Deducing the quantity of acid in a solution
Sofia Gaggiotti Chemistry coursework: Deducing the quantity of acid in a solution 20/03/2008 Index Aim and Background information 3 Hazards 3 Protection 4 Method 5 Previous calculations 5 Making the Solution 6 Equipment needed 6 Quantities of materials needed 8 Procedure 8 Making the Titration 9 Equipment needed 10 Procedure 13 References 15 Results and calculations 16 Evaluation 19 Chemistry coursework: Deducing the quantity of acid in a solution Aim and background information The aim of this experiment is to find how to develop and determine an accurate, precise and reliable concentration of an acid rain solution. 1 To do this, we are going to make first a solution of sodium carbonate with distilled water and then a titration in order to calculate the concentration of sulphuric acid in a solution. Solution: a solution is a homogeneous mixture composed of two or more substances. In this mixture, a solute is dissolved in a solvent. Solutions are characterized by interactions between the solvent phase and solute molecules or ions that result in a net decrease in free energy. 2 Titration: a titration is a laboratory technique by which we can determine the concentration of an unknown reagent using another reagent that chemically reacts with the unknown. At the equivalence point (or endpoint) the unknown reagent has been reacted with the known reagent.
The Effects of Strong and Weak Acids on the Order of a Reaction.
Aim To investigate the effect strong and weak acids have on the rate of a reaction and its order. Introduction What is a chemical reaction? This is the first question that needs to be answered before tackling this investigation. A chemical reaction is the process which results in the chemical conversion of one substance into another. These reactions can be placed into two groups; exothermic and endothermic reactions. If the energy given out of the reaction is greater than the energy taken in, the reaction is known as an 'Exothermic Reaction'. Similarly, if the energy taken in is greater than the energy given out, the reaction is known as an 'Endothermic Reaction'. The easiest way to determine if a reaction is Exo/Endothermic is to observe any temperature changes within or after the reaction has taken place. If the surrounding temperature drop, the reaction is exothermic and if the temperature increases, the reaction is exothermic. Although it is true that every substance has the potential to be converted into another, it is also true that before a reaction happens, certain criteria needs to be met. For a reaction to happen, the particles must collide with the correct amount of energy - also known as the 'Activation Energy'. The Activation energy is the lowest amount of energy a particle needs in order for it to successfully collide with another and for the reaction to take
Titration-chemistry OCR
Chemistry AS-level Titration coursework Aim: The aim of this GCE chemistry investigation was to find out the accurate concentration of sulphuric acid in a solution using, titrations. This acid solution is thought to have a concentration between 0.05 and 0.15 mol dm-3, but as part of this investigation I was asked to find out the accurate concentration of sulphuric acid. Fair testing: Definition: 'Fairness' implies that the outcome of the activity truly depends on what is being investigated, and is not being distorted by other external factors. Therefore a fair test is one where all the variables are kept constant or the same, except the variable that is being investigated. A variable is anything that can change and which may influence the outcome of the investigation. List of variables: The different variables are: > Amount of sulphuric acid > Concentration of sulphuric acid > Mass of alkali- anhydrous sodium carbonate (2.65g) > Indicator Variables that needs to be controlled: The variable that needs to be controlled are as follows: > The mass of the alkali (this has to be determined first before the titration) > The amount of sulphuric acid. These variable needs to be controlled because even the slightest miss calculation of the mass of the alkali of the amount of sulphuric will bring about a huge change in the values that represent the titration.
Determining the concentration of acid in a given solution
Determining the concentration of acid in a given solution Planning 4 I have been given a sample of sulfuric (VI) acid solution with a concentration between 0.05 and 0.15 mol dm-³. I am going to find out the accurate concentration of the sulfuric acid. To find out the concentration of the acid I will react it with a known volume and concentration of a base and see how much base was needed to neutralise the acid. The acid is a strong acid which means that I know all the H+ ions have been disassociated and are in the solution. The H+ ions will react with the OH- ions in the alkali which will neutralise the solution. I am provided with solid, hydrated sodium carbonate with the formula Na2CO3·10H2O.1 This is a readily available base and I can dilute it down to achieve the concentration I want to react with the acid. The formula of the reaction that will take place is H2SO4 (aq) + Na2CO3 (aq) --> Na2SO4 (aq) + CO2 (g) + H2O (l) So 1 mole of H2SO4 reacts with 1 mole of Na2CO3. A titration will give me the most reliable and accurate results with the available equipment. To do my titration I will need: A Burette 7 I will need a burette to add the sodium carbonate to the sulfuric acid solution. The burettes provide me with very accurate results of volume of solution added. The class set of burettes measure 50cm3. I want to do a titration
Chemistry Iodine Clock
AIM To investigate how the rate of reaction varies using the Iodine Clock experiment with changes in temperature, different concentrations of substrates and the use of transition metals. BACKGROUND THEORY The iodine clock reaction was first studied by Augustus Harcourt and William Esson. They studied the reaction between iodide and hydrogen peroxide (1) In the experiment Potassium Peroxodisulphate (K2S2O8) is used instead of Hydrogen Peroxide, in which the Peroxodisulphate ions react with the iodide ions from the Potassium Iodide solution to form Sulphate ions and iodine. It can be represented by this half equation S2O82-(aq) + 2I-(aq) 2SO42-(aq) + I2(aq) The reaction involves the oxidation of the iodide ions to iodine molecules. Sodium thiosulphate increases the time taken for the iodide ions to turn to iodine. All the Sodium thiosulphate has to be used up before the colour of the starch to change. Sodium thiosulphate changes the iodine to iodide ions, without sodium thiosulphate the reaction would be too fast for getting reliable results. The reaction between the Sodium thiosulphate and the iodine can be shown as: 2S2O32-(aq) + I2(aq) S4O62-(aq) + 2I-(aq) Rates of reaction The rate of reaction is a measure of how fast a reaction occurs. If the reaction fast then the rate of reaction is high but if the reaction is slow then the rate of reaction is
Finding Out how much Acid there is in a Solution
Finding out How Much Acid there is in a Solution When a metal is extracted from its ore, a waste product is often sulphur dioxide (SO2). This is then converted into sulphuric acid (H2SO4) and sold. To sell sulphuric acid, its accurate concentration must be known. In this investigation, I will use a titration method to attempt to find the accurate concentration of a sample of sulphuric acid thought to have a concentration of between 0.05 and 0.15 mol dm-3. The chemicals which I will use to do this will be solid anhydrous sodium carbonate (Na2Co3) and an indicator. Finding out How Much Acid there is in a Solution - Plan Quantities of Chemicals Required In this investigation, the chemical reaction used will be the neutralisation reaction between sulphuric acid and sodium carbonate: H2SO4 (aq) + Na2CO3 (aq) --> Na2SO4 (aq) + CO2 (g) + H2O (l) As the sodium carbonate has to be aqueous for this reaction, I will need to make up a solution of sodium carbonate before I begin the titration. I will need to choose an appropriate concentration for this solution and an appropriate volume of it to make up. As there is a 1:1 ratio between the moles of sulphuric acid and sodium sulphate used in this reaction, I should make up a solution of sodium carbonate of similar solution to that of the sulphuric acid. Assuming that the concentration of the sulphuric acid is around 0.1 mol dm-3, this
Investigating the enthalpy change of different fuels when combusted.
Investigating the enthalpy change of different fuels when combusted. Aim: The aim of this experiment is to see how the enthalpy changes vary when different alcohols are combusted in standard conditions. The alcohols used will be: Ethanol, Propan-1-ol, Butan-1-ol, Pentan-1-ol and Hexan-1-ol. These alcohols all have the OH functional group on the first Carbon atom of the molecule. Background Knowledge The enthalpy change of combustion (also shown as ?Hc) is a measure of energy when one mole of a fuel burns completely in air, at a standard temperature and pressure. This standard temperature is 298 Kelvin and 1ATM pressure. Maintaining these conditions would be complicated; therefore the experiment will be carried out in normal conditions. Any drastic alterations to these conditions will need to be taken care of to maintain a degree of accuracy. As combustion is exothermic (heat is transferred to the environment) all of the enthalpy changes will be negative. The formula for enthalpy change is: Energy Transferred= Heat capacity of water x Change in water temp x mass of water. Or E=MC?T Hess's Law. "the enthalpy change for any chemical reaction is independent of the intermediate stages, provided the initial and final conditions are the saeme for each route." This basically means that in an enthalpy cycle, detours can be made to reach the final products and the total
Steel Corrosion In Concrete Costal Structures ERT
Steel Corrosion inside Reinforced Concrete Costal Structures Chemistry 2012 ________________ Contents .0 Introduction 2.0 Background Information 3.0 Why does Steel corrode in a costal environment? 4.0 Method of Corrosion Prevention 4.1 Epoxy Coating 4.2 Cathodic Protection System 5.0 Conclusion 6.0 Appendix 7.0 Bibliography ________________ .0 Introduction Steel has been around since BC times however it has only been with the relatively recent invention of the Bessmer process in the mid-19th century which has turned it into the mass produced, inexpensive material it is today. More than 1.3 billion tons of steel is produced annually (Kolb, 2004 ), it is one of the most common materials in the world being used in everything from buildings and infrastructure to weapons and machines (The Steel Reinforcement Institute of Australia , 2008). Corrosion is a chemical or electrochemical reaction between a material, usually a metal, and its environment which results in deterioration of the material and its properties. For steel embedded in concrete, corrosion occurs mainly in the form of rust which is the oxidization of iron(III). The formation of rust is two to four times the original volume of the steel that has corroded and it maintains none of the good mechanical properties that make it useful
Aim To study the effect of concentration of iodide ion solution on the rate of iodide ion I- oxidation by peroxodisulphate ion S2O82- using iodine clock reaction
INVESTIGATING THE RELATIONSHIP BETWEEN CONCENTRATION OF REACTANTS AND RATE OF REACTION USING IODINE CLOCK REACTION Aim To study the effect of concentration of iodide ion solution on the rate of iodide ion I- oxidation by peroxodisulphate ion S2O82- using iodine clock reaction Introduction In an iodine clock reaction, two clear solutions would be added together in a common container where no apparent reaction takes place. After a short delay, at a sudden, the clear solution would turn into a blue-black solution. In this experiment, two clear solutions - potassium iodide, KI and sodium peroxodisulphate, Na2S2O8 - would be added together, with delaying additives, where a blue-black product solution would be observed. The aim of this experiment is to measure the different time taken to form the blue-black solution for different concentration of potassium iodide solution used. The different rates of reaction for each concentration can then be determined because they are the reciprocal of the times taken. The chemical reaction that takes place is a redox reaction where iodide ion is oxidized and peroxodisulphate ion is reduced. The full ionic equation for the reaction is represented by: I- (aq) + S2O82- (aq) › I2 (aq) + 2SO42- (aq) * all potassium and sodium ions are spectator ions. However, without any delaying mechanism, the formation of the
Paper chromatography
Introduction It is suspected that a rival company producing felt tip pens is stealing ideas for new colour from primary colour, a leading felt tip pen manufacturer. The company requires proof before it starts making allegations and requires you to devise a test to determine whether the colours have been stolen. Somebody on the inside of the rival company has supplied the company with same prototype from the rival company for you to test whether the rival felt tip pen manufacturer is stealing ideas for new colours from the other company. Aim The aim of this coursework is to find if the rival company is stealing the other company's new idea. To determine if they have stolen news ideas for a new felt tip, I well perform to simple tests however effective (paper chromatography and thin layer chromatography). I well reform tests on the prototype and the company's felt tip to see any simulates. Paper chromatography Paper chromatography is one method for testing the purity of compounds and identifying substances. Paper chromatography is a useful technique because it is relatively quick and requires small quantities of material. Paper chromatography is an analytical technique for separating and identifying compounds that are or can be colored, especially pigments. This method has been largely replaced by thin layer chromatography, however it is still a powerful teaching