How Does the Concentration of the Sodium Thiosulfate Affect the Rate of Reaction to Hydrochloric Acid?

Then in the last test tube fill it up with 5ml of sodium sulphate. Then after that carefully pour the sodium carbonate solution into the test tube labelled copper chloride solution examining the result and recording appropriately.

thiosulfate anion needed to react with each mole of hypochlorite anion in the bleach sample.

First, one 80 mL beaker was labeled “HCl” and filled with 30 mL of hydrochloric acid. Another 80 mL beaker was filled with 30 mL of sodium thiosulfate and labeled “Na2S2O3”. Finally, a 250mL beaker was filled with 25 mL of tap water.

Hypothesis: If the concentration of an substrate is increased then the time it takes for the yeast spheres to rise will decrease because there is more substrate for the enzyme to break down, creating more oxygen, faster.

Question: How does changing enzyme concentration or temperature affect the reaction time of enzyme activity?

8. Repeat step 7 with H2SO4, except that you should use a 10 mL graduated cylinder of H2SO4 and adding 15 mL water.

8. The Hydrochloric Acid was carefully poured into the beaker with the Sodium Thiosulfate. Once the liquids had made contact, three seconds were waited until the stop watch was started.

When it is almost neutralized, pour possible minimum amount of sodium hydroxide for a fair result.

If the hydrochloric acid has a greater concentration (2.0 M), there will be a greater reaction rate than with a lower concentration (1.0 M, 0.5 M, 0.1 M). This is because if there is a greater concentration, the chance of the reactants colliding is greater, thus leading to a faster reaction and therefore a faster reaction rate. (Clark, Jim)

The rate of reactions can be sped up by increasing the temperature, increasing the surface area, increasing the concentration and catalysts.

The data supports the hypothesis that an exponential relationship will be found between the change in temperature and the reaction rate, and that the highest temperature will have the fastest rate of reaction. The data also supports the hypothesis that as the concentration of Potassium Iodine increases so will the reaction rate, and vice versa for an increase in Sodium Thiosulphate concentration. The hypothesis that the Iron (II) ions will affect the reaction rate, and that the optimal amount will be about 0.1M of catalyst was partially supported.

Science Coursework – What factors effect the rate of reaction between magnesium and hydrochloric acid? Background Knowledge There are four factors that can affect the rate of reaction and they all rely on the collision theory. This is basically how hard and how often particles collide with each other. The more and harder they collide, the faster the reaction time will be.

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 off a cross from the computer onto a piece of paper, place it under the beaker with the solution in it and record the time taken for the cross not to be visible. The Symbol equation for my experiment is:

the ‘cross’ must be kept the same. The easiest way to do this is to

Hypothesis: If the temperature of the sodium thiosulfate is increased, then the time it takes the precipitate to form will decrease therefore leading to the rate of reaction to increase as well. This can be explained as the temperature increases, the particles in the molecule will be moving more rapidly and hence as they move quicker, they will be colliding with other particles more frequently and with more energy. This energy will likely overcome the activation energy barrier and break the initial bonds and therefore produce a successful reaction and due to the increase in frequency of collisions, the time it takes the precipitate to form will decrease and since the product/precipitate is produced faster, therefore the rate of reaction will increase.