Intro to Chemistry PPT 2 PDF

GENERAL CHEMISTRY BRIDGING CHEMISTRY AND MEDICAL TECHNOLOGY Our Lady of Fatima University INTRODUCTION Overview of Medical Technology Course  MEDICAL TECHNOLOGY “The branch of medicine concerned with the performance of laboratory determinations and analysis used in diagn...

GENERAL CHEMISTRY BRIDGING CHEMISTRY AND MEDICAL TECHNOLOGY Our Lady of Fatima University INTRODUCTION Overview of Medical Technology Course  MEDICAL TECHNOLOGY “The branch of medicine concerned with the performance of laboratory determinations and analysis used in diagnosis and treatment of diseases and maintenance of health” Fagelson (1961)  MEDICAL TECHNOLOGY “The auxiliary branch of laboratory medicine which deals with the examination of various chemical, macroscopic and other medical procedures, techniques which will aid the physician in the diagnosis, study and treatment of disease and in the promotion of health in general” –Philippine Medical Technology Act  MEDICAL TECHNOLOGY It is a branch of laboratory medicine dealing with the examination of the body fluids and tissues with the use of various methods. “It involves the application of natural, physical, a n d biological sciences on the performance of laboratory procedures, which aid in the diagnosis and treatment of disease and the maintenance of health.” – Heinemann MEDICAL TECHNOLOGIST A person who engages in the work of medical technology under the supervision of a pathologist or licensed physician authorized by the Department of Health in places where there is no pathologist and who having passed the prescribed course (Bachelor of Science in Medical Technology/Bachelor of Science in Hygiene) of training and examination is registered under the provision of this RA5527 MEDICAL TECHNICIAN A person certified and registered with the Board as qualified to assist a medical technologist and/or qualified pathologist in the practice of medical technology as defined in this Act.  CAREERS MEDICAL TECHNOLOGISTS IN LABORATORY a. Clinical laboratory Hospital Clinic Independent laboratory b. Sales industry Sales representative – pharmaceutical, equipment, reagents Educational representative c. Research industry Medical center research Industrial research d. Academe College, chemistry, biology, medical sciences e. Veterinary medicine Research Clinics f. Forensic  KEY ATTRIBUTES Physical stamina Good eyesight – normal color vision Manual dexterity Good intellect and aptitude to biological science and caring attitude Communication skills Observant, motivated, precise, good organizational skills Service oriented Patient Honesty, accuracy, skillful Dedicated Emotional, intellectual, spiritual and physically mature X - factor  HISTORY OF MEDICAL TECHNOLOGY Ebers Papyrus (1500 B.C) Hookworm – Book of Ebers papyrus describes the treatment of hookworm disease and infection transmissible to human. Vivian Herrick Intestinal parasite such as taenia and ascaris Hippocrates – Father of Medicine Use of mind and senses as diagnostic tools 4 humors in human body a. Yellow Bile – Serum (Only if you allow blood to clot) b. Phlegm – a whitish layer now called buffy coat. c. Blood – Red Blood Cells d. Black Bile – Dark clot found at the bottom.  HISTORY OF MEDICAL TECHNOLOGY Urine is regarded as composite of the humors proposed by Hippocrates a. Urinalysis b. Uroscopy Contributions of Early Civilizations Greeks a. Diagnosed diabetes Hindu a. Made scientific observations of urine 3 P's of diabetes: Polydipsia – Increase thirst Polyuria – Frequent urination Polyphagia – Rise in appetite  HISTORY OF MEDICAL TECHNOLOGY Chinese a. Immunization by inhaling powder made from smallpox scabs. Romans a. Developed lab tools, forceps, scapels, specula, and surgical needles. Indians a. Toxicology. The science of poisons. Overlapping with biology, chemistry, pharmacology, and medicine Rufus of Ephesus Made the first description of hematuria  HISTORY OF MEDICAL TECHNOLOGY Isaac Judeus a. Kitab al Baul b. Founder of nephrology Jerusalem Code of 1090 a. Failure of physicians to examine patient’s urine was punishable by public beatings Hans and Zaccharias Janssen a. Discovery of microscope Ruth Williams a. Anne Fagelson (14th Century) a.Believed that MT started when a prominent Italian doctor at the University of Bologna employed Allesandra Gillani Allesandra Gillani a. Tasked to perform autopsy and draining of blood  HISTORY OF MEDICAL TECHNOLOGY 15th century a. Discovery of dyes specially aniline dyes Anton van Leeuwenhoek a. Father of Microbiology b. Saw bacteria and classified them as shapes “animalcules” referred to him as microorganisms. Anthanasius Kircher a. Blood of the patients with plagues contains worms. Robert Hooke a. Discovery of cell and published it in his “Micrographia” Marcello Malpighi a. Founding father of modern Anatomic Pathology Jea n Baptiste van Helmont (1577-1644) a.Introduced the gravimetric analysis (specific gravity) of urine by weighing a number of 24-hr urine specimens  HISTORY OF MEDICAL TECHNOLOGY Richard Lower a. blood transfusion from one animal to another is possible Frederick Dekkers a. Observed that proteins in the urine precipitated when boiled with acetic acid William Hewson a. Discovered that plasma could be separated from blood cells when blood clots Matthew Dobson a. Identified sugar in the blood and urine of diabetes Francis Home a. Yeast test for sugar in diabetic urine 19th Century a. Water treatment b. Pasteurization of milk c. Improvement of hygiene  HISTORY OF MEDICAL TECHNOLOGY Rudolf Virchow a. Founder of Archives (collection of records) of Pathology in Berlin Herman Von Fehling a. Fehling’s test/ Fehling’s solution John Snow a. Father of modern epidemiology b. Cholera outbreak in London Louis Pasteur a. Germ Theory of Disease Robert Koch a. Koch's postulates a. tuberculosis – Mycobacterium tuberculosis b. cholera – Vibrio cholerae c. Anthrax – Bacillus anthracis  MEDICAL TECHNOLOGY IN THE PHILIPPINES Introduced by THE 26 MEDICAL INFANTRY OF THE 6 US ARMY. THE First Clinical Laboratory in the Philippines is QUIRICADA ST., Sta. CRUZ, MANILA - MANILA PUBLIC HEALTH - The lab offered training programs to high school graduates as early as FEBRUARY,1944. 1945 THE US ARMY LEFT in JUNE Endorsed it to the NATIONAL DEPARTMENT OF HEALTH The Department rendered the laboratory non-functional for sometime. DR. PIO DE RODA ORGANIZED MANILA PUBLIC HEALTH LABORATORY from the remnants of the deserted laboratory. OCTOBER 1,1945 - With Dr. Mariano Icasiano as his assistant and who was then the MANILA CITY HEALTH OFFICER. 1947 Training of high school graduates to work as medical technicians by Dr. Pio de Roda and Dr. Prudencia de Sta. Ana No period of training was set and no certificates were given.  MEDICAL TECHNOLOGY IN THE PHILIPPINES 1954 A 6 months laboratory training with certificate upon completion was given to the trainees. Dr. Sta. Ana prepared the syllabus for the training program. Medical Technology Education in the Philippines The Training program offered by Dr. Pio De Roda did not last long. The FIRST B.S. Degree course in Medical Technology was offered by the PHILIPPINE UNION COLLEGE and MANILA SANITARIUM. After 2 years, PUC produced its first graduate, Dr. Jesse Umali, now a successful OB-Gynecologist. 1957-1958 Dr. Antonio Gabriel and Dr. Gustavo Reyes of the FACULTY of Pharmacy, University of Sto. Tomas offered medical technology as an elective subject to 4th and 5th year B.S. Pharmacy students. Rev.Fr. Lorenzo Rodriguez Decided to offer it as a course because of the popularity of medical technology among pharmacy students. JUNE 17,1957 Temporary permit was issued by the Dept. of Education, for first to third year student University of the Philippines Offers a similar course but the degree being conferred in B.S. Public Health  MEDICAL TECHNOLOGY IN THE PHILIPPINES June 14,1961 – full recognition of the 4 – year B.S.M.T course was granted by Department of education 1962 – First graduates at Centro Escolar University NOW There are at least 80 schools of med tech recognized by department of education culture and sports “Being weak is Nothing to be A s h a m e d of, but Staying weak is” –Fuegoleon Vermillion  SUMMARY 1. 2. 3. Medical technology is any A medical technologist is A Medical Technician is a technology used to save a highly skilled health medical professional who lives or transform the professional who tests plays a vital part in the health of individuals and looks carefully at health care industry by suffering from a wide blood, other body fluids, providing support for range of conditions. It and tissue samples. physicians and hospitals. involves the application of natural, physical, and biological sciences on the performance of laboratory procedures.  CHAPTER 1 Fundamental Concept in Analytical Procedure Fundamentals in Analytical Procedure Units of measurement Preparation and standardization of solution Chemical reagent and laboratory supply Laboratory math  OBJECTIVES After the course of discussion, students are expected to: Discuss mathematics of Chemistry Recognize and utilize the fundamental quantities and convert units of measurements effectively Solve problems involving measurements in Chemistry Reoriented about the difference of accuracy and precision Understand significant figures and perform simple operations in relation to it.  Units of Measurement Metric system; Based on decimal system; a system of divisions and multiples of tens. m – standard measurement of length, g – standard measurement of weight, L – standard measurement of volume International system (SI units) Standardized system based on seven base units  Base Units of SI System prefix symbol factor Tera T 1012 Giga G 109 Measureme Unit Abbreviation nt name Mega M 106 Length Meter m Kilo k 13 Mass Kilogra kg Hecto h 102 m Deka da 101 Time Second s Deci d 10-1 Amount of Mole mol Centi c 10-2 substance Milli m 10-3 Electrical Ampere A current Micro u 10-6 Temperatur Kelvin K Nano n 10-9 e Pico p 10-12 Luminous Candela cd Femto f 10-15 intensity Atto a 10-18  Units of Measurement Length - the standard unit for measurement of length is meter. 1 meter = 39.37 inches 1in = 2.54 cm Mass – the standard unit for measurement of mass is kilogram 1 kg. = 2.2lbs Volume – the standard unit for measurement of volume is in liters Amount of substance - the standard unit for measurement of amount of substance is mole Temperature K= C+ 273 C = 5/9 (F-32) R= °F + 459.67 C = K- 273 F = 9/5 (C+32)  UNIT OF MEASUREMENT Example: Convert: 328 cm into: a. Yards - 3.587 yds b. Miles – 0.00204 miles c. Feet – 10.76 ft  UNIT OF MEASUREMENT 0.0000011 Example: Convert: 98 𝑚2 into: a. 𝑦𝑑2 - b. 𝑖𝑛2 - 151.9 c. 𝑚𝑚2 − 98,000,000 d. 𝑓𝑡2 - 980,000  UNIT OF MEASUREMENT Example: Convert: 978 𝑚3 into: a. 𝐿– b. 𝑖𝑛3 - c. 𝑈𝑆 𝐺𝑎𝑙𝑙𝑜𝑛 d. 𝑓𝑡3 - 34,537.75  UNIT OF MEASUREMENT EXAMPLE 2 : 576 kg Example: Convert: 567 𝑘𝑔 into: a. 𝑀𝑇 – b. 𝑃𝑜𝑢𝑛𝑑𝑠 – c. 𝑂𝑢𝑛𝑐𝑒𝑠 –  UNIT OF MEASUREMENT Example: Convert: 576 𝑘𝑔/𝑚3 into: a. 𝑙𝑏 - 𝑓𝑡 3 - 0.020736 lb/in^3 𝑙𝑏 b. 𝑖𝑛3 c. 𝑔 - 0.576 g/ml 𝑚𝑙  UNIT OF MEASUREMENT Example: Convert: 98.5 𝑎𝑡𝑚 into: a. 𝑚𝑚𝐻𝑔 – b. 𝑘𝑔𝑓/𝑐𝑚2 - c. 𝑀𝑃𝑎 – d. 𝑙𝑏/𝑖𝑛2 -  UNIT OF MEASUREMENT TEMPERATURE CONVERSION FORMULAS ( °F – 32 ) × 5/9 Degree Celsius (°C ) ( K – 273.15) (°C × 9/5) + 32 Degree Fahrenheit (°F ) Example: ( 1.8 × K) – 459.67 Convert: °F + 459.67 a. 598 °C to °R – ( °C + 273.15) b. 67 °R to K - Kelvin (K) (°R × 5/9) c. 988 °F to °R - 1447. d. 76 °F to °C - 24.4444444444 ( °F + 459.67 ) / 1.8 Rankine (°R) (°C × 9/5 ) + 491.67 °F + 459.67  Fundamental Concept in Analytical Procedure Basic laboratory principles includes: a) Patient preparation b) Proper collection c) Proper specimen handling and processing d) Hiring, Training and Management e) Quality assurance program Reagent, glasswares and plastic wares, equipment, personnel and outcome/result  Reagents What is a reagent? Any substance employed to induce chemical reaction a substance that is used to test for the presence of another substance by causing a chemical reaction with it NOTE: Chemical reagents comes with varying grade of purity MSDS Essential in giving ACCURATE results Spectrograde, nanograde, HPLC grade, – highest purity ACS, USP-NF, NBS, OSRM, CAP, NCCLS,  Material Safety and Data Sheet A Material Safety Data Sheet (MSDS) is a document that contains information on the potential hazards (health, fire, reactivity and environmental) and how to work safely with the chemical product. https://d1yqpar94jqbqm.cloudfront.net/styles/media _middle/s3/images/SampleMSDS.JPG?itok=vpkdl0X d  Reagents Techniques on use and storage: Optimal storage condition Can be used directly or needed reconstitution Safety hazard MSDS  Types of Reagent Reagent grade (RG) or Analytical grade (AR) These chemicals met specifications designed to permit use in quantitative and qualitative analysis  Types of Reagent Chemical pure grade (CP) Purity is usually delivered by measurement of melting point or boiling point  Types of Reagent Standard - a. Primary Standard- highly purified chemicals which maybe weighed out directly for the preparation of solutions of selected concentration or for the standardization of solutions of unknown strength b. Secondary standard – solutions whose concentration cannot be determined directly from the weight of solute an volume of the solution  Types of Reagent Less pure grade a. Purified grade – in general these chemicals should not be used in clinical determination b. Technical grade – generally used in manufacturing USP and NF – Represents other grades of purity. While they are adequate for human consumption, they may not be pure enough for specific chemical determinations  Water TYPE I REAGENT WATER Use for procedure that use maximum water purity Preparation of standard solution; Ultramicrochemical analyses Measurement of nano or subnanogram concentration Tissue or cell culture methods, electrophoresis, toxicology, TYPE II REAGENT WATER Use for most of clinical laboratory determination., hematology, immunology, microbio TYPE III REAGENT WATER For most of the qualitative measurement Urinalysis, parasitology, histology, washing glassware.  Water A. DISTILLATION – distilled water is being redistilled with alkaline permanganate solution that oxidizes the nitrogenous matter present – Conductivity water B. DOUBLE DISTILLATION -Double-distilled water (abbreviated "ddH2O", "Bidest. water" or "DDW") is prepared by double distillation of water. It was the standard for highly purified laboratory water for biochemistry and trace analysis until combination methods of purification became widespread.  Deionization Also known as demineralized water (DI water, DIW or de-ionized water) Water that has had its mineral ions removed, such as cations from sodium, calcium, iron, copper and anions such as chloride and bromide. Electrodeionization  Water Other processes are also used to purify water, including reverse osmosis carbon filtration# microporous filtration Ultrafiltration ultraviolet oxidation electrodialysis. Processes rendering water potable but not necessarily closer to being pure H2O / hydroxide + hydronium ions include use of dilute sodium hypochlorite, mixed-oxidants (electro-catalyzed H2O + NaCl), and iodine  Measurement of mass Fundamental process in the preparation of standards, reagents, gravimetric analysis, or calibration of volumetric equipment, requiring analytical balances. Mass – is the measure of the quantity of matter a body contain In everyday usage, "mass" is often used interchangeably with weight Principle of mass: balance an unknown mass with a known mass.  Assignment 1. Proper care and maintenance of analytical balance 2. Sequence in weighing a sample using a single pan balance  Measurement of mass Calibration: Class S (weights 1-500mg) Adjustments and realignment  Types of Balance Top loading balances Single pan top balances – principle of weighing by substitution; weighs up to 10kg  Types of Balance Electronic balances highly sensitive; 130kg capacity; principle is based on a strict linear relationship between compensation current and force produced by the load placed on the pan  Measurement of volume Volume – is the measurement of the quantity of matter in a liquid state Clinical laboratory glasswares are used to measure volume  Measurement of volume Glasswares - is an amorphous (non-crystalline) solid material. Glasses are typically brittle and optically transparent 5 types a. High thermal resistant b. High silica glass c. High alkali resistant glass d. Standard flint glass e. Low actinic glass  GLASSWARES High thermal resistant / Borosilicate glasswares a type of glass with the main glass-forming constituents' silica and boron oxide. are known for having very low coefficients of thermal expansion (~3 × 10−6 /°C at 20°C), making them resistant to thermal shock. Low alkali content and free from magnesia-lime-zinc element – not used for strong alkali Such glass is less subject to thermal stress and is commonly used for the construction of reagent bottles. Kimax, pyrex (515),vycor (900) – washing and ignition technique  GLASSWARES High silica Glass – 96% Comparable to fused quarts in its thermal endurance, chemical stability, electrical characteristics Radiation resistant and good optical quality Used in precision analytical work and can also used for optical reflectors and mirrors Corex - cuvette  GLASSWARES High alkali resistant glass Not as resistant as pyrex to heat therefore need to heat and cool carefully Used to handle strong alkali solution  GLASSWARES Standard Flint glass high thermal with red color added as an integral part Used for light sensitive reagents  GLASSWARES Low actinic glass / soda Lime glass Composed of mixture of the oxides of silicon, calcium and sodium Poor resistance to high temperature Pipette, regular tubes and glasswares  MEASURING VESSEL Graduated cylinder Biuret/ Burette A long and straight sided Long cylindrical cylindrical piece of glassware graduated pipettes with calibration. with stopcock (glass or Used to measure where less Rubber) accuracy is needed Used for titration  MEASURING VESSEL Volumetric flasks Beaker Are frequently used for Wide straight sided preparation of standard cylindrical vessels that are solutions available in many sizes Measures liquid volume Used generally for mixing accurately and for reagent preparation  Measuring vessel Erlenmeyer Flask Test tubes Are often used for Test tubes comes in different preparing reagents sizes depending on their and titration purposes intended use Chemical reaction medium  Cleaning laboratory glasswares Rinse and immediately placed in a weak detergent Chromic acid with sodium or potassium dichromate, concentrated sulfuric acid and distilled water https://www.youtube.com/watch?v=X9HRNI9kX2Q  HOT AIR STERILIZER Used the principle of dry heat 160 degrees for 1-2 hours  PIPETTES Another type of volumetric glassware used extensively in the laboratory. Calibration are according to deliver or transfer a specific volume from one vessel to another Types of pipette According to manner of calibration According to graduation Specialized pipettes Micropipettes Unopette Capillary pipette Automatic pipettor  PIPETTES According to calibration: 1. To deliver (TD) – calibrated to deliver the amount of fluid designated on the pipette; this volume will flow out of the pipette by gravity. Calibration is usually performed by measuring the amount of water delivered by the pipette. 2. To contain (TC) – calibrated by introducing exact amount of volume or weight of mercury it contains exact amount however does not deliver the exact volume  PIPETTES According to calibration: 3. To blow out pipette – similar to TD except that the volume is obtained when the last drop is being blown out. An etched or frosted ring indicated this calibration 4. Calibrated between the marks – exact volume is calibrated to fill the volume between 2 calibrates points on the pipette  PIPETTES According to graduations: 1. Volumetric or transfer pipette – has a cylindrical bulb located midway the mouthpiece and the tip. a. Ostwald –Folin pipette similar to volumetric pipette but has a larger buld closer to delivery tip and it has an etched ring that indicates that it is a blow out - Used to measure viscous substance ex. Blood and serum  PIPETTES According to graduations: 2. Measuring or graduated pipette – plain narrow tube draw out to a tip and graduated uniformly along its length; calibrated to deliver fractional quantity, specifically reagents. Types a. Mohr b. Serologic Pipette  Pipettes Micropipettes Calibrated to contain or to wash out the pipettes 1 lambda = 1uL = 0.001mL Example of micropipettes a. Kirk transfer pipette – TC b. Self filling transfer pipette – TC c. Lang levy pipette - TD d. Overflow pipette - TC  Pipettes Unopette A special disposable micropipette used in the hematology laboratory It is self filling pipette accompanied by polyethylene reagent reservoir A capillary pipette is fitted in a plastic holder and fill automatically with blood by means of capillary action.  Pipettes Capillary pipette Inexpensive, disposable micropipette It is filled up to the calibrated line by capillary action and measured liquid is delivered by positive pressure as with a medicine dropper  Pipettes Automated pipettor Allows rapid, repetitive measurement and delivery of predetermined volumes of reagents or specimens 0.5-500 uL  Pipetting technique Check pipette before using – wet, chipped or broken Hold properly between thumb and forefinger Wipe the pipette with a soft tissue or lint free cloth Hold the pipette vertically Do not mouth pipette Read the meniscus Bottom of the meniscus Upper meniscus Eye level  Method of separating solids from liquid Centrifugation separates substances with different densities by centrifugal force Substance is separated into precipitate and supernatant Speed is usually given in revolutions per minute More satisfactory than filtration The faster the speed the longer the radius, the better quality of the filtrate Parts: Tachometer – calibrator Loader – balance sets of test tube placers Knobs – break, speed regulator, timer  Centrifugation Types of Centrifuge table top model, floor model, refrigerated centrifuge, ultracentrifuge, cytocentrifuge, serofuge. two traditional centrifuge used in the laboratory: Horizontal head centrifuge / swinging bucket Fixed angle head centrifuge ex. Microhematocrit centrifuge Centrifuge speed – rpm The number of revolutions per minute and the centrifugal force generated are expressed as 600rpm – 7300rcf  Centrifugation Factors that affect centrifugation: To balance the centrifuge Cover the specimen being processed Used proper centrifuge tubes Always checked for the rubber cushion Cover the centrifuge while rotating Do not try to stop the centrifuge with your bare hands Centrifuge should be checked, cleaned and lubricated regularly Method of separating solids from liquid Filtration Usually accomplished by gravity, pressure or suction Gravity filtration – filter paper folded into conical shape or 60 degree cone Funnel Porcelain Buchner funnel Porous Glass filters  Preparation of solution SOLUTE – refers to the substance being dissolved which may be a solid, liquid or gas SOLVENT – refers to the substance in which solute is being dissolved, which in most cases are liquid The concentration of solutions refers to the weight or volume of the solute present in a specific amount of the solvent or a solution. Percentage Molarity Normality  PERCENT COMPOSITION What percent of each element is present in a compound. 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 % 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 = × 100 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 𝑚𝑜𝑙𝑒 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 % 𝑚𝑜𝑙𝑒 𝑋 = × 100 𝑡𝑜𝑡𝑎𝑙 𝑚𝑜𝑙𝑒 𝑜𝑓 𝑡ℎ𝑒 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑  PERCENT COMPOSITION Steps in Solving: 1. Determine the chemical formula of the given compound. 2. Determine the atomic mass of each element. 3. Determine how many atoms are there for each element. Do your mathematics. 4. Get the molecular mass of the entire compound. 5. Substitute to the formula. Do your mathematics.  PERCENT COMPOSITION Example 1: Give the percent composition of sodium and bromine in sodium bromide. Sodium =𝑁𝑎+ Bromine=𝐵𝑟− Chemical Reaction: 𝑁𝑎+ + 𝐵𝑟− 𝑵𝒂𝑩𝒓 Step 1: 𝑁𝑎𝐵𝑟 Step 2/3: Na : 22.99 × 1 = 22.99 𝑔 Br : 79.904 × 1 = 79.904 𝑔 Step 4: 22.99 + 79.904 = 102.894 𝑔  PERCENT COMPOSITION Step 5: 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 % 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 = × 100 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 22.99 𝑔 % 𝑁𝑎 = × 100 102.894 𝑔 % 𝑵𝒂 = 𝟐𝟐. 𝟑𝟒𝟑 79.904 𝑔 % 𝑜𝑓 𝐵𝑟 = × 100 102.894 𝑔 % 𝑩𝒓 = 𝟕𝟕. 𝟔𝟓𝟕 Checking: % Na + %Br = 100 22.343 + 77.657 = 100  PERCENT COMPOSITION Example 2: Give the percent composition of Nitrogen in ammonium sulfate. Ammonium =𝑁𝐻4+ Sulfate = 𝑆𝑂42− Chemical Reaction: 𝑁𝐻+ + 𝑆𝑂2− (𝑵𝑯𝟒)𝟐𝑺𝑶𝟒 4 4 Step 1: (𝑁𝐻4)2𝑆𝑂4 Step 2/3: N : 14.007 × 2 = 28.014 𝑔 H : 1.008 × 8 = 8.064 𝑔 S : 32.06 × 1 = 32.06 𝑔 O : 15.999 × 4 = 63.996 𝑔 Step 4: 28.014 + 8.064 + 32.06 + 63.996 = 132.134 𝑔  PERCENT COMPOSITION Step 5: 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 % 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 = × 100 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 28.014 𝑔 % 𝑁= × 100 132.134 𝑔 % 𝑵 = 𝟐𝟏. 𝟐𝟎𝟏𝟐 % 𝑯 = 𝟔. 𝟏𝟎𝟐𝟗 % 𝑺 = 𝟐𝟒. 𝟐𝟔𝟑𝟐 % 𝑶 = 𝟒𝟖. 𝟒𝟑𝟐𝟕 21.2012 + 6.1029 + 24.2632 + 48.4327 = 100  PERCENT COMPOSITION Example 3: Give the percent composition of Copper, Oxygen and Hydrogen in copper (II) hydroxide. Copper =𝐶𝑢2+ Hydroxide =𝑂𝐻− Chemical Reaction: 𝐶𝑢2+ + 𝑂𝐻− 𝑪𝒖(𝑶𝑯)𝟐 Step 1: 𝐶𝑢(𝑂𝐻)2 Step 2/3: Cu : 63.55 × 1 = 63.55 𝑔 H : 1.008 × 2 = 2.016 𝑔 O : 15.999 × 2 = 31.998 𝑔 Step 4: 63.55 + 2.016 + 31.998 = 97.564 𝑔  PERCENT COMPOSITION Step 5: 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 % 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑋 = × 100 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 63.55 𝑔 % 𝐶𝑢 = × 100 97.564 𝑔 % 𝑪𝒖 = 𝟔𝟓. 𝟏𝟑𝟕 % 𝑯 = 𝟐. 𝟎𝟔𝟔 % 𝑶 = 𝟑𝟐. 𝟕𝟗𝟕 65.137 + 2.066 + 32.797 = 100  PERCENT CONCENTRATION Concentration is often expressed in terms of relative units. a. Mass percent (m/m or w/w) b. Volume percent (v/v) c. Mass/Volume percent (m/v)  PERCENT CONCENTRATION a. Mass/Mass or Weight/Weight 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 %= × 100 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 b. Volume/Volume 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 %= × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 c. mass/volume 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) %= × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝑙)  PERCENT CONCENTRATION Example 1: m/m Problem A saline solution with a mass of 355 g has 36.5 g of NaCl dissolved in it. What is the mass/mass percent concentration of the solution? Given Solution Solute = 36.5 g NaCl 𝑚 36.5 𝑔 𝑁𝑎𝐶𝑙 Solution = 355 g solution 𝑝𝑒𝑟𝑐𝑒𝑛𝑡 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 % 𝑚 = 355 𝑔 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 × 100 Unknown Answer %m/m = ? 10.2817 % Formula 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑝𝑒𝑟𝑐𝑒𝑛𝑡 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 ( % ) = × 100 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛  PERCENT CONCENTRATION Example 2 : m/m Problem If you are about to make 3000.0g of a 5.00% solution of sodium chloride. Given Solution Solution = 3000 g % m/m Solution = 5 % NaCl 5 𝑔 𝑁𝑎𝐶𝑙 𝑔 𝑁𝑎𝐶𝑙 𝑠𝑜𝑙𝑢𝑡𝑒 = 3000𝑔 𝑁𝑎𝐶𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 × 100 𝑔 𝑜𝑓 𝑁𝑎𝐶𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Unknown Solute = ? g NaCl Answer 150 g NaCl Assumption - mass percent 𝑚 can 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒as a co nversion factor in the form of: be expressed 𝑝𝑒𝑟𝑐𝑒𝑛𝑡 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 ( % ) = 𝑔 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 × 100 𝒈 𝒔𝒐𝒍𝒖𝒕𝒆 𝑚 100 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑜𝑟 𝟏𝟎𝟎 𝒈 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏 𝑔 𝑠𝑜𝑙𝑢𝑡𝑒 Thus, 5 𝑔 𝑁𝑎𝐶𝑙 𝒎𝒂𝒔𝒔 𝒔𝒐𝒍𝒖𝒕𝒆= 0.05 (5%), 5.00 % 100 𝑔 𝑁𝑎𝐶𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝟓% = × 𝟏𝟎𝟎 𝟑𝟎𝟎𝟎. 𝟎 Formula 𝑚 𝑔 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 g % 𝑚𝑎𝑠𝑠 𝑁𝑎𝐶𝑙 = 𝑔 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 × 𝑚 100 = 𝑔 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑚𝑎𝑠𝑠 𝑠𝑜𝑙𝑢𝑡𝑒 100  PERCENT CONCENTRATION 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 Example 3 : m/m Problem 𝑚 %= 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 × 100 What is the percent by mass solution when 10 grams of silver nitrate will be dissolved in 750 ml water? Given Solute = 10 g 𝐴𝑔𝑁𝑂3 Solvent = 750 ml water Solution 𝒈 Assumption: 𝟕𝟓𝟎 𝒎𝒍 𝒘𝒂𝒕𝒆𝒓 × 𝟏 = 𝟕𝟓𝟎 𝒈 𝒘𝒂𝒕𝒆𝒓 Density of water: without temp: at room 20 deg C 𝒎𝒍 : 1g/ml or 1000 kg/cu.m, even at 25 deg C To be exact : 997 kg/ cu.m 𝑚 10 𝑔 𝐴𝑔𝑁𝑂3 𝑝𝑒𝑟𝑐𝑒𝑛𝑡 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 % = × 100 𝑚 (10 𝑔 + 750 𝑔 )𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Unknown %m/m = ? Answer Formula 1.3158 % 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑝𝑒𝑟𝑐𝑒𝑛𝑡 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 ( % ) = × 100 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛  PERCENT COMPOSITION Example 3 : m/m Problem What is the percent-by-mass, %(m/m), concentration of sucrose in a solution made by dissolving 7.6 g of sucrose in 83.4 g of water? Given Solute = 7.6 g 𝑠𝑢𝑐𝑟𝑜𝑠𝑒 Solution Solution= 7.6 + 83.4 g 𝑚 7.6 𝑔 𝑠𝑢𝑐𝑟𝑜𝑠𝑒 𝑝𝑒𝑟𝑐𝑒𝑛𝑡 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 % = × 100 Unknown 𝑚 7.6 𝑔 + 83.4 %m/m = ? Formula Answer 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 8.352 % sucrose 𝑝𝑒𝑟𝑐𝑒𝑛𝑡 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 ( % )= × 100 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛  PERCENT CONCENTRATION Example 1: W/V Problem Physiologic or isotonic saline is a 0.9% aqueous solution of NaCl. 0.9% saline = 0.9 g of NaCl diluted to 100 mL of deionized water, where NaCl is the solute and deionized water is the solvent. What is the % w/v of a solution that has 7.5 g of sodium chloride diluted to 100 mL with deionized water? Solution Given mass solute= 7.5 g NaCl 𝑤 7.5 𝑔 𝑁𝑎𝐶𝑙 Volume solution= 100 ml solution % = × 100 𝑣 100 𝑚𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Unknown Answer % w/v = ? 7.5 % Formula 𝑤 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) % = × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝑙)  PERCENT CONCENTRATION Example 2 : W/V Problem Normal saline solution that is used to dissolve drugs for intravenous use is 0.92%(m/v) NaCl in water. How many grams of NaCl are required to prepare 35.0mL of normal saline solution? Given %m/v = 0.92 % Solution Volume solution= 35 ml solution 𝑚𝑎𝑠𝑠 𝑠𝑜𝑙𝑢𝑡𝑒 Unknown 0.92 % = × 100 Mass solute = ? 35 𝑚𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Answer Formula 0.322 g NaCl 𝑤 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) % = × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝑙)  PERCENT CONCENTRATION 𝑚 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) Example 3 : W/V Problem 𝑣 %= 𝑣𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝑙) × 100 What volume of solution would be needed to deliver 3.0 mg of a drug if the concentration of the drug in the solution was 3.5% (m/v)? 𝟏𝒈 Given 𝟑. 𝟎 𝒎𝒈 = 𝟎. 𝟎𝟎𝟑 𝒈 𝟏𝟎𝟎𝟎 𝒎𝒈 Solution %m/v = 3.5 % Mass of solute = 3.0 mg 0.003 3.5 % = × 100 𝑚𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Unknown Volume of the solution = ? Answer 0.0857ml solution Formula 𝑤 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) % = × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝑙)  PERCENT CONCENTRATION Volume in volume percent solution (V/V) – used when both solute and solvent are liquid. It refers to the amount of solute in mL in 100 mL of solvent 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 % = × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛  PERCENT CONCENTRATION Example 1: V/V Problem If 10% V/V HAc solution contains 10 mL of HAc per 100 mL of solution. Prepare 200ml of 5% acetic acid solution Given %v/v= 5 % acetic acid Solution volume solution= 200 ml solution 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 5% = × 100 Unknown 200 𝑚𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Vol solute = ? Answer 10 ml acetic acid Formula 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 % = × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛  PERCENT COMPOSITION Example 2 : V/V Problem Calculate the volume percent, %(v/v), of solute in the following solution: 20.0 mL of methyl alcohol in enough water to give 475 mL of solution. Given volume solute= 20 ml MetOH Solution volume solution= 475 ml solution 𝑣 20 𝑚𝑙 𝑠𝑜𝑙𝑢𝑡𝑒 % = × 100 Unknown 𝑣 475 𝑚𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 % v/v= ? Answer 4.211% Formula 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 % = × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛  PERCENT CONCENTRATION Example 3 : V/V Problem Rubbing alcohol is commonly used as an antiseptic for small cuts. It is sold as 70% (v/v) solution of isopropyl alcohol in water. What volume of isopropyl alcohol is used to make 500mL of rubbing alcohol? Solution Given % v/v= 70 % 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 volume solution= 500 ml solution 70 % = × 100 500 𝑚𝑙 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Unknown Answer Volume solute = ? 350 ml solute Formula 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 % = × 100 𝑣 𝑣𝑜𝑙𝑢𝑚𝑒 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 REVIEW CHEMICAL STOICHIOMETRY is the quantitative relationship among the amounts of reacting chemical species  STOICHIOMETRY Example 1: The Mole 𝑀𝑜𝑙𝑒𝑠 = 𝑀𝑎𝑠𝑠 𝐺𝑖𝑣𝑒𝑛 𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑀𝑎𝑠𝑠 How many moles are in 23 g of HCl? Step 1: Determine the chemical compound. HCl Step 2: Determine the molecular mass of the compound. Do your mathematics. H = 1.008 g Cl = 35.45 g HCl = 36.458 g/mol Step 3. Solve for the unknown. 1 𝑚𝑜𝑙 𝐻𝐶𝑙 𝑀𝑜𝑙𝑒𝑠 𝐻𝐶𝑙 = 23 𝑔 𝐻𝐶𝑙 × = 0.6309 𝑚𝑜𝑙𝑒𝑠 𝐻𝐶𝑙 36.458 𝑔 𝐻𝐶𝑙  STOICHIOMETRY 𝑀𝑜𝑙𝑒𝑠 = 𝑀𝑎𝑠𝑠 𝐺𝑖𝑣𝑒𝑛 𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑀𝑎𝑠𝑠 Example 2 : The Mole How many moles are in 120 g sucrose? Step 1: Determine the chemical compound. 𝐶12𝐻22𝑂11 Step 2: Determine the molecular mass of the compound. Do your mathematics. C = 12.01 × 12 = 144.12 H = 1.008 × 22 = 22.176 O = 15.999 × 11 = 175.989 𝐶12𝐻22𝑂11 = 342.285 g/mol Step 3. Solve for the unknown. 1 𝑚𝑜𝑙 𝐶12𝐻22𝑂11 𝑀𝑜𝑙𝑒𝑠 𝐻𝐶𝑙 = 120 𝑔 𝐶12𝐻22𝑂11 × = 0.3506 𝑚𝑜𝑙𝑒𝑠 𝐶12 𝐻22 𝑂11 342.285 𝑔 𝐶12𝐻22𝑂11  STOICHIOMETRY Example 3 : The Mole How many grams of sodium carbonate is in 0.43 mole ? Step 1: Determine the chemical compound. 𝑁𝑎2𝐶𝑂3 Step 2: Determine the molecular mass of the compound. Do your mathematics. Na = 22.99 × 2 = 45.98 𝑀𝑎𝑠𝑠 𝐺𝑖𝑣𝑒𝑛 𝑀𝑜𝑙𝑒𝑠 = C = 12.01 𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑀𝑎𝑠𝑠 O = 15.999 × 3 = 47.997 𝑁𝑎2𝐶𝑂3 = 105.987 g/mol 𝑀𝑜𝑙𝑒𝑠 × 𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑀𝑎𝑠𝑠 = 𝑀𝑎𝑠𝑠 𝐺𝑖𝑣𝑒𝑛 Step 3. Solve for the unknown. 𝑔 𝑁𝑎2𝐶𝑂3 0.43 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎2 𝐶𝑂3 × 105.987 = 45.5744 𝑔 𝑁𝑎2 𝐶𝑂3 𝑚𝑜𝑙𝑒 𝑁𝑎2𝐶𝑂3  STOICHIOMETRY Example 4 : The Mole How many grams of silver nitrate are in 2.21 moles of silver nitrate? Step 1: Determine the chemical compound. 𝐴𝑔𝑁𝑂3 Step 2: Determine the molecular mass of the compound. Do your mathematics. Ag = 107.868 g 𝑀𝑎𝑠𝑠 𝐺𝑖𝑣𝑒𝑛 N = 14.007 g 𝑀𝑜𝑙𝑒𝑠 = O = 15.999 × 3 = 47.997 𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑀𝑎𝑠𝑠 𝐴𝑔𝑁𝑂3 = 169.872 𝑔/𝑚𝑜𝑙 𝑀𝑜𝑙𝑒𝑠 × 𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑀𝑎𝑠𝑠 = 𝑀𝑎𝑠𝑠 𝐺𝑖𝑣𝑒𝑛 Step 3. Solve for the unknown. 𝑔 𝐴𝑔𝑁𝑂3 2.21 𝑚𝑜𝑙𝑒𝑠 𝐴𝑔𝑁𝑂 3 × 169.872 = 375.417 𝑔 𝐴𝑔𝑁𝑂 3 𝑚𝑜𝑙𝑒 𝐴𝑔𝑁𝑂3  STOICHIOMETRY Example 5 : The Avogadro’s Number (6.02 × 1023 𝑎𝑡𝑜𝑚𝑠, 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠, 𝑖𝑜𝑛𝑠, 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛𝑠, 𝑖𝑜𝑛 𝑝𝑎𝑖𝑟𝑠, 𝑠𝑢𝑏𝑎𝑡𝑜𝑚𝑖𝑐 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠) 𝑚𝑜𝑙𝑒 How many molecules are in 2.0 moles of a compound? 6.02 × 1023𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠 𝑋 = 2.0 𝑚𝑜𝑙𝑒𝑠 × 𝑚𝑜𝑙𝑒 𝑿 = 𝟏. 𝟐𝟎𝟒 × 𝟏𝟎𝟐𝟒𝐦𝐨𝐥𝐞𝐜𝐮𝐥𝐞𝐬 Example 6: How many moles are in 3.28 × 1024 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠? 1 𝑚𝑜𝑙𝑒 𝑋 = 3.28 × 1024 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠 × 6.02 × 1023𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠 𝑿 = 𝟓. 𝟒𝟒𝟖𝟓 𝒎𝒐𝒍𝒆𝒔  STOICHIOMETRY CHALLENGE! How many molecules are in 83 g of potassium permanganate ? STEP 1 : Determine the chemical compound. (𝑲𝑴𝒏𝑶𝟒) STEP 2 : Determine the Molecular Weight. Do your Mathematics. K = 39.098 Mn =54.938 O =15.999 × 4 = 63.996 𝐾𝑀𝑛𝑂4 = 158.032 𝑔/𝑚𝑜𝑙 STEP 3 : Determine the number of moles. 1 𝑚𝑜𝑙 𝐾𝑀𝑛𝑂4 𝑀𝑜𝑙𝑒𝑠 𝐾𝑀𝑛𝑂4 = 83 𝑔 𝐾𝑀𝑛𝑂4 × = 0.5252 𝑚𝑜𝑙𝑒𝑠 𝐾𝑀𝑛𝑂4 158.032 𝑔 𝐾𝑀𝑛𝑂4 STEP 4 : Moles to Molecules 6.02 × 1023𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠 𝑋 = 0.5252 𝑚𝑜𝑙𝑒 𝐾𝑀𝑛𝑂4 × 𝑚𝑜𝑙𝑒 𝟐𝟑 𝑿 = 𝟑. 𝟏𝟔𝟐 × 𝟏𝟎 𝐦𝐨𝐥𝐞𝐜𝐮𝐥𝐞𝐬  STOICHIOMETRY CHALLENGE! How many grams of sodium hydroxide is in 3.35 × 1024 𝑖𝑜𝑛𝑠? STEP 1 : Determine the chemical compound. (𝑵𝒂𝑶𝑯) STEP 2 : Determine the Molecular Weight. Do your Mathematics. Na = 22.99 O =15.999 H =1.008 𝑁𝑎𝑂𝐻 = 39.997 𝑔/𝑚𝑜𝑙 STEP 3 : Determine the number of moles. 1 𝑚𝑜𝑙𝑒 𝑁𝑎𝑂𝐻 𝑀𝑜𝑙𝑒𝑠 𝑁𝑎𝑂𝐻 = 3.35 × 1024𝑖𝑜𝑛𝑠 × = 5.5648 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎𝑂𝐻 6.02 × 1023 𝑖𝑜𝑛𝑠 STEP 4 : Moles to grams 39.997 𝑔 𝑁𝑎𝑂𝐻 𝑋 = 5.5648 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎𝑂𝐻 × 1 𝑚𝑜𝑙𝑒 𝑿 = 𝟐𝟐𝟐. 𝟓𝟕𝟒𝟕 𝐠 𝐍𝐚𝐎𝐇  Molarity A molar solution of a substance is defined as a solution containing one gram molecular weight ( one mole of the solute in one liter solution) of the substance per liter of the solution Molarity is equal to the number of moles of solute per liter of solution (solvent) The molecular weight of one compound is obtained by adding the atomic weights of the component elements in their proper proportions in the formula MOLARITY  MOLARITY 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 𝑙𝑖𝑡𝑒𝑟 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Example 1: Determine the molarity when 2.25 moles of KMnO4 are dissolved in enough water to give 450 mL of solution. 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 𝑙𝑖𝑡𝑒𝑟 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 2.25 𝑚𝑜𝑙𝑒𝑠 𝐾𝑀𝑛𝑂4 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 1𝐿 450 𝑚𝑙 × 1000 𝑚𝑙 𝑴𝒐𝒍𝒂𝒓𝒊𝒕𝒚 = 𝟓 𝑴  MOLARITY 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 𝑙𝑖𝑡𝑒𝑟 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Example 2: What is the molarity of the solution that contains 35.29 g of silver sulfate that has been dissolved to get 652 ml solution? STEP 1 : Determine the chemical compound. (𝐴𝑔2𝑆𝑂4) STEP 2: Determine the molecular weight. Do your mathematics. Ag = 107.868 × 2 = 215.736 𝑔 S = 32.06 g O = 15.999 × 4 = 63.996 𝑔 𝑔 𝐴𝑔2𝑆𝑂4 = 311.792 𝑚𝑜𝑙 STEP 3: Solve for the missing value. 1 𝑚𝑜𝑙 𝐴𝑔2𝑆𝑂4 𝑀𝑜𝑙𝑒𝑠 𝐴𝑔2𝑆𝑂4 = 35.29 𝑔 𝐴𝑔2𝑆𝑂4 × = 0.1132 𝑚𝑜𝑙𝑒𝑠 𝐴𝑔2 𝑆𝑂4 311.792 𝑔 𝐴𝑔2𝑆𝑂4 STEP 4: Solve for the unknown. 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 𝑙𝑖𝑡𝑒𝑟 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 0.1132 𝑚𝑜𝑙𝑒𝑠 𝐴𝑔2𝑆𝑂4 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 1𝐿 652 𝑚𝑙 × 1000 𝑚𝑙 𝑴𝒐𝒍𝒂𝒓𝒊𝒕𝒚 = 𝟎. 𝟏𝟕𝟑𝟔 𝑴  MOLARITY 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 𝑙𝑖𝑡𝑒𝑟 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Example 3: If 162.35 g aluminum hydroxide are dissolved in 6750 mL of solution, what is the concentration of the solution? STEP 1 : Determine the chemical compound. (𝐴𝑙(𝑂𝐻)3) STEP 2: Determine the molecular weight. Do your mathematics. O = 15.999 × 3 = 47.997 𝑔 Al = 26.982 g H = 1.008 × 3 = 3.024 𝑔 𝑔 𝐴𝑙(𝑂𝐻)3 = 78.003 𝑚𝑜𝑙 STEP 3: Solve for the missing value. 1 𝑚𝑜𝑙 𝐴𝑙(𝑂𝐻)3 𝑀𝑜𝑙𝑒𝑠 𝐴𝑙(𝑂𝐻)3 = 162.35 𝑔 𝐴𝑙(𝑂𝐻)3 × = 2.081 𝑚𝑜𝑙𝑒𝑠 𝐴𝑙(𝑂𝐻) 3 78.003 𝑔 𝐴𝑙(𝑂𝐻)3 STEP 4: Solve for the unknown. 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 𝑙𝑖𝑡𝑒𝑟 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 2.081 𝑚𝑜𝑙𝑒𝑠 𝐴𝑙(𝑂𝐻)3 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 = 1𝐿 6750 𝑚𝑙 × 1000 𝑚𝑙 𝑴𝒐𝒍𝒂𝒓𝒊𝒕𝒚 = 𝟎. 𝟑𝟎𝟖 𝑴  Mole solute MOLALITY Kg molality solvent Molality is the number of moles of solute per kilogram solvent. Since the density of water is about one kilogram per liter, molality is approximately equivalent to molarity for dilute aqueous solution at this temperature. It is only approximation and doesn’t apply when the solution is at different temperature, isn’t diluted or uses solvent other than water.  𝑁𝑜 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 𝑠𝑜𝑙𝑢𝑡𝑒 𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑀) = 𝐿 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑁𝑜 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 𝑠𝑜𝑙𝑢𝑡𝑒 𝑚𝑜𝑙𝑎𝑙𝑖𝑡𝑦 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑚) = 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 Where; 𝑤𝑒𝑖𝑔ℎ𝑡 𝑖𝑛 𝑔𝑟𝑎𝑚𝑠 𝑚𝑜𝑙𝑒𝑠 = 𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑤𝑒𝑖𝑔ℎ𝑡  𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑙𝑖𝑡𝑦 = 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 MOLALITY Example 1: What is the molality of a solution that contains 48 grams of sodium chloride and 250 mL of water? STEP 1 : Determine the chemical compound. (𝑁𝑎𝐶𝑙) STEP 2: Determine the molecular weight. Do your mathematics. Na = 22.99 g Cl = 35.45 g NaCl = 58.44 g/mol STEP 3: Solve for the missing value. 1 𝑚𝑜𝑙 𝑁𝑎𝐶𝑙 𝑀𝑜𝑙𝑒𝑠 𝑁𝑎𝐶𝑙 = 48 𝑔 𝑁𝑎𝐶𝑙 × = 0.8214 𝑚𝑜𝑙𝑒 𝑁𝑎𝐶𝑙 58.44 𝑔 1𝑔 𝑤𝑎𝑡𝑒𝑟 1𝑘𝑔 250 𝑚𝑙 𝑤𝑎𝑡𝑒𝑟 × = 250 𝑔 𝑤𝑎𝑡𝑒𝑟 × = 0.250 𝑘𝑔 𝑚𝑙 𝑤𝑎𝑡𝑒𝑟 1000𝑔 STEP 4: Solve for the unknown. 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑙𝑖𝑡𝑦 = 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 0.8214 𝑚𝑜𝑙𝑒𝑠 𝑀𝑜𝑙𝑎𝑙𝑖𝑡𝑦 = 0.250 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 𝑴𝒐𝒍𝒂𝒍𝒊𝒕𝒚 = 𝟑. 𝟐𝟖𝟓𝟔 𝒎  𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑙𝑖𝑡𝑦 = 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 MOLALITY Example 2: Calculate the molality of 22.22 grams of permanganate dissolved in 1L water. STEP 1 : Determine the chemical compound. (𝑀𝑛𝑂−4 ) STEP 2: Determine the molecular weight. Do your mathematics. Mn = 54.938 g O = 15.999 × 4 = 63.996 𝑔 𝑀𝑛𝑂4− = 118.934 g/mol STEP 3: Solve for the missing value. − − 1 𝑚𝑜𝑙 𝑀𝑛𝑂4− 𝑀𝑜𝑙𝑒𝑠 𝑀𝑛𝑂4 = 22.22 𝑔 𝑀𝑛𝑂4 × = 0.1868 𝑚𝑜𝑙𝑒 𝑀𝑛𝑂4− 118.934 𝑔 𝑀𝑛𝑂4− 1 𝑘𝑔 𝑤𝑎𝑡𝑒𝑟 1 𝐿 𝑤𝑎𝑡𝑒𝑟 × = 1 𝑘𝑔 𝐿 𝑤𝑎𝑡𝑒𝑟 STEP 4: Solve for the unknown. 𝑚𝑜𝑙𝑒 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑙𝑖𝑡𝑦 = 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 0.1868 𝑚𝑜𝑙𝑒𝑠 𝑀𝑛𝑂4− 𝑀𝑜𝑙𝑎𝑙𝑖𝑡𝑦 = 1 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 𝑴𝒐𝒍𝒂𝒍𝒊𝒕𝒚 = 𝟎. 𝟏𝟖𝟔𝟖 𝒎  NORMALITY Number of gram or mole equivalents of solute which are present in one liter of a solution. Similarly, normality is mainly used in three common situations: a. To determine the concentrations in acid- base chemistry. b. Used in precipitation reactions to measure the number of ions which are likely to precipitate in a given reaction. c. It is used in redox reactions to find the number of electrons which a reducing or an oxidizing agent can donate or accept.  NORMALITY 𝑵𝒖𝒎𝒃𝒆𝒓 𝒐𝒇 𝒆𝒒𝒖𝒊𝒗𝒂𝒍𝒆𝒏𝒕 𝒈𝒓𝒂𝒎(𝒈) 𝑵𝒐𝒓𝒎𝒂𝒍𝒊𝒕𝒚 𝑵 = 𝒗𝒐𝒍𝒖𝒎𝒆 𝒐𝒇 𝒕𝒉𝒆 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏 (𝑳) 𝑊𝑒𝑖𝑔ℎ𝑡 𝑜𝑓 𝑆𝑜𝑙𝑢𝑡𝑒 𝑁𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑔𝑟𝑎𝑚 𝑒𝑞𝑢𝑖𝑣𝑎𝑙𝑒𝑛𝑡𝑠 = 𝐸𝑞𝑢𝑖𝑣𝑎𝑙𝑒𝑛𝑡 𝑤𝑒𝑖𝑔ℎ𝑡 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑾𝒆𝒊𝒈𝒉𝒕 𝒐𝒇 𝑺𝒐𝒍𝒖𝒕𝒆 𝑵= 𝑬𝒒𝒖𝒊𝒗𝒂𝒍𝒆𝒏𝒕 𝒘𝒆𝒊𝒈𝒉𝒕 (𝑽𝒐𝒍𝒖𝒎𝒆 𝒊𝒏 𝑳) 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 × 𝑀𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑁= 𝐸𝑞𝑢𝑖𝑣𝑎𝑙𝑒𝑛𝑡 𝑚𝑎𝑠𝑠 𝑁 = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 × 𝐵𝑎𝑠𝑖𝑐𝑖𝑡𝑦 = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 × 𝐴𝑐𝑖𝑑𝑖𝑡𝑦  STEPS IN CALCULATING NORMALITY Find the information about the equivalent weight of the reacting substance or the solute. Find out the number of gram equivalent of solute by calculation. Calculate the volume in liters. Then calculate normality using the formula.  NORMALITY Example 2: Calculate the normality of NaOH solution formed by dissolving 0.2 g NaOH to make 250 ml solution. STEP 1: Get the molarity. 0.2 𝒈 𝑵𝒂𝑶𝑯 × 1 𝑚𝑜𝑙𝑒 𝑁𝑎𝑂𝐻 39.996 𝒈 𝑵𝒂𝑶𝑯 = 0.0200 𝑀 250 𝑚𝑙 × 1 𝐿 1000 𝑚𝑙 STEP 2: Multiply to the number of atoms of “H”. 𝟎. 𝟎𝟐𝟎𝟎 𝑴 × 𝟏 = 𝟎. 𝟎𝟐𝟎𝟎 𝑵.  NORMALITY Example 3: Calculate the normality of 1.4 𝑀 𝐻2𝑆𝑂4. STEP 1: Multiply to the number of atoms of “H”. 𝟏. 𝟒 𝑴 × 𝟐 = 𝟐. 𝟖 𝑵. Solutions Standard Solution that contains a known exact amount of the substance being measured Prepared from a high quality reference material w/ measured, known amount of fixed and known chemical composition Working standard Is prepared from stock standard solution and most often employed in the actual determination Blank solutions Contain the reagent but not the sample or standard to check on the accuracy of the reagent Thank you!!! INORGANIC CHEMISTRY ERRORS IN SCIENTIFIC MEASUREMENTS Our Lady of Fatima University ACCURACY AND PRECISION ACCURACY AND PRECISION Precision - Refers to reproducibility or how close the measurements are to each other. Accuracy - Refers to how close a measurement is to the real value. precise and accurate precise but not accurate ACCURACY AND PRECISION random error systematic error Systematic Error - Random Error - Values that are either all In the absence of systematic error, higher or all lower than the some values that are higher and actual value. some that are lower than the actual value. Rules for Determining Which Digits are Significant All digits are significant except zeros that are used only to position the decimal point. Make sure that the measured quantity has a decimal point. Start at the left of the number and move right until you reach the first nonzero digit. Count that digit and every digit to it’s right as significant. Zeros that end a number and lie either after or before the decimal point are significant; thus 1.030 ml has four significant figures, and 5300. L has four significant figures also. Numbers such as 5300 L are assumed to only have 2 significant figures. A terminal decimal point is often used to clarify the situation, but scientific notation is the best!  Significant Digits Determine the number of significant figures in each quantity. a. 0.0030 – 2 sf b. 0.1044 – 4 sf c. 53,069 – 5 sf d. 54,280,000. – 8 sf - 5.4280000× 107 e. 0.00120 – 3 sf - 1.20 × 10−3 f. 0.00004715 – 4 sf - 4.715 × 10−5 g. 57,600. – 5 sf - 5.7600 × 104 h. 0.0000007160 – 4 sf - 7.160 × 10−7  Addition and Subtraction of Significant Digits For addition and subtraction. The answer has the same number of decimal places as there are in the measurement with the fewest decimal places. Example 1: 83.5 + 23. 28 + 101.12 = Example 2 : 1078.21 + 31.122+ 101.1 + 21.2 + 59.897 =1291.529 = Example 3: 1.1+ 2.22 + 3.333 + 4.4444 + 5.55555 = 16.65295 = Example 4 : 1.23 + 2.345 + 3.4567 +4.56789 + 5.678912 = 17.278502 = Example5 : 865.9 – 2.8121 = 863.0879 = Example 6 : 1234.56 -7.8901 = 1226.6699 =  Multiplication and Division of Significant Digits For multiplication and division. The number with the least certainty limits the certainty of the result. Therefore, the answer contains the same number of significant figures as there are in the measurement with the fewest significant figures. Example 1: 9.2 × 6.8 × 0.3744 = 23.422464 = 23 Example 2 : 0.223 × 2.112 × 347.44 = 163.6359014 = 164 Example 3 : 987.21 = 30.65869565 = 30.7 32.2  Rounding Off Rulings If the digit removed is more than 5, the preceding number increases by 1. 5.379 rounds to 5.38 if three significant figures are retained and to 5.4 if two significant figures are retained. If the digit removed is less than 5, the preceding number is unchanged. 0.2413 rounds to 0.241 if three significant figures are retained and to 0.24 if two significant figures are retained. If the digit removed is 5, the preceding number increases by 1 if it is odd and remains unchanged if it is even. 17.75 rounds to 17.8, but 17.65 rounds to 17.6. (a) If the 5 is followed only by zeros, rule 3 is followed; if the 5 is followed by nonzeros, rule 1 is followed: 17.6500 rounds to 17.6, but 17.6513 rounds to 17.7 Be sure to carry two or more additional significant figures through a multistep calculation and round off only the final answer. GENERAL CHEMISTRY MATTER A N D ITS PROPERTIES Our Lady of Fatima University  DISCUSSION OVERVIEW Preliminary Objectives Assessment Introduction Discussion Summary Assessment Home Work  OBJECTIVES After the course of discussion, students are expected to: Visualize the particulate structure of matter; Recognize that substances are made up of smaller particles Be reoriented on the phases of matter alongside with its respected innate characteristics and relate with other theoretical concepts previously discussed and those to be discussed in the succeeding lessons; Be cognizant of the physical and chemical properties of matter and distinguish the intensive and extensive properties of matter; Classify the forms of matter based on it’s physical and chemical properties; Perform laboratory experiments or case analysis on the topic under discussion and Immersed in the research and scientific discussions in relation to the fundamentals of matter. INTRODUCTION The Matter and Its Properties  CHEMISTRY Study of MATTER and its COMPOSITION, PROPERTIES and TRANSFORMATIONS including the energy changes that accompanies along with it. Matter is anything that occupies space and that has a mass  PROPERTIES MASS VOLUME WEIGHT A measure of how The amount of space A measure of the much matter is in an that matter force of gravity on an object. occupies. object.  PROPERTIES FREEZING BOILING MELTING POINT POINT POINT Temperature at Basically the range The temperature at which the liquid form at which the solid which a liquid of an element or changes its state changes into a solid. compound is at into a liquid. equilibrium with the gaseous form.  PROPERTIES DENSITY COMPOUND A substance made The measurement of of two or more how much mass of a elements chemically substance is combined in a set contained in a given ratio. volume..  Properties of Matter Physical Properties are the properties that are observed without changing the composition of a substance though their form might change. PHYSICAL PROCESS Properties of Matter Chemical Properties are the properties observed when a matter is involved in a chemical change. This property revolves around the composition of material. Properties of Matter  PHYSICAL CHANGE A change that affects one or more physical properties of a substance. Do Not form new substances. Can often be Undone  CHEMICAL CHANGES A change that occurs when one or more substances are changed into entirely new substances with different properties. Can Not change back under normal conditions (some can be changed back by other chemical means)  5 SIGNS CHEMICAL CHANGES Odor Production Change in Temperature a. Exothermic-energy is released during the chemical change b.Endothermic- energy is absorbed causing a decrease in temperature Change in Color Formation of Bubbles Formation of a Precipitate  PRACTICE (a) Frost forms as the temperature drops on a humid winter night. (b) A cornstalk grows from a seed that is watered and fertilized. (c) Dynamite explodes to form a mixture of gases. (d)Perspiration evaporates when you relax after jogging (e)A silver fork tarnishes slowly in air.  ENERGY Capacity to do work Potential Energy - energy due to the position of the object or energy from a chemical reaction Kinetic Energy - energy due to the motion of the object SCIENTIFIC APPROACH TO CHEMISTRY SCIENTIFIC APPROACH TO CHEMISTRY Natural phenomena and measured events; universally Observations : consistent ones can be stated as a natural law. Hypothesis: Tentative proposal that explains observations. revised if experiments do not support it Experiment: Procedure to test hypothesis; measures one variable at a time. Model (Theory): Set of conceptual assumptions that explains data from altered if accumulated experiments; predicts related phenomena. predictions do not support it Further Experiment: Tests predictions based on model.  Properties of Matter Intensive Properties are the properties which is independent on the amount or size of the material. Extensive Properties are the properties which are dependent on the amount of material. https://www.thoughtco.com/intensive-vs-extensive- properties-604133  Properties of Matter Characteristics of a substance regardless of its shape and size are called intrinsic properties. Characteristics of a substance which pertains only to it’s appearance including shape, length, mass and temperature are called extrinsic properties. https://sciencenotes.org/intrinsic-and-extrinsic-properties- of-matter/  GENERAL CHEMISTRY 1 Classification of Matter  Physical States https://quizizz.com/admin/quiz/613795c897e458001db9c728/the-states-of-matter Physical States  TEMPERATURE AND PRESSURE Depending on the temperature and pressure of the surroundings, many substance can exist in each of the three physical states and undergo changes. https://stock.adobe.com/ee/search/images?k=states%20of%20 matter  Physical States Plasma – have no fixed shape or volume, and are less dense than solids or liquids. But unlike ordinary gases, plasmas are made up of atoms in which some or all of the electrons have been stripped away and positively charged nuclei, called ions, roam freely. Bose Einstein Condensate - group of atoms cooled to within a hair of absolute zero. Atoms are hardly moving relative to each other; they have almost no free energy to do so. Fermionic Condensate - a superfluid phase formed by fermionic particles at low temperatures. Quark-Gluon Plasma - a state of matter in which the elementary particles that make up the hadrons of baryonic matter are freed of their strong attraction for one another under extremely high energy densities.  Composition https://www.slideshare.net/ewalenta/ch-2-classification-of-matter-ppt  PURE SUBSTANCE Consists of one type of atom, molecule or fixed set of atoms or ions Element consists only of one type of atom. Compound is the chemical combination of two or more different atoms in fixed proportions. https://www.enaco.com.pe/es/sugerencias-y- consultas?ss=5_5_5_21_41&pp=what+is+a+molecule&ii=2159815  IMPURE SUBSTANCE Consists of physically combined elements and/or compounds Homogenous Mixture has a uniform appearance. Heterogenous Mixture phase boundaries are visible. https://www.thoughtco.com/heterogeneous-and- homogeneous-mixtures-606106  Physical Properties A property of matter that can be observed or measured without changing the identity of the matter. Density Malleability Ductility Solubility State Thermal Conductivity  DENSITY Amount of mass in a given volume The density of one substance is usually different from that of another substance.  DENSITY A bar of copper has a mass of 216 g and a volume of 24 𝑐𝑚3. Calculate the density. Given: Mass = 216 g Volume = 24 𝑐𝑚3 Unknown: 𝜌=? Formula: 𝑀 𝜌 = 𝑉 Solution: 216 𝑔 𝜌 = 24 𝑐𝑚 3 Answer: 𝒈 𝝆 =𝟗 𝒄𝒎𝟑  DENSITY The volume of a candy bar is 55 𝑐𝑚3. The mass of the candy bar is 70 g. What s the density of the candy bar? Given: Mass = 70 g Volume = 55 𝑐𝑚3 Unknown: 𝜌=? Formula: 𝑀 𝜌 = 𝑉 Solution: 70 𝑔 𝜌 = 55 𝑐𝑚 3 Answer: 𝒈 𝝆 = 𝟏. 𝟐𝟕𝟐𝟕𝟑 𝒄𝒎𝟑  DENSITY An ice cube has a volume of 36 𝑐𝑚3. If the ice cube has a mass of 33.2 g, what is the density of the ice cube? Given: Mass = 33.2 g Volume = 36 𝑐𝑚3 Unknown: 𝜌=? Formula: 𝑀 𝜌 = 𝑉 Solution: 33.2 𝑔 𝜌 = 36 𝑐𝑚 3 Answer: 𝒈 𝝆 = 𝟎. 𝟗𝟐𝟐𝟐 𝒄𝒎𝟑  DENSITY At 4⁰C, pure water has a density of 1g/mL (1 g/𝑐𝑚3). Suppose that you have 2 liters of pure water at this temperature. What is the mass of this water? Given: Volume = 2 L 𝜌= 1g/ml Unknown: Mass = ? Formula: 𝑀 = 𝜌×𝑉 Solution: 1𝑔 1000𝑚𝑙 𝑀= ×2𝐿 𝑚𝑙 1𝐿 Answer: 𝝆 = 𝟐𝟎𝟎𝟎𝒈  DENSITY ASSIGNMENT 1. What is the mass of ethyl alcohol that exactly fills a 200.0 mL graduated cylinder. The density of ethyl alcohol is 0.789 g/mL. 2. What is the volume of a silver metal that has a mass of 2500.0 g. The density of silver is 10.5 g/𝑐𝑚3.  MALLEABILITY DUCTILITY The ability to be pounded The ability to be drawn or into thin sheets. pulled into a wire  THERMAL SOLUBILITY CONDUCTIVITY The ability to dissolve in The ability to transfer thermal another substance. energy from one area to another. Heat or make warmer, Grind or smash & Stir or mix  CHEMICAL PROPERTIES A property of matter that describes a substance based on its ability to change into a new substance with different properties. Combustibility Flammability Reactivity a. Acids b. Bases c. Oxidation  GENERAL CHEMISTRY 1 Generalization and Summary of Discussion  SUMMARY 1. 2. 3. Chemistry as a branch of Matter can be classified In comparison mixtures science deals with the into 2 by means of its can be separated using study of matter alongside physical state and physical means which it’s properties, composition. Composition compound needs to composition and deals with solution and undergo chemical transformations that chemical composition of interference and reaction accompanies the the matter while physical to be separated. reactions taking over it. state are subdivided into the physical attibutes of the matter.  GENERAL CHEMISTRY 1 QUIZ 1  QUIZ 1 1. What is a matter? a. Building block of all organism b. Anything that can be viewed by naked eye c. Molecules that makes up everything d. None of the above 2. Which of the following is a list of compound? a. H2O, CO2, and b. Au, Ag and brass c. Brick, sand and concrete d. H, NO2 and O2 3. The temperature at which a substance changes from a liquid to a gas a. Freezing point b. Melting point c. Boiling point d. Condensation point  QUIZ 1 4. The amount of space something takes up a. Density b. Volume c. Mass d. Pound Force 5. All matters contains particles which are called… a. Units b. Cell c. Atoms d. Molecules 6. Tearing a piece of paper into 100 pieces is an example of… a. Physical change b. Chemical Change c. Size Reduction d. Particle Technology  QUIZ 1 7. Burning a piece of paper is a classic example of… a. Physical Change b. Chemical Change c. Incineration d. Combustion 8. A reaction occurs, and the product is different from what you started with is an example of… a. Physical Change b. Chemical Change c. Chemical Kinetics d. Chemical Reaction 9. Steel hardness is an example of… a. Intensive Property b. Extensive Property c. Tensile Strength d. Material Science  QUIZ 1 10. Which of the following is an example of homogenous mixture? a. Stainless steel b. Aluminum pan c. Hydrogen gas d. Gold Necklace Bonus It is a unit operation typically use to separate a mixture containing volatile components. It involves evaporation followed by condensation. DISTILLATION  REFERENCES General Chemistry - Department of Education. (n.d.). Retrieved July 17, 2022, from https://www.deped.gov.ph/wp-content/uploads/2019/01/General-Chemistry-1-and- 2.pdf Emspak, J. (2016, May 5). States of matter: Plasma. LiveScience. Retrieved July 17, 2022, from https://www.livescience.com/54652-plasma.html Emspak, J. (2018, August 3). States of matter: Bose-Einstein condensate. LiveScience. Retrieved July 17, 2022, from https://www.livescience.com/54667-bose-einstein- condensate.html#:~:text=A%20Bose%2DEinstein%20condensate%20is,enter%20the %20same%20energy%20states. EngineerPH EducatorPH Follow. (n.d.). DepEd SHS STEM general chemistry modules quarters 1-2 by CDO. SlideShare a Scribd company. Retrieved July 17, 2022, from https://www.slideshare.net/walanoone/deped-shs-stem-general-chemistry- modules-quarters-12-by-tapayan What is fermionic condensate and how it is formed? - byju's. (n.d.). Retrieved July 17, 2022, from https://byjus.com/question-answer/what-is-fermionic-condensate-and-how- it-is-formed/ Why is dissolving salt in water a chemical change and sugar in water a physical change? Quora. (n.d.). Retrieved July 17, 2022, from https://www.quora.com/Why-is- dissolving-salt-in-water-a-chemical-change-and-sugar-in-water-a-physical- change THANKS Do you have any questions? [email protected] 0956-355-2613 Batangas State University The National Engineering University CREDITS: This presentation template was created by Slidesgo, including icons by Flaticon, and infographics & images by Freepik