Final NB 2016-2017 Turley

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Part 5: Molarity Molarity (M) is the most common measure of concentration. The concentration of most solutions you see in the lab are expressed in terms of molarity. Just like g/L, molarity calculations require that you know either the volume or density of the resulting solution. Notes: -Moles of solute divided by liters of solution - 1 mL equals .0001 L -Make sure you change grams to moles Using Density to Calculate Molarity If the volume of the resulting solution is not known, molarity is calculated as follows: Convert the volume of solvent to grams. (The simulation does this step for you.) Determine the total mass of the solution (mass of solute + mass of solvent). Convert the solution mass to volume in milliliters, using its density (volume = mass / density). Convert the solution volume to liters (divide by 1000). Convert solute grams to moles. Calculate the molarity (moles solute / L solution). Reinforcing What You've Learned 1. 35.0 g potassium dichromate are dissolved in 354.0 g distilled water. What is the concentration of the resulting solution, expressed as percent by mass? 9.00% 2. A chemist discovers that 2587.0 g distilled water are contaminated with 13.0 g NaNO3. What is the concentration of NaNO3, expressed in ppm? 5.00 X 10 3 3. 175.00 g H2SO4 are added to 61.49 g distilled H2O. What is the molality of the resulting solution? 29.04m 4. 225 g NaBr are dissolved in 525 g distilled water. If the volume of the resulting solution is 584 mL, what is its concentration when expressed in g/L? 385g/L 5. 470.0 g Na2CO3 are dissolved in 4230.0 g distilled water. What is the molarity of the resulting solution (D = 1.1029 g/mL)? 1.1561 M Applying What You've Learned MS M L Of S 6. Think about the equations for mass percent and parts/million. Consider how you might convert between these two measures of concentration. Mass percent = ppm ÷ 10,000 ppm = mass percent X .0001 7. Think about the equations for grams/liter and molarity. Consider how you might convert between these two measures of concentration. Pyramid Cover one and divide or times grams / L = molarity X molar mass molarity = grams / L ÷ molar mass 130
Glossary Concentration: Amount of dissolved solute in a given amount of solvent or solution. Density: Amount of matter per unit volume. Density is calculated by dividing an object's mass by its volume. Mass: Amount of matter an object contains or, more scientifically, the measure of an object's resistance to changes in motion. The SI (Systéme International) unit for mass is the kilogram. In the lab, mass is often measured in grams. Mass percent: Also referred to as percent by mass and, occasionally, weight percent or percent by weight. Mathematically, mass % = (mass of solute / mass of entire solution) x 100. Molar mass: Mass of a compound, calculated by adding up the individual masses for its component atoms, which are obtained from the periodic table of the elements. Molar mass is expressed in grams/mole and is sometimes referred to as molecular mass (for molecular compounds) or formula mass (for ionic compounds). Molality (m): Moles of solute per kilogram of solvent. Mathematically, m = moles of solute / kilogram of solvent. Molarity (M): Moles of solute per liter of solution. Mathematically, M = moles of solute / liter of solution. Mole (mol): Counting unit used to express the large numbers of particles, such as atoms or molecules, that are involved in chemical processes. One mole of particles contains 6.02 x 10 particles. The mass of one mole of an element, in grams, is equivalent to the atomic mass for that element, as indicated on the periodic table. Parts per million (ppm): Measure of concentration often used for dilute solutions. Mathematically, ppm = (mass of solute / mass of solution) x 10. Solubility: Measure of the maximum amount of solute that can be dissolved in a given amount of solvent at a given temperature, forming a stable solution. Solute: Dissolved substance in a solution. The solute is generally the solution component present in the lesser amount. Solution: Homogeneous mixture in which one substance has been dissolved in another. Solvent: Substance in which a solute is dissolved to form a solution. The solvent is generally the solution component present in the greater amount. Volume: Amount of space an object occupies. The SI (Systéme International) unit for volume is the cubic meter. In the lab, volume is often measured in cubic centimeters, milliliters, or liters. SAS Curriculum Pathways VLab #866 131
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Honors Chemistry Class Policies and
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Unit 1 (22 days) Chapter 1 Introduc
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Chapter 1 Unit 1 Introduction to Ch
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Looking at Ions We haven’t talked
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In the space below, write the unabb
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Create groups for these Scientist a
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Define Atomic Size: Atomic Size Ato
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Define Electronegativity: Electrone
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50 Unit 3 Chapter 25 Nuclear Chemis
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Name ____________________ Go to the
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C 2 H 6 O Ethanol CH 3 CH 2 O Step
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Trigonal Pyramidal Molecular Geomet
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Final NB 2016-2017 Turley

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