Question 1. (2.0 pts)
Decide whether the following statements are true or false.
 Conductivity of KCl solution will decrease with the increasing of its
concentration.
 Overpotential of H2 on Cu electrode is 0.23 V. H+ species will be reduced at –0.23
V of electrode potential at normal condition with H2SO4 as electrolyte.
 Due to the ion strength effect, HCL solution pH value will decrease if the
solution is contaminated by another strong electrolyte.
 Percent dissociation (𝛼) of a weak electrolyte will increase if the increasing of its
concentration, at a certain temperature.
Question 2. (1.5 pts)
Design a cell which overall reaction is 2AgCl (s) + H2 (g) → HCl (aq.)+ 2Ag (s) and
calculate its standard electromotive force (emf).
Question 3. (0.5 pts)
Calculate the emf of the cell which the HCl concentration is 0.03 M (HCl is used as
an electrolyte).
Question 4. (0.5 pts)
Using Debye-Huckel limiting law, define the mean ionic activity coefficient of HCl in
its 0.03 M solution.
Question 5. (0.5 pts)
Determine the equilibrium constant of reaction in cell at normal condition.
Given the following data for question 6 and 7: Prepare a 0.05 M Al2(SO4)3 solution
at 30 oC. Assume that Al2(SO4)3 is strong electrolyte.
Question 6. (1.0 pts)
Fill in the blank: The Van’t Hoff factor (i) of given solution is ………….
Question 7. (1.0 pts)
Define the osmotic pressure of the given solution.
Question 8. (2.5 pts)
Write the cell reaction, electrode half reaction and calculate the emf of the following
cell:
Zn| ZnSO4 (aq) || AgNO3 (aq) | Ag
Question 9. (0.5 pt)
In cathodic protection, the object is connected to a metal with a more negative
standard potential (such as magnesium, oMg2+ / Mg = -2.36 ). V The magnesium acts
as a sacrificial anode, supplying its own electrons to the iron and becoming oxidized
to Mg2+ in the process. From the above concept, choose metal (among Zn, Pb, Cu
metals) work as a sacrificial anode to protect oil pipelnes that are made from steel.