(i) Laboratory procedures, safety regulations, scientific notations, plotting of data and finding of slope and intercept.
(ii) Determination of formula and composition of a suitable hydrate (CuSO4 5H2O, NiSO4 7H2O etc)
(iii) Determination of the density of a liquid / solution by density bottle / pycnometer method.
(iv) Determination of molecular weight of substances like CHCl3, CCl4 by Victor Meyer’s method.
(v) Determination of molecular weight of organic salts by chemical method.
(vi) Determination of heats of solution of simple salts by calorimeter.
(vii) Determination of heats of solution of sparingly soluble samples in water by measuring solubility as a function of temperature (application of Vants-Hoff equation).
(viii) Determination of distribution coefficients of benzoic acid between (i) hexane and octane (ii) ether and water.
(ix) Determination of heat of neutralization of HCl with NaOH.
(x) Preparation of primary and secondary standard solutions.
(xi) Standardization of HCl acid solution by sodium carbonate solution
(xii) Standardization of NaOH solution by potassium hydrogen phthalate / oxalic acid
(xiii) Standardization of NaOH solution by potassium hydrogen phthalate / oxalic acid
(xiv) Standardization of KMnO4 solution by sodium oxalate
The aim of this experiment is to standardize 0.1N Sodium Hydroxide (NaOH) which is an unstandard substance, by using standardized Hydrochloric acid (Na2CO3).
The aim of this experiment is to standardize 0.1N Sodium Hydroxide (NaOH) which is an unstandard substance, by using standardized Hydrochloric acid (Na2CO3).
Preparation of the LAB reagents
How to prepare:
For the Qualitative analysis (identification) of anions and cations from inorganic salt solutions.
1. For sulphate (SO42¯) identification
a. Dilute (6M) Hydrochloric acid (HCl)
b. 0.1M Barium chloride (BaCl2) or Barium nitrate {Ba(NO3)2¬} solution
2. For halide ions identification
a. Dilute nitric acid (2M)
b. 5% Silver nitrate (AgNO3) solution
c. Dilute ammonium hydroxide solution (2M)
d. Concentrated ammonium hydroxide solution (~9M)
3. For nitrate ion identification
a. Concentrated Hydrochloric acid (37%) {÷Conc. Sulphuric acid }
b. 5% Ferrous sulphate (FeSO4) solution
4. For Acetate ion identification
a. Dilute Hydrochloric acid
b. 0.2M Ferric chloride (FeCl3) solution
A. For group I cations
a. Dilute hydrochloric acid (6M)
b. Ammonia solution (9M)
c. Potassium chromate (1M)
B. For group II cations
a. Nitric acid (6M)
b. Stannous chloride (0.1M)
c. Concentrated Ammonia solution (9M)
d. Dilute Ammonia solution (2M)
e. Dilute Sodium hydroxide solution (2M)
C. For group III cations
a. Ammonia solution (9M)
b. Ammonia solution (2M)
c. Potassium ferricyanide (K3[Fe(CN)6]) [250 mg in 10 mL]
d. Potassium thiocyanate [250 mg in 10 mL]
e. Sodium hydroxide (2M)
f. Sodium hydroxide (10M)
This is a general presentation about Argentometric Titration or well known as Precipitation Titration. Contain Mohr Methods, Volhard Methods, and Fajans Methods.
Polarographic technique is applied for the qualitative or quantitative analysis of electroreducible or oxidisable elements or groups.
It is an electromechanical technique of analyzing solutions that measures the current flowing between two electrodes in the solution as well as the gradually increasing applied voltage to determine respectively the concentration of a solute and its nature.
The principle in polarography is that a gradually increasing negative potential (voltage) is applied between a polarisable and non-polarisable electrode and the corresponding current is recorded.
Polarisable electrode: Dropping Mercury electrode
Non-polarisable electrode: Saturated Calomel electrode
From the current-voltage curve (Sigmoid shape), qualitative and quantitative analysis can be performed. This technique is called as polarography, the instrument used is called as polarograph and the current-voltage curve recorded is called as polarogram
Microbiological quality of drinking water Mirko Rossi
Lecture on microbiological quality methods for drinking water for the faculty of Veterinary Medicine, University of Helsinki; Course in Environmental Health
a) Assay of acetyl salicylic acid in aspirin tablets.
b) Assay of sodium salicylate tablets
c) Determination of potency of penicillin tablets.
d) Non- aqueous assay of phenobarbitone tablets.
e) Determination of calcium in solid & liquid dosage form by complexometric titration.
f) Assay of promethazine hydrochloride.
g) Assay of methamphetamine hydrochloride
h) Assay of aluminum hydroxide gel.
i) Assay of milk of magnesia
j) Assay of magnesium and aluminum from antacid preparation.
k) Determination of iodine value, saponification value, acid value and R.M. value of oils and fats.
Preparation of the LAB reagents
How to prepare:
For the Qualitative analysis (identification) of anions and cations from inorganic salt solutions.
1. For sulphate (SO42¯) identification
a. Dilute (6M) Hydrochloric acid (HCl)
b. 0.1M Barium chloride (BaCl2) or Barium nitrate {Ba(NO3)2¬} solution
2. For halide ions identification
a. Dilute nitric acid (2M)
b. 5% Silver nitrate (AgNO3) solution
c. Dilute ammonium hydroxide solution (2M)
d. Concentrated ammonium hydroxide solution (~9M)
3. For nitrate ion identification
a. Concentrated Hydrochloric acid (37%) {÷Conc. Sulphuric acid }
b. 5% Ferrous sulphate (FeSO4) solution
4. For Acetate ion identification
a. Dilute Hydrochloric acid
b. 0.2M Ferric chloride (FeCl3) solution
A. For group I cations
a. Dilute hydrochloric acid (6M)
b. Ammonia solution (9M)
c. Potassium chromate (1M)
B. For group II cations
a. Nitric acid (6M)
b. Stannous chloride (0.1M)
c. Concentrated Ammonia solution (9M)
d. Dilute Ammonia solution (2M)
e. Dilute Sodium hydroxide solution (2M)
C. For group III cations
a. Ammonia solution (9M)
b. Ammonia solution (2M)
c. Potassium ferricyanide (K3[Fe(CN)6]) [250 mg in 10 mL]
d. Potassium thiocyanate [250 mg in 10 mL]
e. Sodium hydroxide (2M)
f. Sodium hydroxide (10M)
This is a general presentation about Argentometric Titration or well known as Precipitation Titration. Contain Mohr Methods, Volhard Methods, and Fajans Methods.
Polarographic technique is applied for the qualitative or quantitative analysis of electroreducible or oxidisable elements or groups.
It is an electromechanical technique of analyzing solutions that measures the current flowing between two electrodes in the solution as well as the gradually increasing applied voltage to determine respectively the concentration of a solute and its nature.
The principle in polarography is that a gradually increasing negative potential (voltage) is applied between a polarisable and non-polarisable electrode and the corresponding current is recorded.
Polarisable electrode: Dropping Mercury electrode
Non-polarisable electrode: Saturated Calomel electrode
From the current-voltage curve (Sigmoid shape), qualitative and quantitative analysis can be performed. This technique is called as polarography, the instrument used is called as polarograph and the current-voltage curve recorded is called as polarogram
Microbiological quality of drinking water Mirko Rossi
Lecture on microbiological quality methods for drinking water for the faculty of Veterinary Medicine, University of Helsinki; Course in Environmental Health
a) Assay of acetyl salicylic acid in aspirin tablets.
b) Assay of sodium salicylate tablets
c) Determination of potency of penicillin tablets.
d) Non- aqueous assay of phenobarbitone tablets.
e) Determination of calcium in solid & liquid dosage form by complexometric titration.
f) Assay of promethazine hydrochloride.
g) Assay of methamphetamine hydrochloride
h) Assay of aluminum hydroxide gel.
i) Assay of milk of magnesia
j) Assay of magnesium and aluminum from antacid preparation.
k) Determination of iodine value, saponification value, acid value and R.M. value of oils and fats.
B. Pharm. (Honours) Part-III Practical, Analytical Pharmacy,MANIKImran Nur Manik
a) Assay of acetyl salicylic acid in aspirin tablets.
b) Assay of sodium salicylate tablets
c) Determination of potency of penicillin tablets.
d) Non- aqueous assay of phenobarbitone tablets.
e) Determination of calcium in solid & liquid dosage form by complexometric titration.
f) Assay of promethazine hydrochloride.
g) Assay of methamphetamine hydrochloride
h) Assay of aluminum hydroxide gel.
i) Assay of milk of magnesia
j) Assay of magnesium and aluminum from antacid preparation.
k) Determination of iodine value, saponification value, acid value and R.M. value of oils and fats
Assay of sodium hydroxide solution.pptxnedalalazzwy
sodium hydroxide is useful for its ability to alter fats. It is used to make soap and as a main ingredient in household products such as liquid drain cleaners. Sodium hydroxide is usually sold in pure form as white pellets or as a solution in water.
Standardization of Acids and bases.
2. Determination of pKa and pKb values
3. Preparation of solutions of different pH & buffer capacities.
4. Determination of phase diagram of binary systems.
Determination of distribution coefficients.
6. Determination of molecular weight by Victor Meyer’s Method.
7. Determination of heats of solutions by measuring solubility as a function of temperature
(Van’t Hoff equation.)
A. Qualitative analysis of metal ions and acid radicals:
Na+, K+, Ca+2, Ag+, Mn+4, Fe+2, Fe+3, Co+2, Mg+2, Al+3, Cu+2 and acid radicals CO3,
halides, Citrate
SO4-2, NO3-, SO3-2, etc.
B. Identification of inorganic drugs in their formulation:
1. Ca+2, from supplied preparations
2. Fe+2 from supplied preparations
3. Al+3 from supplied preparations
4. Mg+2 from supplied preparations
5. K+ from supplied reparations
6. Na+ from supplied preparations
C. Conversion of different water insoluble or sparingly soluble drugs into water soluble
forms:
1. Na/ K – salicylate from salicylic acid
2. Na/ K – benzoate from benzoic acid
3. Na/ K – citrate from citric acid
Plants in complimentary and traditional systems of medicine MANIKanikImran Nur Manik
Plants in complimentary and traditional systems of medicine: Introduction-different types of
alternative systems of treatments (e.g. Ayurvedic, Unani and Homeopathic medicine). Contribution
of traditional drugs to modern medicines. Details of some common indigenous traditional drugs:
Punarnava, Vashaka, Anantamul, Arjuna, Chirata, Picrorhiga, Kalomegh, Amla, Asoka, Bahera,
Haritaki, Tulsi, Neem, Betel nut, Joan, Karela, Shajna, Carrot, Bael, Garlic, Jam and Madar.
Crude drugs: A general view of their origin, distributions, cultivation, collection, drying and
storage, commerce and quality control.
a) Classification of drugs.
b) Preparation of drugs for commercial market
c) Evaluation of crude drugs.
d) Drug adulteration.
Carbohydrate and related compounds: Sugars and sugar containing drugs. Sucrose,
dextrose, glucose, fructose etc. Polysaccharides and polysaccharide containing drugs,
Starches, dextrins etc. Gums and mucilages, tragacanth, acacia, sterculia, sodium
alginate, agar and cellulose.
Volatile oils and related terpenoids-Methods of obtaining volatile oils,
chemistry, their medicinal and commercial uses, biosynthesis of some important
volatile oils used as drugs.
New Directions in Targeted Therapeutic Approaches for Older Adults With Mantl...i3 Health
i3 Health is pleased to make the speaker slides from this activity available for use as a non-accredited self-study or teaching resource.
This slide deck presented by Dr. Kami Maddocks, Professor-Clinical in the Division of Hematology and
Associate Division Director for Ambulatory Operations
The Ohio State University Comprehensive Cancer Center, will provide insight into new directions in targeted therapeutic approaches for older adults with mantle cell lymphoma.
STATEMENT OF NEED
Mantle cell lymphoma (MCL) is a rare, aggressive B-cell non-Hodgkin lymphoma (NHL) accounting for 5% to 7% of all lymphomas. Its prognosis ranges from indolent disease that does not require treatment for years to very aggressive disease, which is associated with poor survival (Silkenstedt et al, 2021). Typically, MCL is diagnosed at advanced stage and in older patients who cannot tolerate intensive therapy (NCCN, 2022). Although recent advances have slightly increased remission rates, recurrence and relapse remain very common, leading to a median overall survival between 3 and 6 years (LLS, 2021). Though there are several effective options, progress is still needed towards establishing an accepted frontline approach for MCL (Castellino et al, 2022). Treatment selection and management of MCL are complicated by the heterogeneity of prognosis, advanced age and comorbidities of patients, and lack of an established standard approach for treatment, making it vital that clinicians be familiar with the latest research and advances in this area. In this activity chaired by Michael Wang, MD, Professor in the Department of Lymphoma & Myeloma at MD Anderson Cancer Center, expert faculty will discuss prognostic factors informing treatment, the promising results of recent trials in new therapeutic approaches, and the implications of treatment resistance in therapeutic selection for MCL.
Target Audience
Hematology/oncology fellows, attending faculty, and other health care professionals involved in the treatment of patients with mantle cell lymphoma (MCL).
Learning Objectives
1.) Identify clinical and biological prognostic factors that can guide treatment decision making for older adults with MCL
2.) Evaluate emerging data on targeted therapeutic approaches for treatment-naive and relapsed/refractory MCL and their applicability to older adults
3.) Assess mechanisms of resistance to targeted therapies for MCL and their implications for treatment selection
These lecture slides, by Dr Sidra Arshad, offer a quick overview of physiological basis of a normal electrocardiogram.
Learning objectives:
1. Define an electrocardiogram (ECG) and electrocardiography
2. Describe how dipoles generated by the heart produce the waveforms of the ECG
3. Describe the components of a normal electrocardiogram of a typical bipolar leads (limb II)
4. Differentiate between intervals and segments
5. Enlist some common indications for obtaining an ECG
Study Resources:
1. Chapter 11, Guyton and Hall Textbook of Medical Physiology, 14th edition
2. Chapter 9, Human Physiology - From Cells to Systems, Lauralee Sherwood, 9th edition
3. Chapter 29, Ganong’s Review of Medical Physiology, 26th edition
4. Electrocardiogram, StatPearls - https://www.ncbi.nlm.nih.gov/books/NBK549803/
5. ECG in Medical Practice by ABM Abdullah, 4th edition
6. ECG Basics, http://www.nataliescasebook.com/tag/e-c-g-basics
Report Back from SGO 2024: What’s the Latest in Cervical Cancer?bkling
Are you curious about what’s new in cervical cancer research or unsure what the findings mean? Join Dr. Emily Ko, a gynecologic oncologist at Penn Medicine, to learn about the latest updates from the Society of Gynecologic Oncology (SGO) 2024 Annual Meeting on Women’s Cancer. Dr. Ko will discuss what the research presented at the conference means for you and answer your questions about the new developments.
Flu Vaccine Alert in Bangalore Karnatakaaddon Scans
As flu season approaches, health officials in Bangalore, Karnataka, are urging residents to get their flu vaccinations. The seasonal flu, while common, can lead to severe health complications, particularly for vulnerable populations such as young children, the elderly, and those with underlying health conditions.
Dr. Vidisha Kumari, a leading epidemiologist in Bangalore, emphasizes the importance of getting vaccinated. "The flu vaccine is our best defense against the influenza virus. It not only protects individuals but also helps prevent the spread of the virus in our communities," he says.
This year, the flu season is expected to coincide with a potential increase in other respiratory illnesses. The Karnataka Health Department has launched an awareness campaign highlighting the significance of flu vaccinations. They have set up multiple vaccination centers across Bangalore, making it convenient for residents to receive their shots.
To encourage widespread vaccination, the government is also collaborating with local schools, workplaces, and community centers to facilitate vaccination drives. Special attention is being given to ensuring that the vaccine is accessible to all, including marginalized communities who may have limited access to healthcare.
Residents are reminded that the flu vaccine is safe and effective. Common side effects are mild and may include soreness at the injection site, mild fever, or muscle aches. These side effects are generally short-lived and far less severe than the flu itself.
Healthcare providers are also stressing the importance of continuing COVID-19 precautions. Wearing masks, practicing good hand hygiene, and maintaining social distancing are still crucial, especially in crowded places.
Protect yourself and your loved ones by getting vaccinated. Together, we can help keep Bangalore healthy and safe this flu season. For more information on vaccination centers and schedules, residents can visit the Karnataka Health Department’s official website or follow their social media pages.
Stay informed, stay safe, and get your flu shot today!
Lung Cancer: Artificial Intelligence, Synergetics, Complex System Analysis, S...Oleg Kshivets
RESULTS: Overall life span (LS) was 2252.1±1742.5 days and cumulative 5-year survival (5YS) reached 73.2%, 10 years – 64.8%, 20 years – 42.5%. 513 LCP lived more than 5 years (LS=3124.6±1525.6 days), 148 LCP – more than 10 years (LS=5054.4±1504.1 days).199 LCP died because of LC (LS=562.7±374.5 days). 5YS of LCP after bi/lobectomies was significantly superior in comparison with LCP after pneumonectomies (78.1% vs.63.7%, P=0.00001 by log-rank test). AT significantly improved 5YS (66.3% vs. 34.8%) (P=0.00000 by log-rank test) only for LCP with N1-2. Cox modeling displayed that 5YS of LCP significantly depended on: phase transition (PT) early-invasive LC in terms of synergetics, PT N0—N12, cell ratio factors (ratio between cancer cells- CC and blood cells subpopulations), G1-3, histology, glucose, AT, blood cell circuit, prothrombin index, heparin tolerance, recalcification time (P=0.000-0.038). Neural networks, genetic algorithm selection and bootstrap simulation revealed relationships between 5YS and PT early-invasive LC (rank=1), PT N0—N12 (rank=2), thrombocytes/CC (3), erythrocytes/CC (4), eosinophils/CC (5), healthy cells/CC (6), lymphocytes/CC (7), segmented neutrophils/CC (8), stick neutrophils/CC (9), monocytes/CC (10); leucocytes/CC (11). Correct prediction of 5YS was 100% by neural networks computing (area under ROC curve=1.0; error=0.0).
CONCLUSIONS: 5YS of LCP after radical procedures significantly depended on: 1) PT early-invasive cancer; 2) PT N0--N12; 3) cell ratio factors; 4) blood cell circuit; 5) biochemical factors; 6) hemostasis system; 7) AT; 8) LC characteristics; 9) LC cell dynamics; 10) surgery type: lobectomy/pneumonectomy; 11) anthropometric data. Optimal diagnosis and treatment strategies for LC are: 1) screening and early detection of LC; 2) availability of experienced thoracic surgeons because of complexity of radical procedures; 3) aggressive en block surgery and adequate lymph node dissection for completeness; 4) precise prediction; 5) adjuvant chemoimmunoradiotherapy for LCP with unfavorable prognosis.
Title: Sense of Smell
Presenter: Dr. Faiza, Assistant Professor of Physiology
Qualifications:
MBBS (Best Graduate, AIMC Lahore)
FCPS Physiology
ICMT, CHPE, DHPE (STMU)
MPH (GC University, Faisalabad)
MBA (Virtual University of Pakistan)
Learning Objectives:
Describe the primary categories of smells and the concept of odor blindness.
Explain the structure and location of the olfactory membrane and mucosa, including the types and roles of cells involved in olfaction.
Describe the pathway and mechanisms of olfactory signal transmission from the olfactory receptors to the brain.
Illustrate the biochemical cascade triggered by odorant binding to olfactory receptors, including the role of G-proteins and second messengers in generating an action potential.
Identify different types of olfactory disorders such as anosmia, hyposmia, hyperosmia, and dysosmia, including their potential causes.
Key Topics:
Olfactory Genes:
3% of the human genome accounts for olfactory genes.
400 genes for odorant receptors.
Olfactory Membrane:
Located in the superior part of the nasal cavity.
Medially: Folds downward along the superior septum.
Laterally: Folds over the superior turbinate and upper surface of the middle turbinate.
Total surface area: 5-10 square centimeters.
Olfactory Mucosa:
Olfactory Cells: Bipolar nerve cells derived from the CNS (100 million), with 4-25 olfactory cilia per cell.
Sustentacular Cells: Produce mucus and maintain ionic and molecular environment.
Basal Cells: Replace worn-out olfactory cells with an average lifespan of 1-2 months.
Bowman’s Gland: Secretes mucus.
Stimulation of Olfactory Cells:
Odorant dissolves in mucus and attaches to receptors on olfactory cilia.
Involves a cascade effect through G-proteins and second messengers, leading to depolarization and action potential generation in the olfactory nerve.
Quality of a Good Odorant:
Small (3-20 Carbon atoms), volatile, water-soluble, and lipid-soluble.
Facilitated by odorant-binding proteins in mucus.
Membrane Potential and Action Potential:
Resting membrane potential: -55mV.
Action potential frequency in the olfactory nerve increases with odorant strength.
Adaptation Towards the Sense of Smell:
Rapid adaptation within the first second, with further slow adaptation.
Psychological adaptation greater than receptor adaptation, involving feedback inhibition from the central nervous system.
Primary Sensations of Smell:
Camphoraceous, Musky, Floral, Pepperminty, Ethereal, Pungent, Putrid.
Odor Detection Threshold:
Examples: Hydrogen sulfide (0.0005 ppm), Methyl-mercaptan (0.002 ppm).
Some toxic substances are odorless at lethal concentrations.
Characteristics of Smell:
Odor blindness for single substances due to lack of appropriate receptor protein.
Behavioral and emotional influences of smell.
Transmission of Olfactory Signals:
From olfactory cells to glomeruli in the olfactory bulb, involving lateral inhibition.
Primitive, less old, and new olfactory systems with different path
These simplified slides by Dr. Sidra Arshad present an overview of the non-respiratory functions of the respiratory tract.
Learning objectives:
1. Enlist the non-respiratory functions of the respiratory tract
2. Briefly explain how these functions are carried out
3. Discuss the significance of dead space
4. Differentiate between minute ventilation and alveolar ventilation
5. Describe the cough and sneeze reflexes
Study Resources:
1. Chapter 39, Guyton and Hall Textbook of Medical Physiology, 14th edition
2. Chapter 34, Ganong’s Review of Medical Physiology, 26th edition
3. Chapter 17, Human Physiology by Lauralee Sherwood, 9th edition
4. Non-respiratory functions of the lungs https://academic.oup.com/bjaed/article/13/3/98/278874
micro teaching on communication m.sc nursing.pdfAnurag Sharma
Microteaching is a unique model of practice teaching. It is a viable instrument for the. desired change in the teaching behavior or the behavior potential which, in specified types of real. classroom situations, tends to facilitate the achievement of specified types of objectives.
New Drug Discovery and Development .....NEHA GUPTA
The "New Drug Discovery and Development" process involves the identification, design, testing, and manufacturing of novel pharmaceutical compounds with the aim of introducing new and improved treatments for various medical conditions. This comprehensive endeavor encompasses various stages, including target identification, preclinical studies, clinical trials, regulatory approval, and post-market surveillance. It involves multidisciplinary collaboration among scientists, researchers, clinicians, regulatory experts, and pharmaceutical companies to bring innovative therapies to market and address unmet medical needs.
TEST BANK for Operations Management, 14th Edition by William J. Stevenson, Ve...kevinkariuki227
TEST BANK for Operations Management, 14th Edition by William J. Stevenson, Verified Chapters 1 - 19, Complete Newest Version.pdf
TEST BANK for Operations Management, 14th Edition by William J. Stevenson, Verified Chapters 1 - 19, Complete Newest Version.pdf
Tom Selleck Health: A Comprehensive Look at the Iconic Actor’s Wellness Journeygreendigital
Tom Selleck, an enduring figure in Hollywood. has captivated audiences for decades with his rugged charm, iconic moustache. and memorable roles in television and film. From his breakout role as Thomas Magnum in Magnum P.I. to his current portrayal of Frank Reagan in Blue Bloods. Selleck's career has spanned over 50 years. But beyond his professional achievements. fans have often been curious about Tom Selleck Health. especially as he has aged in the public eye.
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Introduction
Many have been interested in Tom Selleck health. not only because of his enduring presence on screen but also because of the challenges. and lifestyle choices he has faced and made over the years. This article delves into the various aspects of Tom Selleck health. exploring his fitness regimen, diet, mental health. and the challenges he has encountered as he ages. We'll look at how he maintains his well-being. the health issues he has faced, and his approach to ageing .
Early Life and Career
Childhood and Athletic Beginnings
Tom Selleck was born on January 29, 1945, in Detroit, Michigan, and grew up in Sherman Oaks, California. From an early age, he was involved in sports, particularly basketball. which played a significant role in his physical development. His athletic pursuits continued into college. where he attended the University of Southern California (USC) on a basketball scholarship. This early involvement in sports laid a strong foundation for his physical health and disciplined lifestyle.
Transition to Acting
Selleck's transition from an athlete to an actor came with its physical demands. His first significant role in "Magnum P.I." required him to perform various stunts and maintain a fit appearance. This role, which he played from 1980 to 1988. necessitated a rigorous fitness routine to meet the show's demands. setting the stage for his long-term commitment to health and wellness.
Fitness Regimen
Workout Routine
Tom Selleck health and fitness regimen has evolved. adapting to his changing roles and age. During his "Magnum, P.I." days. Selleck's workouts were intense and focused on building and maintaining muscle mass. His routine included weightlifting, cardiovascular exercises. and specific training for the stunts he performed on the show.
Selleck adjusted his fitness routine as he aged to suit his body's needs. Today, his workouts focus on maintaining flexibility, strength, and cardiovascular health. He incorporates low-impact exercises such as swimming, walking, and light weightlifting. This balanced approach helps him stay fit without putting undue strain on his joints and muscles.
Importance of Flexibility and Mobility
In recent years, Selleck has emphasized the importance of flexibility and mobility in his fitness regimen. Understanding the natural decline in muscle mass and joint flexibility with age. he includes stretching and yoga in his routine. These practices help prevent injuries, improve posture, and maintain mobilit
- Video recording of this lecture in English language: https://youtu.be/lK81BzxMqdo
- Video recording of this lecture in Arabic language: https://youtu.be/Ve4P0COk9OI
- Link to download the book free: https://nephrotube.blogspot.com/p/nephrotube-nephrology-books.html
- Link to NephroTube website: www.NephroTube.com
- Link to NephroTube social media accounts: https://nephrotube.blogspot.com/p/join-nephrotube-on-social-media.html
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b) Secondary Standard Substance: Secondary standard substances are the substances from
which standard solution cannot be prepared by directly weighting and then dissolving in suitable
solvent. Examples are:
iv. The gram equivalent weight is large.
iii. The substances are stable both in solid or liquid state.
ii. The molecular weight of the substance corresponds to the chemical formula.
i. They are chemically pure substance.
Criteria of Primary Standard substance:
I t
a) · Primary Standard substance: Primary standard substances are substances from which
standard solution can be prepared directly by taking weight at an electrical balance and then
dissolving that substance in distilled water or any other suitable solvent. Examples are:
Standard solution: In the case of volumetric analysis, the solution whose strength is known
is called standard solution. Standard solution can be prepared directly from primary standard
substance by taking exact weight and then dissolving in distilled water.
PRINCIPLE:
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/ ~ a) Preparation of pritnary standard solution of Sodium thiosulfate (Na2S03), Oxalic acid
{(COOH)z. 2H20}, Potassium dichromate (K2Cr201).
b) Preparation of secondary standard solution of Sulfuric acid (H2S04), Hydrochloric acid
(HCl) and Acetic acid (CH3COOH).
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Secondarystandard substance:
i. Sulfuric acid (H:~S04)
ii. Hydrochloric acid (HCI}
iii. Nitric acid (HNQ3)
iv. Acetic acid (CH3COOH)
v. Sodium hydroxide (NaOH)
vi. Distilled water (H20)
iv. Potassium dichromate (K2Cr201)
iii. Sodium oxalate (NaOOC-COONa)
ii. Oxalic acid (HOOC-COOH)
i. Sodium carbonate (Na2C03)
Primarystandardsubstance:
Reagent:
Concentrationterm:Normal solution.
S2 = Strength of secondary standard solution
V2 = Volume of secondary standard solution ·
S1 =Strength of primary standard solution
V1 = Volume of primary standard solutionWhere,
In this case, the appropriate weight of the substance under test is taken and then dissolved in
distilled water and dil~te solution is prepared. This solution is then standardized with primary
standard solution and then its strength is determined by using the following equation:
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Page 5 of 23
v. Preparation of standard O.l(N) Sodium thiosulfate solution: The gram equivalent
weight of this substance is 158. So, to prepare 100ml of 0.1 (N) solution of Na2S203, we need
(158 + 100) = l.58gm ofNa2S203.
iv. Preparation of standard O.l(N) Potassium dichromate (K2Cr201) solution: The gram
equivalent weight of potassium dichromate is _f;j ~-b6 = 49. So, to prepare 1OOml of 0.1 (N)
potassium dichromate solution we need (49 + I00) = 0.49gm K2Cr201.
Now weigh 0.49gm of K2Cr207 in the electrical balance and dissolved it in 50ml of distilled
water in lOOml volumetric flask and shake gently. Then make the volume up to the mark with
distilled water.
iii. Preparation of standard O.l(N) Sodium oxalate solution: The gram equivalent weight
of this substance is 170 + 2 = 85. So, to prepare IOOml ofO.l(N) solution of sodium oxalate, we
need (85 + 100) = 0.85gm of sodium oxalate.
Now weigh 0.85gm of sodium oxalate in the electrical balance and dissolved it in 50ml of
distilled water in 1OOml volumetric flask and shake gently. Then make the volume up to the
mark with distilled water.
ii. Preparation of standard O.l(N) Oxalic acid solution: The gram equivalent weight of
oxalic acid is 126 + 2 = 63. So, to prepare IOOml of 0. l(N) solution of oxalic acid, we need (63 +
100) = 0.63gm of oxalic acid.
Now weigh out 0.63gm of oxalic acid in the electrical balance and dissolved it in 50ml of
distilled water in lOOml volumetric flask and shake gently. Then make the volume up to the
mark with distilled water. ·
Apparatus:
i, Balance
ii. Measuring cylinder
iii. Funnel
iv. Volumetric flask
Procedure:
a) Primary Standard Substance:
i. Preparation of standard O.l(N) Na2C03 solution: The gram equivalent weight of
Na2C03 is 53.50. 53 + 100 = 0.53 gram ofNa2C03 is needed to prepare O. l(N) lOOml solution of
Na2C03. ·..t ·~__:---~----------- -------------·----------------------···---------_,
Now 0.5fgm of Na2C03 was weighed in the electrical balance and dissolved it in 50ml of~-----------------:-;:_,,___ --------------·--------- -....
distilled water in. l_OOml volumetric flask and shake gently. Then make the volume up to the
mark with distilled water.
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Imran
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Manik
7. Mass = volume x density
Thus density ofHCI is 1.055. So, to prepare lOOml O. l(N) solution of CH3COOH the needed
volume of CH3COOH is (0.6 + 1.055) = 0.56ml = 0.6ml.
Now~ take lOOml volumetric flask, which contains 50ml of distilled water and 0.6ml of
CH3COOH is added slow,Iy. Then make the volume up to the mark with distilled water.
Page 6 of 23
iii. Preparation of standard O.l(N) Acetic acid (CH3COOH) solution: The gram
equivalent weight of CH3COOH is 60. So, to prepare lOOml of O. l(N) acetic acid solution (60 +
100) = 0.6gm of 100% CH3COOH is needed. But CH3COOH is liquid and secondary standard
substance. So its volumetric measurement is needed which may be obtained by the following
equation:
Mass = volume x density
Thus density ofHCI is 1.18. So, to prepare lOOml O. l(N) solution of HCI the needed volume
of32% HCI is (1.14 + 1.18) = 0.966ml = lml.
Now take lOOmlvolumetric flask, which contains 50ml of distilled water and I ml of HCl is
added slowly. Then make the volume up to the mark with distilled water.
ii. Preparation of standard O.l(N) HCI solution: The gram equivalent weight of HCl is
36.5. So, to prepare lOOmlof O. l(N) HCI solution (36.5 + 100) = 0.365gm of 100% HCI acid is
needed. Since HCl is not 100% pure, it is 32% pure. So to prepare lOOml of O. l(N) HCI solution
{(100 x 0.365) + 32} = l.14gm HCI is needed. But HCl is liquid and secondary standard
substance. So its volumetric measurement is needed which may be obtained by the following
equation:
b) Secondarystandard substance
i. Preparation of standard O.l(N) Sulfuric acid solution: The gram equivalent weight of
H2S04 is (98 + 2) = 49. So, to prepare lOOml ofO.l(N) H2S04 solution (49 + 100) = 0.49gm of
100% H2S04 acid is needed. Since H2S04 is not 100% pure, it is 98% pure. So to prepare 1OOml
ofO. I(N) H2S04 solution {(100 x 0.49) -'!,_ 98} = 0.5gm H2S04 is needed. But H2S04 is liquid and
secondary standard substance. So its volumetric measurement is needed which may be obtained
by the following equation:
Mass = volume x density
Thus density of H2S04 is 1.89. So, to prepare lOOml 0. l(N) H2S04 the needed volume of
98% H2S04 is 0.5 + 1.89 = 0.2645ml
Now take lOOml volumetric flask, which contains 50ml of distilled water and 0.2645ml of
H2S04 is added slowly. Then make the volume up to the mark with distilled water.
Now weigh l.58grrt of Na2S203 in the electrical balance and dissolved it in 50ml of distilled
water in lOOmlvolumetric flask and shake gently. Then make the volume up to the mark with
distilled water.
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8. Page 7 of 23
1L
Precaution:
i. Acid should be poured very slowly to the water. If acid is poured to water very rapidly
then the flask will be heated and may burst.
ii. Concentrated acid should be measured with measuring cylinder pipette as accurately as
possible.
iii. The surface of the funnel should be washed into flask with distilled water so that no acid
loss occurs.
ii. Preparationof standardO.l(N) KOHsolution: The gram equivalent weight of KOH is
56. So, to prepare lOOml ofO. l(N) KOH solution, we need (56 -i- 100) = 0.56gm of KOH.
Now take 50ml of distilled water in a conical flask and shake gently>until the KOH granules
dissolved completely. Then pour this solution to 1OOml volumetric flask and rinse the conical
flask into the volumetric flask and make the volume up to the mark with distilled water.
iv. Preparation of standard O.l(N) NaOH solution: The gram equivalent weight of NaOH
is 40. So, to prepare lOOmlofO. l(N) NaOH solution, we need (40 + 100) = 0.4gm ofNaOH.
Now take lOOml volumetric flask, which contains 50ml of distilled water and 0.4gm of
NaOH is added slowly and shake gently until the NaOH granules dissolved completely. Then
make the volume up to the mark with distilled water.
Md.
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9. Page 8 of 23
/'., Procedure:
i. Filling the burette: A clear and dried burette is filled with O. l(N) acid solution and mark
is adjusted with respect to zero.
ii. Placement of O.l(N) acid solution in conical flask by pipette: A clear and dried conical
flask is used to take 0.l(N) Na2C03 solution from the volumetric flask to the conical flask. Take
lOml of O. l(N) Na2C03 solution in a conical flask, add IOml of distilled water and 2-3 drops of
Apparatus: '-i
a) Conical flask e) Volumetric flask
b) Pipette f) Beaker
c) Burette g) Measuring cylinder
d) Funnel
Chemicals:
1-ar-b. l(N) H2S04 (secondary standard solution)
L-bt--0.1 (N) HCl (secondary standard solution)
/? c) O. I(N) CH3COOH (secondary standard solution)
Ld) O. l(N) Na2C03 (primary standard solution)
e) Indicator - methyl orange (for H2S04, HCl)
-Phenolphthalein (for CH3COOH)
S2 =Strength ofbase solution
V2 =Volume of base solution
S1 = Strength of acid solution
V1 =Volume of acid solutionWhere,
Principle:
This can be considered as the neutralization reaction between a strong base {e.g. 0.1 (N)
Na2C03} and strong acid {e.g. 0.1(N) HCl, 0.1(N) H2S04 etc.} of course CH3COOH is a weak
and organic acid. The following reactions take place between them.
H+. + OH- ~ H20
To determine the strength of the acid the following equation is used:
V1S1 = V2S2
Experiment -1/:
Determination of ltrength of O. l(N) H2S04, O. l(N) HCl, O. l(N) Acetic acid (CH3COOH)
solution by standard Od(N) sodium carbonate (Na2C03) solution.
Md.
Imran
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Manik
10. ml
(N).; ·i
I
I
-L.
ml
(N)
O)·~
1
0
()r~
(...,'h· /
//
s-en_,,
I,.
~rr,·
V1 =Volume of acid =
S1 = Strength ofacid =
V2 =Volume ofbase =
S2 = Strength of base =
Where,
Solution no. Volume, of base Initial burette reading F.B.R Difference Mean
2 io 0 0·'2. ~'L.
2 10 ~ ·'L .~· b 9·lt ~·~
2 to ti· (:, 2-1· b 9'·~'
Where, V1 =Volume ofacid = <6· b ml"'?
S1 = Strength of acid = 1. (N)
-~
V2 =Volume ofbase = Q mlr
'--- S2 =Strength ofbase = C) r 1 (N)
'
We know, V1S1 = V2S2
iL
0 S - V2S2 0)<. ·'1
b· 2..i (N)r 1--- = =
' v: <6· l 4I
-,
Thus, strength ofacid (H2S04) = O•Z~ (N)·/ t-
~· '7I ~<~
Table for O.l(N) HCI · e
Solution no. Volume of base Initial burette reading F.B.R Difference Mean
I IO 0 <6·1 ~·t
1 10 g.t_ b·~ cg. '2. g. l(,
I 10 (,.':) 2-~·a g.'l_ --
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x..
methyl orange. The colour becomes yellow. Add 1 Oml distilled water and 3-4....~~
phenolphthalein for CH]COOH. This colour becom_!s red.
·- iii. Wipe out the bottom of the conical flask and place a piece ofwhite paper below it. Take
initial burette reading. Now add drops of acid solution from the burette to the conical flask along
with gentle shaking. A drop of acid solution will make it orange colour but this colour will fade
away rapidly. When the end point reaches, then the colour become orange. Taken the final
burette reading and fill the table for each acid.
Md.
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11. Page 10 of 23
i. Taken necessary step to prevent from the stop cork of burette.
ii. Acid solution from burette should be added slowly.
iii. Not more than 3-4 drops of methyl orange should be used.
iv. Difference of acid solution between two titrations should not vary more than 0.2ml. If it
is high, repeat the titration.
v. In case of titration of CH3COOH used phenolphthalein indicator.
--
Precaution:
(N)
(N)
(N)
e t'2. ~
O· 07
0·';>1-
../Result:
a) Strength ofH2S04 {O. l(N)} =
b) Strength ofHCI {O. l(N)} =
c) Strength ofCH3COOH {O.l(N)} =
I -1
f !
i '--
-L
L
Where, V1 = Volume of acid = 7.-, ml
S1 =Strength of acid = 41 (N)
V2 =Volume of base = t0 ml
S2 =Strength of base = o.t (N)
We know, V1S1 = V2S2
0 S - V2S2 toi--0·1
0·~1-r, 1--v,- = = (N)
-1-·?I
Thus, strength of acid (CH3COOH) = 0·1~7- (N)/L
Solution no. Volume of base Initial burette reading F.B.R Difference Mean
3 10 C) ::;. i--,:.
3 10 1- -.
'lt·~ 1--·? i·~
3 10 ~·~ 2·<'h 1·~
L
Thus, strength of ad~ (HCl) = a· l 0 7-- (N)
tTableforO.t(N)C~,coo?r--
--
L
= o- l01- (N)
to~ ·'.
=
9. ':l
We know,
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12. Page 11of23
ii. Placement of O.l(N) standard oxalic acid solution in conical flask by pipette: A clear
and dried conical flask is used to take O. l(N) oxalic acid solution from the volumetric flask. Add
- Procedure:
i. Filling the burette: A clear and dried burette is filled with 0.1 (N) basic solution and
lower meniscus of the solution is adjusted to zero.
e) Volumetric flask
f) Stand clamp
g) Measuring cylinder
Apparatus:"
a) Conical flask
b) Pipette
c) Burette ·
d) Funnel
e) Indicator - Phenolphthalein
O. l(N) KOH (secondary standard solution)
O, l(N) NaOH (secondary standard solution)
O. l(N) NH40H (secondary standard solution)
O. l(N) 'oxalic acid (primary standard solution)
Chemicals:
a)
b)
-a
I
I .L_.
S2 = Strength of acid solution
V2 =Volume of acid solution
S1 =Strength of base solution
V1 =Volume of base solutionWhere,
Ir + OH-~ H20
acid base water
The calculation is performed by using the following equation:
V1S1 = V2S2
Principle:
Standardization of strong base by oxalic acid can be considered as neutralization reaction
between strong base and weak acid. Phenolphthalein should be used as indicator. The following
reaction takes place.
Experiment - 3: '
Determination of strength of O. l(N) Potassium hydroxide (KOH), O. l(N) Ammonium
hydroxide (NH40H), 0.1 {N) Sodium hydroxide (NaOH) by standard oxalic acid.
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13. Page 12 of 23
O·~~ ml
1 (N)
V1 =Volume of base =
S1 =Strength of base =
Where,
Solution no. Volume of acid Initial burette reading F.B.R Difference Mean
2 ·- 10 C) lO•i IO· I
2 10 1.0·t 2· 1i lO·~~
2 10 2-t I 1 1>·0 0·0)
l_
Where, V1 =Volume ofbase = g.1 ml
S1 =Strength ofbase = '2. (N)
V2 = Volume of acid = LO ml~
S2 = Strength of acid = Q., (N)
We know, V1S1 = V2S2
o s - v2s2 l0-1- ().I
a.,i. ~r 1--.-. = = (N), v: <l.. II
Thus, strength of base (KOH) = 0-~:9 (N)
Table for O.l(N) NaOH
Solution no. Volume of acid Initial burette reading F.B.R Difference Mean
I IO 0 <3·1- ~·
1 10 t·1. l~· '?> ~-2- s.t
1 10 ((;·~ l~·~ g.o
Table for O.l(N) KOH
iii. Titration: .
a) The bottom ofthe conical flask is wiped and a piece of white paper is placed below it.
b) Take initial burette reading.
c) Add drop by drop NaOH solution from the burette to the conical flask along with gentle
shaking. Each drop produces a pink colour which disappears rapidly.
d) At the end point the colour of the solution becomes pink which remain for long time.
e) Take the final burette reading and fill the table, from which we can calculate the strength
of solution.
I~
lOml of distilled wafer and 3-4 drops of phenolphthalein solution to it. The solution remains
colourless.L
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14. Page 13 of 23
i. The necessary step should be taken to prevent the breaking of stop cork of the burette.
ii. Acid solution from burette should be added slowly.
iii. Not more than 3-4 drops of phenolphthalein should be used.
iv. Difference of acid solution between two titrations should not vary more than 0.2ml. If it
is high, repeat the titration.
'L..
L
We know, V1S1 = V2S2
0 S - V2S2
01-0.'
o. _'2.'5' (N)r, i-V = g =
1
Thus, strength of base (NH40H) = O·'_'L~ (N)
.>
Result:
.>a) Strength ofH2S04 {O.l(N)} = 0·'l'3 (N)
b) Strength ofHCI {O. I(N)} = C·OOJ1. (N)
~
c) Strength of CH3COOH {0.1 (N)} = CJ ·l'L~ (N)
Precaution:
L
,.._
Where, V1 =Volume of base = s ml
Si= Strength of base = 'l (N)~
V2 =Volume of acid = 0 ml
S2 = Strength of acid = ().I (N)
L
Solution no. Volume of acid Initial burette reading F.B.R Difference Mean
3 10 0 ~-9 1-· °)
3 10 ~·~ b <8· I g
3 10 (, ~~ s
'r '--
Table for O.l(N) NH40H
V2 = Voh.ime of acid = 0 ml
t.., S2 = Strength of acid = 0.1 (N)
-
We know, ViS1 = V2S2
L__
Oi' S _ V2S2 01-0·1
r 1--- = = 0- o~ 9-. (N)
' v. le)·~'?I
Thus, strength of base (NaOH) = 0 · OC{)f (N)
• I
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15. Page 14 of 23
Solution no. Volume of acid Initial burette reading F.B.R Difference Mean
1 10 C) ~'2. t~
1 10 '2. 2-15 i 12.·~'?
1 10 'L*'! ~ 1--- ..2_
Table for O.l(N) NaOH
•
i. Determination of standard 0.1 (N) oxalic acid solution.
ii. Determination of strength of 0.1 (N) NaOH solution by oxalic acid solution.
iii. Calculation ofstrength of 0.1 (N) NaOH by titration.
iv. Standardization of 0.1(N) HCl with standardized NaOH solution.
v. Calculation ofstrength ofO. l(N) HCI by titration.
e) Volumetric flask
f) Stand clamp
g) Measuring cylinder
h) Beaker
i. O. l(N) Potassium hydroxide (KOH)
ii. O. l(N) Hydrochloride acid (HCl)
iii. O. l(N) Oxalic acid solution
iv. Indicator - methyl orange and phenolphthalein
Apparatus:
a) Conical flask
b) Pipette
c) Burette
d) Funnel
Procedure:
H+ +OH.~ H20
As both acid and alkali are secondary standard substance, so anyone of them must be
standardized by primary standard solution.
Calculation is done by the following equation:
VS= V1S1
Where, S = Strength ofacid
V = Volume of acid
S1 =Strength of base
V1 =Volume of base
Chemicals:
Principle:
During the standardization of a strong base with a strong acid neutralization reaction takes
place by this way:
Experiment - 4:
The standardization ofstrong base {secondary standard solution O. l(N) NaOH} with strong
acid {secondary standard sdlution O. l(N) HCl}
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16. Page 15 of 23
Precaution:
i, Take necessary step to prevent breaking the stop cork of the burette.
ii. Acid solution from the burette is slowly added.
iii. Not more than 3-4 drops of phenolphthalein should be used.
iv. Difference of basic solution between two titrations should not vary more than 0.2ml. If it
is high, repeat the titration.
L
•
'
r I
L
(N)
vs ~™-0-1
Or, S1 = ~
2
= • ~ . {, - .>"l 0 ~
Thus, strength of acid (HCI) =1C (N) /
Result. /
i. Strength ofNaOH {O.l(N)} = 0 · 0<6 (N) "' /
ii. Strength ofHCl {O. l(N)} = 6. tO~ (N) / _
' '
~' '---
r 1
L
We know,L
Where, V1 =Volume of base = 0 ml
S1 = Strength of base =
o.. ' (N)
V2 =Volume of acid = 9. (, ml
S2 = Strength of acid = 'l (N)
'
i
L
Solution no. Volume of base Initial burette reading F.B.R Difference Mean
3 IO C) ~·~ 9·~
3 IO ~·Lt & . 0) ~-? ~.{:,
3 IO ~· 0) 1-~·1-- 9.g
TableforO.l(N) HCI
Where, V1 = Volume ofacid = 0 ml;
'-- S1 = Streng!h ofacid = 0· (N)
V2 = Volurrie of base = 12..'?1 ml
S2 =Strengih of base = ·'l (N)
~-
We know, V2S2 = V1S1
o s - v;s1
01'0·
r, 2-V =
'2-·~'.
= . (N)
2
Thus, strength of base (NaOH) = 0. 0<6 ( (N)
T.
Md.
Imran
Nur
Manik
17. Now let the amount of solid MH taken for the experiment is n gm of molecular weight M
Page 16 of 23
:. Total heat absorbed= (M1S1 - M2S2) (T2 - T1) cal= Q cal (say)
Where, M1 =mass of the solution
M2 = mass ofthe calorimeter + stirrer + thermometer
S1 = specific heat of solution
S2 = specific heat of glass
T1 = Initial temperature
T2 = Final temperature
Theory:
Since the heat which is evolved or absorbed on dissolving a substance depends on amount of
water or other solvent employed, the statement of the heat of solution has· a definite meaning.
Only when the concentration of the solution formed is given. If the dilution is so great that
further dilution is unaccompanied by any heat effect, then the heat measured per mole ofsolute
is known as the heat of solution at infinite dilution, usually, however, it will not be possible to
determine this heat of solution directly and one therefore must state the number of molesof
water in which one mole of solute is dissolved. Further a clear definition must be made between
the quantity known as the integral heat of solution (which is the heat obtained when I mole is
dissolved in X moles of solvent) and the different heat of solution. The latter is the heat change
per mole of the solute when an infinitesimal amount of solute is dissolved in a large amount of
solution of stated concentration.
The dissolution of most of the solid salt (MA) in water is an endothermic process. This
means that a definite amount of heat energy is necessary for the decomposition of MA into M
1
and A- ions and hence to go into solution. The heat absorbed in the reaction must be equal to the
heat loss due to the decrees of temperature of the solution in the calorimeter and other glass and
with the calorimeter through (T2 - T1)°C. this is exactly equal to the sum of the masses of the
parts multiplied by their specification.
Principle:
When solids are dissolved into H20 or any other solvent heat is either absorbed or evolved.
Heat of the solution is the heat content change of the solvent when one mole ofa solute is
dissolved in it. It depends on the concentration of the resulting solution. The integral heat of a
solution is the total heat content change for dissolving one mole completely that is when the
solution is complete.
. '---
L
i
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''----
Experiment- 5:
~ Determination of integral heat of solution of Potassium chloride (KCI), Potassium nitrate
(KN03), Ammonium chloride (NH4CI) and Sodium chloride (NaCl).
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18. / Page 17 of 23
Mass of calorimeter + Stirrer + Thermometer (M2) =
Molecular weight of KCI (M) = .f.. Lt 1 ~
i_(), ~ gm
Calculation:
ForKCI
Mass of KCl (W) =
Procedure:
i. 200ml of distilled water is taken into a pre-weighed calorimeter with stirrer and
thermometer.
ii. The temperature of the contents of the calorimeter was noted and recorded.
iii. 1 Ogm of supplied solid sample was weighed using a rough balance.
iv. Supplied sample added quickly to the calorimeter.
v. The temperature recorded after 30 seconds interval at the time the solution was stirred
quickly. The temperature time recording continued for 15 minutes.
vi. The final weight of calorimeter with its whole content was taken. The differences
between the weight of calorimeter and final weight give the weight of the solution.
vii. The temperature time curve was drawn and corrected final temperature was taken from
the graph in case of each supplied sample.
iii. Solid NH4CJ
iv. Solid N&CI
L
L
.f
L Chemicals:
i. Solid KCI
ii. Solid KNQ3
iv. Rough balance
v. Measuring flask
vi, Stop watch
Apparatus:
i. Calorimeter
ii. Stirrer
iii. Thermometer
w:. Number of moles = -
M
For the dissolution of moles of the salt MA, the amount of heat absorbed Q cal (say).
w:. For one mole of MA, the heat absorbed H = Q x -
M
H = -1-{M (M1S1 +M2S2)(1~ -1;)}Kcal
1000 w -
i
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19. ·- -~)
Page 18 of 23
Specific heat of solution (S1) = 1
Specific heat of glass (S2)= 0.16
Mass of solution (M1) =f~3-~~)m {~g +. ~ ~1oi r
gmMass of solution + Calorimeter + Stirrer+ Thermometer (M3) =
Mass of calorimeter + Stirrer + Thermometer (M2) = ~ ~ ? gm
Molecular weight of NH4CI (M) = '5'3 ·'i"
ForNH.,CI
Mass of NH4Cl (W) = ! 0 gm
The total heat absorbed:
H= _l_ {M(M1 S1 +M~S2 )(T2 -1;)}Kcal
1000 fV_ -
~ 1 ·) ~f-t·'i (2.0lS·(.)(l +(i73f..-O·I~) (Z·1- - 21J1K...u-'
1000 o·~ ~
-z - L_. C. 2.. ~(.o..l
Time (min) 8 8.5 9 9.5 10 10.5 11 11.5 12 12.5 13 LU 14 14.5 15
Temp(°C)
1Yt 21·1- l·1- 2.·f- 2l ·7- 2·1 2Y1- 2·l- 2Yl- 21·1 2·'.1- 219- 2·/ 21·+ 21·J
Time (min 'C 0.5 I 1.5 2 2.5 3 3.5 4 4.5 5 5.5 6 6.5 7 7.5
Tcmp(0C)
~ 22-"i 21·} 2FI- 2.1·1- Z1- .2..1·°7- 2Y7- 21-7 2.F1- 21·7- 2J·1- '2 .-,.. 2. ·7- 2Ft 2-·~
Final temperature (T2) = '2.~•1- °C
Initial temperature (T1) = · ?.~ °C
Specific heat of solution (S1) =
Specific heat of glass (S2).= 0.16
Mass of solution (M1) = 2.0&.<, gm
L
gmMass of solution + Calorimeter + Stirrer+ Thermometer (M3) = C ~ ' 'L
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23. ·.~
Page 20 of 23
Result:
Heat ofKCl solution absorbed per mole=
Heat ofNH4Cl solution absorbed per mole=
Heat of KN03 solution absorbed per mole=
Heat of NaCl solution absorbed per mole =
Kcal
Kcal
Kcal
Kcal
- l..· (,L_
-S- - 2- b
-7· I~
~ ,.(:,)
The total heat absorbed:
H= -1-{M (M1S1 +M2S~)(1~ -li)}Kcal
1000 JV -
t i~ 5~: (Li 5·~ 7 I-t /.ii l.·'!l >< O :I 4) ( 31 - ->tf U.-
-z - 1· ~ S' ~~G-'
L·i
Time (min e o.s 1 1.5 2 2.5 3 3.5 4 4,5 5 5.5 6 6,5 7 7.5
Temp (°C)
31. ~IS ; ~' .,,' ~ ~ ~ ~I ~" ~' '3' ~I 3 1 ~1
Time (min) 8 8.5 9 9.5 10 10.5 11 11.5 12 12.5 l3 13.5 14 14.5 15
Temp (°C) ,, ')' ~' ~' ~' ~) ">l '3 I ~' '3' ~' "31 ~' ~1 "S
gm
For NaCl
Mass of NaCl (W) = i 0 gm
Molecular weight of NaCl (M) = 5<6·)
Mass of calorimeter + Stirrer + Thermometer (M2) = 4.t b· ~ gm
Mass of solution+ Calorimeter+ Stirrer+ Thermometer (M3) = C~t · S-
Mass of solution (M1) = 21r· C. gm
Specific heat of solution (S1) = I
Specific heat of glass (S2) = 0.16
Initial temperature (T1) = ~ 'l °C
Final temperature (T2) = 31 °C
~[!· I
'
Ll
:1f .
H= lO~O {: (M,S, +M2S,)(7;-1;)}Kcal
e: _i_ ~ to1 ~(1,t>~., "I,..- 4,~t·t~ ().
.1000 lo
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Md.
Imran
Nur
Manik
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25. Page-21 of 23
Procedure:
i. Preparation of solution of 0.1 (N) oxalic acid, H2S04, HN03, HCl and NaOH.
ii. Find out the exact concentration of supplied acid and base and suppose that they are (a)
and (b) respectively.
iv. NaOH or KOH
v. Methyl orange
vi. Distilled water
Reagent:
i. Oxalic acid
ii. HCl, H2S04, HN03
iii. Phenolphthalein
f) Volumetric flask
g) Stop watch
h) Beaker 250ml.
Apparatus:
a) Conical flask
b) Pipette
c) Burette
d) Calorimeter, thermometer and stirrer
e) Measuring cylinder 1OOml and 1 Oml
Principle:
Heat of neutralization is defined as heat evolved when one gram equivalent of an acid is
completely neutralized by a base.
In dilute solution strong acid and strong base and the salt produced remain completely
dissolved. So the neutralization reaction may be represented as:
H+ + A" + B+ + Off = H20 + B+ + A
Therefore, the neutralization between strong acid and strong base may also be called as
formation of one mole ofwater. So, the heat change accompanying this reaction is constant.
In order to obtain the heat of neutralization according to the quantitative definition:
Let, W 1 = mass of mixture
W2 =mass of calorimeter with stirrer and thermometer
S1 =specific heat of mixture
S2 = specific heat of calorimeter
T1 = initial temperature
T2 = final temperature
lfVml ofHCl with strength Sis neutralized by NaOH, the heat of neutralization is as:
£H= v~s {cw1s1 +w2s2)(T2-1;)}ca1
Experiment - 6:
Determination of heat of neutralization between a strong base and strong acid.
~
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.L~
Md.
Imran
Nur
Manik
26. Page 22 of 23
t 0 ml
O·()i (N)
9,4 ml
1 (N)
'
V1 =Volume ofNaOH =
S1 =Strength NaOH =
V2 =Volume ofHCI =
52 =Strength ofHCl =
Where,
0
Number of Volume of Strength of I.B.R F.B.R Difference Mean
experiment Na OH NaOH
1 10 c~oi 0 0·1t 9·~
2 10 o o i 9,Lt &·~ 0. S"' 9· f:,
3 10 C)· Qi I~~ 2J~; 1-- 0·&
Number of Volume of Strength of LB.R F.B.R Difference Mean
experiment oxalic acid oxalic acid
I 10 0·{ 0 I 'L l i._
-··
2 10 6·1 .z. 2) 1') I~.')'
3 10 6·1 'l '5 )1- 'L
Table for oxalic acid and NaOH
iii. Take 100/a ml of the supplied acid and 100/b ml of supplied base in two separate flask.
iv. Pour one of these solutions into the previously cleaned and weighed calorimeter and note
down the temperature at a regular interval of time.
v. Plot the graph temperature versus time in order to find out the true final temperature after
the correction for heat loss bf reaction.
vi. Find out the correct final temperature and calculate heat of neutralization according to the
equation.L
t
·L
Where, V1 =Volume of oxalic acid = 10 ml- S1 =Strength of oxalic acid = (.). (N)
V2 =Volume ofNaOH = 1-:>~ ml
S2 = Strength of NaOH = 'l (N)
We know, V1S1 = V2S2
0 S - V.S1
O"'- O· .
o .()rg_.r 2--- =
'2 ·~'> = (N)
' v2
Thus, strength of base (NaOH) = () -~~1 (N)
-:Table for O.l(N) HCI
Md.
Imran
Nur
Manik
27. Page 23 of 23
Result: Heat of neutralization ofHCl = ~- 2 6 Cal
. :. L.H = - I~· '& f, Cal
I
i
Thus, heat ofneutralization: L.H = -.-1- {CWiSI + w2s2 )(T2 - Ti)}Cal
f· xS
Or L.H= 1 ) (2..._i:i<. +~o?• 2~D·9 (~Q·S"-J.o)
• 1·t<?>·I> Lr)( a.o'IS~ 1 L
Time (min) 8 8.5 9 9.5 10 10.5 l l 11.5 12 12.5 13 13.5 14 14.5 15
Temp(°C) >o·) 'JO.S 3l>T -so.r YiS 30.J 30.S "},l•S" ~us ~OS '1~.S- 30.S '30.5" 3) S'"' 10-')
Time(min 0 0.5 l l.5 2 2.5 " 3~ 3.5., 4 4.5 5 5.5 6 6.5 7 7.5
Tempec>
- ,
~ '}O·J' ~()·S- '30·l ~o·) 10.s ~-d·J ~u<v 3()·!$" ';l.O·s ~-S- 3V·f' ':O·S ltl·~ ~Cl-S- <3.<l·.J
t-
gm
Now, Mass of calorimeter + Stirrer+ Thermometer (W'!) =
Mass of solution+ Calorimeter+ Stirrer+ Thermometer (W3) =
~~on(Wi)= 2J·i gm
Specific heat of solution (S1) ". 1
Specific heat of glass (S2) = _ · 0.16
Initial temperature (Ty = ':>() °C
Final temperature (T2) = )Cl -:S-°C -· ,.r- .,,,,,.,,..
Let, volume'V' of exact Q.l(N) HCl solution was,,____ '--v-->
Vx 0-0B~ = lQlJj._ C>-1
Or, V=t~-O~ml
,(1() )()O·) -:-·
0- ~~·· (
V1S1 =VS -..
V =Volume ofi':JaOH = r l.q&- ~t ml
S =Strength NaOH = a.oil (N)
V2 =Volume ofHCl = lQ.2.-- ml
S2 =Strength ofHCl = b·i (N)
Then,
Where,
(N)
= (N)
V1S1 = V2S2
0 . s - i'iS1
r1 2-V
. 2
Thus, strength ofacid (HCI) =
We know,
-
·'
. I
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L
Md.
Imran
Nur
Manik