Sodium thiosulphate

Title: The effect of Hydrochloric Acid volume with Sodium Thiosulphate on the reaction rate. Introduction: Research Question: How does changing the volume of Hydrochloric Acid on Sodium Thiosulphate effect the time taken for the ‘X’ Mark to dissapear? The rate of a chemical reaction is the time required for a given quantity of reactant to be changed to product. The unit of time may be seconds, minutes, hours, days or years. For a chemical reaction to occur it needs to have a collision, and it is

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 of the prepared Sodium thiosulphate solution

Reaction Rates of Sodium Thiosulphate and Hydrochloric Acid at Various Concentrations Introduction/ plan ------------------ I am experimenting into the reaction rates of Sodium Thiosulphate and Hydrochloric acid when under different concentrations. Both Sodium Thiosulphate and Hydrochloric acid are clear solutions but when they react together they produce a cloudy solution, the solution become so cloudy you cannot see through it. To measure the rate of reaction I am going to print

concentration affects the rate of reaction between Hydrochloric Acid and Sodium Thiosulphate Chemistry Coursework How Concentration Affects a Reaction Aim: The aim of this experiment is to find out how concentration affects the rate of reaction between Hydrochloric Acid and Sodium Thiosulphate. Introduction: This experiment will be carried out by drawing a cross on a piece of paper and mixing hydrochloric acid and sodium thiosulphate together to see if the cross disappears. The concentration of hydrochloric

Investigating Reaction Rates of Sodium Thiosulphate and Hydrochloric Acid Aim: To investigate the rate of reaction of Sodium Thiosulphate and Hydrochloric acid. In this investigation I will be varying the concentration of Sodium Thiosulphate only and not the Hydrochloric acid concentration. In this investigation I will use the following word equation: Sodium Thiosulphate + Hydrochloric acid In this investigation I will use the following symbol equation:

The Factors Controlling the Rate of the Sodium Thiosulphate and Acid Reaction Planning I am investigating the factors controlling the rate of thiosulphate / acid reaction. The reaction that will be taking place will follow the rate at which sulphur is formed in the reaction of sodium thiosulphate with dilute hydrochloric acid. In the experiment the sulphur will appear as an extremely fine precipitate. This will slowly be followed by a milky appearance in the reaction

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

In 1839, Herschel was the first to use a new product, sodium thiosulphate, to fix images forever. This was later implemented by Fox Talbot and then Daguerre for his own daguerreotype. In 1851 Scott Archer learnt that you could use collodion -soluble guncotton dissolved in a mixture of ether and alcohol- to attach solver compounds to glass, the negative/positive process became dominate. The photographer would have to prepare the collodion glass plates and expose them while they were still wet. Processing

(HCl) and Sodium Thiosulphate (Hypo solution). There are multiple ways to test the rate of reaction between two substances, however the experiment we will be conducting involves placing a conical flask directly over a black coloured ‘x’ and recording the time it takes for the ‘x’ to become invisible after the two solutions react with each other. This is simple and direct as multiple tests can be undertaken at different concentration levels and multiple temperatures. Sodium Thiosulphate and Hydrochloric

of 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