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东 南 大 学 考 试 卷(B卷)  

2013-04-27 14:59:10|  分类: 化学尖端 |  标签: |举报 |字号 订阅

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东 南 大 学 考 试 卷(B卷)

 


课程名称

Analytical Chemistry

考试学期

10-11-3

得分

 

 

适用专业

样    卷

考试形式

闭卷

考试时间长度

120分钟

 

(可携带计算器)

 

 

题号

得分

 

 

 

 

一、 选择题(每题2分,共15题,共30分)

1. In which one is there 4 significant figures:   (     B       )

A. 0.125             B. 0.001305        C. 3.05×104         D. 0.0305

2. Write answer with the correct number of digits for the equation log (2.20 × 10-10) = ? (  D   )

A. -9.6576          B. -9.66            C. -9.7             D. -9.658

3. Which of the following choices cannot function as a Bronsted-Lowry acid?(   B   )

A. H2O        B.  NH3      C. HSO3-       D. HOCl      E. HI

4. Two aqueous solutions are mixed: 25ml of HCl (pH=1) and 25ml of HCl (pOH=13).What is the pH value of the resulting solution?( A  )

A. 1     B. 13     C.  7     D.  6

5. What is the pH of 0.10 mol/L H2Se solution that has the stepwise dissociation constants Ka1=1.3×10-4 and Ka2=1.0×10-11? (  A  )

A. 2.44     B.  3.89     C.  4.89     D.  5.50

6. The value of Ksp for Fe(OH)3 is 2.6 × 10–39. What is the solubility of Fe(OH)3 in mol/L? (      )

A. 1.7 × 10–10 mol/L    B. 5.1 × 10–20 mol/L    C. 2.9 × 10–20 mol/L    D. 9.9 × 10–11 mol/L

7. The Cl- content is directly analyzed by Mohr’s method at pH=11, introducing (   A  ) in the final result.

A.a positive error    B.a negative error   C.an uncertain error     D.no change

8. What is the electrode potential at the equivalence point for Ce4+ titrated with Fe2+( Eθ’ (Fe3+/Fe2+) =0.68V,  Eθ’(Ce4+/Ce3+)=1.44V)?( B  )V.

A. 0.38       B. 1.06        C. 1.32        D. 1.49        E. 0.89

 

9. For the reaction: Ce4+ +Fe2+ Ce3+ +Fe3+ ( Eθ’ (Fe3+/Fe2+) =0.68V,  Eθ’(Ce4+/Ce3+)= 1.44V), lgKθ’=?(    A      )

        

              

10. Which statement is incorrect?

11. What is the pH of a buffer solution

12. For which should the solubility of AgCl in the following solution be lowest?

13. Indicate how many significant figures there are in:

(a)  0.305 0 (b)  0.003 050 (c)  1.003 × 104

solution:(a)  4 (b)  4 (c)  4

14. Round each number as indicated:

(a)  5.124 8 to 4 significant figures:5.125

15. Which buffer system will have the greatest buffer capacity at pH 8.5?

16. What is the concentration of total free EDTA ion at

 

二、填空题(第1题8分,第2题3分,第3题3分,第4题8分,第5题8分,共30分)

1. Write each answer with the correct number of digits:

(a)  3.021 + 8.99 = 12.01

2. Identify the Br?nsted-Lowry acids on both sides of the reaction:

3. Identify the conjugate acid-base pairs in the reaction:

4. Calculate the concentration of H+ and the pH of:  (a) 0.001 0 mol/L HClO4

5. What fraction of the total H+ in this solution is derived from dissociation of water? 

6. Given that the Ka value for   HA  is          , calculate Kb for   A-  

7. Write a charge balance equation for an aqueous solution of HA- 

8. Write a mass balance equation for an aqueous solution of HA- 

9. Write a proton balance equation (PBE) for an aqueous solution of HA- 

10. Consider the titration of 20.00mL of 0.02132 mol·L-1 KCl with 0.02010 mol·L-1 AgNO3(Ksp(AgCl)=1.6×10-10). At the equivalence point, the volume of added AgNO3:      ; pAg+ :      . When the volume of added AgNO3 is 20.00 mL, pAg+ :      . When the volume of added AgNO3 is 27.60 mL, pAg+ :        .

11. Calculate the maximum lgαY(H) values for effectively titrated 0.02 mol·L-1 A2+, B2+ and C2+ with 0.02 mol·L-1 EDTA, respectively, the results are: A2+      ,  B2+      ,  C2+      .  Calculate the minimum pH values are: A2+      ,  B2+      ,  C2+      .  Consider the titration of 0.02 mol·L-1 A 2+ with 0.01 mol·L-1 EDTA at pH 10, p A =        at the equivalence point.

Mn+

A2+

B2+

C2+

lgKMY

 

 

 

 

pH

1.0

2.0

3.0

4.0

5.0

6.0

7.0

8.0

9.0

10.0

11.0

12.0

lgαY(H)

18.01

13.51

10.6

8.44

6.45

4.65

3.32

2.27

1.28

0.45

0.07

0.01

12. How many milligrams of oxalic acid dihydrate, H2C2O4·2H2O (FM 126.07 g·mol-1), will react with 1.00 mL of 0.027 3 mol·L-1 ceric sulfate (Ce(SO4)2) if the reaction is:   H2C2O4 + 2Ce4+→2CO2 + 2Ce3+ + 2H+    (sometimes the reaction equation is not given)

13. Find the concentration of free Ca2+ in 0.050 M CaY at pH 10.00

14. What fraction of free EDTA is in the form Y4- at pH 10.00

15. If a c M solution of a base has pH =   , find Kb for the base.

 

三、计算题(每题10分,5题任选4题,共40分)

1. Calcium concent in a mineral was analyzed five times by the same method:0.0271,0.0282,0.0279,0.0271,0.0275. Calculate the following. (a) mean (b) median (c) percent average deviation (relative average deviation) (d) percent standard deviation(relative standard deviation, coefficient of variation, CV).

2. Using the Q test, decide whether the value 1.956 should be rejected from the set of results:

3. How to prepare a buffer solution of 450mL pH=4.70 by the mixing of 0.1mol/L HAc solution and 0.1mol/L NaAc solution?(Ka(HAc)=1.8×10-5)

4. In an acidic solution, 1.00mL KHC2O4·H2C2O4 solution reacts with 2.00mL KMnO4 standard solution (T(FeSO4·H2O/KMnO4)=0.01125 g/mL). Calculate the volume of 0.2115mol/L NaOH solution required to react with the 20.00 mL KHC2O4·H2C2O4 solution completely. (M(FeSO4·H2O)=169.93 g/mol)

5. A mixture weighing 27.73 mg containing only FeCl2 (FM 126.75 g·mol-1) and KCl (FM 74.55 g·mol-1) required 18.49 mL of 0.02237 mol·L-1 AgNO3 for complete titration of Cl-. Find the mass of FeCl2 and the weight percent of Fe in the mixture.

Solution:

6. Given:Eθ of Cu2+/Cu+ couple is 0.16V, Kspθ of CuI is 1.1×10-12. Calculate the conditional electrode potential of Cu2+/Cu+ couple supposing that the concentration of KI is 1mol/L.

Eθ’=0.87V

7. a solution prepared by mixing 0.100 mol/L A with an equal volume of B

8. Calculate the concentration of free metal ion at

9. Consider the titration of 20.00 mL of c1 mol·L-1 KBr with c2 mol·L-1 AgNO3.  Calculate pAg+ at the following volumes of added AgNO3: (a)  20.00 mL (b)  Veq (c)  22.60 mL

10. Calculate how many milliliters of c1 M HCl should be added to how many grams of sodium acetate dihydrate (NaAc·2H2O, FM=118.06 g/mol) at 5?C to prepare V mL of c2 M buffer, pH 5.00.  At 5?C, pKw = 14.734 and pKa for acetic acid is 4.770.

11. Find the pH of c M H2A. Calculate the concentration of each form of H2A in this solution.

12. Find the conditional formation constant for CaY at pH 10.00.


13. A sample that may be a mixture of A and B is titrated with the two-indicator methods.

Identify the mixture and calculate the percentage of each component.

 

可能涉及的专业词汇:

FM (分子量或摩尔质量), dissolve(使溶解), the diprotic acid, the complexation titration, the precipitation titration, Condition equilibrium constant, Condition electrode potential, buffered, iodometry method, The product(产物),The conjugate acid(共轭酸), the strong base(强碱),buffer solution(缓冲溶液),the proton balance equation (PBE,质子平衡式),solubility(溶解度), solubility product constant(溶度积常数),  calculate the molar solubility(计算摩尔溶解度), precipitation(沉淀), formation constant(稳定常数), dissociation constant(离解常数), equilibrium constant(平衡常数), titrate(滴定), the maximum pH value(最大pH值), the minimum pH value(最小pH值), the excess (过量),cell potential(电池电动势), cathode(阴极,正极,positive electrode) , anode(阳极,负极),negative electrode, fraction of dissociation,to reach the methyl orange (MO) end point, to reach the phenolphthalein (PP) end point.etc.

 

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