The OH- ions remain in the solution as Chlorine gas is given off. .
2Cl- 2e- + Cl2 (g).
This is an OXIDATION reaction.
.
The positive ions go to the cathode, which is negatively charged and the negative ions go to the anode, which is positively charged. We can see here that the electrodes act as magnets, as the opposite charges attract and the like charges repel. .
Apparatus: The experiment will be set up as below.
.
Fair Test: To make this a fair test, I will make sure I use the same beaker, spatula, .
electrodes, scales, ammeter, power pack, measuring cylinder and wires. .
Also, I will make sure that the distance between the electrodes are the same .
during each experiment, which will be 5cm. I will also ensure that the .
amount of water put into each experiment is constant at 60ml. .
Method: First I will set up the apparatus as shown above. Then I will weigh different amounts of sodium chloride (NaCl) starting at 0.25g then increasing the .
amount by 0.25g until I reach 2g. To these eight different levels of NaCl I .
will add 60ml of water (H20), this will create the solution. I will then stir the .
solution until all of the salt has dissolved. When it is clear that all the salt has.
dissolved I will place the electrodes into the solution, spaced apart at 5cm.
When they are in place, I will read the ammeter to measure the current .
flowing between the electrodes and record them in a table.
I will repeat this with all the different amounts of NaCl and then repeat the.
entire process again 3 times. This will enable me to obtain more accurate .
results and work out an average, which I will use to plot a graph.
Results: .
Mass of NaCl (g) 1st Test.
(amps) 2nd Test.
(amps) 3rd Test.
(amps) Average.
(amps).
25 0.12 0.13 0.15 0.13.
5 0.18 0.18 0.19 0.19.
75 0.19 0.21 0.20 0.20.
1 0.23 0.24 0.22 0.23.
1.25 0.25 0.28 0.25 0.26.
1.5 0.37 0.36 0.36 0.36.
1.75 0.41 0.40 0.40 0.40.
2 0.47 0.46 0.45 0.46.
-------------------PLEASE SEE GRAPH-------------------.
