∵ Zn Zn2+ + 2e-
Cu2+ + 2e- Cu ∴ n=2
For the Zn(s)/Zn2+(aq) half-cell, = -0.76V
For the Cu(s)/Cu2+(aq) half-cell,
Ecell = ER - EL
= {(+0.34) + 0.0295 log [Cu2+(aq)]} – {(-0.76)}
= (1.10) + 0.0295 log [Cu2+(aq)]
When the voltage of the cell system is measured, the concentration of Cu2+ can be determined by the above equation. Therefore, the solubility product can be calculated by the above principle.
Purposes:
To determine the solubility product of copper(II) iodate(V) at room temperature and pressure by e.m.f. measurement.
Apparatus and Reagents Used:
Chemical Reactions Involved:
The equation of dissolution of copper(II) iodate(V):
Cu(IO3)2(s) + aq Cu2+(aq) + 2IO3-(aq)
The equation of redox reaction between Zn and Cu2+:
Cu2+(aq) + Zn(s)Zn2+(aq) + Cu(s)
Procedures:
1. 50 drops of 1M ZnSO4(aq) were placed into a well of the well-plate;
2. 25 drops of 0.3M KIO3(aq) were placed into an empty well next to the well containing the 1M ZnSO4(aq), by using a clean Jumbo pipette;
3. The plastic pipette used in step(2) was cleaned. By using the same plastic pipette, 25 drops of 0.15M CuSO4(aq) were added and stirred well with a micro-stirrer or toothpick. 5 minutes were waited to attain equilibrium;
4. The two wells were connected by a strip of filter paper moistened with saturated KNO3(aq);
5. A clean homemade copper wire electrode and a clean zinc plate electrode were placed into the well containing the pale blue suspension and the well containing the 1M ZnSO4(aq) respectively;
6. The prepared galvanic cell was connected to a DMM. The steady voltage developed was recorded.
Observations:
When the galvanic cell completed in step(5) was connected to the DMM, a steady voltage was developed.
Data and results:
Temperature of the aqueous solution = 26℃
E.m.f. of the cell formed by Zn(s)/Zn2+(aq, 1M) and Cu(s)/Cu(aq, saturated) = 0.997V
Discussions:
1. The expression of the Ksp of copper(II) iodate(V) = [Cu2+(aq)]eqm [IO3-]2eqm
2. By the equation evaluated in the introduction,
Ecell = (1.10) + 0.0295 log [Cu2+(aq)] = 0.997V
0.0295 log[Cu2+(aq)] = -0.103
log[Cu2+(aq)] = -3.492
∴ [Cu2+(aq)]eqm = 3.225 × 10-3 moldm-3
Concentration of Cu2+(aq) in the saturated pale blue suspension = 3.225 × 10-3 moldm-3
3. By the equation of dissolution of copper(II) iodate(V),
Cu(IO3)2(s) + aq Cu2+(aq) + 2IO3-(aq)
[Cu2+(aq)] : [IO3-(aq)] = 1 : 2
∴[IO3-(aq)]eqm = 2 × 3.225 × 10-3 = 6.450 × 10-3 moldm-3
Concentration of IO3-(aq) in the saturated pale blue suspension = 6.450 × 10-3 moldm-3
4. The value for Ksp of Cu(IO3)2
= [Cu2+(aq)]eqm [IO3-]2eqm
= (3.225 × 10-3) × (6.450 × 10-3)2
= 1.34 × 10-10 mol3dm-9
5. From the data of the Faculty of Chemistry and Technology, University of Split, the literature value of Ksp of Cu(IO3)2 is 6.94 × 10-8 mol3dm-9 [1]. Obviously, the literature value was much larger than the experimental value. The discrepancy came from several reasons:
① The experimental temperature was 26℃, which was different from the expected room temperature 25℃. As temperature is the main factor of Ksp, the discrepancy of Ksp was caused by the difference of temperature;
② The low quality of copper and zinc electrode may affected the e.m.f. taken from the DMM, so the Ksp result was also affected;
③ The concentration of solutions prepared may be different with the expected value. The e.m.f. given out may not equal to the theoretical values, so the Ksp obtained may be different.
Conclusion:
By the e.m.f. method, the solubility product of copper(II) iodate(V) at room temperature and pressure was determined. Ksp for = 1.34 × 10-10 mol3dm-9
Reference:
[1] : Solubility Product Constants, Faculty of Chemistry and Technology, University of Split http://www.ktf-split.hr/periodni/en/abc/kpt.html
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