In this experiment, we aim to investigate the effect of sodium carbonate on hard water.
GCSE CHEMISTRY COURSEWORK: INVESTIGATING HARD WATER . PLANNING Aim In this experiment, we aim to investigate the effect of sodium carbonate on hard water. Method Firstly, 25.00cm3 of a sample of water was pipetted into a clean conical flask. The pipette was used because this measures and delivers a very accurate amount of liquid (to the nearest hundredth of a cm3, or 0.01cm3), but care had to taken to make sure it was not held by the bulge, as this could have made the amount inaccurate (as body temperature heats the apparatus up and makes it expand). Also, the pipette is used to avoid spillage, as the thin tube can put the water straight into the appropriate container. Furthermore, a pipette filler was used for safety purposes, because blowing or sucking could get unwanted and potentially dangerous substances into the mouth. 0.500g of sodium carbonate (a white powder) was added to the water, having been carefully weighed on an electronic balance - this was very exact and had a cover to maximise accuracy (it protected the balance from being affected by wind or other particles). The balance measured the mass of the powder to the nearest thousandth of a gram (i.e. 0.001g). Then a burette on a stand was obtained, a considerable amount of soap solution funnelled into it through the top (so the level reached near the top) and 1cm3 of the solution added to the water. The
An investigation into the factors affecting the rate of reaction of indigestions tablets with acid.
Chemistry Coursework, An investigation into the factors affecting the rate of reaction of indigestions tablets with acid. Planning, To start the investigation I thought about what affected rates of reaction. I managed to come up with 4 ideas: Surface area 2 Temperature 3 Concentration 4 Mixing of the substances (stirring) I decided to do 2 different preliminary experiment so I could chose the best variable to investigate and see what equipment was necessary to provide us with an accurate set of data. Our first Preliminary experiment was testing what affect heat had on the rate of reaction. I planned a basic experiment, * I took a heatproof mat and placed a Bunsen burner on it. * I then put a tripod directly above the Bunsen burner on which I placed a conical flask with a bung and delivery tube tightly attached on. * I fed the delivery tube into a bowl of water. * Then a measuring cylinder was filled up with water, (to the very top of the cylinder) the cylinder was then turned upside down whilst a hand was placed over the open hole of the cylinder with pressure letting no water out. It was the placed under the water in the bowl (hole first). * I removed the hand that was covering the hole of the tube when it was under the water of the bowl. The water remains inside the cylinder all the way to the top, this will allow us to see how much gas is given off by the
DECOMPOSITON OF HYDROGEN PEROXIDE WITH HEAVY METAL CATALYSTS
DECOMPOSITON OF HYDROGEN PEROXIDE WITH HEAVY METAL CATALYSTS Aim: Various metal oxides will be added to the hydrogen peroxide and the production of oxygen of the reaction mixture will determine catalysis. The volume of oxygen evolved will be observed and recorded to measure the reaction rate and the reaction rates of the different metal oxides will be compared. Scientific Background: Catalysis is the process by which the activation energy is lowered to allow the reaction to occur at less extreme conditions, during the process the catalyst does not under go any overall change. The catalyst reduces the activation energy by using a chemical route with activation energy less then the route, which would otherwise be taken in the absence of the catalyst. During catalysis the reacting substance usually undergoes a change or changes in oxidation state, therefore the catalyst must also be able to change its oxidation state. The s & p block metals possess or exhibit only one oxidation state. The reason being that their oxidation state depends on the removal of electrons from their outermost shell. The further removal of electrons will result in the penetration of stable inner shells that are filled with electrons. This would require an excessive amount of energy. As a result of this, the catalysts are not able to enter their different oxidation states and this therefore does not
In this experiment I am finding out how much sulphuric acid is present in sodium carbonate solution.
AS Chemistry Coursework Aim: In this experiment I am finding out how much sulphuric acid is present in sodium carbonate solution. How I will find the accurate concentration of sulphuric acid I am to find the accurate concentration of sulphuric acid ranging between 0.05 and 0.15-mol dm-3, I am provided with solid, anhydrous sodium carbonate, and range of indicators. The indicator which I will be using in my experiment is methyl orange, because it is used in most titrations, and it changes colour as a mid strength acid. It has sharper end point then universal indicators. The pH of methyl orange is 3.1 - 4.4. This is the chemical balanced equation that will take place, during my experiment. Equation: H2SO4 (aq) + Na2COaq) › Na2SO4 (aq) + H2O (l) + CO2 (g) From looking at the equation we can see that one mole of aqueous sulphuric acid reacts with one mole of sodium carbonate. (These are the reactants). This forms the (products) which is one mole of aqueous sodium carbonate, one mole of water and one mole of carbon dioxide. The balanced chemical equation is in a 1:1 ratio. Choosing the concentration of sodium carbonate solution The concentration of sodium carbonate which I will choose will be 0.1 mol dm-3, I have chosen this concentration because it is halfway between 0.05 and 0.15 moldm-3 of sulphuric acid concentration, I added, 0.05 and 0.15 and found out the
The aim of this experiment is to find out the concentration of a solution of acid rain. It is to be assumed that the concentration is approximately 0.1 moles dmˉ . Using a standard solution
AN EXPERIMENT TO FIND THE CONCENTRATION OF SAMPLE OF ACID RAIN Planning:- AIMS:- The aim of this experiment is to find out the concentration of a solution of acid rain. It is to be assumed that the concentration is approximately 0.1 moles dm¯ ³. Using a standard solution of sodium carbonate and then titrating this solution against the sample of acid rain, to find the exact molarity of the acid rain, using a suitable indicator that shows when the acid neutralises. sodium carbonate + sulphuric acid --> sodium sulphate + carbon dioxide + water Na2CO3 (aq) + H2SO4 (aq) --> Na2SO4 (aq) + CO2 (g) + H2O (l) RISK ASSESSMENT:- . In this experiment there is a hazardous and corrosive chemical, which acts as an irritant: sulphuric acid (0.1 molar), so goggles need to be worn. If any does go on the skin, wash off immediately with water (care needs to be taken at all times). 2. Anhydrous sodium carbonate is also an irritant, and therefore needs to be washed off immediately with water (care needs to be taken at all times). 3. Goggles must to be worn for the full duration of this experiment because of the chemicals involved. 4. Make sure to wipe down the surfaces after use, for the acid solution, if spilt will mark the surfaces or harm others. 5. After the experiment is completed, make sure to wash ones hands, so as not to carry hazardous chemicals left on your
Determination of the relative atomic mass of lithium.
Determination of the relative atomic mass of lithium. Aim: To determine the relative atomic mass of lithium. Analysis (method 1):) * (1) Calculate the number of moles of hydrogen. Conclusion so far: Since I have only this experiment once, method 1, there are no other results, only one set of results. Due to this fact there cannot be any anomalous results because there are not any other results to compare it to. The reason why I only did the experiment once was that was a lack of time, thus no average can be made. Plus I can conclude that since I have only done the experiment once, it could be an anomalous result itself. * During this experiment I will assume (from source of information) that 1 mole of gas occupies 24000 cm3 at r.t.p. (room temperature and pressure). The balanced formula I will be using for this experiment will be: 2Li(s) + 2H20(l) 2LiOH(aq) + H2(g) So to figure out the number of moles of hydrogen I am going to use an equation gained from my knowledge. n = Vcm3 24000 n = 224 = 0.00933 Moles 24000 The "224Cm3" or the volume was obtained from my results table (later on ). * (2) Deduce the number of moles for lithium. From looking at the balanced equation from above, we can simply look at it and tell that the ratio is 2 : 1, which means I can say there are two moles of Lithium and one mole of Hydrogen.
Aspirin Investigation
OBJECTIVES The objectives of this investigation are: ) Research available literature on aspirin with reference to synthesis, history, and medical use. 2) Prepare a pure sample of aspirin starting with oil of wintergreen as the initial compound. 3) Verify the identity and measure purity of the manufactured aspirin using a range of techniques. 4) Devise additional investigations into manufacture, properties or usage of Aspirin. Background Information Aspirin or acetylsalicylic acid is made from salicylic acid, found in the bark of the willow tree, which was used by the ancient Greeks and Native Americans, among others, to counter fever and pain. Salicylic acid is bitter and irritates the stomach. The German chemist Felix Hoffman synthesized the acetyl derivative of salicylic acid in 1893 in response to the urging of his father, who took salicylic acid for rheumatism. Aspirin is currently the first-choice drug for fever, mild to moderate pain, and inflammation due to arthritis or injury. It is a more effective analgesic than codeine. Aspirin causes insignificant gastrointestinal bleeding that can over time, however, cause iron deficiency; gastric ulcers may also occur with long-term use. Complications can be avoided by using enteric-coated aspirin, which does not dissolve until reaching the intestine. Aspirin should not be given to children who have chicken pox or
The Use of Volumetric Flask, Burette and Pipette in Determining the Concentration of NaOH Solution
Title The Use of Volumetric Flask, Burette and Pipette in Determining the Concentration of NaOH Solution Objective * To determine the number of ionizable hydrogen in an unknown acid. * To determine the equivalent weight of an unknown acid. * To determine the enthalpy change for the ionization of an unknown acid. * To use the technique of volumetric analysis or titration to determine the concentration of a given NaOH solution. Theory And Background In 1855, the German chemist, Friedrich Mohrn defined titration as the "weighing without scale" method because this process allows determination of the concentration of a sample without using complex instrumentation. A manual titration requires high accuracy and precision, both in the preparation of the material, and the use of different precisely dosed reagents. The operation must be repeated at least 3 times to obtain a reliable measured value. This procedure makes the manual analytical technique very long and fastidious. Titration is the quantitative measurement of an analyte in solution by reacting it completely with a standardized reagent. For example, a given volume of a solution of unknown acidity may be titrated with a base of known concentration until complete Neutralization has occurred. Acids and bases react until one of the reactants is consumed completely. A solution of base of known
Energy Change Associated With Neutralisation
Energy Change Associated With Neutralisation * Aim In this investigation I am trying to find out how energy is transferred from the reactants to the product and if any of it is released as heat energy. In the investigation my aim is to examine the change in temperature in a neutralisation reaction, specifically the change from the start temperature of the acid and the alkali to the finish temperature of the neutral solution. I would like to produce an unbiased and fair set of results. I would like to produce results which match my prediction and the scientific theory behind them. I would like there to be an obvious trend in the results and a pattern which can be easily be used to predict further results when changing the strength of the acid. Preferably there would be no anomalous figures. I aim to undertake a safe and well-planned investigation after which I will be able to arrive at a thorough and decisive conclusion. I aim to take the right amount of measurements for there to be an accurate result, not to take too many unnecessary ones. I aim to take the temperatures of all the solutions before the reaction and the temperature of the product afterwards so as to ensure that the temperature difference is measured correctly. My overall aim is to perform a safe, well-planned, precise and conclusive investigation into the temperature changes during neutralisation. *
Indigestion Tablets Investigation
Plan Variables . Temperature of water 2. Amount of time between measurements 3. Volume of acid 4. Type of acid 5. Concentration of acid 6. Mass of indigestion tablet 7. Number of indigestion tablets 8. Size/shape of indigestion tablet 9. Type of indigestion tablet 0. Agitation given to boiling tube Apparatus 00cm3 measuring cylinder boiling tubes 25cm3 measuring cylinder Indigestion tablets 250cm3 beaker delivery tube M hydrochloric acid stand Stop clock thermometer Electric kettle trough Diagram Method The apparatus will be set up as shown in the diagram above. Then I intend to- . measure the starting temperature of water. 2. add the indigestion tablet to the boiling tube. 3. measure the volume of gas produced every 15 seconds until the reaction finishes (I will know that it has finished because there will be no more bubbles evolved or when I get 3 consecutive readings that are the same). 4. repeat the experiment with 6 different temperatures of water, following steps 1-4. To ensure a fair test To ensure a fair test I will keep all the variables the same apart from the one I am testing. This variable is temperature. I am finding out if the temperature of a reaction affects the rate of the reaction. Amount of time between measurements I will measure the volume of gas produced every 15 seconds for 8 minutes or until the
