Sodium thiosulphate solution

Preparation of Standard Volumetric Solutions 1. 0.1N Sodium thiosulphate solution Reagents: Sodium thiosulphate crystals, Potassium dichromate (primary standard NIST certified), Sulphuric acid, Potassium iodide , Starch Solution (1%): Weigh 1g of soluble starch and mix it with 100ml of boiled water. Procedure • Weigh 25 g of sodium thiosulphate crystals and transfer it in a 1000 ml volumetric flask. • Dissolve it in minimum amount of distilled water and make up the volume to 1000 ml. Standardization

The Potassium Iodide particles will increase and the frequency of their collisions with Hydrogen Peroxide particles will also increase, causing them to react quicker. I hypothesize that as I increase the concentration of the Potassium Iodide Solution, the rate at which the blue-black starch complex covers the ‘X’ marking on the tile, will also increase until a point where the rate will remain the same due to all the particles having already finished reacting. 1

reaction that lead to chemical equilibrium and explore also the impact of concentration of reactants and temperature on rates. In this experiment, hydrogen peroxide and sulphuric acid are added to a another solution of potassium iodide, sodium thiosulphate and starch. After a lag, the combined solution turns a deep blue colour. The reactions occurring are as follows. (1) 3I-(aq)+H2O2 (aq)+2H+I3-(aq)+2H2O(l) Hydrogen peroxide is an oxidising agent that oxidises iodide ions to iodine in acidic medium

Introduction Chemistry is a branch of science commonly defined as “the study of the structure, properties, and reactions of the chemical elements and the compounds they form” (The American Heritage Science Dictionary, 2002). This definition is very general and covers a range of study areas, including those that are an asset to society. Chemical reactions are studied by many chemists as they common occurrences in everyday life (Stewart, 2014). Without chemical reactions people would be unable to

Rate of Reaction of Dilute Hydrochloric Acid and Sodium Thiosulphate To investigate the change in rate of reaction between DILUTE HYDROCHLORIC ACID and SODIUM THIOSULPHATE as the concentration varies. PLAN A chemical reaction takes place over a specific period of time i.e. which is the time for the reactants to be formed into the products. If the reactants take a relatively short time to form the products, the reaction is known as a FAST one. The RATE of that particular reaction

either a gaseous or as sodium or calcium hypochlorite. The chlorine is added to water to help prevent people from getting sick from disease-producing microorganisms. The chlorine that is added and reacts with the organic material and metals in the water is the chlorine demand for the water as it will not be available for any disinfection that keeps people from getting sick while in the pool. The residual test is

concentration of sodium thiosulphate the higher the reaction rate. The graph above shows the reaction rate compared to the sodium thiosulphate solution is almost a straight line showing the relationship of the sodium thiosulphate and the rate of reaction. 2. Explain why the results were the way they were The higher the sodium thiosulphate concentration the faster the rate of the chemical reaction as more particle collide. The graph shows a liner relationship as the sodium thiosulphate concentration

An experiment to investigate the effect of changing the concentration of hydrochloric acid on the rate of reaction with sodium thiosulpahte. Aim I am trying to find out how the concentration of hydrochloric acid affects the reaction time with sodium thiosulpahte. If a clear solution of sodium thiosulphate is mixed with hydrochloric acid then a reaction will occur where a creamy-yellow precipitate of sulphur is produced. H20 Text Box: + Text Box: + Text Box: + Na2S203 2HCL

of a reaction, according to the collision theory of reacting particles: temperature, concentration (of solution), pressure (in gases), surface are (of solid reactants), and catalysts. I have chosen to investigate the

The solution mixture was stirred until the KI dissolves. 10. The reaction mixture was titrated in the conical flask with the sodium thiosulphate solution until it just turns pale yellow. 11. 3 drops of freshly prepared starch solution were added to the conical flask. 12. The titration was continued until it just changes from dark blue to colorless. The final reading was recorded in Table 1. It was a first trial titration to estimate the volume of the sodium thiosulphate solution required