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**1. Calculate the equilibrium constant for the reaction, 2Fe ^{3+} + 3I^{-} 2Fe^{2+} + I_{3}^{-}. The standard reduction potentials in acidic conditions are 0.77 and 0.54 V respectively for Fe^{3+}/Fe^{2+} and I_{3}^{-} /I^{-} couples.**

**2. Find the solubility product of a saturated solution of Ag _{2}CrO_{4} in water at 298 K if the emf of the cell Ag|Ag^{+} (satd. Ag_{2}CrO_{4} soln.)||Ag^{+}(0.1 M)|Ag is 0.164 V at 298 K. [JEE-1998]**

**5. Copper sulphate solution (250 mL) was electrolysed using a platinum anode and a copper cathode. A constant current of 2 mA was passed for 16 mintue. It was found that after electrolysis, the absorbance (concentration) of the solution was reduced to 50% of its original value. Calculate the concentration of copper sulphate in the solution to begin with. [JEE-2000]**

**6. The following electrochemical cell has been set up**

**Pt _{(I)}|Fe^{3+}, Fe^{2+}(a=1)||Ce^{4+}, Ce^{3+}(a=1)|Pt_{(II)}**

** = 0.77 V and = 1.61 V**

**If an ammetter is connected between the two platinum electrodes. Predict the direction of flow of current. Will the current increase or decrease with time? [JEE-2000**

**10. The standard potential of the following cell is 0.23 V at 15ºC & 0.21 V at 35ºC**

**Pt|H _{2}(g)|HCl(aq)|AgCl(s)|Ag(s) [JEE-2001]**

**(i) Write the cell reaction.**

**(ii) Calculate DHº, DSº for the cell reaction by assuming that these quantities remain unchanged in the range 15ºC to 35ºC.**

**(iii) Calculate the solubility of AgCl in water at 25ºC. Given standard reduction potential of the Ag ^{+}/Ag couple is 0.80 V at 25ºC**

**13. Two students use same stock solution of ZnSO _{4} and a solution of CuSO_{4}. The e.m.f of one cell is 0.03 V higher than the other. The conc. of CuSO_{4} in the cell with higher e.m.f value is 0.5 M. Find out the conc. of CuSO_{4} in the other cell . [JEE-2003]**

**17. (a) Calculate DG _{f}^{0} of the following reaction**

**Ag ^{+}(aq) + Cl^{-}(aq) ® AgCl(s)**

**given D _{f}Gº (AgCl) = - 109 kJ/mole,**

**D _{f}Gº (Cl^{-}) = - 129 kJ/mole,**

**D _{f}Gº (Ag^{+}) = 77 kJ/mole**

**Represent the above reaction in form of a cell**

**Calculate Eº of the cell. Find log _{10}K_{SP} of AgCl**

**(b) 6.539 × 10 ^{-2} g of metallic Zn (amu = 65.39) was added to 100 ml of saturated solution of AgCl.**

**Calculate log _{10}, given that**

**Ag ^{+} + e^{-} ® Ag Eº = 0.80 V ; Zn^{2+} + 2e^{-} ® Zn Eº = - 0.76 V**

**Also find how many moles of Ag will be formed? [JEE-2005]**

**21. We have taken a saturated solution of AgBr. K _{sp} of AgBr is 12 × 10^{-14}. If 10^{-7} mole of AgNO_{3} are added to 1 litre of this solution find conductivity (specific conductance) of this solution in terms of 10^{-7} S m^{-1}mole^{-1}.**

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