Lab report: Le Châtelier's Principle
Introduction:
Please refer to the lab manual.
Aim:
To investigate the state of equilibrium of chemicals.
Procedure:
A. Equilibrium of Fe3+ and SCN- with Fe(SCN)2+
Please refer to the lab manual
B. Equilibrium of Ni2+ and NH3 with Ni(NH3)62+
Please refer to the lab manual
C. Equilibrium involving solubility of inorganic salts
(a) Solubility of Barium Oxalate
Please refer to the lab manual
(b) Solubility of Copper(II) Hydroxide
Please refer to the lab manual
D. Equilibrium of Co2+ and Cl- with CoCl42-
Please refer to the lab manual
Results:
A. Equilibrium of Fe3+ and SCN- with Fe(SCN)2+
Color tube 1:Light blood red color
Color tube 2:Blood red color
Color tube 3:Light red
B. Equilibrium of Ni2+ and NH3 with Ni(NH3)62+
Color before addition of NH3 :Green
Color after addition of NH3 : Blue
Color after addition of HCl: Light green
C. Equilibrium involving solubility of inorganic salts
(a) Solubility of Barium Oxalate
Color of BaCl2 Solution: Colorless
Color of BaC2O4 precipitate: White
Color after addition of HCl: Colorless
Color after addition of NH3: White
(b) Solubility of Copper(II) Hydroxide
Color of CuCl2 solution: Blue
Color of Cu(OH)2 precipitate: Dark blue
Color after addition of HCl: Colorless
Color after addition of NaOH: Blue
D. Equilibrium of Co2+ and Cl- with CoCl42-
Color of Co(NO3)2 solution: Red
Color after addition of HCl: Blue
Color after addition of H2O: Pink
Color after heating: Blue
Color after cooling: Pink
Questions:
1. Use Le Châtelier's Principle to explain the different colors found in the following equilibria.Show all chemical equations
(a) Fe3+ and SCN- with Fe(SCN)2+
Fe3+ + SCN- ⇌ Fe(SCN)2+
When the amount of Fe3+ions increases, the equilibrium is disrupted, causing it to shift to the right. More SCN- are reacted wih the Fe3+ ions to form more Fe(SCN)2+ , causing the blood red color to be darker.
(b) Ni2+ and NH3 with Ni(NH3)62+...