you reach about 18cm. Then start letting out the hydrochloric solution in 1cms. And as the solution is near to turning green (Neutral) let the solution out in shorter measurements (i.e. 0.5cm) 8. Record the results and then repeat the whole process twice more. Roziana Wan Ramli 10S Chemistry Coursework Set B3 Mrs
GCSE Coursework: Acid Rain Experiment
Daniel Ellis 10TYL\10C1 GCSE Coursework: Acid Rain Experiment Background: Burning fossil fuels makes acid rain. Most fossil fuels contain sulphur as an impurity. When we burn the fuel, the sulphur is oxidised. It turns into sulphur dioxide (SO2) gas. Power stations burning coal or oil give off most sulphur dioxide. This is the main cause of acid rain. The gas dissolves in rainwater, and reacts with oxygen in the air, to form sulphuric acid. Here are the following effects of acid rain on: . FORESTS - Trees are damaged and even killed. Over half the forests in Germany are dead or dying. 2. FISH - Hundreds of lakes in Norway and Sweden now have no fish left in them at all. Aluminium, which is normally "locked" in the soil, dissolves in acid rain. It then gets washed into the lakes, where it poisons the fish. 3. BUILDING - Acid rain attacks buildings and metal structures. Limestone buildings are most badly affected. Plan: In this experiment we are trying to find out the rates of reaction on limestone when different concentrates of acid are added to it. The equation for this reaction is: Calcium dioxide + hydrochloric acid = Carbon dioxide + water + Calcium Chloride. Factors that effect the rate of reaction are:
The effect of temperature on the rate of a reaction can be studied using the reaction between sodium thiosulphate solution and dilute hydrochloric acid.
Saeed Sattar The Thiosulphate Reaction Plan The effect of temperature on the rate of a reaction can be studied using the reaction between sodium thiosulphate solution and dilute hydrochloric acid. Sodium + Dilute --> Sodium + Water + Sulphur + Sulphur Thiosulphate Hydrochloric Chloride Dioxide Acid When sodium thiosulphate solution and dilute hydrochloric acid are mixed, the solution goes cloudy. Eventually, it is not possible to see a cross through the beaker. Preliminary Tests Test 1: We are going to be using thiosulphate at 0.25 maulers and 2.0 maulers. We will keep the temperature the same, which will be room temperature. We will do both the tests at the same time and see how long it takes to disappear. Test 2: We will keep the concentration levels the same, but we will change the temperatures. We will heat the dilute hydrochloric acid to 80ºC and place it in one beaker. In another beaker we will cool the dilute hydrochloric acid to 20ºC. We will do both the tests at the same time and see how long it takes to disappear. The reason we are doing these tests to test the different speeds at which they react. Prediction I predict that the higher the concentration, the faster the faster the 'x' will disappear. Reasons for prediction Method Fair Test Results
To investigate how the volume of Hydrochloric acid Affects the rate at which a reaction takes place.
Chemistry Coursework. AIM: To investigate how the volume of Hydrochloric acid Affects the rate at which a reaction takes place. EQUATIONS: Magnesium+hydrochloric acid=magnesium chloride+hydrogen Mg+2HCl=MgCl2+H2 Method: I have been asked to produce a piece of coursework that measures the rate at which a strip of magnesium is dissolved by hydrochloric acid. I have been asked to vary one aspect of the fair test and I chose to vary the volume of hydrochloric acid as I realised that it will give me a clear indication on how the rate of the reaction is affected by the volume of hydrochloric acid. First of all I got all of the following equipment plus the relevant safety equipment (goggles to protect my eyes and an apron to protect my body from splashing); * strip of magnesium * Hydrochloric acid * Measuring cylinder * Stopwatch * Beaker Once the equipment had been collected I set-up the experiment. I used 2cm lengths of magnesium for each experiment as I realised that when using smaller amounts of hydrochloric acid the magnesium would take too long to dissolve and it would be a waste of time. I decided against 1cm because I thought that maybe when larger quantities of hydrochloric acid were used the experiment would be over too
Original Writing Poetry Story of My Life Each day goes down in history, wets its feet,bathes in the clear or murky stream, drinks deep,
Story of My Life Each day goes down in history, wets its feet, bathes in the clear or murky stream, drinks deep, comes out to join past days on the other bank. We go in with the bathing day, every morning, brace the shiver on our skin, taste the slaking of thirst, find footing on mossy rock. Climb out with sleep. Waking, we're back on the first bank, wading with a new day into the kaleidoscopic water. Days far from either bank are barely seen and seem unseeing. There is no recording of them that knows the cold and quenching of their moment in the water. Yet I cannot let them go, nor bear the strong suggestion formed by their fading figures that they have let us go and that those coming cannot be foretold anything actual of water, flesh, or stone. Publisher holds out a large envelope says, Sorry. We can't publish your autobiography. Man sighs, says, Story of my life. All these words, then, are only for the stream? The stream is everything? The stream is not enough? The specters on the banks are deaf but
Working out the concentration ofThiosulphate solution and amount of HCl to be used
Working out the concentration of Thiosulphate solution and amount of HCl to be used I will firstly work out the concentration of Thiosulphate solution: Volume of Thiosulphate = 50 cm3 40g/ litre = 40 grams in 1000 cm3 Relative Molecular Mass (RMM) of Thiosulphate = 158 g Concentration: Mole of Thiosulphate contains 158 grams in 1000 cm3 0.25 Moles of Thiosulphate contains 40 grams in 1000 cm3 Therefore the concentration of Thiosulphate = 40/ 158 = 0.25 moles of Thiosulphate in 1000 cm3 Number of moles in 50 cm3 of thiosulphate: 0.25 moles in 1000 cm3 in 50 cm3, moles = 50/ 1000 = 0.05 moles Therefore number of moles of thiosulphate in 50 cm3 = 0.0125 I will now calculate the number of moles of Thiosulphate needed to react with hydrochloric acid: Na2S2O3 + 2HCl 2NaCl (aq) + H2O + SO3 + S(s) 50 cm3 / 0.0125 Number of moles of HCl = 2 x 0.0125 = 0.025 I will now work out the volume of HCl, which I will use for my experiment: Moles of HCl needed = 0.025 Concentration = 2 moles Volume = moles/ concentration = 0.025/ 2 m = 12.5
