Worksheet – Experiment 3
Equilibrium
October 24th, 2020
Data, Graphs, Results and Discussion:
This discussion is primarily about the topic of equilibrium, which according to Chang's book is
defined as: “Chemical equilibrium is reached when the rates of reactions in one direction and
another are equal, and the concentrations of reactants and products remain constant. Chemical
equilibrium is a dynamic process.” Raymond Chang,“Chemistry”,14,McGraw Hill,
623(2013).
, It began with procedure 1, the objective of which is to have observations of 3 test tubes in order
to be able to determine the qualitative changes of these reactions and to see if a precipitate was
achieved. For the first test tube the mixture was between Ag+ and Na2CO3, On this first
reaction, after Ag+ has reacted with Na2CO3, the color of the reaction passes from a colorless
solution to an orange or brownish solution. After this the reaction was made a net ionic equation.
For the second reaction the combination in the test tube was first to add Pb+ and then the NaCl
was added. For the second reaction, after Pb2+ has reacted with NaCl ,the color of the reaction
passes from a colorless solution to a white solution. After this the reaction was made a net ionic
equation. For the third and last reaction, combine between Sb3 + and Na2S. For the third
reaction, after Sb3+ has reacted with Na2S ,the color of the reaction passes from a colorless
solution to a light orange with yellow solution. After this the reaction was made a net ionic
equation. The equations for each reaction are found below in the calculations section.
For procedure 2, based on 3 main components which are attached to the table. 15 reactions were
carried out, which had to make the observation of whether when combining both ractives a
precipitate was formed.
+ 2+ 2+
𝐴𝑔𝑁𝑂3 (𝐴𝑔 ) 𝑃𝑏 (𝑁𝑂3) 2
(𝑃𝑏 ) 𝐶𝑎 (𝑁𝑂3)2 (𝐶𝑎 )
2− Produces a pinkish Produces a white Produces a white
𝑁𝑎2𝐶𝑂3 (𝐶𝑂3 ) precipitate precipitate. precipitate.
2−
𝑁𝑎2𝑆 (𝑆 ) Produces a dark Produces a black NR
brown precipitate precipitate
𝑁𝑎𝑂𝐻 (𝑂𝐻 )
− Produces a light NR Produces a white
brown precipitate precipitate.
𝑁𝑎2𝑆𝑂4 (𝑆𝑂4 )
2− NR Produces a white NR
precipitate.
−
𝑁𝑎𝐶𝑙 (𝐶𝑙 ) Produces a white Produces a white NR
precipitate precipitate.
At the time of completing all the reactions, some of them can be seen that no precipitate was
formed, for example in box D. In which the solution remained colorless. Similar situations
happened in the space box H, L, N, O. For this case, there is no need to write the reaction,
because if no reaction occurs, there is no product formed. Due to the fact that the components are
in both the left and right side.
For procedure 3, a list of reactions that started from just one was carried out. You start first with
Cu2 + it is observed that the solution is light blue, intermediate yellow pH, which indicates an
Equilibrium
October 24th, 2020
Data, Graphs, Results and Discussion:
This discussion is primarily about the topic of equilibrium, which according to Chang's book is
defined as: “Chemical equilibrium is reached when the rates of reactions in one direction and
another are equal, and the concentrations of reactants and products remain constant. Chemical
equilibrium is a dynamic process.” Raymond Chang,“Chemistry”,14,McGraw Hill,
623(2013).
, It began with procedure 1, the objective of which is to have observations of 3 test tubes in order
to be able to determine the qualitative changes of these reactions and to see if a precipitate was
achieved. For the first test tube the mixture was between Ag+ and Na2CO3, On this first
reaction, after Ag+ has reacted with Na2CO3, the color of the reaction passes from a colorless
solution to an orange or brownish solution. After this the reaction was made a net ionic equation.
For the second reaction the combination in the test tube was first to add Pb+ and then the NaCl
was added. For the second reaction, after Pb2+ has reacted with NaCl ,the color of the reaction
passes from a colorless solution to a white solution. After this the reaction was made a net ionic
equation. For the third and last reaction, combine between Sb3 + and Na2S. For the third
reaction, after Sb3+ has reacted with Na2S ,the color of the reaction passes from a colorless
solution to a light orange with yellow solution. After this the reaction was made a net ionic
equation. The equations for each reaction are found below in the calculations section.
For procedure 2, based on 3 main components which are attached to the table. 15 reactions were
carried out, which had to make the observation of whether when combining both ractives a
precipitate was formed.
+ 2+ 2+
𝐴𝑔𝑁𝑂3 (𝐴𝑔 ) 𝑃𝑏 (𝑁𝑂3) 2
(𝑃𝑏 ) 𝐶𝑎 (𝑁𝑂3)2 (𝐶𝑎 )
2− Produces a pinkish Produces a white Produces a white
𝑁𝑎2𝐶𝑂3 (𝐶𝑂3 ) precipitate precipitate. precipitate.
2−
𝑁𝑎2𝑆 (𝑆 ) Produces a dark Produces a black NR
brown precipitate precipitate
𝑁𝑎𝑂𝐻 (𝑂𝐻 )
− Produces a light NR Produces a white
brown precipitate precipitate.
𝑁𝑎2𝑆𝑂4 (𝑆𝑂4 )
2− NR Produces a white NR
precipitate.
−
𝑁𝑎𝐶𝑙 (𝐶𝑙 ) Produces a white Produces a white NR
precipitate precipitate.
At the time of completing all the reactions, some of them can be seen that no precipitate was
formed, for example in box D. In which the solution remained colorless. Similar situations
happened in the space box H, L, N, O. For this case, there is no need to write the reaction,
because if no reaction occurs, there is no product formed. Due to the fact that the components are
in both the left and right side.
For procedure 3, a list of reactions that started from just one was carried out. You start first with
Cu2 + it is observed that the solution is light blue, intermediate yellow pH, which indicates an
