ab 1.2b – Worksheethoduloz nl sl Name:anlov ient) noitulce to J1 ni bavloaie Lab Period:tw nottuleenConcentrations and Dilutions Reviewean noReading: Silverthorn 7e Fig. 2.7 p. 42Student Learning Objectives:Explain the different ways concentration is expressedDefine all terms usedExplain the concept of a mole and Avogadro's number for ionizing and non-ionizing solutesCalculate molarity, grams, molecular weight, and volumes in problemsMake the calculations necessary to perform serial dilutions.Use the concept of a mole to calculate the number of moles or grams to be used in chemical reactions.Physiologists spend a lot of time working with chemical solutions needed for various lab techniques. You therefore needto know how to make up solutions of known concentrations and to make appropriate dilutions of these solutions.Concentration: the amount of solute present per unit of solvent.stomSolute: the minor component of a solution; the substance dissolved in another substance (e.g. NaCl dissolved inwater)Solvent: the major component of a solution; the substance that does the dissolving: in physiology this is alwayswater.Concentration is expressed several ways:Mass Percent (%):Amount (mass) dissolved in total volume: e.g. a 2 % solution of NaCl consists of 2 g of NaCl dissolved in 100 mlof water (total volume).An isotonic saline solution used for an IV contains approx. 0.9% NaCl.This is 0.9g NaCl dissolved in a total volume of 100ml waterMilligram per cent (mg/dL)mg /dL = number of milligrams of a substance in 100 ml of solution, e.g. glucose 80 mg/dL in blood. Note:clinically units are expressed as mg/dL (also known as mg %).Molarity:Molarity (M) is equal to the number of moles of a substance per liter of solution (mol/L)First, what is a mole? Just like a dozen is 12 of anything, a mole is 6.02 x 1023 (Avogadro's number) of anything.We don't usually count molecules or atoms directly because there are so many of them. Instead we countmoles of molecules or atoms.Different molecules are composed of different numbers and types of atoms. One mole of a particular type ofmolecule equals the molecular weight (MW) of that molecule in grams.1 mole of any substance has the same number of molecules:This number (the number of molecules in one mole) is Avogadro's number (6.02 x 1023)HOWEVER: If a compound ionizes (i.e. splits into two or more separate ions when dissolved in water),then there will be 1 mole of each ion in the solution. For example, 1 mole of NaCl dissolved in waterproduces a solution with 1 mole (6.02 x 1023) of Na* ions and 1 mole (6.02 x 1023) of Cl ions. onvert between grams and moles. In this case, the MW of a molecule is the conversion factor,A 0.1 M solution contains (0.1 x 58.5 g) /L= 5.85 g /L (it is more dilute than a 1M solution)ince 1 mole of each type of molecule equals the MW of that substance (in grams), we can use dimensional analysis toSince molarity has uswe are adding outardelsow dwe mustthát molecule (in grams) dissolved in 1 L of solution (final volume).NotCalculating molecular weight (Mw)of the molecule.weight of Cl = 35.5 grams.Question: What is the MW of NaCl?grams = 1 Mole of NaClQuestion: How many molecules of NaCl are in 58.5 g NaCl?Examples:1. Calculate the number of grams of potassium permanganate (KMnOa) in 1 mole of potassium permanganate:Add the molecular weight (in grams) of each atom in the molecule: 1 mole of K = 40.08 g, 1 mole of Mn = 55 g, 1 moleO = 16 g (But be careful: from the molecular formula for potassium permanganate, there are 4 oxygen atoms in onemolecule of potassium permanganate.)grams in 1 mole of KMNO42. How many grams of glucose are in 1 mole of glucose (C6H1206)?MW of C = 12 g, H = 1 g, and O = 16 g.MW of glucose:grams.Calculating MolarityHere we will review how to calculate molarity and determine how many grams of a substance are needed to mekasolutions of varying molarity.A 1M solution has the MW of the molecule (in grams) dissolved 1L (final volume)Since 58.5g of NaCl is equal to 1 mole of NaCI, a 1M solution of NaCl contains 58 5 c NesuA 2M solution contains (2 x 58.5 g) /L = 117 g /L (it is twice as concentrated as a 1McelNote: In practice, we can only weigh out grams. We cannot weigh out molesaWe can convert grams of NaCl to moles of NaCl using the following formula.1mole Nacigrams NaCl x(Eq. 1)MW of NaCl (grams Nacl)ice that the units of grams cancel and we are left with units of moles

Molecular weight of any molecule is defined as sum of atomic weights of all the atoms present in…

Question: What is the MW of NaCl? grams = 1 Mole of Nacl Question: How many molecules of NaCl are in 58.5 g NaCl? Examples: . Calculate the number of grams of potassium permanganate (KMNO.) in 1 mole of potassium permanganate: Add the molecular weight (in grams) of each atom in the molecule: 1 mole of K = 40.08 g, 1 mole of Mn = 55 g, 1 mole O = 16 g (But be careful: from the molecular formula for potassium permanganate, there are 4 oxygen atoms in one molecule of potassium permanganate.) %3D grams in 1 mole of KMNO4

Question: What is the MW of NaCl? grams = 1 Mole of Nacl Question: How many molecules of NaCl are in 58.5 g NaCl? Examples: . Calculate the number of grams of potassium permanganate (KMNO.) in 1 mole of potassium permanganate: Add the molecular weight (in grams) of each atom in the molecule: 1 mole of K = 40.08 g, 1 mole of Mn = 55 g, 1 mole O = 16 g (But be careful: from the molecular formula for potassium permanganate, there are 4 oxygen atoms in one molecule of potassium permanganate.) %3D grams in 1 mole of KMNO4

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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