This means that it was mostly in the form of CH3COOH. When the NaOH was added, the amount of CH3COOH that was dissociated to form acetate ions and H+ ions increased. These ionised protons (H+) reacted with the added OH from the NaOH and formed H2O, which then neutralised them (Joesten, M. 2007). Where the slope of the graph was shallow, the pH changes very slowly with the addition of NaOH and this was where the CH3COOH displayed its maximum buffering ability. This occurred when the pH was resisting change from the addition of NaOH, and it occurred at this point because the amount of CH3COOH was equal to the amount of acetate ions (CH3COO-) (Thorne, A.
The accuracy of titration results depends very much on the correct detection of the end point. Chemicals: Ethanedioic acid-2-water crystals Dilute sodium hydroxide solution Phenolphthalein Deionized water Apparatus: Beakers (100 cm3 ) x 4 Conical flasks (250 cm3 ) Pipette (25.0 cm3 ) Pipette filler Burette (50.0 cm3 ) Stand and clamp Volumetric flask (250.0cm3 ) Wash bottle White tile Glass rod Weighing bottle Electronic balance Stopper Chemical Reaction involved: Procedures: 1. Clean all the glassware involved in this experiment (e.g. burette, pipette, conical flasks, weighing bottle, volumetric flask, etc.) with deionized water as directed by the teacher.
Introduction Kinetics is the discovery and study of the reaction rates of chemical reactions. These reaction rates involve the pace or rate at which a reaction progresses. Many specific conditions can affect the reaction rate value; furthermore, the factors include the concentration of the reactants, the polarity of the solvent, and temperature1. The rate of reaction can be determined and studied using a rate law, an equation that correlates the rate with concentrations and a rate constant. This experiment’s reaction involving t-butyl chloride has a first order reaction rate, which means that the reaction’s rate law equation is the first order equation shown below.
RATES OF CHEMICAL REACTIONS REACTION ORDER FOR IODATE ION OBJECTIVE: To determine the order of a KIO3-NaHSO3 reaction with respect to the iodate ion. To determine a difference on the rate of the reaction when the solution is 10oC higher than a room temperature. BACKGROUND: The rate of a chemical reaction is the speed at which reactants are converted to products. Some reactions are very fast and some are very slow. In order for a chemical reaction to occur, particles of the reactants involved must collide with one another at the correct angle and with the correct amount of energy.
PLANNING Investigating the Kinetics of the reaction between Iodide ions and Peroxodisulphate (VI) ions By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in potassium iodide) to react fully with Peroxodisulphate ions (in potassium Peroxodisulphate). I will do three sets of experiments changing first the concentration of iodide ions, then the concentration of Peroxodisulphate ions and finally the temperature of the solution in which the reaction is taking place. From these results, I hope to draw conclusions as to the effects of these changes to the environment of the reaction on the rate and also determine the order of the reaction and the activation enthalpy. Background information The rate of a reaction is determined by a number of factors. These include: pressure, temperature, concentration of reactants, surface area of reactants, presence of a catalyst and radiation.
I predict that as the temperature of the acid increases so will the rate of reaction. This is because for two substances to react they have to have a successful collision which means the have to collide with a minimum amount of energy which is called the activation energy. This diagram shows how the particles will react with each other with the minimum amount of energy (activation energy): The higher the temperature of the acid the faster the acid particles will be moving around as they’ll have more energy and there will more collisions. This energy will also allow there to be more successful collisions and so more carbon dioxide will be formed in smaller amount of time. Therefore the rate of reaction will be faster.
Factors Affecting the Equilibrium Reaction of Iron (III) and Thiocyanate ions Research Question How does the change in temperature of Iron (III) Thiocyanatoiron, containing iron (III) ions Fe3+ (aq) and thiocyanate ions SCN¬¬- (aq), affect the absorbance of the solution? - Temperature at 25 °C, 30 °C, 35 °C, 40 °C, 45 °C, 50 °C, 55 °C, and 60 °C (equilibrate the Iron (III) Thiocyanatoiron (aq) in various temperatures using a digital water bath, and temperature checked using a digital thermometer connected to a data logger) - Production rate of thiocynate ion measured by the degree of change in color using a colorimeter after 600 seconds since the reactants are mixed. - The quantitative data of the absorbance of the solution will allow the determination of the concentration of the Iron (III) Thiocyanatoiron using the Beer–Lambert Law. The difference in concentration of the solution per temperature point provides the precise effect of temperature on the reaction’s equilibrium position. Introduction This experiment investigates how changing a factor that affects the equilibrium reaction, in this case temperature, affects the equilibrium position.
enzymeThis is shown in the diagram opposite. The Maxwell-Boltzmann Distribution and activation energy For a reaction to take place particles have got to collide with energies greater than or equal to the activation energy for the reaction, this can be marked on Maxwell-Boltzmann Distribution. I have chosen to investigate the effect concentration has on a reaction. I chose this because it is the easier to prepare and will provide the most accurate set of results. Equipment --------- Hydrochloric acid (5cm3) Sodium thiosulphate Paper with black cross on Conical flasks Goggles Water Pipette Measuring cylinder Method To provide fair accurate results it is important to ensure that the same printed cross is used for each experiment.
From this reaction, the equilibrium constant can be calculated by using the ratio of the product of the products over the product of the reactants. Thus Keq= [C]*[D] / [A] * [B]. Some reversible reactions reach equilibrium faster than others such as that of Iron (III) ion (Fe3+) with thiocyanate ion (SCN-) that forms thiocyanatoiron(III) (FeSCN2+). In this reversible reaction Fe3+ reacts with SCN- to produce FeSCN2+ in water. For this reaction A is the iron (III) ion, B is the thiocyanate ion and C is the thiocyanato iron (III).
Standardising: 1.) Rinse burette with distilled water and then with a little of the dilute HCl solution. 2.) Drain burette into your waste beaker and fill it with acid. 3.)