EBK BASIC CHEMISTRY5th EditionTimberlake Publisher: PEARSONISBN: 8220101472335
EBK BASIC CHEMISTRY
Solutions for EBK BASIC CHEMISTRY
Problem 1.2QAP:
Write a one-sentence definition for each of the following: chemistry chemical 1.2 Ask two of your...Problem 1.3QAP:
Obtain a bottle of multivitamins and read the list of ingredients. What are four chemicals from the...Browse All Chapters of This Textbook
Chapter 1 - Chemistry In Our LivesChapter 1.1 - Chemistry And ChemicalsChapter 1.2 - Scientific Method: Thinking Like A ScientistChapter 1.3 - Learning Chemistry: A Study PlanChapter 1.4 - Key Math Skills For ChemistryChapter 1.5 - Writing Numbers In Scientific NotationChapter 2 - Chemistry And MeasurementsChapter 2.1 - Units Of MeasurementChapter 2.2 - Measured Numbers And Significant FiguresChapter 2.3 - Significant Figures In Calculations
Chapter 2.4 - Prefixes And EqualitiesChapter 2.5 - Writing Conversion FactordChapter 2.6 - Problem Solving Using Unit ConversionChapter 2.7 - DensityChapter 3 - Matter And EnergyChapter 3.1 - Classification Of MatterChapter 3.2 - States And Properties Of MatterChapter 3.3 - TemperatureChapter 3.4 - EnergyChapter 3.5 - Specific HeatChapter 3.6 - Energy And NutritionChapter 4 - Atoms And ElementsChapter 4.1 - Elements And SymbolsChapter 4.2 - The Periodic TableChapter 4.3 - The AtomChapter 4.4 - Atomic Number And Mass NumberChapter 4.5 - Isotopes And Atomic MassChapter 5 - Electronic Structure Of Atoms And Periodic TrendsChapter 5.1 - Electromagnetic RadiationChapter 5.2 - Atomic Spectra And Energy LevelsChapter 5.3 - Sublevels And OrbitalsChapter 5.4 - Orbital Diagrams And Electron ConfigurationsChapter 5.5 - Electron Configurations And The Periodic TableChapter 5.6 - Trends In Periodic PropertiesChapter 6 - Ionic And Molecular CompoundsChapter 6.1 - Ions: Transfer Of ElectronsChapter 6.2 - Ionic CompoundsChapter 6.3 - Naming And Writing Ionic FormulasChapter 6.4 - Polyatomic IonsChapter 6.5 - Molecular Compounds: Sharing ElectronsChapter 7 - Chemical QuantitiesChapter 7.1 - The MoleChapter 7.2 - Molar MassChapter 7.3 - Calculations Using Molar MassChapter 7.4 - Mass Percent CompositionChapter 7.5 - Empirical FormulasChapter 7.6 - Molecular FormulasChapter 8 - Chemical ReactionsChapter 8.1 - Equations For Chemical ReactionsChapter 8.2 - Balancing A Chemical EquationChapter 8.3 - Types Of Chemical ReactionsChapter 8.4 - Oxidation–reduction ReactionsChapter 9 - Chemical Quantities In ReactionsChapter 9.1 - Conservation Of MassChapter 9.2 - Calculating Moles Using Mole–mole FactorsChapter 9.3 - Mass Calculations For ReactionsChapter 9.4 - Limiting ReactantsChapter 9.5 - Percent YieldChapter 9.6 - Energy In Chemical ReactionsChapter 10 - Bonding And Properties Of Solids And LiquidsChapter 10.1 - Lewis Structures For Molecules And Polyatomic IonsChapter 10.2 - Resonance StructuresChapter 10.3 - Shapes Of Molecules And Polyatomic Ions (vsepr Theory)Chapter 10.4 - Electronegativity And Bond PolarityChapter 10.5 - Polarity Of MoleculesChapter 10.6 - Intermolecular Forces Between Atoms Or MoleculesChapter 10.7 - Change Of StateChapter 11 - GasesChapter 11.1 - Properties Of GasesChapter 11.2 - Pressure And Volume (boyle's Law)Chapter 11.3 - Temperature And Volume (charles's Law)Chapter 11.4 - Temperature And Pressure (gay-lussac's)Chapter 11.5 - The Combined Gas LawChapter 11.6 - Volume And Moles (avogadro's Law)Chapter 11.7 - The Ideal Gas LawChapter 11.8 - Gas Laws And Chemical ReactionsChapter 11.9 - Partial Pressures (dalton's Law )Chapter 12 - SolutionsChapter 12.1 - SolutionsChapter 12.2 - Electrolytes And NonelectrolytesChapter 12.3 - SolubilityChapter 12.4 - Solution ConcentrationsChapter 12.5 - Dilution Of SolutionsChapter 12.6 - Chemical Reactions In SolutioonsChapter 12.7 - Molality And Freezing Point Lowering/
boiling Point ElevationChapter 12.8 - Properties Of Solutions: OsmosisChapter 13 - Reaction Rates And Chemical EquilibriumChapter 13.1 - Rates Of ReactionsChapter 13.2 - Chemical EquilibriumChapter 13.3 - Equilibrium ConstantsChapter 13.4 - Using Equilibrium ConstantsChapter 13.5 - Changing Equilibrium Conditions Le Chatelier's PrincipleChapter 13.6 - Equilibrium In Saturated SolutionsChapter 14 - Acids And BasesChapter 14.1 - Acids And BasesChapter 14.2 - Brønsted–lowry Acids And BasesChapter 14.3 - Strengths Of Acids And BasesChapter 14.4 - Dissociation Constants For Acids And BasesChapter 14.5 - Dissociation Of WaterChapter 14.6 - The Ph ScaleChapter 14.7 - Reactions Of Acids And BasesChapter 14.8 - Acids-base TitrationChapter 14.9 - BuffersChapter 15 - Oxidation And ReductionChapter 15.1 - Oxidation And ReductionChapter 15.2 - Balancing Oxidation–reduction Equations Using Half-reactionsChapter 15.3 - Electrical Energy From Oxidation– Reduction ReactionsChapter 15.4 - Oxidation–reduction Reactions That Require Electrical EnergyChapter 16 - Nuclear ChemistryChapter 16.1 - Natural RadioactivityChapter 16.2 - Nuclear ReactionsChapter 16.3 - Radiation MeasurementChapter 16.4 - Half-life Of A RadioisotopeChapter 16.5 - Medical Applications Using RadioactivityChapter 16.6 - Nuclear Fission And FusionChapter 17 - Organic ChemistryChapter 17.1 - AlkanesChapter 17.2 - Alkenes, Alkynes, And PolymersChapter 17.3 - Aromatic CompoundsChapter 17.4 - Alcohols And EthersChapter 17.5 - Aldehydes And KetonesChapter 17.6 - Carboxylic Acids And EstersChapter 17.7 - Amines And AmidesChapter 18 - BiochemistryChapter 18.1 - CarbohydratesChapter 18.2 - Disaccharides And PolysaccharidesChapter 18.3 - LipidsChapter 18.4 - Amino Acids And ProteinsChapter 18.5 - Protein StructureChapter 18.6 - Proteins As EnzymesChapter 18.7 - Nucleic AcidsChapter 18.8 - Protein Synthesis
Book Details
For courses in introductory, preparatory, and basic chemistry. Engages First Time Chemistry Students Basic Chemistry introduces students to the essential scientific and mathematical concepts of general chemistry. With accessible language and a moderate
Sample Solutions for this Textbook
We offer sample solutions for EBK BASIC CHEMISTRY homework problems. See examples below:
According to question: Mass of ethylene glycol = 120 g Mass of liquid = 450 g Therefore, percentage...During the doctor visit of Person G; he complained about feeling tired. The blood test showed the...Breakfast: Food consumed and the corresponding energy value: 1 Banana = 110 kcal 1 cup non-fat milk...The group number of an element is determined by the number of its valence electrons. The electron...For a neutral atom, the number of protons is always equal to the number of electrons. The number of...Magnesium is a second group element belonging to the alkaline earth metal family. To obtain stable...Atomic mass of C = 12 g/mol Atomic mass of H = 1 g/mol Atomic mass of N = 7 g/mol Atomic mass of O =...The chemical reaction that takes place during cellular respiration is the combustion of glucose to...Given: Mass of naphthol = 2.2 x 102 kg Molar mass of naphthol = 144.17 g/mol Equality: 1 kg = 1000 g...
The mass of the nitrogen gas is 15.8 g. The amount of heat required to vaporize 1 g of the nitrogen...As per the ideal gas equation: PV = nRT -(1)P = pressure ; V = volume n = number of moles = m...The stock solution is 2.5% mass by volume. This means 2.5 g of chlorpromazine is present in 100 mL...For the dissociation of slightly soluble compounds, there exists equilibrium between dissolved and...Given: [H3O+] = 2.0 × 10-4 M pH is a logarithmic scale which specify the acidity or basicity of the...Given information: The reaction between hydrogen gas and oxygen gas results in the formation of...The activity of the radioactive dye injection for Simone is 74MBq 1Ci = 37000 MBq 74MBq ×1Ci37000...Polychlorotrifluoroethylene, PCTFE, is a polymer in nature, made up from the chlorotrifluoroethylene...Given information: The Rebecca’s prescription for Pravachol was 80 mg daily. Equality factors are: 1...
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