Sodium thiosulfate

By using the scatter plot graphs it was clear to see that as the temperature of the sodium thiosulfate raised in the water baths the quicker the reaction occurred this is because of collision theory. Collision theory is the cause of all reactions between particles (atoms). For a reaction to occur the atoms have to collide with each other. Not just collide, but collide each other in the correct place and the correct orientation for the reaction to occur. These atoms then need to exceed activation

the sodium thiosulfate affect the rate of reaction to hydrochloric acid? contents page 1: contents, aim, prediction, equation, diagram page 2: equipment, preliminary experiments page 3: page 4: page 5: page 6: page 7: page 8: Aim: In my investigation I am trying to find out how the rate of reaction between sodium thiosulfate and hydrochloric acid gets affected but the concentration of the thiosulfate. Prediction: My prediction is that the increased concentration of the thiosulfate will

Volumetric Flask and covered with a lid. To homogenize the solution, the Volumetric flask was repeatedly inverted and shaken. Finally, the Potassium Iodate solution was ready. Next, the Sodium thiosulfate solution was prepared in a similar manner. First, 1.20 grams of Sodium thiosulfate and 0.04 grams of Sodium Carbonate were weighed added into the 100 ml Volumetric flask. Further, the deionized water was added until the mark of the neck of the volumetric flask and the lid was placed on the top

Sample calculations: The way we measured the amount of DO depended on the amount of drops it took to make our yellow water sample(as seen in Section 3) clear using the Sodium Thiosulfate Solution. One drop was equal to one ppm, so if it took 5 drops of the Sodium Thiosulfate Solution to turn the water sample clear, the amount of dissolved oxygen in it was 5 ppm. Likewise, to gather averages, we used data from day 1 and day 2. Combine the average results by adding all them and dividing by the amount

vitamin C an amount of KIO3 solution with a known concentration had it’s iodine “freed” with the chemicals KI and H2S04, this allowed the iodine to react with the dissolved vitamin C tablet. This was then titrated against a primary standard of sodium thiosulfate at a concentration of 0.01102*10-5¬¬M. These chemicals cause the following reactions3: KIO3(aq) + 5KI(aq) +3H2SO¬4(aq) -> 3I2(aq) + 3K2SO4(aq) + 3H2O(l) 2Na2S2O3(aq) + I2(aq) -> 2NaI(aq) + Na2S4O6(aq) Since the volume of KIO3 solution and so

with increasing temperature. Conversely, the reaction rate of virtually all reactions decreases with decreasing temperature. In this experiment, to investigate study the effect concentration and temperature of the reactant on the reaction rate, Sodium Thiosulfate will be reacted with dilute Hydrochloric Acid. The reaction is carried out in a conical flask placed on a piece of white paper. The white paper has a black cross on it. At the beginning of the reaction, both compounds are clear and, the cross

Vitamin C Investigation Aim: I want to find out whether the concentration of Vitamin C in Golden Circle Pineapple juice changes over time. Hypothesis: My hypothesis for this investigation will argue that the Vitamin C level in Golden Circle Pineapple juice will decrease over time. Chemical information and safety surrounding the use of these substances. Previous scientific work: CHEEKY NANDOS Vitamin C: Vitamin C (ascorbic acid) is a water-soluble vitamin, which is needed by the body to

Experiment A1: Kinetics of the Reaction between Acetone and Iodine The key aim of this experiment was to determine the rate equation for the acid-catalysed iodination of acetone and to hence consider the insinuations of the mechanism of the rate equation obtained. The stoichiometric equation for the reaction between iodine and acetone is below, followed by the rate equation (where x,y,z and k are the values to be obtained): I2 + CH3COCH3 CH3COCH2I + HI -d[I2]/dt = k [I2]x [CH3COCH3]y [H+]z

INTRODUCTION: The purpose of this two-part experiment was to “determine the mass percent of sodium hypochlorite in a commercial chlorine bleach sample” (lab website). Titration is used in this lab twice. In Part one, students will use the solution of KIO3 primary standard and use this solution to standardize a solution containing sodium thiosulfate. When the KI is added to the solution, it forms a brown/yellow color. Then students used titration to add Na2SO3 to make the color go from brown/yellow

A2 Chemistry Coursework Section 1 Aims: I aim to find out the order of reaction with respect to [H2O2] and [2I-]. I aim to find out the activation enthalpy of the reaction by finding the rate of reaction at different temperatures using the Arrhenius Equation. The experiment will go as follows: Into a conical flask put 15cm3 of distilled water and add 2cm3 of [X]moldm-3 potassium iodide (KI) solution and 1cm3 of 2moldm-3 sulphuric acid. Then add to this 2.5cm3 of 5vol (0.42moldm-3) hydrogen