化学专业英语练习题(8页).doc

-化学专业英语练习题-第 8 页Final Examination Paper . Monochoice questions依数性6. The red blood cell will be shrinkable in which solution listed below?（ ） g·L-1CaCl2·2H2O(Mr147)B. ·L-1NaHCO3(Mr84.0) g·L-1NaCl D. 224g·L-1C3H5O3Na(Mr112)11. There are four water solutions of the equal volume in which there are equal mass of glucose, CaCl2, NaHCO3 and sucrose respectively. Then whose freezing-point is the lowest? ( )Mr(glucose)180( HAc)60(Na2CO3)106 (CaCl2) 111A. GlucoseB. HAcC. CaCl2 D. Na2CO312. Which choice listed below is isotonic solution? ( )A. 5% glucose solution and 5% sucrose solutionB. 1 mol·L-1 glucose solution and 0.5 mol·L-1 sucrose solutionC. 0.5 mOsmol·L-1 urea solution and 0.5 mOsmol·L-1 NaCl solutionD. 0.5 mol·L-1 MgSO4solution and 0.5 mol·L-1 CaCl2 solution电解质9. We learn that the Ka of HF is 3.53×10-4 and the Kb of NH3·H2O is 1.79×10-5, then which option following is true?( )A. NH4 is a stronger acid than HFB. NH4 is a weaker acid than HFC. the acidic strength of NH4 and HF are equal.D. can not do the compare13. A solution was prepared by mixing equal volume of 0.10mol·kg1NH4Cl and 0.10mol·kg1NH3·H2O, its ionic strength ( I ) is ( ) mol·kg1. B. 0.075 C. 0.10 D. 0.15 14. 0.10mol NaOH and 0.10mol HAc are dissolved into distilled water together, please calculate the pH of this solution( ) (Ka(HAc)=1.74×105)(A) 10.28 B. 11.28 C. 8.88 D. 12.28 15. There is 1L 0.1mol·L1H2CO3 solution with the addition of 0.5ml 0.1mol·L1 HCl solution. Which choice listed below is true? ( )A. pH decrease, dissociation degree of H2CO3 decrease. B. pH decrease, dissociation degree of H2CO3 increase.C. pH increase, dissociation degree of H2CO3 increase.D. pH increase, dissociation degree of H2CO3 decrease.缓冲溶液16.The buffer range of a buffer solution prepared by mixing 500ml 0.4mol·L-1 H2CO3 solution and 200ml 0.4mol·L-1 NaOH is about ( ). (pKa1=6.37; pKa2=10.25 )3.12 B. 6.218.21 C. 11.3213.32 D. 5.377.37. 19. If you mix two solutions of equal volume in each option listed below, which option has no buffer action. （ ）mol·L-1HCl和0.2mol·L-1KClB. 0.02mol·L-1HCl和0.04mol·L-1NH3·H2OC. 0.01mol·L-1KH2PO4和0.2mol·L-1Na2HPO4D. 0.01mol·L-1NaOH和0.02mol·L-1HAc20. The most important ACID resistant in the plasma of human being is （ ）A. H2PO4- B. HPO42- C. HCO3- D. H2CO3 21. The color of the solution is orange with the addition of methyl orange indicator. In order to keep the pH of the solution stable, which buffer system listed below is the best? ( )mol·L-1 HAc 0.1mol·L-1 NaAc (Ka = 1.8×10-5)B. 0.1mol·L-1 NH3·H2O 0.1mol·L-1 NH4Cl (Kb = 1.8×10-5)C. 0.1mol·L-1 NaH2PO4 0.02mol·L-1 Na2HPO4 (Ka = 6.2×10-8)D. 0.1mol·L-1 HCN 0.02mol·L-1 NaCN (Ka = 4.9×10-10).Fill the blank. (Please fill your answers into the blanks following)1. When the HCl standard solution is used to titrate a sample solution which containing NaHCO3 and Na2CO3, the indicator is(1) in the first step of the titration，the indicator is (2) in the second step of the titration (pKa1=6.35；pKa2=10.33) 2.A 2.05 g sample of white phosphorus was dissolved in of carbon disulfide,CS2. The of the carbon disulfide solution was found to be 1.59. The molecular weight of the phosphorus is (3) g·mol-1 in solution? The formula of molecular phosphorus is (4) mol·L-1 (boiling-point elevation constant Kb of CS2=2.4; Mr(P)=31).Calculation1. A sample of 0 mL of water and titrated with 0.0633 M NaOH solution. The volume of base required to reach the equivalence point was 18.4 mL. (a) Calculate the molar mass of the acid. (b) After 10.00 mL of base had been added in the titration, the pH was determined to be 5.87. What is the Ka of the unknown acid? Final Examination Paper . Monochoice questions依数性6. The osmotic pressure of a solution prepared by the equal volume of 8.4%（g/ml）NaHCO3 and 18%（g/ml）glucose (C6H12O6) is equal to the osmotic pressure of ( ). Mr(glucose)180 (NaHCO3)84mol·L-1sucrose solution C. 1mol·L-1glucose solutionD. 1 mol·L-1 CaCl2 solution 7. Which of the following statements is a logical deduction ( )A. if a nonvolatile solute is added to water, the boiling point of the solution will be 100.B. the addition of a volatile solute will change the boiling point of the water.C. atmospheric pressure will affect the composition of the aqueous solution.D. if a nonvolatile solute is added to water, the freezing point of the solution will be lower than that of water.电解质8. Which species is the strongest acid that can exist in aqueous solution? ( )A. NaOH B. Na2CO3C. OH- D. KOH9. A 0.1 mol·L-1 solution of potassium acetate, KC2H3O2, has a lower pH than a 0.1 mol·L-1 solution of potassium cyanide, KCN. From this, you can correctly conclude that ( ) A. hydrocyanic acid, HCN, is a weaker acid than acetic acid, HC2H3O2.B. hydrocyanic acid, HCN, is less soluble in water than acetic acid, HC2H3O2.C. the cyanide ion, CN, is a weaker base than the acetate ion, C2H3O2.D. acetate ion, C2H3O2, partially dissociates to form hydronium ion, H3O+.10. The factor that does not affect on the activity coefficient has ( )A. ionic concentration B. charge on the ionC. ionic strengthD. Ka or Kb11.The pH of mixed solution by 0.10mol·L1NH30mol/L NaOH is about ( ).（Kb=1.8×10-5）A. 9 B. 1 C. 6 D. 1312. The solubility of BaSO4 is not changed when it was dissolved in ( ).A. 1mol·L1KCl solutionB. 2mol·L1 Na2SO4 solutionC. pure waterD. no answer13. There is 1L 0.4mol·L1Na2CO3 solution with the addition of 1.0 ml 0.1mol·L1 HCl solution. Which choice listed below is true? ( )A. pH decrease, dissociation degree of CO32- decrease. B. pH decrease, dissociation degree of CO32- increase.C. pH increase, dissociation degree of CO32- increase.D. pH increase, dissociation degree of CO32- decrease.14. 25, the Ksp of Ag2CrO4 is 1.12×10-12, so the concentration of Ag+ ions in the saturate solution of Ag2CrO4 is ( )A.×10-5mol·L-1 B. 1.21×10-5mol·L-1C. 1.21×10-4mol·L-1 D. 6.54×10-4mol·L-1缓冲溶液15.The buffer range of a buffer solution in which there are the same concentrations of Na2HPO4 and NaH2PO4 is about. (pKa1=2.12; pKa2=7.21 pKa3=12.32) Which one is wrong? ( ).B. 6.21D. all the choice above 16. To determine the content of Mg2+ and Ca2+ ions in tap water, in order to keep the pH =10, which buffer system listed below is the best? ( )mol·L-1 HAc 0.1mol·L-1 NaAc (Ka = 1.8×10-5)B. 0.1mol·L-1 NH3·H2O 0.1mol·L-1 NH4Cl (Kb = 1.8×10-5)C. 0.1mol·L-1 NaH2PO4 0.02mol·L-1 Na2HPO4 (Ka = 6.23×10-8)D. 0.1mol·L-1 H2CO3 0.02mol·L-1 NaHCO3 (Ka = 4.3×10-7)17. The most important ACID resistant in the plasma of human being is （ ） A. H2PO4- B. HPO42- C. HCO3- D. H2CO3 18. If you mix two solutions of equal volume in each option listed below, which option has no buffer action. （ ）mol·L-1HCl and 0.2mol·L-1KClB. 0.02mol·L-1HCl and0.04mol·L-1NH3·H2O·L-1KH2PO4and 0.2mol·L-1Na2HPO4D. 0.01mol·L-1NaOH and 0.02mol·L-1HAc.Fill the blank. (Please fill your answers into the blanks following)1. the theoretical range of color change of a weak basic indicator is (1) which Kb is 1.0×104 2 g sample of the protein hemoglobin is dissolved in enough water to make 1 L (kg) of solution. The osmotic pressure of the solution is measured at 25 kPa. The molecular mass of hemoglobin is (2) and the molality of the hemoglobin solution is (3) .Final Examination Paper . Monochoice questions1. 依数性How much is the normal freezing points of the solution in which NaCl is dissolved in 135mLof water ? Kf =1.86 K·kg·mol-1 , Mr(NaCl)=58.5 ( )A. -9.89B. 19.89C. 9.89D. 19.89 2. If you want to have osmosis between two dilute solutions separated by semipermeable membrane, which choice listed below is wrong.（ ）A.Both of the two osmotic pressure are not equal. B. Both of the two osmolarity are not equal. C.Both of the two solutions are not isotonic.D. Both of the two molality are not equal.3. In 500mL normal saline water, the osmolarity of the Cl- ions is ( ) mOsmol·L1 Mr(Cl)=35.5A. 77B. 196C. 154D. 3084. The minimum mass of NaCl that would have to be added to 1.200×103 g H2O so the resulting solution would not freeze outside on a cold day(-10) is ( ) ( Kf =1.86 K·kg·mol-1 , MrNaCl=58.5)A.B. C.D.5. 电解质There is 1L 0.1mol·L1 HAc solution with the addition of 0.5mL 0.1mol·L1 NaCl solution. Which choice listed below is true? ( )A. pH decrease, dissociation degree of HAc decrease. B. pH decrease, dissociation degree of HAc increase.C. pH increase, dissociation degree of HAc increase.D. pH increase, dissociation degree of HAc decrease.6. What is ionic strength ( I ) for the solution that contains 0.10 mol·kg1NaCN and 0.10 mol·kg1HCN ( ).mol·kg1B. 0.050mol·kg1C. 0.20mol·kg1D. 0.10mol·kg1 7. Ksp for SrSO4 is 4.0×10-8 at certain temperature. How much is the solubility of SrSO4 in H2O. ( )×10-8 mol·L-1B. 2.0×10-4 mol·L-1C. 8.0×10-8 mol·L-1D. 1.0×10-4 mol·L-18. Which substance can use as ampholyte in different solvent?( )A. NaNO3B. HAcC. NaClD. NaOH9. 缓冲溶液Which option of the following determines the capacity of a buffer ( )A. Conjugate acid-base pairB. Buffer-component ratioC. Buffer rangerD. pKa of the acid component 10. The buffer range of a buffer solution prepared by mixing 100mL 0.2mol·L-1 H2A solution and 100mL 0.3mol·L-1 NaOH is about ( ). (pKa1=4.00; pKa2=9.00 )5.00B. 5.007.00D. 9.0011.00 11. If two solutions are mixed in equal volume in each option listed below, which option has no buffer action? （ ） mol·L-1 NaOH and 0.2 mol·L-1 KClB. 0.2 mol·L-1 HCl and 0.4 mol·L-1 NH3·H2OC. 0.1 mol·L-1 H3PO4 and 0.1 mol·L-1 Na2HPO4D. 0.1 mol·L-1 NaOH and 0.2 mol·L-1 HAc12. To prepare a buffer of pH 9, which buffer system listed below is the best? ( ) mol·L-1 HAc 0.1 mol·L-1 NaAc (pKa = 4.75)B. 0.1 mol·L-1 NH3·H2O 0.1 mol·L-1 NH4Cl (pKb = 4.75)C. 0.1 mol·L-1 H2CO3 0.15 mol·L-1 NaOH (pKa1=6.37; pKa2=10.25 )D. 0.1 mol·L-1 HCN 0.02 mol·L-1 NaCN (pKa = 9.5). Simple answer question1. 酸碱滴定Can 0.1000 mol·L-1 formic acid (HCOOH) of 20.00 mL be titrated by 0.1000 mol·L-1 NaOH standard solution directly? Please give reasons. What indicator can be used to signal endpoint (pKa)? （5 marks）2. 电解质溶液Pivaic acid is a monoprotic weak acid. A 0.100 mol·L-1 solution of pivalic acid has a pH=3.00. What is the pH of 0.100 mol·L-1 sodium pivalate at the same temperature? 3. How many significant figures are there in each of the following numbers (assume that each number is a measured value)?Final Examination Paper . Monochoice questions1. 酸碱滴定If you had to do the calculation of (22.83-21.43)/1.4000, what would be the correct result of significant figure? ( )A. B. C. D. 2. If the KHIn of a weak acidic indicator is 1.0×10-5, what is the color transition pH range of this indicator? ( )A. 4-6B. 6-8C. 7-9D. 8-10 3. What result would be if NaOH solution was standardized against potassium hydrogen phthalate, the measured concentrations of the NaOH solution in the cases that the mass of potassium hydrogen phthalate should be 0 g, but was recorded as 0 g by mistake? ( )A. highB. lowC. unchangeD. uncertain 4. How many grams of potassium hydrogen phthalate (KHC8H4O4) primary standard substance are required to standardize about 25 mL of 0.1 mol·L-1 NaOH solution? ( ) Mr(KHC8H4O4)204 g·mol-1A. B.gC. gD. g5. 依数性How much is the normal freezing points of the solution in which of urea is dissolved in 66.7 mL of water ? Kf =1.86 K·kg·mol-1 , Mr(CON2H4)=60.0 ( ) A. -B. 0C.D. 6. The osmolarity of 1000 mL officinal solution in which it contains NaHCO3 of ·L -1 and KCl of 5.79 g·L -1 is ( ) mOsmol·L1. Mr(NaHCO3)=84, Mr(KCl)B. C. 309D. 6107. A hemoglobin (Hb) solution of 1L is prepared by dissolving of Hb into water. If the osmotic pressure of the solution is found to be 1.33kPa at 25. The molar mass of hemoglobin is ( ) .A. 537B. ×10-4C. 2×104D. 1008. 电解质8,9,10,11,12,13,14There is 1L 0.1mol·L1 NaHCO3 solution with the addition of 0.1mol NaCl solid. Which choice listed below is true? ( )A. pH unchanged, dissociation degree of HCO3 unchange. B. pH decrease, dissociation degree of HCO3 increase.C. pH increase, dissociation degree of HCO3 increase.D. pH increase, dissociation degree of HCO3 decrease.9. what is ionic strength ( I ) for mol·kg1 NaCl solution ( ) mol·kg1.A. 0.025 mol·kg1B. 0.050mol·kg1C. 0.20mol·kg1D. 0.10mol·kg1 10. In a saturated solution of calcium phosphate, the concentration of ion is 3.3×10-7 mol·L-1. the Ksp of Ca3(PO4)2 is ( )A.×10-7B. 1.65×10-7C. 9.9×10-21D. 1.3×10-32 11. Which substance can use as strong base in glacial acetic acid ?( )A. HAcB. NH3C. H2OD. H3PO412. A solution is 0.15 mol·L-1 in Pb2+ and 0.20 mol·L-1 in Ag+. If a solid of Na2SO4 is added slowly to this solution until the Ag+ starts to precipitate as the sulfate. What is SO42- concentration reached at least at this point? ( ) Ksp for PbSO4 = 2.53×10-8, Ag2SO4 =1.20×10-5.A. ×10-8B. 2.53×10-8C. 3.0×10-4D. 1.20×10-5 13. pH of solution in which 0.2 mol·L1 H3PO4 solution and 0.2 mol·L1 Na3PO4 solution are mixed in the same volume is ( D ) (Ka1= 7.5×10-3 , Ka2= 6.3×10-8 , Ka3= 2.2×10-13)A. 12.8B. 1.32C. 2.12D. 14. 125.0 mL of 0.40 mol·L-1 propanic acid, HPr, is diluted to 500.0 mL. What will the final pH of the solution be? (Ka=1.0×10-5) ( )A. 3B. 11C. 5D. 9 缓冲溶液 15. The buffer range of a buffer solution prepared by mixing 100ml 0.2mol·L-1 H3PO4 solution and 100ml 0.5mol·L-1 NaOH is about ( ). (pKa1=; pKa2=; pKa3= )A. 3.16B. 8.21C. 8.0010.00D. 16. The color of the solution is yellow with the addition of methyl orange indicator and red with the addition of methyl red. In order to keep the pH of the solution stable, which buffer system listed below is the best? ( )mol·L-1 HAc 0.1mol·L-1 NaAc(pKa = )B. 0.1mol·L-1 NH3·H2O 0.1mol·L-1 NH4Cl(pKb = )C. 0.1mol·L-1 NaH2PO4 0.1mol·L-1 Na2HPO4(pKa2= )D. 0.1mol·L-1 HCN 0.1mol·L-1 NaCN(pKa = 9.5)17. Which of 0.1 mol·L-1 NaOH in the following solution? ( ) mol·L-1 mol·L-1 NaAc(pKa = ) mol·L-1 NH3·H2 mol·L-1 NH4Cl(pKb = ) mol·L-1 H2CO3 0.15 mol·L-1 NaOH(pKa1=6.37; pKa2=10.25 ) mol·L-1 HCN 0.02 mol·L-1 NaCN(pKa = 9.5)18. To pr