Essential Maths for Medics and Vets Reference Materials Module 2. Amount and Concentration.


 Shona McCoy
 2 years ago
 Views:
Transcription
1 2 Amount and concentration: making and diluting solutions 2 Amount and concentration; making and diluting solutions... 2A Rationale... 2B Distinguishing between amount and concentration, g and %w/v... 2C Distinguishing between amount and concentration, moles and molar...2 2D Practice converting g/l to M and vice versa...3 2E Diluting Solutions...5 2F Practice calculating dilutions...6 Summary of learning objectives...7 2A Rationale Biological and biochemical investigations rely completely upon being able to detect the concentration of a variety of substances. For example, in diabetics it is important to know the concentration of glucose in the blood and you may also need to be able to calculate how much insulin would need to be dissolved in a certain of saline so as to give the right amount in a ml injection. It is also vitally important that you perform these calculations quickly, reliably and accurately. This section aims to help you understand how to go about doing these calculations and to give you plenty of practice so that you can do them quickly and reliably. 2B Distinguishing between amount and concentration, g and %w/v The amount of a substance is often measured by how much it weighs i.e. in g or mg or kg etc. The concentration is the amount divided by the it is dissolved in. amount concentration= For example you might dissolve 0.9g of sodium chloride in 00mL of water. Sometimes this is referred to as 0.9% w/v since it is 0.9g weight divided by 00mL and w/v stands for weight per. The concentration of this solution could be described as g/ml or 9 mg/ml. Alternatively you could notice that if 0.9g is dissolved in 00mL, then 9g would be dissolved in 000ml (=L) and the concentration could also be written as 9g/L Page of 7
2 2C Distinguishing between amount and concentration, moles and molar Another way of representing the amount of a substance is to use the concept of mole. A mole is simply x 0 23 molecules (this is Avogadro s number ) Eggs come in dozens (2), molecules come in moles (6 x 0 23 ) The mass of a mole of molecules is the formula weight in grams. This is sometimes called molar mass with symbol M. Sometimes it is referred to as molecular weight. Sometimes it is called relative molecular mass since the mass of a carbon element is designated to be 2 and other molecules or elements are given masses relative to that. The molar mass of a small molecule such as an amino acid (eg glycine is NH 2 CH 2 COOH and has molecular mass = g.mol  ) is much less than the molar mass of a protein (eg haemoglobin has molecular mass ~ g.mol  ) x 0 23 glycine molecules (or mole) would weigh g whereas x 0 23 haemoglobin molecules (or mole) would weigh ~64500g (or 64.5kg) The important thing to remember for calculations is that the molecular weight/molecular mass/molar mass call it what you will has the units of g.mol  To convert between an amount in g and an amount in moles, Amount (in g) = Amount (in mol) x Molar Mass (g.mol  ) Sometimes the term Dalton is used for molecular mass. For example the molecular mass of glycine is 75 Da while the molecular mass of haemoglobin is 64.5kDa (or Da). The concentration of a solution of mole dissolved in L is M ( one molar ) M = mole litre Don t confuse this symbol M for mol/l with M for molar mass. It s unfortunate they have been used for two quite different things. In the case of glucose, a M solution would have mole = 80 g dissolved in L. So another way of saying that is M glucose solution = 80 g/000 ml = 0.8 g/ml Alternatively you could call it 8 % (w/v). You need to be able to convert easily and accurately between different ways of expressing concentration. Page 2 of 7
3 2D Practice converting g/l to M and vice versa Example : Converting g/l to M You have weighed out 20 g KCl (formula weight of KCl is g.mol  ) and dissolved it in 500 ml, what is the concentration in M? Work out how many moles are equivalent to 20 g. Rearranging: Amount (in g) = Amount (in mol) x Molar Mass (g.mol  ) Amount (in moles) = amount (in g) molar mass (in g.mol  ) 20g gmol. = = mol Now work out the concentration by dividing the amount (in mol) by the (in L) Concentration (M) = amount (in mol) (in L) = mol 0.5L = M Example 2. Converting M to g/l You have a M solution of NaCl, what is the concentration in % (w/v)? M = mol / L mol of NaCl = g.mol  Concentration (M) = mol L = 58.44g L = 5.844g 00 ml = 5.8% (w/v) Page 3 of 7
4 Example 3. You are given 580 mg of adrenaline and need to make a mm solution. What of water do you need to dissolve it in? The molar mass of adrenaline is 83.2 g.mol  First you need to convert 580 mg to moles: Amount (in moles) = amount (in g) molar mass (in g.mol  ) 0.58g = mol 83.2 gmol. = Then work out the by rearranging the equation: Concentration (M) = amount (in mol) (in L) becomes: Volume (in L) = amount (in mol) concentration (in M) Volume (in L) = mol 0.00 mol.l  = 3.66 L Example 4. You have a mm solution of adrenaline and wish to dispense a which contains 0 mg. What do you need to dispense? First convert 0mg to moles: Amount (in moles) = amount (in g) molar mass (in g.mol  ) 0.0g 83.2 gmol. = 5.46 x 05 mol = Page 4 of 7
5 = = = amount concentration 5.46 x 05 mol x 03 mol.l x 02 L = L = 54.6 ml Example 5. You want to make 0 ml of a 5 mm solution of adrenaline, how much should you weigh out? Amount = x concentration = 0.0 L x 5 x 03 mol.l  = 5 x 05 mol = 5 x 05 mol x 83.2 g.mol  = 96 x 05 g = 9.6 mg 2E Diluting Solutions Simple Dilutions Make a :0 dilution (say this as a one in ten dilution ). Take part of your stock solution and add 9 parts of solvent (usually water but sometimes alcohol or other organic solvent). If your original sodium chloride solution is M, and you dilute it :0, then you might take 0ml of M NaCl and 90ml water, ( = 00) or you could take ml of M NaCl and 9ml water, ( + 9 = 0) or 0.2 ml M NaCl and.8ml water ( = 2) In all cases you are diluting by the same factor. The concentration of the resulting solution is M /0 = 0.M where 0 is the dilution factor. [Although it is really quite obvious, you can convince yourself that the resulting concentration is 0.M by the following: Take 0 ml of M NaCl, how much NaCl is there in that? Answer: amount concentration= amount = concentration Amount in 0ml = 0ml x mol.l  x 0.00 L.mL  = 0.0mol So imagine that you are taking 0ml which has 0.0mol salt in it, and you put it into a total of 00ml. Page 5 of 7
6 amount 0.0mol concentration = 0.M = 0.00L = ] For example, a :5 dilution = unit of diluent + 4 unit s of solvent; dilution factor = 5 :2 dilution = unit of diluent + unit of solvent; dilution factor = 2 :7.4 dilution = unit of diluent unit s of : dilution factor = 7.4 Serial Dilutions Serial dilutions are a quick and convenient way to prepare a wide range of concentrations. Typically, they are done in powers of 0 or 00 (but not always). So for example: Take a mm stock solution of adrenaline, dilute it :0 (0.ml + 0.9ml) to give a 0.mM solution dilute this :0 to give a 0.0mM solution dilute this :0 to give a 0.00mM solution dilute this :0 to give a 0.000mM solution and so on This approach allows you to prepare very dilute solutions from a concentrated stock much more accurately than the alternative. 2F Practice calculating dilutions The most common task you will be asked to do is to prepare a particular concentration from a stock solution. So say you are asked to prepare 0.32M sucrose from a M sucrose stock. There are two ways of approaching this and these are illustrated below. Think about them both and then choose whichever makes the most sense for you. Method : Step : work out what the dilution factor is.. /0.32 = 3.25 Step 2: turn this into of diluent and solvent.. part of M sucrose plus 2.25 parts water gives 3.25 parts of 0.32M sucrose Page 6 of 7
7 you could write this as ml x M sucrose ml water 3.25ml x 0.32M sucrose or you could scale it up to whatever you want, say 32ml x M sucrose + 68ml water 00 ml x 0.32M sucrose Method 2: The alternative method is this: Start by noticing that amount = concentration x or A = C.V Now if you take a V of your concentrated solution (concentration = C) Then the amount you have in your pipette is A. Now if you put that amount into a new V2, the amount is still constant, but now because you have a bigger, the concentration C2 = A/V2. But from before, A = C.V, so C.V = C2.V2 What this is saying is that if the amount is the same in both solutions, then their concentrations and s must be related. You can use this relationship to calculate the required V2 to get a particular concentration. Taking our earlier example, C = M, V = ml, C2 (the desired concentration) = 0.32M what is the resulting? M x ml = 0.32M x V2. V2 = 0.32 ml V2 = 3.25ml What about if you were asked to make 00ml of 0.32M sucrose? Now you have C=M, C2 = 0.32M, V2 = 00ml and V is the unknown. M x V = 0.32M x 00ml V = 32ml Summary of learning objectives At the end of this section you should be able to: a. To understand the difference between amount and concentration b. To be able to calculate the concentration of a solution in a variety of formats including M, g/l, %v/v, %w/v c. To be able to quickly and reliably convert from one unit to another d. To be able to quickly and reliably calculate the appropriate way to prepare a dilution Page 7 of 7
Calculations involving concentrations, stoichiometry
Calculations involving concentrations, stoichiometry MUDr. Jan Pláteník, PhD Mole Unit of amount of substance the amount of substance containing as many particles (atoms, ions, molecules, etc.) as present
More informationElement of same atomic number, but different atomic mass o Example: Hydrogen
Atomic mass: p + = protons; e  = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass
More informationMolarity is used to convert between moles of substance and liters of solution.
Appendix C Molarity C.1 MOLARITY AND THE MOLE The molar mass is the mass of a mole of a pure substance while the molarity, M, is the number of moles of a pure substance contained in a liter of a solution.
More informationCalculation of Molar Masses. Molar Mass. Solutions. Solutions
Molar Mass Molar mass = Mass in grams of one mole of any element, numerically equal to its atomic weight Molar mass of molecules can be determined from the chemical formula and molar masses of elements
More informationChapter 3. Stoichiometry of Formulas and Equations
Chapter 3 Stoichiometry of Formulas and Equations Chapter 3 Outline: Mole  Mass Relationships in Chemical Systems 3.1 The Mole 3.2 Determining the Formula of an Unknown Compound 3.3 Writing and Balancing
More informationLab Math Solutions, Dilutions, Concentrations and Molarity
Lab Math Solutions, Dilutions, Concentrations and Molarity Stanimila Nikolova, PhD Molecular Quality Improvement Program NBS Molecular Training Class April 25, 2016 National Center for Environmental Health
More informationSample Exercise 13.1 Predicting Solubility Patterns
Sample Exercise 13.1 Predicting Solubility Patterns Predict whether each of the following substances is more likely to dissolve in the nonpolar solvent carbon tetrachloride (CCl 4 ) or in water: C 7 H
More informationUnit 2: Quantities in Chemistry
Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C12 and C13. Of Carbon s two isotopes, there is 98.9% C12 and 11.1% C13. Find
More informationFormulas, Equations and Moles
Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule
More informationThe Mole Concept. A. Atomic Masses and Avogadro s Hypothesis
The Mole Concept A. Atomic Masses and Avogadro s Hypothesis 1. We have learned that compounds are made up of two or more different elements and that elements are composed of atoms. Therefore, compounds
More informationChapter 4. Chemical Composition. Chapter 4 Topics H 2 S. 4.1 Mole Quantities. The Mole Scale. Molar Mass The Mass of 1 Mole
Chapter 4 Chemical Composition Chapter 4 Topics 1. Mole Quantities 2. Moles, Masses, and Particles 3. Determining Empirical Formulas 4. Chemical Composition of Solutions Copyright The McGrawHill Companies,
More information2 Stoichiometry: Chemical Arithmetic Formula Conventions (1 of 24) 2 Stoichiometry: Chemical Arithmetic Stoichiometry Terms (2 of 24)
Formula Conventions (1 of 24) Superscripts used to show the charges on ions Mg 2+ the 2 means a 2+ charge (lost 2 electrons) Subscripts used to show numbers of atoms in a formula unit H 2 SO 4 two H s,
More informationChemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.
1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.
More informationLaboratory Math II: Solutions and Dilutions
Slide 1 Laboratory Math II: Solutions and Dilutions Philip Ryan, PhD PostDoctoral Fellow National Cancer Institute, NIH Welcome to the National Institutes of Health, Office of Intramural Training & Education
More informationMolarity and Serial Dilutions Student Handout
Molarity and Serial Dilutions Student Handout Background information: Atomic and Molecular Weight Everything in the world is made up of atoms. Think of atoms as the building blocks for larger structures.
More informationSolutions: Molarity. A. Introduction
Solutions: Molarity. A. Introduction... 1 B. Molarity... 1 C. Making molar solutions... 2 D. Using molar solutions... 4 E. Other molebased concentration units [optional]... 6 F. Answers... 7 A. Introduction
More informationChemical Calculations: Formula Masses, Moles, and Chemical Equations
Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic
More informationThe core material is Sect BD. The rest is optional; do individual sections as suits your interests or needs.
Solutions: Percentage. A. Introduction... 1 B. Comparisons; ratios; the idea of percentage... 1 C. The units of percent... 3 D. Weight percentage, %(w/w)... 5 E. Volume percentage, %(v/v)... 6 F. Weight/volume
More informationMolarity. Why? Learning Objectives. Success Criteria. Prerequisites. Vocabulary
Why? Molarity When a substance (solute) is dissolved in a solvent, a solution is formed. A chemist often needs to know how much solute is present in a given volume of solution. In this activity you will
More informationA dozen. Molar Mass. Mass of atoms
A dozen Molar Mass Science 10 is a number of objects. A dozen eggs, a dozen cars, and a dozen people are all 12 objects. But a dozen cars has a much greater mass than a dozen eggs because the mass of each
More informationReview of Basic Concepts, Molarity, Solutions, Dilutions and Beer s Law
Review of Basic Concepts, Molarity, Solutions, Dilutions and Beer s Law Aqueous Solutions In Chemistry, many reactions take place in water. This is also true for Biological processes. Reactions that take
More informationChemical calculations
Chemical calculations Stoichiometry refers to the quantities of material which react according to a balanced chemical equation. Compounds are formed when atoms combine in fixed proportions. E.g. 2Mg +
More informationThere is a simple equation for calculating dilutions. It is also easy to present the logic of the equation.
Solutions: Dilutions. A. Dilutions: Introduction... 1 B. The dilution equation... 2 C. The logic of the dilution equation... 3 D. Should you memorize the dilution equation?  Attention X11 students...
More informationConcentration of a solution
Revision of calculations Stoichiometric calculations Osmotic pressure and osmolarity MUDr. Jan Pláteník, PhD Concentration of a solution mass concentration: grams of substance per litre of solution molar
More informationU3LM2BWS Molar Mass and Conversions
U3LM2BWS Molar Mass and Conversions Name: KEY 1. The molar mass of chlorine is: 2 x 35.45 g/mol Cl = 70.90 g/mol Cl 2 (Remember that chlorine exists as a diatomic molecule in nature) 2. The molar mass
More informationChapter 6 Notes. Chemical Composition
Chapter 6 Notes Chemical Composition Section 6.1: Counting By Weighing We can weigh a large number of the objects and find the average mass. Once we know the average mass we can equate that to any number
More informationName Date Class. SECTION 16.1 PROPERTIES OF SOLUTIONS (pages 471 477)
16 SOLUTIONS SECTION 16.1 PROPERTIES OF SOLUTIONS (pages 471 477) This section identifies the factors that affect the solubility of a substance and determine the rate at which a solute dissolves. Solution
More informationMass and Moles of a Substance
Chapter Three Calculations with Chemical Formulas and Equations Mass and Moles of a Substance Chemistry requires a method for determining the numbers of molecules in a given mass of a substance. This allows
More informationn molarity = M = N.B.: n = litres (solution)
1. CONCENTRATION UNITS A solution is a homogeneous mixture of two or more chemical substances. If we have a solution made from a solid and a liquid, we say that the solid is dissolved in the liquid and
More informationConcentration Units The concentration of a dissolved salt in water refers to the amount of salt (solute) that is dissolved in water (solvent).
Concentration Units The concentration of a dissolved salt in water refers to the amount of salt (solute) that is dissolved in water (solvent). Chemists use the term solute to describe the substance of
More informationPercent Yield = Actual yield of product x 100% Theoretical yield of product
Yields of Chemical Reactions In the stoichiometry examples so far we have made the unstated assumption that the reaction goes to completion, that all reactants are converted to products. In actual fact,
More informationMore on ions (Chapters 2.1 and )
More on ions (Chapters 2.1 and 3.5 3.7) Ion: an atom or molecule that has a net electrical charge. Examples: Na + (sodium ion), Cl  (chloride), NH 4 + (ammonium). Anion: a negative ion, formed when electrons
More informationSolutions and Their Concentrations
Chapter 8 Solutions and Their Concentrations Solutions for Practice Problems Section 8.3 Student Tetbook page 305 1. Problem What is the concentration in percent (m/v) of each solution? (a) 14.2 g of potassium
More informationHow to Make Simple Solutions and Dilutions
How to Make 1. Simple Dilution (Dilution Factor Method based on ratios) A simple dilution is one in which a unit volume of a liquid material of interest is combined with an appropriate volume of a solvent
More informationMole  Mass Relationships in Chemical Systems
Chapter 3: Stoichiometry Mole  Mass Relationships in Chemical Systems 3.1 The Mole 3.2 Determining the Formula of an Unknown Compound 3.3 Writing and Balancing Chemical Equations 3.4 Calculating the Amounts
More informationFormulas, Equations, and Moles. + "reacts with" "to produce" Equations must be balanced. Equal amounts of each element on each side of the equation.
Chapter 3 Formulas, Equations, and Moles Chemical Equations 2 2 + 2 2 2 reactants products + "reacts with" "to produce" coefficients  indicate amount of substance Equations must be balanced. Equal amounts
More information2 The Structure of Atoms
CHAPTER 4 2 The Structure of Atoms SECTION Atoms KEY IDEAS As you read this section, keep these questions in mind: What do atoms of the same element have in common? What are isotopes? How is an element
More information0.279 M Change g to mol: g/mol = mol Molarity = mol L = mol 0.325L = M
118 ChemQuest 39 Name: Date: Hour: Information: Molarity Concentration is a term that describes the amount of solute that is dissolved in a solution. Concentrated solutions contain a lot of dissolved solute,
More informationSolution Making. Some general guidelines to follow when making solutions
Solution Making One goal of the laboratory exercises in this course is for you to develop competence in laboratory procedures. Among the most fundamental of these procedures is preparation of solutions,
More informationColligative Properties: Freezing Point Depression and Molecular Weight
Purpose: Colligative Properties: Freezing Point Depression and Molecular Weight The first purpose of this lab is to experimentally determine the van't Hoff (i) factor for two different substances, sucrose
More informationConcentration. The concentration of a solution is the amount of solute dissolved in a specific amount of solution.
Concentration The concentration of a solution is the amount of solute dissolved in a specific amount of solution. can be represented as mass percent, volume percent, mass/volume percent, or molarity. Mass
More informationOther Units for Solution Concentrations
OpenStaxCNX module: m51016 1 Other Units for Solution Concentrations OpenStax College This work is produced by OpenStaxCNX and licensed under the Creative Commons Attribution License 4.0 By the end of
More informationScientific Calculations
Scientific Calculations Preparing Solutions One of the most common tasks in laboratory One of the greatest sources of error and variance Need to get concentrations right if we want to draw conclusions
More informationCalculating Atoms, Ions, or Molecules Using Moles
TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary
More informationPerforming Calculatons
Performing Calculatons There are three basic units for measurement in the organic laboratory mass, volume, and number, measured in moles. Most of the other types of measurements are combinations of them,
More informationMolecular Formula: Example
Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical
More informationHow much does a single atom weigh? Different elements weigh different amounts related to what makes them unique.
How much does a single atom weigh? Different elements weigh different amounts related to what makes them unique. What units do we use to define the weight of an atom? amu units of atomic weight. (atomic
More informationBalance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O
Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent
More informationOrganic Chemistry Calculations
Organic Chemistry Calculations There are three basic units for measurement in the organic laboratory mass, volume, and number, measured in moles. Most of the other types of measurements are combinations
More information25 ppb diluted 5 ml in 100 ml 500 ppb undiluted 5.00 x 105 g in g = %
1. If a solution is determined to be 25 ppb magnesium and this was formed by dissolving 0.5436 g of an unknown solid into 100 ml and then diluting 5 ml of that solution into a 100 ml volumetric flask.
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of
More informationPart One: Mass and Moles of Substance. Molecular Mass = sum of the Atomic Masses in a molecule
CHAPTER THREE: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS Part One: Mass and Moles of Substance A. Molecular Mass and Formula Mass. (Section 3.1) 1. Just as we can talk about mass of one atom of
More informationMajor chemistry laws. Mole and Avogadro s number. Calculating concentrations.
Major chemistry laws. Mole and Avogadro s number. Calculating concentrations. Major chemistry laws Avogadro's Law Equal volumes of gases under identical temperature and pressure conditions will contain
More informationSample problems: A. What s the concentration of a solution containing 0.1 moles of NaCl in 0.25 liters of water?
EEWWWW. CHEMISTRY!! Or, dumb math problems Dr. Moss says I gotta know how to do for lab. I m not going to collect these assignments and grade them. However, there WILL be at least one math question on
More informationChemical Equations and Calculations
Chemical Equations and Calculations A chemical equation is a shorthand way of indicating what is going on in a chemical reaction. We could do it the long way Two molecules of Hydrogen gas react with one
More informationFrom the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116)
Chem 112 Solutions From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116) 1. Which of the following compounds are nonelectrolytes? A. NaF
More informationChemical Conversions and Problems
Chemical Conversions and Problems Contents: Temperature Conversions: pg. 1 Basic Unit Conversions: pg. 13 Chemical Quantity Conversions: pg. 35 Density: pg. 56 Percent Composition & Empirical & Molecular
More information12A. A Molar Mass from FreezingPoint Depression
12A. A Molar Mass from FreezingPoint Depression Time: 2 hours Required chemicals and solutions: Reagent Requirement/5 Pairs Preparation of 1 L p C 6 H 4 Cl 2 2.0 g Cyclohexane 100 ml Other required materials:
More informationThe Mole. Chapter 2. Solutions for Practice Problems
Chapter 2 The Mole Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the full set of
More informationConcentration of Solutions and Molarity
Concentration of Solutions and Molarity The concentration of a solution is a measure of the amount of solute that is dissolved in a given quantity of solvent. A dilute solution is one that contains a small
More informationProgramme in mole calculation
Programme in mole calculation Step 1 Start at the very beginning Atoms are very small indeed! If we draw a line 1 metre long, 6,000,000,000 (6 billion) atoms could be lined end to end. So a scientist cannot
More informationChapter 14. Mixtures
Chapter 14 Mixtures Warm Up What is the difference between a heterogeneous and homogeneous mixture? Give 1 example of a heterogeneous mixture and 1 example of a homogeneous mixture. Today s Agenda QOTD:
More informationChemical Calculations
Moles and Molecules Moles and Chemical Reactions Moles, Chemical Reactions, and Molarity All done as UNIT CONVERSIONS!!! and practice, practice, practice CHM 1010 Sinex 1 Mass moles particles conversions
More informationChapter 13. Properties of Solutions
Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2
More informationLecture 3: (Lec3A) Atomic Theory
Lecture 3: (Lec3A) Atomic Theory Mass of Atoms Sections (Zumdahl 6 th Edition) 3.13.4 The Concept of the Mole Outline: The mass of a mole of atoms and the mass of a mole of molecules The composition of
More informationLecture Topics Atomic weight, Mole, Molecular Mass, Derivation of Formulas, Percent Composition
Mole Calculations Chemical Equations and Stoichiometry Lecture Topics Atomic weight, Mole, Molecular Mass, Derivation of Formulas, Percent Composition Chemical Equations and Problems Based on Miscellaneous
More informationPREPARING LABORATORY SOLUTIONS AND REAGENTS I. Dr.Sarita Mangukiya GMCS
PREPARING LABORATORY SOLUTIONS AND REAGENTS I Dr.Sarita Mangukiya GMCS INTERPRETING RECIPES DEFINITIONS: SOLUTES  substances that are dissolved SOLVENTS  substance in which solutes are dissolved (usually
More information4. Magnesium has three natural isotopes with the following masses and natural abundances:
Exercise #1 Atomic Masses 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. In a sample that contains 90.0% new and 10.0% old pennies,
More informationThe Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon12? Molar Mass of Atoms 3/1/2015
The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical
More informationLecture 6: Lec4a Chemical Reactions in solutions
Lecture 6: Lec4a Chemical Reactions in solutions Zumdahl 6 th Ed, Chapter 4 Sections 16. 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
More informationChapter 4 Chemical Composition. Moles of Various Elements and Compounds Figure 4.8
Chapter 4 Chemical Composition Mole Quantities Moles, Masses, and Particles Determining Empirical and Molecular Formulas Chemical Composition of Solutions 41 Copyright The McGrawHill Companies, Inc.
More informationCh. 6 Chemical Composition and Stoichiometry
Ch. 6 Chemical Composition and Stoichiometry The Mole Concept [6.2, 6.3] Conversions between g mol atoms [6.3, 6.4, 6.5] Mass Percent [6.6, 6.7] Empirical and Molecular Formula [6.8, 6.9] Bring your calculators!
More informationMOLAR MASS AND MOLECULAR WEIGHT Themolar mass of a molecule is the sum of the atomic weights of all atoms in the molecule. Molar Mass.
Counting Atoms Mg burns in air (O 2 ) to produce white magnesium oxide, MgO. How can we figure out how much oxide is produced from a given mass of Mg? PROBLEM: If If 0.200 g of Mg is is burned, how much
More informationStoichiometry Dr. M. E. Bridge
Preliminary Chemistry Course Stoichiometry Dr. M. E. Bridge What is stoichiometry? The meaning of the word: The word stoichiometry comes from two Greek words: (meaning element ) and (meaning measure )
More information12.1 Expressing Concentration
12.1 Expressing Concentration The Amount of Solute in the solvent Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Expressing Concentration Components of Solution Mixtures: Variable components, retains
More informationCh. 10 The Mole I. Molar Conversions
Ch. 10 The Mole I. Molar Conversions I II III IV A. What is the Mole? A counting number (like a dozen) Avogadro s number (N A ) 1 mole = 6.022 10 23 representative particles B. Mole/Particle Conversions
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 9 The Mole Concept by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 9 1 Avogadro s Number Avogadro
More information4.4 Calculations Involving the Mole Concept
44 Section 43 Questions 1 Define Avogadro s constant, and explain its significance in quantitative analysis 2 Distinguish between the terms atomic mass and molar mass 3 Calculate the mass of a molecule
More informationBasics 6page 1. Basics 6: Solutions
Basics 6page 1 Basics 6: Solutions Basics 6page 2 Solutions: A Reprise A solution is a homogeneous mixture of 2 or more pure substances. What makes a mixture homogeneous/ We understand that the word
More informationMolarity. OpenStax College
OpenStaxCNX module: m51014 1 Molarity OpenStax College This work is produced by OpenStaxCNX and licensed under the Creative Commons Attribution License 4.0 By the end of this section, you will be able
More informationPercent Composition. Percent Composition the percentage by mass of each element in a compound. Percent = Part Whole x 100%
Percent Composition Percent Composition the percentage by mass of each element in a compound Percent = Part Whole x 100% Percent composition of a compound or = molecule Mass of element in 1 mol x 100%
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
A.P. Chemistry Practice Test: Ch. 11, Solutions Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Formation of solutions where the process is
More informationWe know from the information given that we have an equal mass of each compound, but no real numbers to plug in and find moles. So what can we do?
How do we figure this out? We know that: 1) the number of oxygen atoms can be found by using Avogadro s number, if we know the moles of oxygen atoms; 2) the number of moles of oxygen atoms can be found
More informationSYMBOLS, FORMULAS AND MOLAR MASSES
SYMBOLS, FORMULAS AND MOLAR MASSES OBJECTIVES 1. To correctly write and interpret chemical formulas 2. To calculate molecular weights from chemical formulas 3. To calculate moles from grams using chemical
More informationQuantitative aspects of chemical change: Moles and molar mass
OpenStaxCNX module: m38717 1 Quantitative aspects of chemical change: Moles and molar mass Free High School Science Texts Project This work is produced by OpenStaxCNX and licensed under the Creative
More informationChemical Quantities: The Mole Chapter 7 Assignment & Problem Set
Chemical Quantities: The Mole Name WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Quantities: The Mole 2 Study Guide: Things You Must Know
More informationChapter 3 Calculation with Chemical Formulas and Equations
Chapter 3 Calculation with Chemical Formulas and Equations Practical Applications of Chemistry Determining chemical formula of a substance Predicting the amount of substances consumed during a reaction
More informationF321 MOLES. Example If 1 atom has a mass of 1.241 x 1023 g 1 mole of atoms will have a mass of 1.241 x 1023 g x 6.02 x 10 23 = 7.
Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol 1.
More informationName Block THE MOLE. Who s Counting Lab. Mole Notes. Mole Calculations. Mixed Mole Conversions. % Comp, Emp, and Molecular Calcuations
Name Block THE MOLE Who s Counting Lab Mole Notes Mole Calculations Mixed Mole Conversions % Comp, Emp, and Molecular Calcuations Mole Notes, Part 1 1. The Mole is just a long word for changing units
More informationFormula Stoichiometry. Text pages
Formula Stoichiometry Text pages 237250 Formula Mass Review Write a chemical formula for the compound. H 2 CO 3 Look up the average atomic mass for each of the elements. H = 1.008 C= 12.01 O = 16.00 Multiply
More informationPRACTICE WITH YOUR LEARNING ASSISTANT!
PRACTICE WITH YOUR LEARNING ASSISTANT! An object has a mass of 20.0 g. When it is submerged in a graduated cylinder initially containing 85.0 ml of water, the water level rises to 95.0 ml. What is the
More informationMatter. Atomic weight, Molecular weight and Mole
Matter Atomic weight, Molecular weight and Mole Atomic Mass Unit Chemists of the nineteenth century realized that, in order to measure the mass of an atomic particle, it was useless to use the standard
More informationThe component present in larger proportion is known as solvent.
40 Engineering Chemistry and Environmental Studies 2 SOLUTIONS 2. DEFINITION OF SOLUTION, SOLVENT AND SOLUTE When a small amount of sugar (solute) is mixed with water, sugar uniformally dissolves in water
More information4.1 Percent Composition
Chapter 4 Page 1 4.1 Percent Composition Thursday, September 22, 2011 5:33 PM Percent composition of mass (percent composition) = the portion of the total mass contributed by each element. This is consistent
More informationChapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions This chapter uses the concepts of conservation of mass to assist the student in gaining an understanding of chemical changes. Upon completion of Chapter
More informationConcept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.
Chapter 3. Stoichiometry: MoleMass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of
More informationCHAPTER 13: ANSWERS TO ASSIGNED PROBLEMS Hauser General Chemistry I revised 8/03/08
CHAPTER 13: ANSWERS TO ASSIGNED PROBLEMS Hauser General Chemistry I revised 8/03/08 13.21 The solubility of Cr(NO 3 ) 3 9 H 2 O in water is 208 g per 100 g of water at 15 C. A solution of Cr(NO 3 ) 3
More informationTutorial 4 SOLUTION STOICHIOMETRY. Solution stoichiometry calculations involve chemical reactions taking place in solution.
T27 Tutorial 4 SOLUTION STOICHIOMETRY Solution stoichiometry calculations involve chemical reactions taking place in solution. Of the various methods of expressing solution concentration the most convenient
More informationMultiple Choice questions (one answer correct)
Mole Concept Multiple Choice questions (one answer correct) (1) Avogadro s number represents the number of atoms in (a) 12g of C 12 (b) 320g of sulphur (c) 32g of oxygen (d) 12.7g of iodine (2) The number
More informationLab 9. Colligative Properties an Online Lab Activity
Prelab Assignment Before coming to lab: Lab 9. Colligative Properties an Online Lab Activity Chemistry 162  K. Marr Revised Winter 2014 This lab exercise does not require a report in your lab notebook.
More information