Rate of reaction between Na2 S2O3 and HCI
Answers
The reaction between Sodium thiosulphate (Na2S2O3) and hydrochloric acid (HCl)
To produce a colloidal solution of sulphur, where the solution obtained is translucent.
The reaction occurs as follows:
Na2S2O3 (aq) + 2HCl (aq) → 2NaCl (aq) + H2O(l) + SO2 (g) + S(s)
The above reaction when written in its ionic form:
S2O3-2 (aq) + 2H+ (aq) → H2O (l) + SO2 (g) + S(s)
As the temperature of the system increases or as the concentration of reacting species increases the rate of precipitation of sulphur also increases. As the concentration increases, molecular collisions per unit time of the reacting species increase which can result in increased chances of product formation. This results in an increase in the rate of precipitation of sulphur. Similarly, on increasing the temperature, the kinetic energy of the reacting species increases, so the number of collisions that result in the formation of products increase leading to a faster rate of reaction.
Answer:
Explaination:-
To Study the Effect of Concentration on the Rate of Reaction Between Sodium Thiosulphate and Hydrochloric Acid
Theory
According to the law of mass action, rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants. In other words, the rate of reaction increases with the increase in the concentration of the reactants. The effect of concentration of reactants on rate of a reaction can be studied easily by the reaction between sodium thiosulphate and hydrochloric acid.
Na2S203 + 2HCl ——–> S(s) + 2NaCl(aq) + SO2(g) + H2O (l)
The insoluble sulphur, formed during the reaction, gives a milky appearance and makes the solution opaque. Therefore, rate of reaction can be studied by measuring the time taken to produce enough sulphur to make some mark invisible on a paper kept under the conical flask in which the reaction is carried out.
Apparatus
Pipette (10 ml), stop-watch, two burettes and five conical flasks (100 ml).
Materials Required
0.1 M Na2S2O3 solution and 1 M HCl solution.
Procedure
Wash the conical flasks with water and label them as 1, 2, 3, 4 and 5 respectively.
With the help of a burette, add 10, 20, 30, 40 and 50 ml of 0.1 M Na2S2O3 solution to the flasks 1, 2, 3, 4 and 5 respectively.
Now add 40, 30, 20 and 10 ml of distilled water to the flask 1, 2, 3 and 4 respectively so that volume of solution in each flask is 50 ml.
Take 10 ml of 1M HCl in a test tube with the help of a burette.
Add 10 ml of hydrochloric acid taken in a test tube to the conical flask No. 1 containing 10 ml of 0.1 M Na2S2O3 and 40 ml of distilled water and start the stop-watch.
When half of the hydrochloric acid solution has been added. Shake the contents of the conical flask and place it on the tile with a cross mark as shown in Fig.
to-study-the-effect-of-concentration-on-the-rate-of-reaction-between-sodium-thiosulphate-and-hydrochloric-acid-1
Go on observing from top to downwards in the flask and stop the stop-watch when the cross mark just becomes invisible. Note down the time.
Repeat the experiment by adding 10 ml of 1M HCl to flasks 2, 3,4 and 5 and record the time taken in each case for the cross to become just invisible.
Observations
Record the observations in a tabular form as given below :
to-study-the-effect-of-concentration-on-the-rate-of-reaction-between-sodium-thiosulphate-and-hydrochloric-acid.
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