Aim: To investigate how the rate of reaction between Sodium Thiosulphate and Hydrochloric acid is affected by changing the concentration.

Background:

THE REACTION: when Sodium Thiosulphate reacts with hydrochloric acid

sulphur is produced. The sulphur forms in very small particles and

causes the solution to cloud over and turn a yellow colour. This

causes the cross to fade and eventually disappear.

Sodium Thiosulphate + Hydrochloric acid »» Sulphur + Sodium Chloride +

Sulphur Dioxide + Water

NA2S2O3 + 2HCL »» S + 2NaCl + SO2 + H2O

(aq) + (aq) »» (s) + (aq) + (g) + (l)

PREDICTION: As the concentration of Sodium Thiosulphate increases the

length of time for cross to disappear decreases (inverse). This is

because the increase of concentration of Sodium Thiosulphate will

increase the rate of reaction between Hydrochloric acid and sodium

Thiosulphate particles.

SCIENTIFIC REASONS FOR PREDICTION: the results from preliminary

experiments support the prediction made.

From the results you can see that there is a directly proportional

relationship between the concentration and the rate of reaction. If

you increase the concentration then the rate of reaction will also

increase.

METHOD:

1. Set up apparatus as in preliminary experiment.

2. Record the temperature of the room.

3. Add the first of the concentrations of sodium Thiosulphate to the

flask. As you add 10cm3 of HCL and start the stopwatch

4. Watch the solution as it clouds over. Once the cross has

disappeared stop the clock.

5. Record the time in a results table

6. Repeat the above steps for the other concentration of sodium

Thiosulphate. Repeat the experiment 3 times for each of the

concentrations.

7. Record all results in a table and work out the rate by dividing 1

by the average time for each.

This extract was taken from the link below:

This experiment is testing how the rate of reaction is affected when concentration is changed. The theory is said that increasing the concentration can increase the rate of reaction by increasing the rate of molecular collisions. The phenomenon behind all of this is the collision theory and how it plays a big role in this investigation. The higher the concentration the less time/faster it will take for the system to turn into equilibrium, and if concentration id decreased, time taken for the solution to go cloudy increases.

Hypothesis: The higher the concentration the faster the rate of reaction will be and the time taken to reach equilibrium will decrease. A more diluted concentration will have a longer rate of reaction and a longer time to reach equilibrium.

Apparatus:

Method:

Gathered all the apparatus needed for the experiment.

Using a weight balance we measure out 8g of Sodium thiosulphate, that we added too 200cm³ of water. We mixed the solution until all the crystals were dissolved.

Then you pour 50 cm³, 40 cm³, 30 cm³, 20 cm³, and 10 cm³ of the solution into five identical conical flasks. Then you add water to the other conical flasks so that the total volume in each flask in 50 cm³. Make sure to label the flasks so you know which one has so much concentration.

Once that’s done, you must now take a beaker and add 35 cm³ of concentrated Hydrochloric acid to 65 cm³ of water to make a diluted solution.

Now take a piece of paper and draw a black cross on it, and then place one of the flasks on the paper (do one flask at a time). Using a measuring cylinder measure out 5 cm³ of the hydrochloric solution, and add this to the flask. Immediately stir the flask and start the stop watch. One person should do this part.

As soon as you can’t see the cross any more stop the stopwatch, and record the results in a table. Repeat this with all the flasks.

Results:

The rate of reaction is measured by dividing 1 by the time taken for the reaction to take place.

Number of moles of sulphur used: n= m/M

n= 8/32 = 0.25 mols

Discussion: