DEPARTMENT OF CHEMISTRY – PERIYAR MANIAMMAI …



|COURSE CODE |XAC104/XAC204 |L |T |P |C |

|COURSE NAME |APPLIED CHEMISTRY |3 |1 |1 |5 |

|PREREQUISITES |Nil |L |T |P |H |

|C:P:A |2.8:0.8:0.4 |3 |2 |2 |7 |

|COURSE OUTCOMES |DOMAIN |LEVEL |

|CO1 |Identify and describe the various water quality parameters and methods to purify water in |Cognitive |Remember |

| |context with boilers and domestics usage. |Psycomotor |Perception |

|CO2 |Explain the fundamental principles of electrochemical reactions, its applications in redox |Cognitive |Understand Set |

| |reactions and calculate the different electrochemical processes. |Psycomotor | |

|CO3 |Interpret the types of corrosion, use and measure its control by various methods including |Cognitive |Apply |

| |protective techniques. |Psycomotor Affective |Mechanism Receive |

|CO4 |Describe, Illustrate and Discuss the generation of energy in batteries, nuclear reactors, |Cognitive |Remember |

| |solar cells, fuel cells and anaerobic digestion. | |Analyse |

| | |Affective |Respond |

|CO5 |Apply and measure the different types of spectral techniques for quantitative chemical |Cognitive |Remember |

| |analysis and list nanomaterials for various engineering processes. | |Apply |

| | |Psycomotor |Mechanism |

| |Theory Part |

| |

| |

|UNIT – I WATER TECHNOLOGY |

|7 + 8 +9 |

| |

|Sources and types of water – water quality parameters – BIS and ISO specifications- hardness: types and estimation of hardness (problems) – |

|alkalinity: types and estimation (problems) – boiler feed water – requirements – disadvantages of using hard water in boilers – internal treatment, |

|external treatment – demineralization process – desalination using reverse osmosis – domestic water treatment – Effluent treatment processes in |

|industries |

| |

|UNIT – II ELECTROCHEMISTRY |

|8+5 +15 |

| |

|Basic concepts of conductance – Kohlraush’s law and conductometric titrations –electrode potentials– Nernst equation: derivation and problems – |

|reversible and irreversible cells – electrolytic and electrochemical cells – emf and its measurements – types of electrodes-reference electrodes – |

|primary and secondary – glass electrode – determination of pH using quinhydrone and glass electrodes – electrochemical series and its applications –|

|Galvanic cells and concentration cells – potentiometric titrations - redox titrations. |

| |

| |

|UNIT – III CORROSION AND PROTECTIVE COATINGS |

|9 + 4 +3 |

| |

|Corrosion- causes- types-chemical, electrochemical corrosion (galvanic, differential aeration), corrosion in electronic devices, corrosion control -|

|material selection and design aspects - electrochemical protection – sacrificial anode method and impressed current cathodic method. |

|Protective coatings: paints- constituents and functions - electroplating of copper and gold, Electroless plating - Distinction between |

|electroplating and electroless plating, |

|advantages of electroless plating, electroless plating of nickel and copper on PCB. |

| |

| |

|UNIT –IV ENERGY STORAGE DEVICES AND NUCLEAR ENERGY |

|12 + 7+0 |

| |

|Energy storage devices – Batteries: Types – primary (dry cell, alkaline cells) and secondary (lead acid, Ni-Cd and Lithium ion batteries) - |

|Supercapacitors – Fuel cells-Hydrogen-Oxygen fuel cell- Solar cells . |

|Nuclear energy: nuclear fission and fusion –chain reaction and its characteristics – nuclear energy and calculations (problems) – atom bomb –Nuclear|

|reactor- light water nuclear power plant – breeder reactor- Weapon of mass destruction- nuclear, radiological, chemical and biological weapons. |

|Disarmament - National and International Cooperation- Chemical Weapon Convention (CWC), Peaceful Uses of Chemistry. Bio fuels: biomethanation- |

|anaerobic digestion process, biomass: sources and harness of energy. |

| |

|UNIT –V SPECTROSCOPY AND NANOCHEMISTRY |

|9 +6 +3 |

| |

|Electromagnetic spectrum - Lambert law and Beer-Lambert’s law (derivation and problems) – molecular spectroscopy -UV- visible spectroscopy: |

|electronic transitions - chromophores and auxochromes – instrumentation (block diagram) - applications – IR spectroscopy: principle – fundamental |

|modes of vibrations – calculations of vibrational frequency – IR spectrophotometer instrumentation (block diagram) – applications of IR |

|spectroscopy. |

|Nanochemistry - Basics - distinction between molecules, nanoparticles and bulk materials; size-dependent properties. Nanoparticles: Nanocluster, |

|nanorod, nanotube and nanowire. Synthesis ; properties and applications of nano materials-Buckminister fullerenes, CNT‟S(Single walled carbon nano |

|tubes and Multi-walled carbon tubes)-Graphene- advantages and applications. |

| |

| |

|TEXT BOOKS |

| |

|1. Jain and Jain , “A Text book of Engineering Chemistry”, Dhanapatrai Publications,New Delhi,    2011. |

|2. Gadag and NityanandaShetty , “Engineering Chemistry”, I.K International publishing |

|House Pvt. Ltd, 2010. |

|3. P. Atkins, J.D. Paula , “Physical Chemistry” , Oxford University Press, 2009. |

|4. S. S. Dara, S. S. Umare, “A Text Book of Engineering Chemistry”, S. Chand Publishing, 2011 |

|5. C.P. Poole and F.J. Owens, “Introduction to Nanotechnology”, , Wiley, New Delhi ,2007. |

| |

|REFERENCE BOOKS |

| |

|Puri B R Sharma L R and Madan S Pathania, “ Principles of Physical Chemistry”, Vishal |

|publishing Co., Edition 2004 |

|2. Kuriocose, J C and Rajaram, J, “Engineering Chemistry”, Volume I/II, Tata McGraw- |

|     Hill Publishing Co. Ltd. New Delhi, 2000 |

| |

|E Resources - MOOCs: |

| |

| |

| |

| |

| |

| |

| |

| |

|Laboratory Part 30 hrs |

| |

|Determination of total hardness, temporary and permanent hardness of water by EDTA method. |

|Determination of alkalinity of water sample. |

|Determination of chloride content of water sample by Argentometric method. |

|Conductometric titration of a strong acid with a strong base. |

|Determination of strength of hydrochloric acid by pH metric method. |

|Conductometric precipitation titration using barium chloride and sodiumsulphate. |

|Determination of strength of iron by potentiometric method using dichromate. |

|Potentiometric acid-base titration using quinhydrone electrode. |

|Corrosion inhibition efficiency by weight loss method. |

|Estimation of iron by colorimetric method. |

|CO1 |

|CO1 |

|CO1 |

|CO2 |

|CO2 |

|CO2 |

|CO2 |

|CO2 |

|CO3 |

|CO5 |

| |

|REFERENCE BOOKS |

|Mendham, Denney R.C,. Barnes J.D and Thomas N.J.K., “Vogel’s Textbook of Quantitative Chemical Analysis”, 6th Edition, Pearson Education, 2004. |

|Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. “Experiments in Physical Chemistry”, 8th Ed.; McGraw-Hill: New York, 2003. |

|Sirajunnisa.A., Sundaranayagi.S.,Krishna.,Rajangam.R.,Gomathi.S., “Applied Chemistry Lab Manual”, Department of Chemistry, PMU Press, Thanjavur, |

|2016. |

| |

|E Resources - MOOCs: |

|1. |

|2. |

|3. |

| |

| |

|LECTURE |

|TUTORIAL |

|PRACTICAL |

|TOTAL |

|HOURS |

| |

|HOURS |

|45 |

|30 |

|30 |

|105 |

| |

| |

| |

Table 1 :Mapping of CO’s with PO’s:

| |PO1 |

|1.1.1 |Able to identify and apply various purification steps in water purification for boiler feed and for domestic supply |

|1.1.2 |Able to derive the Nernst equation and find the electrode potential of unknown cell. |

|1.1.3 |Apply the concept of electrode potential in corrosion of machineries and electronic devices and its control. |

|1.1.4 |Apply the concept of electrode potential and design primary and secondary batteries. |

|1.1.5 |Apply the concept of nuclear fission reaction for energy generation. |

|1.1.6 |Apply anaerobic digestion process to obtain bio-energy. |

|1.1.7 |Describe the different types of spectral & nano techniques and their applications to qualitative and quantitative |

| |chemical analysis |

|PI 2.1 |An ability to design and conduct experiments, as well as to analyze and interpret data |

|2.1.1 |Able to design and estimate various water quality parameters such as hardness, alkalinity and chloride ions in the given |

| |water sample. |

|2.1.2 |Apply the principles of Kohlraush’s law and find the strength of strong acid, mixture of strong acid-weak acid and BaCl2|

| |by conductometric titrations. |

|2.1.3 |Find the strength of Fe2+ by potentiometric titrations |

|2.1.4 |Able to standardize the pH-meter and determine strength of unknown acid solution by measuring pH of a solution. |

|2.1.5 |Ability to standardize the calorimeter and find the strength of unknown iron solution by plotting calibration graph. |

|PI 3.1 |An ability to design a system, component, or process to meet desired needs within realistic constraints such as economic,|

| |environmental, social, political, ethical, health and safety, manufacturability, and sustainability |

|3.1.1 |Able to design a batch type water purification unit. |

|3.1.2 |Able the design and accomplish electroplating of copper and electroless plating of nickel to control corrosion. |

|3.1.3 |Able to construct a laboratory model of biomethanation unit to produce biogas and nuclear reactor disarmament with |

| |peaceful uses of chemistry using chemical weapon convention. |

|3.1.4 |Able to construct a primary battery cell. |

|PI 4.1 |An ability to function on multidisciplinary teams. |

|4.1.1 |Ability to analyze water sample from various units such as municipal water, industrial water and surface water and solve |

| |the water contamination problem by applying the purification process with support from environmental and civil |

| |engineering. |

|4.1.2 |Ability to understand corrosion of materials including electronic corrosion and involve in corrosion control with |

| |inter-disciplinary works. |

|PI 5.1 |An ability to identify, formulate, and solve engineering problems. |

|5.1.1 |Able to consolidate the water quality parameters and apply suitable techniques to solve water contamination problem. |

|5.1.2 |Able to identify the type of corrosion and apply suitable method to control corrosion problem. |

|5.1.3 |Able to identify suitable energy source by comparing the advantages and disadvantages. Able to take effort to improve |

| |renewable energy source, such as solar cells. |

|PI 6.1 |An ability to develop professional and ethical responsibility. |

|6.1.1 |Able to understand the ethical responsibility in analyzing the water sample. |

|6.1.2 |The method to be implemented for water purification should not be harmful to the society. |

|6.1.3 |Ability to develop the professional and ethical responsibility in making batteries and other energy sources. |

|6.1.4 |Able to understand the ethical responsibility of handing chemicals and glass apparatus. |

|PI 7 |An ability to communicate effectively. |

|7.1.1 |Able to justify and communicate suitable method adopted to purify water. |

|7.1.2 |Able to explain the instrumental principle and methodology applied in conductometer, potentiometer, pH meter and |

| |calorimeter. |

|7.1.3 |Able to compare and explain different energy storage devices. |

|PI 8 |An ability to create the impact of engineering solutions in a global, economic, environmental, and societal context. |

|8.1.1 |Ability to create solutions to purify water in terms of environmental and societal service. |

|8.1.2 |Ability to apply suitable method to solve corrosion in machineries. |

|8.1.3 |Ability to apply knowledge in generating energy in economically viable method. |

|PI 9 |Recognition of the need for, and an ability to engage in life-long learning. |

|9.1.1 |Able to recognize the need for improving the technique for purification of water. |

|9.1.2 |Ability to find improved method to control corrosion. |

|9.1.3 |Ability to apply various instrumental methods for qualitative and quantitative analysis. |

|PI 10 |An ability to describe the solutions for complex problems. |

|10.1.1 |Ability to suggest suitable solutions for water purification under abnormal water contaminant in boilers. |

|10.1.2 |Ability to propose improved method for corrosion control in complex situation. |

|10.1.3 |Ability to recommend suitable anode and cathode for batteries. |

|PI 11.1 |An ability to use the techniques, skills, and modern engineering tools necessary for engineering practice. |

|11.1.1 |Ability to use skill of handling instruments is helpful for engineering practices. |

|11.1.2 |Ability to use the technique of preparing different concentrations of solutions is useful in engineering practices. |

|PI 12.1 |Updation of the technical needs in a challenging world in equipping themselves to maintain their competence through life |

| |long learning |

|12.1.1 |Ability to carry out the fundamental and applications of chemistry through their life. |

Table 3: Assessment Template

| | |Marks |Weightage |Weightage |Weightage |

|S.No. |Task | | |Formative |Summative |

|1 |CA 1 (Class Test- 1) |15 |11.25 |37.5 | |

|2 |CA 2 (Class Test -2) |15 |11.25 | | |

|3 |CA3 |20 |15 | | |

|4 |CA 4- End Semester |50 |37.5 | | |

| |Pattern (MCQ – 10% + 2 Marks 10% + Descriptive | | | |37.5 |

| |80%) | | | | |

|5 |CIA -1 (Based on observation Note and rubrics |15 |3.75 | | |

| |designed by lab teacher) | | | | |

| | | | |12.5 | |

|6 |CIA-2 (Lab Mid Exam) |15 |3.75 | | |

|7 |CIA -3 or EA-1- Product/Simulation/Design/ |20 |5 | | |

| |Programme/Process | | | | |

|8 |EA-2 End semester exam |50 |12.5 | |12.5 |

| |(External Assessment) | | | | |

| |Total |200 |100 |50 |50 |

| | | | |Pass/Fail determination) |Pass/Fail determination)|

Table 4: COs Versus real marks

|S.No. |Task |Type |Marks |Weightage|CO1 |

| | | | | | |

|1.1.1 |3 |3 |3 |3 |1 |

|2.1.1 |3 |2 |3 | |3 |

|3.1.1 |3 |3 |3 |3 | |

|4.1.1 |3 |3 |3 |3 |2 |

|5.1.1 |3 |3 |3 |3 |2 |

|6.1.1 |1 |2 |1 |3 |1 |

|7.1.1 |2 |3 |3 |3 |2 |

|8.1.1 |3 |3 |3 |3 | |

|9.1.1. |1 |1 |1 |1 |1 |

|10.1.1. |1 | |1 | | |

|11.1.1. |1 | |1 | | |

|12.1.1 |1 |1 |1 |1 |1 | |

|Part B 5 x 2 marks = 10 marks |3.25 |6 |4 |-- | | |

|Part C 2x 15 marks =30 marks |7.5 |15 |15 |-- | | |

|Total 50 Marks |15% |26 |24 | | | |

|CA2 | |CO1 |CO2 |CO3 |CO4 |CO5 |

|Part B 5 x 2 marks = 10 marks |3.25 | | |4 |6 | |

|Part C 2x 15 marks =30 marks33 |7.5 | | |15 |15 | |

|Total 50 Marks |15% | | |23 |27 | |

|CA3 | |CO1 |CO2 |CO3 |CO4 |CO5 |

|Test |3 | |15 | | | |

|Seminar |3 | | |15 | | |

|Assignment I |4 | | | |20 | |

|Quiz |3 | | | | |15 |

|Assignment II |3 | | | | |15 |

|Total 100 marks |20% |20 |15 |15 |15 |30 |

|CA4- End semester Exam | |CO1 |CO2 |CO3 |CO4 |CO5 |

|Participation and Performing |20 |6 |10 |2 | |2 |

|experiment | | | | | | |

|Movement in the Lab, Safety, |20 |6 |10 |2 | |2 |

|maintaining cleanliness | | | | | | |

|Punctuality, Dresscode and |10 |3 |5 |1 | |1 |

|Neatness | | | | | | |

|Submission of Observation Note |10 |3 |5 |1 | |1 |

|Record |10 |3 |5 |1 | |1 |

|Q&A |10 |3 |5 |1 | |1 |

|Total 100 Marks |15 % |30 |50 |10 | |10 |

|CIA2 | |CO1 |CO2 |CO3 |CO4 |CO5 |

|Short Procedure & Model graph |15 |5.625 |9.375 | | | |

|Tabulation & Graph |20 |7.5 |12.5 | | | |

|Calculation |20 |7.5 |12.5 | | | |

|Result |10 |3.75 |6.25 | | | |

|Viva-Voce |15 |7.5 |12.5 | | | |

|Record |10 |3.75 |6.25 | | | |

|Total 100 Marks |15 % |37.5 |62.5 | | | |

|Before CLA4 |10% |10 |10 |10 |10 |10 |

|Total 100 marks |20% |20 |20 |20 |20 |20 |

|EA 2 End | |CO1 |CO2 |CO3 |

|semester | | | | |

|exam | | | | |

Table 15 -Marks distribution list pasted in the observation note book (CIA1)

|S.No. |Criterion |Marks |

| |Aim, Short Procedure, Tabulation, Calculation, result |20% |

| |Participation and Performing experiment |20% |

| |Movement in the Lab, Safety, maintaining cleanliness |20% |

| |Punctuality, Dresscode and Neatness |10% |

| |Submission of Observation Note |10% |

| |Record |10% |

| |Q&A |10% |

| |Total |100 |

Table 16-Rubrics for lab assessment CIA2 Exam

|S.NO |Criterion |

Table 19: Course Plan

|Unit No. |Topic No |

|1 |1.1 |

|2. |2.1 |

| |3.1 |

|4. |4.1 |

| | | |

|1 |The permissible limit of hardness in drinking water is |1 |

| |a) 500 ppm c) 250 ppm d) < 250 ppm | |

|2 |Sea water/Saline water can be purified using the principle------------ |1 |

| |a) osmosis b) filtration c) coagulation d)reverse osmosis | |

|3 |E0 of standard hydrogen electrode is |2 |

| |a) 0 V b) 1.1 V c) 2V d) 1.5V | |

|4 |Which metals are more resistant to corrosion? |3 |

| |a) Noble metals b) Alkaline metals | |

| |c) Alkaline Earth metals d) None of these | |

|5 |Hydrogen bomb works on the principle of ------------ |4 |

| |a) Nuclear fission b) Oxidation c) Nuclear splitting d) Nuclear fusion | |

|6 |---------- nuclei undergoes nuclear fission reaction. |4 |

| |a) Pu238 b) U235 c) U238 d) Pu235 | |

|7 |Intensity of colour can be measured by using |5 |

| |a) Colorimeter b) Potentio meter | |

| |c) Uv Spectroscopy d) NMR spectroscopy | |

|8 |IR Spectroscopy provide valuable information about a) Molecular weight b) |5 |

| |Melting point c) Conjugation d) Functional groups | |

| |PART – B – (5 x 2 = 10 Marks) | |

|1 |Define osmosis. |1 |

| 2 | Calculate the emf of the following cell at 25o C | 2 |

| |  Cu /Cu2+(0.01M) || Cu2+(0.05M)/Cu | |

|3 |State Pilling Bedworth rule. |3 |

|4 |List out any two advantages of lithium battery. |4 |

|5 |Define chromophore with an example. |5 |

| | | |

| |PART – C– (4 x 15 = 60 Marks) | |

|1 |Describe the various processes to remove the impurities of water for domestic supply. |(10) |1 |

|2 |A sample of water contains Mg (HCO3)2 = 73 mgs/lit, Ca (HCO3)2 = 40.5 mgs/lit CaSO4 = 13.6 mgs/lit, MgCl2 = |(5) |1 |

| |9.5 mgs/lit, NaCl = 5.0 mgs/lit. Calculate the carbonate and non-carbonate hardness of the water. (Atomic | | |

| |weights of Ca, Mg, O, C, C l, S and H are 40, 24, 16,12, 35.5, 32 and 1 respectively) | | |

|3 |Describe the process of desalination of sea water using RO method. |(8) |1 |

|4 |100 ml of raw water sample on titration with N/50 hydrochloric acid required 13.0ml of the acid to |(7) |1 |

| |phenolphthalein end point and 16.5ml of the acid to methyl orange end point. Determine the types and amount | | |

| |of alkalinity present in the water sample | | |

|5 |Derive Nernst equation for an electrode potential of the cell. |(8) |2 |

|6 |Discuss the working principle and construction of Daniel cell. |(7) |2 |

|7 |Explain the construction and working of hydrogen electrode. |(8) |2 |

|8 |Distinguish between dry corrosion and wet corrosion. |(7) |3 |

|9 |Illustrate corrosion control by sacrificial anodic protection method. |(10) |3 |

|10 |Describe the construction and principle of lead acid storage battery and mention its uses? |(5) |4 |

|11 |Write short notes on solar cell. |(10) |4 |

|12 |Discuss the principle and instrumentation of a UV-Visible Spectrometer with neat block diagram. |(5) |5 |

|13 |Derive Beer Lambert’s law and its limitations. |(8) |5 |

|14 |Calculate the number of fundamental modes of vibration for the following molecules. |(7) |5 |

| |a) H2O b) NH3 c) HCl d) CO2 | | |

| | | | |

| | | | |

| | | | |

| | | | |

| |PART – D – (2 x 10 = 20 Marks) | | |

|1 |Explain the various components of nuclear reactor with neat diagram. |(10) |5 |

|2 |List out any ten detailed applications of CNT’s. |(10) |5 |

| | | | |

| | | | |

| | | | |

| |Table 21 : Tutorial Details | | |

| | | | |

| |Problems based on Hardness | | |

| |A sample of water contains 100 mgs of MgSO4 per litre. Calculate the hardness in terms of CaCO3 equivalents. | | |

| |Solution | | |

| |Given: The amount of MgSO4 = 100 mgs/lit | | |

| |The amount of hardness producing salt | | |

| |Amount equivalent to CaCO3 = ---------------------------------------------------------- X 100 | | |

| |Molecular weight of hardness producing salt | | |

| |We know that, the molecular weight of MgSO4 = 120 | | |

| |[pic]Amount equivalent to CaCO3 =100 x 100/120 = 83.3 mgs/lit | | |

| | | | |

| |A water sample contains 200 mgs of CaSO4 and 75 mgs of Mg (HCO3)2 per litre. What is the total hardness | | |

| |interms of CaCO3 equivalent? | | |

| |Solution: | | |

| |Name of the hardness producing salts | | |

| |Amount in mgs/lit | | |

| |Molecular weight | | |

| |Amount equivalent to CaCO3 | | |

| | | | |

| |CaSO4 | | |

| |200 | | |

| |136 | | |

| |200 X 100 / 136 = 147 mgs/lit | | |

| | | | |

| |Mg(HCO3)2 | | |

| |75 | | |

| |146 | | |

| |75 x 100 / 146 = 51.4 mgs/lit | | |

| | | | |

| | | | |

| |Temporary Hardness = Mg (HCO3)2 = 51.4 mgs/lit | | |

| |Permanent hardness = CaSO4 =147 mgs/lit. | | |

| |Total hardness = Mg (HCO3)2 + CaSO4 | | |

| |= 51.4 + 147 | | |

| |= 198.4mgs/lit | | |

| | | | |

| |Calculate the carbonate and non-carbonate hardness of a sample water containing the dissolved salts as given | | |

| |below in mgs/lit Mg(HCO3)2 = 10;Ca(HCO3)2 = 40; MgCl2 = 21.; and NaCl = 20 | | |

| |Solution | | |

| |Name of the hardness producing salts | | |

| |Amount in mgs/lit | | |

| |Molecular weight | | |

| |Amounts equivalent to CaCO3 | | |

| | | | |

| |Mg(HCO3)2 | | |

| |10 | | |

| |146 | | |

| |10 X 100 / 146 = | | |

| |6.8 mgs/lit | | |

| | | | |

| |Ca(HCO3)2 | | |

| |40 | | |

| |162 | | |

| |40X 100 / 162 = 24.7 mgs/lit | | |

| | | | |

| |MgCl2 | | |

| |21 | | |

| |95 | | |

| |21 X 100 / 95 = 22.1 mgs/lit | | |

| | | | |

| |NaCl | | |

| |20 | | |

| |NaCl does not contribute any hardness to water, hence it is ignored. | | |

| | | | |

| | | | |

| |Carbonate hardness = Mg(HCO3)2 + Ca(HCO3)2 | | |

| |= 6.8 + 24.7 = 31.5 mgs/lit | | |

| |Non-carbonate hardness = MgCl2 | | |

| |= 22.1 mgs/lit | | |

| |Total hardness = carbonate hardness + Non-carbonate hardness | | |

| |= 31.5 + 22.1 | | |

| |= 53.6 mgs/lit | | |

| |Exercises | | |

| |A sample of water contains the following dissolved salts in mgs/lit. Mg (HCO3)2 = 73; CaCl2=111; Ca | | |

| |(HCO3)2=81 and MgSO4=40. Calculate the temporary and permanent hardness of the water (Atomic weights of Ca, | | |

| |Mg, O, C, Cl, S, H are 40, 24, 16, 12, 35.5, 32 and respectively. | | |

| |Problems based on Alkalinity | | |

| |1. 100 ml of a raw water sample on titration with N/50 H2SO4 required 10.0 ml of the acid to phenolphthalein | | |

| |end-point and 14.0 ml of the acid to methyl orange end-point. Determine the type and extent of alkalinity | | |

| |present in the water sample. | | |

| |Solution: | | |

| |Strength of HCl = 0.02 N | | |

| |phenolphthalein end-point = P = 10.0 ml | | |

| |methyl orange end-point = M = 14.0 ml | | |

| |Since P > [pic] M, | | |

| |the water sample must contain only OH- and CO32- alkalinities and there cannot be any HCO3- alkalinity. | | |

| |i) Volume of std .HCl required for OH- alkalinity = 2P - M | | |

| |= (2 x 10.0) ml - 14 ml | | |

| |= 20 ml- 14.0 ml | | |

| |= 6.0 ml | | |

| |Volume of acid consumed to OH- alkalinity V1 = 6.0 ml | | |

| |ii) Volume of std .HCl required for CO32- alkalinity = 2M – 2P | | |

| |= 2 x 14.0 ml – 2 x 10.0 ml | | |

| |= 24 – 20 | | |

| |Volume of acid consumed to CO32- alkalinity V1 = 4.0 ml | | |

| | | | |

| |1. Calculate the OH- alkalinity | | |

| |Volume of HCl V1 = 6.0 ml | | |

| |Strength of HCl N1 = 0.02 N | | |

| |Volume of water sample V2 = 100 ml | | |

| |Strength of water sample due to OH- alkalinity N2 = ? | | |

| |V1 N1 = V2 N2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |Strength of water sample due to OH- alkalinity = 0.0012 N | | |

| |Amount of OH- alkalinity present in | | |

| |1 litre in terms Of CaCO3 equivalent = Strength of OH- alkalinity | | |

| |[pic]Eq. wt of aCO3 | | |

| |= 0.0012 N [pic]50 | | |

| |= 0.06 gm x 1000 | | |

| |Amount of OH- alkalinity = 60 ppm | | |

| | | | |

| |2. Calculate the CO32- alkalinity | | |

| |Volume of HCl V1 = 4.0 ml | | |

| |Strength of HCl N1 = 0.02 N | | |

| |Volume of water sample V2 = 100 ml | | |

| |Strength of water sample due to CO32- alkalinity N2 = ? | | |

| |V1 N1 = V2 N2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |Strength of water sample due to CO32- alkalinity = 0.0008 N | | |

| |Amount of CO32- alkalinity present in | | |

| |1 litre in terms Of CaCO3 equivalent = Strength of of CO32- alkalinity | | |

| |[pic]Eq. wt of CaCO3 | | |

| |= 0.0008 N [pic]50 | | |

| |= 0.04 gm x1000 | | |

| |= 40 ppm | | |

| |Amount of CO32- alkalinity = 40 ppm | | |

| |Total Alkalinity | | |

| |Total alkalinity = Alkalinity due to OH— + | | |

| |Alkalinity due to CO32- | | |

| |= 60 ppm + 40 ppm | | |

| |= 100 ppm | | |

| |2. A water sample is not alkaline to phenolphthalein but, 100 ml of the sample on titration with N/10 HCl, | | |

| |required 15 ml to methyl orange end point. What are the types and amounts of alkalinity present in the | | |

| |sample. | | |

| |Solution: | | |

| |Strength of HCl = 0.1 N | | |

| |phenolphthalein end point p = 0 | | |

| |methyl orange end point M = 15 ml | | |

| |Since P = 0 | | |

| |The water sample contain only HCO3- alkalinity , | | |

| |Volume of HCl required to HCO3- alkalinity = M | | |

| |M = 15 ml | | |

| |1) Calculate the HCO3- alkalinity | | |

| |Volume of HCl V1 = 15.0 ml | | |

| |Strength of HCl N1 = 0.1 N | | |

| |Volume of water sample V2 = 100 ml | | |

| |Strength of water sample due to HCO3- alkalinity N2 = ? | | |

| |V1 N1= V2 N2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |= 0.015 N | | |

| |Strength of water sample due to HCO3- alkalinity = 0.015 N | | |

| |Amount of HCO3- alkalinity present in | | |

| |1 litre in terms Of CaCO3 equivalent = Strength of HCO3- alkalinity | | |

| |[pic]Eq. wt of CaCO3 | | |

| |= 0.015 N [pic]50 | | |

| |= 0.75 gm x1000 | | |

| |= 750 ppm | | |

| |Amount of HCO3- alkalinity = 750 ppm | | |

| | | | |

| |3. 100 ml of a water sample on titration with 0.02 N H2SO4 gave a titre value of 7.8 ml to phenolphthalein | | |

| |end-point and 15.6m l to methyl orange end-point. Calculate the alkalinity of the water sample interms of | | |

| |CaCO3 equivalent and comment the type of alkalinity present. | | |

| |Solution: | | |

| |Given: | | |

| |Strength of HCl = 0.02 N | | |

| |Volume of the water sample = 100 ml | | |

| |phenolphthalein end point P = 7.8 ml | | |

| |methyl orange end point M = 15.6 ml | | |

| |Given data satisfy the condition P = 1/2 M, Therefore water sample contains only [pic]alkalinity not OH| | |

| |- and HCO3- alkalinity, | | |

| |Volume of HCl required to CO32- alkalinity = 2P | | |

| |= 2 [pic] 7.8 | | |

| |= 15.6 ml | | |

| |Calculation for CO32- Alkalinity. | | |

| |Volume of HCl V1 = 15.6 ml | | |

| |Strength of HCl N1 = 0.02 N | | |

| |Volume of water sample V2 = 100 ml | | |

| |Strength of water sample due to CO32- alkalinity N2 = ? | | |

| |V1 N1 = V2 N2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |Strength of water sample due to CO32- alkalinity = 0.00312 N | | |

| |Amount of CO32- alkalinity present in | | |

| |1 litre in terms Of CaCO3 equivalent = Strength of CO32- alkalinity | | |

| |[pic]Eq. wt of CaCO3 | | |

| |= 0.00312 N [pic]50 | | |

| |= 0.156 gm x1000 | | |

| |= 156 ppm | | |

| |Amount of CO32- alkalinity = 156 ppm | | |

| | | | |

| |4. 100 ml of a raw water sample on titration with N/50 H2SO4 required 7.5 ml of the acid to phenolphthalein | | |

| |end-point and 18.0 ml of the acid to methyl orange end-point. Determine the type and extent of alkalinity | | |

| |present in the water sample. | | |

| |Solution. | | |

| |Strength of HCl = 0.02 N | | |

| |phenolphthalein end-point P = 7.5 ml | | |

| |methyl orange end-point M = 18.0 ml | | |

| |If the data satisfy the condition, P < [pic] M, | | |

| |the water sample must contain both CO32- and HCO3- alkalinities and there cannot be any OH- alkalinity. | | |

| |i) Volume of std .HCl required for CO32- alkalinity = 2P | | |

| |= 2 x 7.5 ml | | |

| |= 15.0 ml | | |

| |Volume of acid consumed to CO32- alkalinity V1 = 15.0 ml | | |

| |ii) Volume of std .HCl required for HCO3- alkalinity = M – 2P | | |

| |= 18.0 ml – 2 x 7.5.0 ml | | |

| |= 3.0 ml | | |

| |Volume of acid consumed to HCO3- alkalinity V1 = 3.0 ml | | |

| |Calculate the CO32- alkalinity | | |

| |Volume of HCl V1 = 15.0 ml | | |

| |Strength of HCl N1 = 0.02 N | | |

| |Volume of water sample V2 = 100 ml | | |

| |Strength of water sample due to | | |

| |CO32- alkalinity N2 = ? | | |

| |V1 N1 = V2 N2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |= 0.003 N | | |

| |Strength of water sample due to CO32- alkalinity = 0.003N | | |

| |Amount of CO32- alkalinity present in | | |

| |1 litre in terms Of CaCO3 equivalent = Strength of CO32- alkalinity | | |

| |[pic]Eq. wt of CaCO3 | | |

| |= 0.003 N [pic]50 | | |

| |= 0.15 gm x 1000 | | |

| |Amount of CO32- alkalinity = 150ppm | | |

| |Calculate the HCO3- alkalinity | | |

| |Volume of HCl V1 = 3.0 ml | | |

| |Strength of HCl N1 = 0.02 N | | |

| |Volume of water sample V2 = 100 ml | | |

| |Strength of water sample due to HCO3- alkalinity N2 = ? | | |

| |V1 N1 = V2 N2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |N2 = 0.0006 N | | |

| |Strength of water sample due to HCO3- alkalinity = 0.0006 N | | |

| |Amount of HCO3- alkalinity present in | | |

| |1 litre in terms Of CaCO3 equivalent = Strength of of HCO3- alkalinity | | |

| |[pic]Eq. wt of CaCO3 | | |

| |= 0.0006 N x 50 | | |

| |= 0.03 gm x1000 | | |

| |= 30 ppm | | |

| |Amount of HCO3- alkalinity = 30 ppm | | |

| |Total Alkalinity | | |

| |Total alkalinity = Alkalinity due to CO32- + | | |

| |Alkalinity due to HCO3- | | |

| |= 160 ppm + 30 ppm | | |

| |= 190 ppm | | |

| |6. 0.25 gm of CaCO3 was dissolved in HCl and the solution made upto one litre with distilled water. 100 ml | | |

| |of the above solution consumed 25 ml of EDTA solution on titration.100 ml of hard water sample required 30 ml| | |

| |of same EDTA solution on titration. 100 ml of this water, after boiling cooling and filtering required 11 ml | | |

| |of EDTA solution on titration. Calculate the temporary permanent and total hardness of water. | | |

| |Calculate the strength of given std water, | | |

| |Amount / Lit | | |

| |Strength of Std Water = _________________________ | | |

| |Molecular Weight | | |

| |Strength of std Water = [pic] | | |

| |Strength of Std water = 0.0025 M | | |

| | | | |

| |Titration: I | | |

| |Standardization of EDTA : | | |

| |Volume of std water V1 = 100 ml | | |

| |Strength of std water M1 = 0.0025M | | |

| |Volume of EDTA V2 = 25 ml | | |

| |Strength of EDTA M2 = ? | | |

| |V1M1 = V2M2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |M2 = 0.01 M | | |

| |Strength of EDTA = 0.01 M | | |

| | | | |

| |Titration: II | | |

| |Estimation of total hardness. | | |

| |Volume of water sample V1 = 100 ml | | |

| |Strength of water sample M1 = ? | | |

| |Volume of std EDTA V2 = 30 ml | | |

| |Strength of b std EDTA M2 = 0.01 M | | |

| |V1M1 = V2M2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |M2 = 0.003 M | | |

| |Strength of hard water sample = 0.003 M | | |

| |Amount of total hardness present in per liter in | | |

| |terms of CaCO3 equivalent = Strength of hard water x M .W OF CaCO3 | | |

| |= 0.003M X 100 | | |

| |= 0.3 gm x1000 | | |

| |Amount total hardness = 300 ppm | | |

| |Titration: III | | |

| |Estimation of permanent hardness. | | |

| |Volume of boiled water V1 = 100 ml | | |

| |Strength of boiled water M1 = ? | | |

| |Volume of std EDTA V2 = 11 ml | | |

| |Strength of b std EDTA M2 = 0.01 M | | |

| |V1M1 = V2M2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |M2 = 0.0011 M | | |

| |Strength of boiled water = 0.0011 M | | |

| |Amount of permanent hardness present in per liter in | | |

| |terms of CaCO3 equivalent = Strength of boiled water x M .W of CaCO3 | | |

| |= 0.0011M X 100 | | |

| |= 0.11 gm x1000 | | |

| |Amount of permanent hardness = 110 ppm | | |

| |Temporary hardness = Total hardness - Permanent hardness | | |

| |Temporary hardness = 300 ppm - 110 ppm | | |

| |Temporary hardness = 190 ppm | | |

| | | | |

| |Problems based on Nernst equation. | | |

| |1) Calculate the reduction potential of the Cu/Cu2+(0.5M) at 25 0C . E0 Cu2+ / Cu = 0.34V | | |

| |Given: | | |

| |[pic]; [Cu2+] =0.5M; n =2; | | |

| |Solution | | |

| |Electrode reaction Cu2+ +2e [pic]Cu | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| | | | |

| |2) Find the oxidation potential of Zn/Zn2+ = 0.2 M electrode at 25 0C .Standard oxidation potential of of | | |

| |Zn/Zn2+ is 0.76V. | | |

| |Given: | | |

| |[pic]; [Zn2+] =0.2M; n =2; | | |

| |Solution | | |

| |Electrode reaction: Zn [pic] Zn2 +2e | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| | | | |

| |3) Calculate the electrode potential of Zinc electrode dipped in 0.1 M ZnSO4 solution at 250C . | | |

| |Given: | | |

| |Concentration of ZnSO4 = 0.1M ; n = 2 ; E 0Zn / Zn2+ = - 0.76V | | |

| |Solution | | |

| |Electrode reaction: Zn2+ + 2e [pic] Zn | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| | | | |

| |4) Calculate the standard e.m.f. of the cell : Cd, Cd2+||Cu2+,Cu and determine the cell reaction. The | | |

| |standard reduction potentials ofCu2+, Cu and Cd2+, Cd are 0.34V and –0.40 volts respectively. Write the cell | | |

| |reaction and predict the feasibility of the cell reaction. | | |

| |Solution. | | |

| |[pic] = E0right – E0 left | | |

| |[pic] = [Std. reduction potential of Cu2+, Cu] | | |

| |– [Std. reduction potentials of Cd2+, Cd] | | |

| |[pic] = E0Cu2+,Cu – E0Cd2+,Cd | | |

| |[pic] = 0.34 V – (– 0.4 V) | | |

| |[pic] = + 0.74 Volts. | | |

| |Left hand electrode (oxidation half cell) reaction is | | |

| |Cd(s) Cd2+ + 2e | | |

| |Right hand electrode (reduction half cell) reaction is | | |

| |Cu2+ + 2e Cu(s) | | |

| |The cell reaction is | | |

| |Cd(s) + Cu2+ (aq) Cd2+(aq) + Cu(s) | | |

| |E0cell is positive. [pic]The cell reaction is feasible. | | |

| | | | |

| |5) Calculate the standard free energy of the cell reaction is the following cell at 250C Zn, Zn2+ [pic] | | |

| |Ni2+, Ni. The standard reduction potentials of Zn2+, Zn and Ni2+, Ni half cells are – 0.76 V and – 0.25 V | | |

| |respectively. | | |

| |Solution | | |

| |[pic] = E0Right – E0Left = – 0.25 – (– 0.76) | | |

| |[pic] = + 0.51 V | | |

| |[pic] is + ve. [pic] = – ve | | |

| |[pic] = – nFE0cell | | |

| |n = 2 electrons | | |

| |[pic] = –2 x 96495 x 0.51 | | |

| |= –97460 Joules | | |

| |[pic] = – 97.46 kJ. | | |

| | | | |

| |6) What is the potential of a half-cell consisting of zinc electrode in 0.01 M ZnSO4 solution 25 0C. E0 = | | |

| |0.763 V. | | |

| |7) Calculate the emf of the cell. | | |

| |Zn | Zn2+ (0.001 M) || Ag+ (0.1 M) | Ag | | |

| |The standard potential of Ag/Ag+ half-cell is + 0.80 V and Zn/Zn2+ is – 0.76 V. | | |

| | | | |

| |8) Calculate the equilibrium constant for the reaction between silver nitrate and metallic zinc. | | |

| |Solution: | | |

| |Cell construction: Zn /Zn2+ / / Ag+ / Ag | | |

| |Step 1 : Write the equation for the reaction | | |

| |2Ag+ + Zn → Zn2+ + 2Ag E0cell = 1.56 V | | |

| |Step 2 : Substitute values in the Nernst equation at equilibrium | | |

| |[pic] = [pic] | | |

| |At the Eqm, [pic]=0, Where K = Equilibrium Constant | | |

| |0 = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = 53 | | |

| |[pic] = 1053 | | |

| | | | |

| |9. Calculate the E.M.F. of the zinc - silver cell [pic]at 25oC when [Zn2+] = 0.10 M and [Ag+] = 10 M. (E0cell| | |

| |at 25 oC = 1.56 volt] | | |

| |Solution: | | |

| |LHSE : oxdn [pic]→ [pic]+ 2e- | | |

| |RHSE : redn [pic]→ [pic] | | |

| |__________________________________ | | |

| |Overall Cell reaction 2Ag+ + Zn → 2Ag + Zn2+ | | |

| |__________________________________ | | |

| |n = 2 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] [Zn]=1, [Ag]=1 | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| | | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| |[pic] = [pic] | | |

| | | | |

| | | | |

| | | | |

| | | | |

| | | | |

| | | | |

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