Loyola College Instrumental Methods Of Chemical Analysis Question Papers Download

Loyola College M.Sc. Chemistry April 2006 Instrumental Methods Of Chemical Analysis Question Paper PDF Download

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             LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – ZOOLOGY & BIOMEDICAL INSTRUMENTATION

LM 32

SECOND SEMESTER – APRIL 2006

                          CH 2901 – INSTRUMENTAL METHODS OF CHEMICAL ANALYSIS

 

 

Date & Time : 28-04-2006/9.00-12.00         Dept. No.                                                       Max. : 100 Marks

 

 

Part-A   ANSWER ALL QUESTIONS (10 ´ 2 = 20)

  1. Define: (i) a mole   (ii) molarity
  2. If drinking water contains 1.5 ppm of NaF, how many liters of water can be fluoridated with 454 g of NaF?
  3. Explain hypsochromic shift with an example.
  4. Sketch and explain the fundamental difference in instrumentation between Flame Emission and Atomic Absorption Spectrometers?
  5. What is optical activity? Give an example.
  6. Compare the energy of the following electromagnetic radiation

(i) Radio wave                 (ii) Infrared rays     (iii) Visible light

  1. Mention the nuclear spin quantum number (I) for 6C12, 1H1
  2. Compare the absorption frequencies of C-C and C=C.
  3. Define ‘base peak’.
  4. What kind of electromagnetic radiation is used to study crystal structure?

 

Part-B   ANSWER ANY FIVE QUESTIONS (5 ´ 8 = 40)

  1. (a) State Beer-Lambert’s law and explain under what conditions it is not applicable.

(b) The molar absorptivity of a particular solute is 2.1 x 104 L cm-1mol-1. Calculate the transmittance through a cuvette with a 5 cm light path for

a 2.0 x 10-6 M solution.

  1. (a) Explain the significance of λmax and ε values in UV-Visible spectroscopy with a suitable example.

(b) Spectrophotometry is a very useful quantitative technique in the applications of biological systems. Can you substantiate this statement with two examples?

  1. Discuss in detail the instrumentation and application of nephelometry.
  2. Explain briefly the principle of ICP AES and its advantages over AAS methods?
    1. Determine the force constant for the C-H bond, given the stretching frequency of the C-H bond as 3000cm-1.

 

  1. Calculate the pH of the following solutions.
  • 10-2 M Ca(OH)2
  • Mixture containing 10-2 M NH4Cl and 10-1 M NH4 Kb of NH4OH is 10-5.
  1. Discuss the applications of isotopic dilution analysis.
  2. Draw the low resolution NMR spectrum of ethyl alcohol and explain.

 

Part-C   ANSWER ANY TWO QUESTIONS (2 ´20 = 40)

 

  1. (a) Define Beer-Lambert’s law explaining the terms involved and state under what conditions it is not applicable.

(b) With a schematic diagram explain the different parts and working of a Double-Beam Spectrophotometer. What are its advantages over a single-beam instrument?                                                                   (10+10)

  1. (a) Discuss the principle and working of an Atomic Absorption Spectrometer and how it can be used in the quantitative determination of lead (Pb2+) in blood.

(b) Give an account of how AAS can be used in studying the toxicological effects of mercury.                                                           (15+5)

  1. (a) Describe the method of determining the pH of a solution using a potentiometer.

(b) Discuss the instrumentation of Gas Chromatography.

  1. (a) Discuss the principle involved in NMR spectroscopy and explain its instrumentation.

(b) Distinguish the following

(i)  CH3   CHCl  CH3      and          CH3  – CH2 -CH2Cl     by NMR

(ii)   CH3  CH2 CHO      and          CH3  -CO -CH3             by IR

(iii)   CH3OH                 and          CH3  CH2 OH             by mass spectrum.

 

 

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Loyola College M.Sc. Chemistry April 2007 Instrumental Methods Of Chemical Analysis Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

LM 36

M.Sc. DEGREE EXAMINATION – ZOOLOGY / BMIS

SECOND SEMESTER – APRIL 2007

CH 2901 – INSTRUMENTAL METHODS OF CHEMICAL ANALYSIS

 

 

 

 

Date & Time: 26/04/2007 / 1:00 – 4:00      Dept. No.                                       Max. : 100 Marks

 

 

Part-A   ANSWER ALL QUESTIONS (10 x 2 = 20)

 

  1. Define: (i) molarity (ii) ppm
  2. Explain Bathochromic shift with an example.
  3. What is the volume of 6M H2SO4 (MW=98 gmol-1) that contains 20 g of H2SO4 solute?
  4. What are the two sources of flames used commonly in Atomic Absorption Spectrometers?
  5. Define the specific rotation of an optically active compound.
  6. Determine the pH of 10-3M Ba(OH)2
  7. Compare the fundamental vibrational frequency of C-O and C=O.
  8. How is the internuclear distance determined by X-ray diffraction studies?
  9. Which of the following will give NMR signal (i) 8O16 and (ii) 6C13
  10. Predict the m/e value for the molecular ion peak of C6H6.

 

 

Part-B   ANSWER ANY FIVE QUESTIONS (5 x8 = 40)

 

  1. (a) State Beer-Lambert’s law and explain under what conditions it is not applicable.

(b) With a schematic diagram indicate the different parts and working of a Double-Beam Spectrophotometer. What are its advantages?                                      (3+5)

  1. With a sketch discuss the principle, parts and working of a fluorimeter and how it is used in the analysis of riboflavin (vitamin B2).
  1. With a diagram outline the principle, parts and working of a cold-vapor atomic absorption spectrometer in the determination of mercury in a given biological sample?
  1. With a schematic diagram discuss the principle, parts and working of a spectropolarimeter. Mention any one application.
  2. How is the fluoride content in water sample estimated using ion selective electrode?
  3. Describe the principle and instrumentation of NMR spectroscopy.
  4. Write an account of ‘Isotopic dilution analysis’.
  5. Calculate the fundamental frequency in the infrared absorption region for the C=C stretching vibration. (k = 9.77 x 105 dynes cm-1; c = 3 x 1010 cms-1)

 

 

 

Part-C   ANSWER ANY TWO QUESTIONS (2 x20 = 40)

 

  1. (a) Discuss in detail the instrumentation and application of nephelometry

 

(b) Discuss the principle and working of an Atomic Absorption Spectrometer

and how it can be used in the quantitative determination of lead (Pb2+) in blood.

(10+10)

  1. Define and explain briefly the following concepts and its importance with a

suitable example:

 

(a) Difference Spectrometry (b) turbidimetry (c) ICP AES   (d) monochromator

(e) hollow-cathode lamp                                                                    (4 each)

 

  1. (a) Discuss the principle and instrumentation of HPLC.

(b) Describe the applications of neutron diffraction.

 

  1. (a) Give an account of the application of IR spectroscopy.

(b) Distinguish the following

H    H                                            H           H

|      |                                              |             |

(i)    H –C—C—O—H           and       H—C—O—C—H    using NMR.

|      |                                              |             |

H    H                                            H           H

H

|

(ii)   CH3 –C—H           and           CH3 –C–OH             using IR

||                                            |

O                                           H

 

 

(iii)   CH3OH                 and          CH3–CH2–OH         using mass spectra.

 

 

 

 

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Loyola College M.Sc. Chemistry April 2008 Instrumental Methods Of Chemical Analysis Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

GH 35

M.Sc. DEGREE EXAMINATION – BIO INSTRUMENT. & ZOOLOGY

SECOND SEMESTER – APRIL 2008

    CH 2901 – INSTRUMENTAL METHODS OF CHEMICAL ANALYSIS

 

 

 

Date : 26/04/2008            Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

PART-A   ANSWER ALL QUESTIONS (10 x 2 = 20)

  1. Define: ppb and Molarity
  2. What is a primary standard solution? Give an example.
  3. Give two important quantitative applications of spectrophotometer in biological systems.
  4. What is the role of ‘flame’ in AAS? Why no ‘flame’ is used in cold vapor AAS technique?
  5. What is optical activity? Give an example.
  6. What is the pH of 0.425M solution of acetic acid if Ka for acetic acid is 1.8 x 10-5 mol L-1?
  7. What are the experimental methods used to determine the crystal structure?
  8. Mention the nuclear spin quantum number (I) for 16O8 and 19F9.
  9. Give examples for stationary liquid, which are used in gas chromatography.
  10. Write the expression for the fundamental vibrational frequency defining the terms in it.

 

PART-B   ANSWER ANY FIVE QUESTIONS (5 x8 = 40)

 

  1. (a) State Beer Lambert’s law and explain under what conditions it is not applicable.

(b) A 7.0 x 10-5 M solution of KMnO4 has a transmittance of 44% when measured in a 2.0 cm

cell at a wavelength of 523 nm. Calculate (a) the absorbance of this solution (b) the molar

absorptivity of KMnO4.                                                                                         (5+3)

  1. Discuss in detail the instrumentation and application of nephelometry in the determination of

phosphate ion.

  1. Explain briefly the principle and instrumentation of ICP AES and its advantages over AAS

methods.

  1. Sketch and describe the working of a typical Fluorimeter and how it can be applied in the

quantitative analysis of riboflavin.

  1. Discuss in detail the composition and role of glass electrode in the working of a pH meter

how the pH of a given solution can be determined using a pH meter.

 

 

  1. (a) In an ESR spectrometer operating at 9.233 GHz, the center of the spectrum of CH3

                   radical occurred at 329.4 mT. Calculate the g-value of the free radical.

(b) Describe the applications of electron diffraction.

  1. Describe the Bragg equation for X-ray crystallography.
  2. Discuss in detail the principle and applications of the isotopic dilution analysis.

 

PART-C   ANSWER ANY TWO QUESTIONS (2 x 20 = 40)

 

  1. (a) With a schematic diagram explain the different parts of a Double-Beam

Spectrophotometer and mention its advantage over single-beam instrument.

(b) What is the basic difference between Optical Rotatory Dispersion (ORD) and Circular

Dichroism (CD)? With a schematic diagram discuss the principle, parts, and working of a

Spectropolarimeter.

 

  1. (a) Discuss the principle and working of an Atomic Absorption Spectrometer and how it can

be used in the quantitative determination of lead (pb2+) in blood.

(b) Describe the composition and working of a Fluoride Ion Selective Electrode and how it

is used in determining the fluoride content of drinking water.

 

  1. (a) Write notes on (i) Thermal conductivity (ii) Electron Capture Detector

(b) Describe the applications of neutron diffraction.

 

  1. (a) Discuss the principle involved in ESR spectroscopy and explain its instrumentation.

(b) How are the following compounds distinguished?

 

 

 

(i)               H3C                               H2C – CH2

C=O    and          |       |

H3C                               H2C – CH2                            by NMR

 

 

(ii)   CH3-CH2-C-H             and   CH2=CH-CH2-OH                       by IR

||

O

 

(iii) CH3-CH2-CH2-C = O      and CH3-C-CH2-CH2-CH2-CH3          by Mass

|

H

 

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Loyola College M.Sc. Chemistry Nov 2012 Instrumental Methods Of Chemical Analysis Question Paper PDF Download

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LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

M.Sc. DEGREE EXAMINATION – CHEMISTRY

SECOND SEMESTER – NOVEMBER 2012

CH 2901 – INSTRUMENTAL METHODS OF CHEMICAL ANALYSIS

 

 

Date : 06/11/2012            Dept. No.                                        Max. : 100 Marks

Time : 1:00 – 4:00

 

PART A

Answer all the questions:                                                                   10×2=20 Marks

 

  1. Define molarity.
  2. State Beer Lambert’s law.
  3. Calculate the pH of 0.01N NaOH.
  4. What is Buffer solution? Give an example.
  5. Mention the principle of HPLC.
  6. State Bragg’s law.
  7. Give an example for Mc-Lafferty rearrangement.
  8. Mention the significance of finger print region in IR spectroscopy.
  9. Define gyroscopic motion.
  10. How many ml of conc.HCl (density = 1.18 g/ml, 36.0 wt% HCl, MW = 36.5) should be diluted to 1litre to produce a 0.100 M solution?

 

PART B

Answer any eight questions:                                                                        8×5=40 Marks

 

  1. What are the requirements of a primary standard?
  2. How is sulphate determined by turbidometry?
  3. Discuss the significance of PMT.
  4. Explain the analysis of riboflavin by spectroflurometry.
  5. Write a short note on circular dichroism with an example.
  6. How is ion selective electrode helpful in the analysis of fluoride in drinking water?
  7. Draw and explain the working principle of a thermal conductivity detector.
  8. Briefly explain the instrumentation of EPR.
  9. Explain the fragmentation pattern of decane.
  10. Discuss the absorption bands of functional groups in IR spectrum.
  11. Explain the method of single crystal XRD determination.
  12. Write short notes on detectors used in HPLC.

 

 

PART C

Answer any four questions:                                                                4×10=40 Marks

 

  1. Draw and explain the working principle of dark beam spectrophotometer.
  2. Briefly discuss the instrumentation of AAS.
  3. a) Explain the instrumentation of turbidometry.
  4. b) How is phosphate determined by turbidometry.
  5. Draw the block diagram and explain the instrumentation of GC.
  6. Explain the fragmentation pattern of
  7. a) benzyl alcohol
  8. b) pentanoic acid
  9. Briefly explain the instrumentation of NMR with a block diagram.

 

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