Theory & Procedure, Kinetics Study on the Reaction between Sodium Thiosulphate and Hydrochloric Acid Class 12 Notes | EduRev

Chemistry Class 12

Class 12 : Theory & Procedure, Kinetics Study on the Reaction between Sodium Thiosulphate and Hydrochloric Acid Class 12 Notes | EduRev

The document Theory & Procedure, Kinetics Study on the Reaction between Sodium Thiosulphate and Hydrochloric Acid Class 12 Notes | EduRev is a part of the Class 12 Course Chemistry Class 12.
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Objective

Our objective is to study the effect of concentration on the rate of reaction between sodium thiosulphate and hydrochloric acid.

The Theory

What is Chemical Kinetics?

For any chemical reaction, its feasibility and extent of reaction are very important. The feasibility of a reaction can be predicted by thermodynamics and the extent can be determined from chemical equilibrium. Like feasibility and extent, it is important to know the rate and the factors affecting the rate of a chemical reaction. The branch of chemistry that deals with the study of reaction rate and its mechanism is called Chemical Kinetics.

What does the rate of a reaction mean?

In all the chemical reactions the reactants are consumed and new products are formed. So the rate of a reaction is defined as the rate of decrease in concentration of any one of the reactants or the rate of increase in concentration of any one of the product.

Consider the hypothetical reaction, R > P.

[R] and [P] are the concentrations of the reactants and the product respectively.

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What are the factors that influence the rate of a reaction?

There are various factors that can affect the rate of a chemical reaction.

  • Temperature
  • Concentration of the reactant
  • Physical state
  • Catalyst

The concentration of the reactant plays an important role in the rate of a reaction. As the concentration of the reactant increases, the number of reacting molecules increases. Because of the increase in the number of molecules, the number of collisions also increases as a result the rate of the reaction increases.

Reaction between Sodium thiosulphate and Hydrochloric Acid

The effect of concentration of the reactant on the rate of a reaction can be studied easily by the reaction between sodium thiosulphate and hydrochloric acid.

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Sodium thiosulphate reacts with dilute acid to produce sulphur dioxide, sulphur and water. Sulphur dioxide is a soluble gas and dissolves completely in aqueous solution. The sulphur formed however is insoluble and exist in the mixture as a white or pale yellow precipitate or a colloid that gives a milky appearance and makes the solution opaque. Therefore the rate of the reaction can be studied by monitoring the opaqueness of the reaction. This can be easily done by measuring the time taken (t) for forming a certain amount of sulphur.

In this experiment, the reaction is carried out by mixing the reactants in a conical flask, and placing the conical flask on the top of a piece of white paper that has a cross mark on it. Before the reaction starts, the mark is clearly visible from the top of the conical flask through the solution. However, as the reaction proceeds, sulphur precipitates that make the solution more opaque and eventually the mark gets completely masked. The time taken (t) for the mark to totally disappear indicates how fast the reaction has occurred.

We can plot a graph between 1/t (in second) and the concentration of sodium thiosulphate by taking 1/t along ordinate axis and concentration of Na2S2Oalong abscissa. The graph should be a straight slopping line.

Theory & Procedure, Kinetics Study on the Reaction between Sodium Thiosulphate and Hydrochloric Acid Class 12 Notes | EduRev

From the graph, it is clear that 1/t is directly proportional to the concentration of Na2S2O3. But 1/t is a direct measure of the rate of the reaction. Therefore the rate of the reaction between Na2S2O3 and HCl is directly proportional to the concentration of Na2S2O3 solution.

Learning Outcomes

  • Students understand the effect of concentration of the reactant on the rate of a chemical reaction.
  • Once the students understand the concept of the experiment and the different steps, they can perform the experiment in the real lab more accurately and quickly.

Materials Required

  • Burettes
  • Conical flasks
  • Stop-watch
  • 0.1M sodium thiosulphate (Na2S2O3) solution
  • 1M HCl
  • Distilled water.

Procedure

Real Lab Procedure

  • Take five clean conical flasks and label them as A, B, C, D and E respectively.
  • Add 10, 20, 30, 40 and 50 ml of 0.1M sodium thiosulphate solution to the flasks A, B, C, D and E respectively.
  • Then add 40, 30, 20 and 10ml of distilled water to the flask A, B, C and D respectively so that volume of solution in each flask is 50ml.
  • Add 10ml of 1M HCl to the conical flask A.
  • When half of the HCl solution has been added to the conical flask, start the stop- watch immediately.
  • Shake the contents of the conical flask and place it on a white tile that has a cross mark at the centre.
  • Go on observing from the top of the flask and stop the stop-watch when the cross marks just becomes invisible. Note down the time.
  • Repeat the experiment by adding 10ml of 1M HCl to flasks B, C, D and E respectively and record the time taken in each case for the cross to become just invisible.

Simulator Procedure (as performed through the Online Labs)

  • You can select the volume of sodium thiosulphate (Na2S2O3) solution using the slider.
  • Drag the measuring jar to the conical flask to pour 0.1 M sodium thiosulphate (Na2S2O3) solution in it.
  • Drag the measuring jar to the conical flask to pour distilled water in it.
  • Click on the stopcock of the burette to add 5 ml hydrochloric acid into the conical flask.
  • Click on the conical flask to shake it.
  • Immediately, click on the stopcock of the burette to add another 5ml hydrochloric acid into the conical flask.
  • You can get the time taken for the disappearance of the cross mark from the stopwatch.
  • You can use the embedded worksheet to enter the values.
  • You can plot a graph using the worksheet.
  • To redo the experiment, click the ‘Reset’ button.

Note: Click on the ‘HELP’ button to see the instructions.

Observations

Flask No.    
 
Volume of Na2S2O3 solution (ml)
Volume of water (ml)
Total volume of solution (ml)
Conc. of Na2S2Osolution (M)
Volume of 1M HCl (ml)
Time (t) taken for cross to become just invisible (s)

1/t
(s-1)
A
10
40
50
0.02
10
 
 
B
20
30
50
0.04
10
 
 
C
30
20
50
0.06
10
 
 
D
40
10
50
0.08
10
 
 
E
50
0
50
0.1
10
 
 

Plotting the Graph

Plot a graph between 1/t (in s-1) and the conc. of Na2S2O3 by taking 1/t along ordinate axis and conc. of Na2S2O3 along abscissa.

Conclusion

  • The graph obtained is a straight line.
  • 1/t is directly proportional to the concentration of Na2S2O3.
  • Rate of the reaction between Na2S2O3 and HCl is directly proportional to the concentration of Na2S2O3, which is one of the reactant.

Precautions

  • The apparatus must be thoroughly clean.
  • Measure the volumes of sodium thiosulphate solution, HCl and distilled water very accurately.
  • Use the same tile with the cross-mark for all observations.
  • Complete the experiment at one time only so that there is not much temperature variation.
  • When half of the HCl has been added to sodium thiosulphate solution, start the stop-watch immediately.
  • View the cross-mark through the reaction mixture from top to bottom and from same height for all the observations.
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