課程名稱︰分析化學一
課程性質︰系訂必修
課程教師︰劉春櫻 教授
開課學院：理學院
開課系所︰化學系
考試日期（年月日）︰01.12.2009
考試時限（分鐘）：120 min
是否需發放獎勵金：是
（如未明確表示，則不予發放）
試題 :
Analytical Chemistry
1. (18%) Briefly distinguish between
(a) Concentration polarization and kinetic polarization
(b) Working eletrode and counter electrode
(c) Charging current and faraday current
(d) Iodometry and iodimetry
(e) Formal potential and standard electrode potential
(f) Ohmic potential and overpotential
2. (4%) Give the algebraic expression for the equivalence point potential in
the titration of iron(II) with K2Cr2O7 in acidic solution.
3. (5%) (A) What is a Jones reductor and what is it used for?
(B) Why is a Walden reductor always used with solutions that contain
appreciable concentrations of HCl?
4. (12%) Describe the source of pH dependence in a glass membrane eletrode.
5. (6%) (A) What is liquid junction potential?
(B) List several sources of uncertainty in pH measurements with a
glass/calomel electrode system.
6. (12%) Explain the principle of operation of ion-selective electrode. How
does a compound electrode (gas sensing probe) differ from a simple
ion selective electrode?
7. (3%) Describe three mechanisms responsible for the transport of dissolved
species to and from an electrode surface.
8. (8%) (A) Define stripping voltammetry.
(B) Why are stripping methods more sensitive than other voltammetric
procedures?
9. (6%) What is a Clark electrode, and how does it work?
10.(12%) Derive an equation that describe the effect of the analytical
concentration of KCl on the solubility of AgCl in an aqueous
solution. Calculate the concentration of KCl at which the solubility
is a minimum.
Note: Ksp=1.82*10^-10; Kd=3.9*10^-4; Kf2(AgCl2 -)=2.0*10^-5;
Kf3(AgCl3 2-)=1
11.(10%) Please explain the following figure.(圖是偵測血糖用的電極構造圖)
12.(9%) Explain the electrochemical behavior of (a) 5mM Cd2+ in 1M HCl and
(b) 1M HCl alone in terms of the following terms indicated:
Half-wave potential, Diffusion current, Residual current.
13.(9%) A cell was set for measuring the formation constant(Kf) of
Hg(EDTA)2-. The right hand conpartment contains 0.500mmol of Hg2+ and
2.00mmol of EDTA in 0.100L buffered to pH 6.00. The left half cell is
a standard hydrogen electrode. The cell voltage is +0.342V. Find the
value for Hg(EDTA)2-.
(Hg2+ + 2e- <-> Hg(l) Eo=0.852V; Kf for Hg(EDTA)2- is 3*10^21;
αY4- for EDTA at pH 6.00 is 1.8*10^-5)
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