PEKA 2 (TITRATION)

Topic :  Acids and Bases

                                                                             

Aim                           :To find the end point in the titration of hydrochloric acid and sodium hydroxide solution using an acid-base indicator

                                  

           

Materials                   :0.1 mol dm^-3 hydrochloric acid, 0.1 mol dm^-3 sodium hydroxide solution, phenolphthalein

Apparatus                :Burette, 25 cm³ pipette, pipette filler, retort stand and clamp, white tile, 250 cm³ conical flask

                                  

Procedure                 :                (Must draw the diagram and list out the procedure)

                                

Result                        :   

Titration set	Estimation	1	2	3
Final burette reading/ cm3
Initial burette reading/ cm3
Volume of hydrochloric acid needed/ cm3

 Discussion                :

Able to write the chemical equations for the reactions correctly    

Able to show the calculation

                                      Able to state a observation and inference  correctly

                                     

                                      Able to state precaution

Conclusion                :

PEKA FORM 4

PEKA 1

ELECTROPLATING


PREPARE THE FORMAT OF REPORT AS BELOW:

Aim                           : To study the electroplating of an object with copper.

Problem statement  

Hypothesis               

Variables                

                                  

Materials                  

Apparatus               

Procedure

Observation           

Set	Electrode		Observation
	Anode	Cathode	Anode	Cathode
I	Iron spoon	Copper
II	Copper	Iron spoon

                                  

                 

Discussion

     

Conclusion    

EXAMPLE OF PEKA

Aim                           :To investigate the effect of concentration of ions on selective discharge of ions at the electrodes

Problem statement   :How does the concentration of ions in hydrochloric acid, HCl affect the discharge of ions at the anode?

Hypothesis               :When the concentration of chloride ion is higher, then the chloride ion will be selectively discharged at anode.

                                    

Variables                  :Manipulated variable  :  Concentration of chloride ion

                                   Responding variable   :    Ion discharged

                                   Constant variable        :    Type of electrolyte, type of electrode, duration of electrolysis

                                  

Materials                   1.0 mol dm^-3 hydrochloric acid, 0.001 mol dm^-3 hydrochloric acid

Apparatus                batteries, carbon electrodes, connecting wires with crocodile clips, ammeter, electrolytic cell, test tubes, litmus paper and splinter

Procedure                 1. A electrolytic cell is filled with 1.0 mol dm^-3 hydrochloric acid until it is half full.

                                   2. The switch is turned on.

                                   3. Gas produced at anode is collected and tested with moist litmus paper and glowing splinter.

                                   4. Observations are recorded.

                                   5. Steps 1 to 4 are repeated by using 0.001 mol dm^-3 hydrochloric acid to replace 1.0 mol dm^-3 hydrochloric acid.

 Observation

Electrolyte	Observation at anode
1.0  mol dm-3 hydrochloric acid	A greenish-yellow gas with pungent smell is released. The gas turns the blue litmus paper to red then to white.
0.001 dm-3 hydrochloric acid	Gas bubbles are released. A colourless gas relight a glowing splinter.

                  
                                  

                                   

Discussion                  :

1.      the aqueous solution of hydrochloric acid consists of hydrogen ions, H+, chloride ions, Cl^- and hydroxide ions, OH^- tat move freely.

2.      During the electrolysis, the Cl^- ions and OH^- ions move to the anode.

a)      Electrolysis of 0.001 dm^-3 hydrochloric acid

The OH^- ions are selectively discharged at anode to form oxygen and water. This is because OH^-ion is lower than Cl^- ion in the electrochemical series.

4OH^-     →  O₂  +  2H₂O  +  4e

b)      Electrolysis of 1.0 mol dm^-3 hydrochloric acid

The Cl^- ions are selectively discharged at anode to form chlorine gas. This is because the concentration of Cl^- ions are higher than OH^- ions.

2Cl^-    → Cl₂  +  2e

Conclusion     : During electrolysis of 1.0 mol dm^-3 hydrochloric acid, the Cl^- ions are selectively discharged at anode instead of OH-.to form chlorine gas due tohigher concetration of Cl^-.The hypothesis is accepted.