DOCSLIB.ORG

Data Booklet

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Data Booklet Chemistry DATA BOOKLET Chemistry DATA BOOKLET Chemistry Data Booklet © Crown copyright, Province of Nova Scotia, 2013 Prepared by the Department of Education and Early Childhood Development The contents of this publication may be reproduced in whole or in part provided the intended use is for non-commercial purposes and full acknowledgment is given to the Nova Scotia Department of Education and Early Childhood Development. Cover image may not be extracted or reused. Cataloguing-in-Publication Data Main entry under title. Chemistry : data booklet / Nova Scotia. Department of Education and Early Childhood Development. ISBN: 978-1-55457-524-4 1. Chemistry—Study and teaching (Secondary). 2. Chemistry—Study and Teaching—Nova Scotia. 3. Science—Study and teaching. I. Nova Scotia. Department of Education and Early Childhood Development. 540.712—dc23 2013 Contents Introduction . 1 Periodic Table of The Elements . .2 Table of Common Polyatomic Ions . .3 Chemistry Notation . 4 Solubility of Some Common Ionic Compounds in Water at 298 1. 5 °K . .4 Flame Colour of Elements . 5 Selected SI (Système International) Prefixes . 5 Table of Selected Standard Electrode Potentials . .6 Acid–Base Indicators at 298.15 °K . .7 Colours of Common Aqueous Ions . 7 Names of the Elements . .8 First Ionization Energy, Electron Affinity, and Electronegativity of the Elements . .9 Covalent Bond Lengths and Bond Enthalpies . 11 Thermodynamic Data of Organic Compounds . 12 Enthalpies of Combustion . 13 Standard Electrode Potentials . .14 Strengths of Organics . 15 Carboxylic acids . 15 Halogenated carboxylic acids . 15 Phenols . 15 Alcohols . 15 Amines . 16 Acid–Base Indicators . .16 Examples of Structural Formulas . 17 Medicines and Drugs . 17 Biological Molecules . 18 Examples of Common Ion Names, Formulas, and Charges . 19 Solubility of Common Compounds in Water . .20 Solubility Product Constants at 25°C . 21 Brønsted-Lowry Acids and Bases . .22 Standard Reduction Potentials of Half-Cells . .23 Acid to Base Indicators . .25 Solubility Table . .26 Standard Heats of Formation at 298.15 K (25°C) . 27 References . .29 iii CHEMISTRY DATA BOOKLET Introduction Chemistry is part of the science curriculum from primary to grade 12 . This chemistry data booklet is intended for student use for class work and assessments . This booklet is helpful for Science 9, Science 10, all chemistry classes, and Food Science 12 . 1 CHEMISTRY DATA BOOKLET 2 Periodic Table of The Elements 1 18 1 1. 01 2 4.00 +1 0 –1 1 H He 2 atomic number average atomic mass* 13 14 15 16 17 hydrogen oxidation states helium 3 6.94 4 9.01 5 10.81 6 12.01 7 14.01 8 16.00 9 19.00 10 20.18 +1 +2 +3 +2 +1 –2 -1 0 Symbol +4 +2 2 –4 +3 Li Be B C N +4 O F Ne +5 element name –1 lithium berylium boron carbon nitrogen –2 oxygen fluorine neon –3 11 22.99 12 24.31 13 26.98 14 28.09 15 30.97 16 32.07 17 35.45 18 39.95 +1 +2 +3 +2 +3 +4 +1 0 +4 +5 +6 +5 3 Transitional Elements –4 –3 –2 +7 Na Mg Al Si P S Cl –1 Ar sodium magnesium 3 45678910 11 12 aluminum silicon phosphorus sulfur chlorine argon 19 39.10 20 40.08 21 44.96 22 47.87 23 50.94 24 52.00 25 54.94 26 55.85 27 58.93 28 58.69 29 63.55 30 65.39 31 69.72 32 72.61 33 74.92 34 78.96 35 79.90 36 83.80 +1 +2 +3 +2 +2 +2 +2 +2 +2 +2 +1 +2 +3 +2 +3 +4 +1 0 +3 +3 +3 +3 +3 +3 +3 +2 +4 +5 +6 +5 4 +4 +4 +6 +4 –3 –2 –1 K Ca Sc Ti V +5 Cr Mn +7 Fe Co Ni Cu Zn Ga Ge As Se Br Kr potassium calcium scandium titanium vanadium chromium maganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton 37 85.47 38 87.62 39 88.91 40 91.22 41 92.91 42 95.94 43 (98) 44 101.07 45 102.91 46 106.42 47 107.87 48 112.41 49 114.82 50 118.71 51 121. 76 52 127.60 53 126.90 54 131.29 +1 +2 +3 +4 +3 +6 +4 +3 +3 +2 +1 +2 +3 +2 +3 +4 +1 0 +5 +6 +3 +4 +5 +6 +5 5 +7 –3 –2 +7 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I –1 Xe rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon CHEMISTRY DATA BOOKLET DATA CHEMISTRY 55 132.91 56 137.33 57 138.91 72 178.49 73 180.95 74 183.21 75 186.21 76 190.23 77 192.22 78 195.08 79 196.97 80 200.59 81 204.38 82 207.20 83 208.98 84 (209) 85 (210) 86 (222) +1 +2 +3 +4 +5 +6 +4 +3 +3 +2 +1 +1 +1 +2 +3 +2 0 +6 +4 +4 +4 +3 +2 +3 +4 +5 +4 6 Cs Ba La Hf Ta W Re +7 Os Ir Pt Au Hg Tl Pb Bi Po At Rn cesium barium lanthanum hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon 87 (223) 88 (226) 89 (227) 104 (261) 105 (262) 106 (266) 107 (264) 108 (269) 109 (268) 110 (271) 111 (272) 112 (277) 113 (282) 114 (285) 115 (288) 116 (289) +1 +2 +3 +4 7 Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv francium radium actinium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium ununtrium flerovium ununpentium livermorium elements 113 and 115 have not yet been officially named Inner Transitional Elements 58 140.12 59 140.90 60 144.24 61 (145) 62 150.36 63 151.96 64 157.25 65 158.93 66 162.50 67 164.93 68 167.26 69 168.93 70 173.04 71 174.97 +3 +3 +3 +3 +2 +2 +3 +3 +3 +3 +3 +3 +2 +3 +4 +3 +3 +3 8 Lanthanoids Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium 90 232.04 91 231.04 92 238.03 93 237.05 94 (244) 95 (243) 96 (247) 97 (247) 98 (251) 99 (252) 100 (257) 101 (258) 102 (259) 103 (262) +4 +5 +3 +3 +3 +3 +3 +3 +3 +3 +3 +2 +2 +3 +4 +4 +4 +4 +4 +4 +3 +3 9 Actinoids +5 +5 +5 +5 Th Pa U +6 Np+6 Pu +6 Am +6 Cm Bk Cf Es Fm Md No Lr thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium *Average atomic mass values in parenthesis represent the mass of the most stable isotope. Table of Common Polyatomic Ions – acetate (ethanoate) CH3COO + ammonium NH4 – benzoate C6H5COO 3– borate BO3 2– carbide C2 2– carbonate CO3 – hydrogen carbonate HCO3 – perchlorate CIO4 – chlorate CIO3 – chlorite CIO2 hypochlorite OCl– or CIO– 2– chromate CrO4 2– dichromate Cr2O7 cyanide CN– hydroxide OH– – iodate IO3 – nitrate NO3 – nitrite NO2 oxalate OOCCOO2– hydrogen oxalate HOOCCOO– – permanganate MnO4 2– peroxide O2 2– persulfide S2 3– phosphate PO4 2– hydrogen phosphate HPO4 – dihydrogen phosphate H2PO4 2– silicate SiO3 2– sulfate SO4 – hydrogen sulfate HSO4 2– sulfite SO3 – hydrogen sulfite HSO3 hydrogen sulfide HS– thiocyanate SCN– 2– thiosulfate S2O3 3 CHEMISTRY DATA BOOKLET Chemistry Notation Symbol Term Unit(s) c specific heat capacity J/(g·°C) or J/(g·K) E° standard electrical potential V or J/C ΔH enthalpy (heat) kJ ΔH°f standard molar enthalpy of formation kJ/mol I current A or C/s Kc equilibrium constant — Ka acid ionization (dissociation) constant — Kb base ionization (dissociation) constant — M molar mass g/mol m mass g n amount of substance mol Q charge C T temperature (absolute) K t temperature (Celsius) °C t time s V volume L c amount concentration mol/L Solubility of Some Common Ionic Compounds in Water at 298.15 °K – – 2– 2– – – Ion Group 1 ions F Cl SO4 CO3 IO3 OH + – 3– 2– NH4 Br PO4 OOCCOO – – 2– NO3 I SO3 – ClO3 – ClO4 – CH3COO Solubility most most most most Group 1 ions Group 1 ions Group 1 ions + + + greater than NH4 NH4 NH4 or equal to 0 1. Co(IO3)2 mol/L Fe2(OOCCOO)3 (very soluble) + + 2+ Solubility less RbClO4 Li Cu Ca most most most 2+ + 2+ than 0 1. mol/L CsClO4 Mg Ag Sr 2+ 2+ 2+ (slightly AgCH3COO Ca Hg2 Ba 2+ 2+ + soluble) Hg2(CH3COO)2 Sr Pb Ag 2+ + 2+ Ba Tl Hg2 2+ 2+ Fe Pb 2+ 2+ Hg2 Ra Pb2+ Note: This solubility table is only a guideline that is established using the Ksp values . A concentration 2+ of 0 1. mol/L corresponds to approximately 10 g/L to 30 g/L depending on molar mass . Hg2 is a polyatomic ion of mercury . 4 CHEMISTRY DATA BOOKLET Flame Colour of Elements Element Symbol Colour barium Ba yellowish green boron B yellowish green calcium Ca yellowish red cesium Cs violet copper Cu blue to green lead Pb blue-white lithium Li red potassium K violet rubidium Rb violet sodium Na yellow strontium Sr scarlet red Note: The flame test can be used to determine the identity of a metal or a metal ion .
Load more

Recommended publications
  • Addendum.Solubility
    Addendum to Hebden: Chemistry 11 SOLUBILITY I. CALCULATING SOLUBILITY AND ION CONCENTRATIONS Once the mass of a substance present in 1 L of a solution has been experimentally measured, calculating the solubility of the substance is straightforward. EXAMPLE: It is experimentally found that 1.00 L of saturated AgBrO3(aq) contains 1.96 g of AgBrO3. What is the molar solubility of AgBrO3? (That is, what is the solubility expressed in moles per litre?) g 1mol –3 [AgBrO3] = 1.96 x = 8.31 x 10 M L 235 .8 g –3 EXAMPLE: The molar solubility of PbI2 is 1.37 x 10 M. Express this value in grams per litre. –3 mol 461.0 g g Solubility (g/L) = 1.37 x 10 x = 0.632 L 1mol L o EXAMPLE: It is experimentally found that 0.250 L of saturated CaCl2 contains 18.6 g of CaCl2 at 20 C. What is the molar solubility of CaCl2? 18.6 g 1mol [CaCl2] = x = 0.670 M 0 .250L 111 .1g Note: Unless otherwise indicated, assume all solutions are at a temperature of 25oC. EXERCISES: o 1. Aluminum fluoride, AlF3 , has a solubility of 5.59 g/L at 20 C. Express this solubility in moles per litre. o 2. Lead (II) chloride, PbCl2 , has a solubility of 0.99 g/100.0 mL at 20 C. Calculate the molar solubility of PbCl2 . –3 o 3. The molar solubility of MgCO3 is 1.26 x 10 M at 25 C. Express this value in grams per litre. –4 o 4.
    [Show full text]
  • Chemistry Curriculum L1
    1 CHEMISTRY The Nature of Chemistry Topic(s) Concepts Competencies (Eligible Anchor Descriptions Vocabulary Textbook Duration (with Standards) Content) Pages (in days) The Scientific 3.2.10.A6: CHEM.A.1.1.1: CHEM.A.1.1: The Nature of Chemistry L1: Ch 1 (p3-27) 2-5 Method • Compare and contrast • Classify physical or • Identify and describe how Analytical chemistry scientific theories. chemical changes within a observable and measurable Biochemistry Laboratory • Know that both direct system in terms of matter properties can be used to Chemistry Procedure(s) and indirect observations and/or energy. classify and describe matter Inorganic chemistry and Safety are used by scientists to and energy. Organic chemistry study the natural world CHEM.A.1.1.2: Physical chemistry The Metric and universe. • Classify observations as Science System, • Identify questions and qualitative and/or Technology Significant concepts that guide quantitative. Figures, and scientific investigations. Scientific Methods and L1 and L2: 2-5 Measurement • Formulate and revise CHEM.A.1.1.3: Laboratory Safety & Teacher and explanations and models • Utilize significant figures to Procedures department using logic and evidence. communicate the Control generated • Recognize and analyze uncertainty in a quantitative Control experiment materials; Flinn alternative explanations observation. Dependent variable Scientific Safetly and models. Erlenmeyer flask (E-flask) Contract • Explain the importance of Graduated cylinder accuracy and precision in Hypothesis making valid Independent variable measurements. Laboratory balance Laboratory burner 3.2.C.A6: Law • Examine the status of Observation existing theories. Science Scientific method • Evaluate experimental Theory information for relevance Variable and adherence to Laboratory equipment science processes.
    [Show full text]
  • Solubility Handbook Collected from Wikipedia by Khaled Gharib ([email protected])
    Solubility handbook Collected from wikipedia by Khaled Gharib ([email protected]) PDF generated using the open source mwlib toolkit. See http://code.pediapress.com/ for more information. PDF generated at: Sat, 31 Mar 2012 09:49:23 UTC Contents Articles What is solubility 1 Solubility 1 Solubility chart 8 Solubility chart 8 Solubility table 10 Solubility table 10 References Article Sources and Contributors 39 Image Sources, Licenses and Contributors 40 Article Licenses License 41 1 What is solubility Solubility Solubility is the property of a solid, liquid, or gaseous chemical substance called solute to dissolve in a solid, liquid, or gaseous solvent to form a homogeneous solution of the solute in the solvent. The solubility of a substance fundamentally depends on the used solvent as well as on temperature and pressure. The extent of the solubility of a substance in a specific solvent is measured as the saturation concentration where adding more solute does not increase the concentration of the solution. Most often, the solvent is a liquid, which can be a pure substance or a mixture.[1] One may also speak of solid solution, but rarely of solution in a gas (see vapor-liquid equilibrium instead). The extent of solubility ranges widely, from infinitely soluble (fully miscible[2]) such as ethanol in water, to poorly soluble, such as silver chloride in water. The term insoluble is often applied to poorly or very poorly soluble compounds. Under certain conditions, the equilibrium solubility can be exceeded to give a so-called supersaturated solution, which is metastable.[3] Solubility is not to be confused with the ability to dissolve or liquefy a substance, because the solution might occur not only because of dissolution but also because of a chemical reaction.
    [Show full text]
  • Treatment Concept for Rdx-Containing Wastewaters Using Activated Carbon with Offline Solvent Biological Regeneration
    TREATMENT CONCEPT FOR RDX-CONTAINING WASTEWATERS USING ACTIVATED CARBON WITH OFFLINE SOLVENT BIOLOGICAL REGENERATION by Rolf M.X. Hesselmann and Michael K. Stenstrom Civil and Environmental Engineering Department University of California, Los Angeles Los Angeles, CA 90095 1994 School of Engineering and Applied Science Report Eng. 94-23 TABLE OF CONTENTS TABLE OF CONTENTS i LIST OF FIGURES m LIST OF TABLES v PREFACE vi ABSTRACT vii 1 .0 INTRODUCTION 1 1 .1 RDX - Properties, Importance, Toxicity, and Environmental Fate 2 1 .2 Physico-Chemical Treatment of RDX Wastes 5 1 .3 Biodegradation of RDX 7 2.0 PROPOSED TREATMENT CONCEPT AND RESEARCH 13 REQUIREMENTS 2 .1 Treatment Concept 13 2.2 Detail Considerations and Research Requirements 16 3 .0 MATERIALS AND METHODS 22 3 .1 Chemicals 22 3 .2 Adsorption and Desorption Experiments 23 3 .2.1 Continuous flow experiments in column reactors 23 3 .2.2 Desorption experiments in batch reactors 24 3 .2.3 Solubility determination 25 3 .3 Inocula 25 3 .4 Incubation Methods and Media 27 i TABLE OF CONTENTS (Cont'd) 3 .5 Analytical Methods 30 4.0 RESULTS 33 4.1 Adsorption and Desorption of RDX 33 4.2 Anaerobic Biodegradation of RDX 39 5.0 DISCUSSION 61 5 .1 Adsorption and Desorption of RDX 61 5 .2 Anaerobic Bioegradation of RDX 66 6.0 CONCLUSIONS AND RECOMMENDATIONS 73 REFERENCES 77 APPENDIX A 84 APPENDIX B 90 ii LIST OF FIGURES Figure 1 .1 Structure, properties, and names of RDX . 3 Figure 1 .2 Proposed intermediates for the anaerobic biodegradation of RDX . 9 Figure 2.1 Proposed treatment scheme using an indirect-offline-bioregeneration 14 (IOBR) of activated carbon .
    [Show full text]
  • 2 Concentration and Solubility
    2 Concentration and Solubility What You’ll Learn 6(E) • what solubility is • about the concentration of Before You Read solutions The labels of some containers of fruit juice say “Not from • three types of solutions concentrate.” What do you think this means? • factors that affect gas solutions Read to Learn Focus Check for Understanding As How much can dissolve? you read this section, highlight Suppose you like your lemonade very sweet. You add a any sentences that you read teaspoon of sugar to it and stir. The sugar dissolves. If you keep more than once. After you finish the section, go back and read adding sugar to the lemonade, you will reach a point when no more the highlighted sentences again. sugar will dissolve in it. The excess sugar crystals fall to the bottom of the glass. They do not go into the solution. You have reached the solubility of sugar in a given amount of water. Solubility (sahl yuh BIH luh tee) is the greatest amount of solute that can dissolve in a specific amount of solvent at a given temperature. Are the solubilities of all substances the same? You can dissolve more than 32 g of salt in 113 g of water at 25°C. But, you can only dissolve about 12 g of baking soda in 113 g water. Salt and baking soda have different solubilities in water. The difference in the solubilities of solutes depends on the nature of the solute and the nature of the solvent. Concentration Suppose you and a friend are making lemonade.
    [Show full text]
  • Solubility Table
    Solubility Table Solutions for Crystal Growth Crystal Growth 101 page 1 • The following table provides data for formulating a saturated solution of the reagents listed at the temperature designated. Reagent Formula MW Temp (°C) g/100 ml [M] Ammonium bromide NH4Br 97.95 15 53.8 5.5 Ammonium chloride NH4Cl 53.49 20 26.7 5.0 Ammonium citrate dibasic (NH4)2C6H6O7 226.19 25 56.54 2.5 Ammonium fluoride NH4F 37.04 20 37.0 10.0 Ammonium formate HCOONH4 63.06 20 63.0 10.0 Ammonium iodide NH4I 144.94 25 94.2 6.5 Ammonium nitrate NH4NO3 80.04 25 90.2 11.2 Ammonium phosphate dibasic (NH4)2HPO4 132.06 25 46.2 3.5 Ammonium phosphate monobasic NH4H2PO4 115.03 25 28.7 2.5 Ammonium sulfate (NH4)2SO4 132.14 20 46.2 3.5 Ammonium tartrate dibasic (NH4)2C4H4O6 184.15 20 36.8 2.0 Barium nitrate Ba(NO3)2 261.34 25 10.2 0.3 Cadmium bromide tetrahydrate CdBr2 • 4H2O 344.28 25 94.0 2.7 Cadmium chloride hemipentahydrate CdCl2 • 2.5H2O 228.35 25 97.2 4.2 Cadmium iodide CdI2 366.22 20 73.0 1.9 Cadmium sulfate hydrate 3CdSO4 • 8H2O 769.52 25 70.3 0.9 Calcium chloride hexahydrate CaCl2 • 6H2O 219.08 25 67.8 3.0 Calcium sulfate dihydrate CaSO4 • 2H2O 172.17 25 0.208 0.01 Cesium bromide CsBr 212.81 22 89.8 4.2 Cesium chloride CsCl 168.36 25 126.3 7.5 Cesium iodide CsI 259.81 23 74.1 2.8 Cesium nitrate CsNO3 194.91 25 26.1 1.3 Cesium sulfate Cs2SO4 361.87 25 129.8 3.5 Citric acid monohydrate HOC(COOH)(CH2COOH)2 • H2O 210.14 25 88.6 4.2 Copper(II) bromide CuBr2 223.35 25 102.5 4.5 Copper(II) chloride dihydrate CuCl2 • 2H2O 170.48 25 80.0 4.6 Copper(II) sulfate pentahydrate
    [Show full text]
  • Solutions and Their Behavior
    Solutions and Their Behavior Shonna Robinson, (ShonnaR) Therese Forsythe, (ThereseF) Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) AUTHORS Shonna Robinson, (ShonnaR) To access a customizable version of this book, as well as other Therese Forsythe, (ThereseF) interactive content, visit www.ck12.org EDITOR Richard Parsons, (RichardP) CK-12 Foundation is a non-profit organization with a mission to reduce the cost of textbook materials for the K-12 market both in the U.S. and worldwide. Using an open-content, web-based collaborative model termed the FlexBook®, CK-12 intends to pioneer the generation and distribution of high-quality educational content that will serve both as core text as well as provide an adaptive environment for learning, powered through the FlexBook Platform®. Copyright © 2014 CK-12 Foundation, www.ck12.org The names “CK-12” and “CK12” and associated logos and the terms “FlexBook®” and “FlexBook Platform®” (collectively “CK-12 Marks”) are trademarks and service marks of CK-12 Foundation and are protected by federal, state, and international laws. Any form of reproduction of this book in any format or medium, in whole or in sections must include the referral attribution link http://www.ck12.org/saythanks (placed in a visible location) in addition to the following terms. Except as otherwise noted, all CK-12 Content (including CK-12 Curriculum Material) is made available to Users in accordance with the Creative Commons Attribution-Non-Commercial 3.0 Unported (CC BY-NC 3.0) License (http://creativecommons.org/ licenses/by-nc/3.0/), as amended and updated by Creative Com- mons from time to time (the “CC License”), which is incorporated herein by this reference.
    [Show full text]
  • Chemistry 20 Unit 3 Lesson 3
    Chemistry 20 Unit 3 Lesson 3 - Concentration as a Percent 84 mins Solubility of Ionic Compounds Solubility Table (Data Booklet) 4+ 2- - ​ ​ Ammonium NH SO3 (NH4)2SO3 (aq) ​ ​ ​ ​ ​ ​ ​ ​ ​ sulphite + - Lithium fluoride Li ​ F LiF ​ ​ ​(s) + - Sodium Na ​ OH NaOH ​ ​ ​(aq) hydroxide 3+ - Niobium (III) Nb ​ Cl NbCl ​ ​ ​3(aq) chloride Percentage Concentration quantity of solute concentration = × 100% Types quantity of solution - % v/v Percent by volume - % w/w Percent by weight Percent by Volume V solute 2L of solution of 5% v/v acetic acid Cv/v = V × 100% solution - What would be the Vsolute? ​ ​ V solute CCH COOH = × 100% 3 V solution V solute CCH COOH ÷ 100% = × 100% ÷ 100% 3 V solution C CH3COOH V solute × V solute = × V solution 100% V solution (C )(V ) CH3COOH solution 100% = V solute (5%)(2L) V solute = 100% = 0.1 L Percentage by Weight m solute Eg. Cw/w = × 100% msolution 0.11% w/w of flouride msolution = 250 g msolute = ? (Cw/w)(msolution) msolute = 100% (0.11%)(250g) msolute = 100% = 0.28g Eg. msolution = 12.0g 0.103 mol of Ag(s) C = ?? mAg = Mn = (107.87 g)(0.103 mol) = 11.1061 g msolute Cw/w = × 100% msolution (11.1061 g) Cw/w = (12.0 g) × 100% = 92.6% Eg. Sol′n of HCl = 500 mL d = 1.50 g/mL n = ? m = dV = (1.50 g/mL)(500 mL) = 750 g m 750 g n = M = 36.46 g/mol = 20.6 mol Extra Examples 6) Cv/v = 70.0% ​ ​ Vsol’n = 500 mL ​ ​ (C )(V ) Cw/w = 25.0% v/v solution ​ ​ V solute = 100% msol’n = 60.0 kg ​ ​ (70.0%)(500 mL) msolute = ?? V = ​ ​ solute 100% msolute Cw/w = × 100% V solute = 350 mL msolution (Cw/w)(msolution) msolute = 100% (25.0%)(60.0 kg ) msolute = 100% 4 msolute = 15.0 kg = 1.50 × 10 g Chemistry 20 - Unit 2 - Concentration as a Percent Name: _________________________________________ You may find the following formulas useful: n V C = solute V Cv/v = V × 100% m = Mn msolution m solute Cw/w = m × 100% d = V solution 1.
    [Show full text]
  • Chem 1319 – WS16 Solubility Worksheet
    Name: __________________________________________ Sec #: _______________ Date: _____________________ Chem 1319 – WS16 Solubility Worksheet A. Solubility Terms Directions: Fill in the blank with the most appropriate term for the definition given. Word Bank: Chemical Change, Compound, Electrolyte, Element, Heterogeneous, Homogenous, Matter, Mixture, Physical Change, Precipitate, Soluble, Solute, Solution, Solvent, Supernate 1. ______________________________ Able to dissolve to a certain extent, usually in reference to water. 2. ______________________________ A homogenous mixture of two substances. 3. ______________________________ Changes that alter the composition of matter. 4. ______________________________ Changes that alter only the state or appearance of a substance, but not the composition. 5. ______________________________ The minor (lesser) component in a solution. 6. ______________________________ A pure substance composed of 2 or more elements in a fixed ratio. 7. ______________________________ A solid, insoluble ionic compound that forms in and separates from a solution. 8. ______________________________ The major (greater) component in a solution. 9. ______________________________ The soluble ionic compound that remains in solution. 10. ______________________________ A mixture that has the same composition throughout. 11. ______________________________ A pure substance that cannot be broken down into simpler substances. 12. ______________________________ Anything that occupies space and has mass. 13. ______________________________ A substance composed of 2 or more components in proportions that vary. 14. ______________________________ A mixture where the composition varies from one region to another. 15. ______________________________ A substance that dissolves readily in water (e.g., alkali metal compounds),to form solutions that conduct electricity. 1 B. Solution Concentration Unit Terms Directions for Matching: Write the letter corresponding to the most appropriate definition for the given word in the blank to the left of the word.
    [Show full text]
  • INTRODUCTION Experimental Protocol References Conclusions Initial Evaporation Results N Solubility Determination Results Future
    EXPERIMENTAL STUDY OF NITROGEN DISSOLUTION IN METHANE- ETHANE MIXTURES UNDER TITAN SURFACE CONDITIONS V. F. Chevrier1, A. Luspay-Kuti2, S. Singh1 1Arkansas Center for Space and Planetary Science, University of Arkansas, Fayetteville, AR 72701, USA. [email protected] 2South West Research Institute, San Antonio, Texas. INTRODUCTION In the past few years there have been significant advances in determining the composition of Titan’s lakes, using vapor-liquid equilibrium calculations with activity models [1], Regular Solution Theory [2,3] and Statistical Associating Fluid Theory [4]. Though, in the absence of relevant datasets at Titan temperature and pressure conditions, the thermodynamic and kinetic parameters are extrapolated values, thus carrying high uncertainty. Using our recent work on experimental measurements of evaporation rates of liquid methane-ethane mixtures [5,6], we present preliminary results on the solubility of N2 in liquid mixtures under conditions relevant to Titan’s surface. Experimental Protocol • The plateau zone at the beginning of the experiment increases with increasing CH4 concentration (Fig. 1). • Titan simulation chamber • Steady-state slope correction removes the hydrocarbon • Temperature: 92-94 K evaporation (Fig. 2A). • The residual mass increase is due to N dissolution (Fig. 2B). • 1.5 bar N2 atmosphere 2 • C2H6 then CH4 condensation Results • Mass loss measurements • N2 solubility is not detected at initial CH4 mole ratio below 0.7 • Continuous P, T, measurements • Time to reach steady state decreases with increasing XCH4 (Fig. 3) • Above XCH4 ~ 0.7 exponential increase of N2 solubility (Table 1, Initial Evaporation Results Fig. 4). Figure 4. Calculated mole fraction of nitrogen in the sample as a function of the initial mole fraction of methane in the methane – ethane liquid (e.g.
    [Show full text]
  • "Electrochemistry in Nonaqueous Solutions"
    Electrochemistry in Nonaqueous Solutions. Kosuke Izutsu Copyright © 2002 Wiley-VCH Verlag GmbH & Co. KGaA ISBNs: 3-527-30516-5 (Hardback); 3-527-60065-5 (Electronic) Kosuke Izutsu Electrochemistry in Nonaqueous Solutions Electrochemistry in Nonaqueous Solutions. Kosuke Izutsu Copyright © 2002 Wiley-VCH Verlag GmbH & Co. KGaA ISBNs: 3-527-30516-5 (Hardback); 3-527-60065-5 (Electronic) Related Titles from WILEY-VCH Bard, A.J., Stratmann, M., Licht, S. (Eds) Encyclopedia of Electrochemistry, Volume VI 2001. ISBN 3-527-30398-7 Kaifer, A.E., Gómez-Kaifer, M. Supramolecular Electrochemistry 1999. ISBN 3-527-29597-6 Memming, R. Semiconductor Electrochemistry 2000. ISBN 3-527-30147-X Günzler, H., Williams, A. (Eds) Handbook of Analytical Techniques 2001. ISBN 3-527-30165-8 Electrochemistry in Nonaqueous Solutions. Kosuke Izutsu Copyright © 2002 Wiley-VCH Verlag GmbH & Co. KGaA ISBNs: 3-527-30516-5 (Hardback); 3-527-60065-5 (Electronic) K. Izutsu Electrochemistry in Nonaqueous Solutions Electrochemistry in Nonaqueous Solutions. Kosuke Izutsu Copyright © 2002 Wiley-VCH Verlag GmbH & Co. KGaA ISBNs: 3-527-30516-5 (Hardback); 3-527-60065-5 (Electronic) Professor Dr. K. Izutsu n This book was carefully produced. Nevertheless, 3-8-23 Motomachi author and publisher do not warrant the informa- Matsumoto 390-0803 tion contained therein to be free of errors. Rea- Japan ders are advised to keep in mind that statements, data, illustrations, procedural details or other items may inadvertently be inaccurate. Library of Congress Card No.: applied for British Library Cataloguing-in-Publication Data: A catalogue record for this book is available from the British Library. Die Deutsche Bibliothek – CIP-Cataloguing-in- Publication Data A catalogue record for this publication is available from Die Deutsche Bibliothek.
    [Show full text]
  • Solubility Table Lab #9
    Lower Merion High School Chemistry Solubility Table Lab #9 Not all reactions that we can write actually occur. For instance, carbon burns to form carbon dioxide. C + O2 Æ CO2 You could also write that carbon dioxide decomposes into carbon and oxygen CO2 ÆC + O2 but we don't expect to suddenly breathe out chunks of carbon. For some reactions we just have to assume that they will occur, but for double displacement reactions we can predict very accurately whether or not they will occur. Predicting Double Displacement Reactions Understanding double displacement reactions requires a mental picture of what is actually going on in the solutions. When an ionic compound dissolves, it breaks up into its ions. For instance sodium chloride dissolved in water is really a solution of sodium ions and chloride ions running around SEPARATELY in the solution. Reactions occur when ions that began in two different solutions get together and form a compound that does NOT have its ions separated. This can be an insoluble ionic compound, water, or a gas (such as H2S). An example: NaCl + AgNO3 ÆNaNO3 + AgCl Silver chloride is a white solid that does not dissolve in water. If you do this reaction, two clear liquids produce a white solid. What is really happening: + - + - + - Na + Cl + Ag + NO3 Æ Na + NO3 + AgCl The ions that make up AgCl are no longer separate. So...something has changed. A counter example: NaBr + KNO3 Æ NaNO3 + KBr is the same as: + - + - + - + - Na + Br + K + NO3 Æ Na + NO3 + K + Br Both products are soluble. Since everything on the right is identical to everything on the left, nothing has happened.
    [Show full text]