An Investigation of the Reaction Between Hcl and Sodium Thiosulphate Essay Example
Science Investigation
Srategy
I am ivestigating the reaction of sodium thiosulphate and hydroclohric acid.
sodium thiosulphate(aq) + Hydroclohric Acid (aq) --> Sodium cloride (aq) + Sulphur Dioxide (g) + Water (l) + Suplhur (s)
Na(2)S(2)O(3) + 2 HCl --> 2NaCl + SO(2) + H(2)O + S
The finished reaction of the 2 clear liquids is cloudy.I will use this change from clear to cloudy as an indicator as to when the reaction is finished.
By using this change , i can see the effect of changing other factors has upon the rate of reaction.I will be sure to only change one factor at a time
(as far as possible) because otherwise i will not know which factors are influencing the rate of the reaction.
I have decided that changing the (molar) Concentration of the hydroclohric acid is the factor im going to investigate.
My Hypothesis is that as i decrease the concentration of the hydroclohric acid, the rate of reaction will also decrease.I Belive This Because Chemical
Reactions occur using the Collision theory (proposed by Max Trautz and William Lewis in 1916 and 1918) .This theory states that the reactant particles must collide, but only a certain fraction of the total collisions (the effective collisions, the molecules that have sufficient energy at the moment of impact to break the existing bonds and form new bonds, Called activation energy) cause the transformation of reactant molecules into product.With a higher concentration of HCl there are more molecules to collide , giving more chances for them to break bonds.
[INSERT PICTURE]
Equipment
3 Burettes ( One for water , One for HCl and the other for sodium thosulphate)
Distilled Water
Beaker(s)
HCl (1 Molar)
Sodium Thosulphate (0.25 molar)
Data Logger
Timer
I have elected to use burettes beacuse these will allow for more accurate measurement ( to within 1/10 ml) And I will be using one for each substance so that there is no cross contamination between the chemicals.I am using
Srategy
I am ivestigating the reaction of sodium thiosulphate and hydroclohric acid.
sodium thiosulphate(aq) + Hydroclohric Acid (aq) --> Sodium cloride (aq) + Sulphur Dioxide (g) + Water (l) + Suplhur (s)
Na(2)S(2)O(3) + 2 HCl --> 2NaCl + SO(2) + H(2)O + S
The finished reaction of the 2 clear liquids is cloudy.I will use this change from clear to cloudy as an indicator as to when the reaction is finished.
By using this change , i can see the effect of changing other factors has upon the rate of reaction.I will be sure to only change one factor at a time
(as far as possible) because otherwise i will not know which factors are influencing the rate of the reaction.
I have decided that changing the (molar) Concentration of the hydroclohric acid is the factor im going to investigate.
My Hypothesis is that as i decrease the concentration of the hydroclohric acid, the rate of reaction will also decrease.I Belive This Because Chemical
Reactions occur using the Collision theory (proposed by Max Trautz and William Lewis in 1916 and 1918) .This theory states that the reactant particles must collide, but only a certain fraction of the total collisions (the effective collisions, the molecules that have sufficient energy at the moment of impact to break the existing bonds and form new bonds, Called activation energy) cause the transformation of reactant molecules into product.With a higher concentration of HCl there are more molecules to collide , giving more chances for them to break bonds.
[INSERT PICTURE]
Equipment
3 Burettes ( One for water , One for HCl and the other for sodium thosulphate)
Distilled Water
Beaker(s)
HCl (1 Molar)
Sodium Thosulphate (0.25 molar)
Data Logger
Timer
I have elected to use burettes beacuse these will allow for more accurate measurement ( to within 1/10 ml) And I will be using one for each substance so that there is no cross contamination between the chemicals.I am using