Solutions for CHM 101 VOL 1 2014 >IC<
Problem 2E:
Aqueous solutions of three different substances, AX, AY, and AZ, are represented by the three...Problem 3E:
4 3 Use the molecular representations shown here to classify each compound as a noneleclrolyte, a...Problem 4E:
The concept of chemical equilibrium is very important Which one of the following statements is the...Problem 5E:
4 5 You are presented with a white solid and told that due to careless labeling it is not clear if...Problem 6E:
Which of the following ions will always be a spectator ion in a precipitation reaction? Cl- , NO3- ,...Problem 7E:
The labels have fallen off three bottles containing powdered samples of metals, one contains zinc,...Problem 8E:
Explain how a redox reaction involves electrons in the same way that a neutralization reaction...Problem 11E:
4.11 Which data set, of the two graphed here, would you expect to observe from a titration like...Problem 12E:
You are titrating an acidic solution with a basic one, and just realized you forgot to add the...Problem 13E:
State whether each of the following statements is true or false. Justify your answer in each case...Problem 14E:
State whether each of the following statements is true or false Justify your answer in each case...Problem 15E:
4.15 We have learned in this chapter that many ionic solids dissolve in water as strong...Problem 17E:
4.17 Specify what ions are present in solution upon dissolving each of the following substances in...Problem 20E:
Acetone. CH3COCH3, is a nonelectrolyte; hypochlorous acid. HClO, is a weak electrolyte. and ammonium...Problem 21E:
4.21 Using solubility guidelines, predict whether each of the following compounds is soluble or...Problem 25E:
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed?...Problem 26E:
Write balanced net ionic equations for the reactions that occur in each of the following cases....Problem 27E:
4.27 Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr,...Problem 33E:
State whether each of the following statements is true or false. Justify your answer in each case....Problem 34E:
State whether each of the following statements is true or false. Justify your answer in each case....Problem 35E:
4.35 Label each of the following substances as an acid, base, salt, or none of the above. Indicate...Problem 36E:
An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The...Problem 38E:
Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong...Problem 39E:
Complete and balance the following molecular equations, and then write the net ionic equation for...Problem 40E:
Write the balanced molecular and net ionic equations for each of the following neutralization...Problem 41E:
Write balanced molecular and net ionic equations for the following reactions, and identify the gas...Problem 42E:
4.42 Because the oxide ion is basic, metal oxides react readily with acids.
Write the net ionic...Problem 43E:
4.43 Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react...Problem 44E:
4.44 As K20 dissolves in water, the oxide ion reacts with water molecules to form hydroxide...Problem 45E:
True or false: If a substance is oxidized, it is gaining electrons. If an ion is oxidized, its...Problem 47E:
Which region of the periodic table shown here contains elements that are easiest to oxidize? Which...Problem 48E:
Determine the oxidation number of sulfur in each of the following substances: barium sulfate. BaSO4,...Problem 49E:
Determine the oxidation number for the indicated element in each of the following substances: Sin...Problem 50E:
Determine the oxidation number for the indicated element in each of the following compounds: Co in...Problem 51E:
Which element is oxidized, and which is reduced in the following reactions? N2(g) + 3 H2(g) 2...Problem 52E:
Which of the following are redox reactions? For those that are, indicate which element is oxidized...Problem 53E:
4.53 Write balanced molecular and net ionic equations for the reactions of
manganese with dilute...Problem 54E:
Write balanced molecular and net ionic equations for the reactions of hydrochloric acid with nickel,...Problem 55E:
Using the activity series (Table 4.5), write balanced chemical equations for the following...Problem 56E:
Using the activity series (Table 4.5), write balanced chemical equations for the following...Problem 57E:
The metal cadmium tends to form Cd2+ ions. The following observations are made: When a strip of zinc...Problem 58E:
4.58 The following reactions (note that the arrows are pointing only one direction) can be used to...Problem 59E:
Is the concentration of a solution an intensive or an extensive property? What is the difference...Problem 61E:
Calculate the molarity of a solution that contains 0.175 mol ZnC12 in exactly 150 mL of solution....Problem 62E:
4.62
Calculate the molarity of a solution made by dissolving 12.5 grams of Na2CrO4 in enough water...Problem 66E:
4.66 The average adult male has a total blood volume of 5.0 L. After drinking a few beers, he has a...Problem 67E:
4.67
How many grams of ethanol, CH2CH2OH should you dissolve in water to make 1.00 L of vodka...Problem 69E:
Which will have the highest concentration of potassium ion: 0.20 M KC1, 0.15 M K2CrO4, or 0.080 M...Problem 83E:
Some sulfuric acid is spilled on a lab bench You can neutralize the acid by sprinkling sodium...Problem 84E:
4.84 The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium...Problem 85E:
A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100 0 mL of water An acid-base...Problem 86E:
4.86 An 8.65-g sample of an unknown group 2A metal hydroxide is dissolved in 85.0 mL of water. An...Problem 87E:
A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. Write...Problem 88E:
4.88 A solution is made by mixing 15.0 g of Sr(OH)2 and 55.0 mL of 0.200 M HNO3.
Write a balanced...Problem 90E:
A 1.248-9 sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCI...Problem 91AE:
4.91 Uranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear...Problem 92AE:
The accompanying photo shows the reaction between a solution of Cd(NO3)2 and one of Na2S What is the...Problem 94AE:
4.94 You choose to investigate some of the solubility guidelines for two ions not listed in Table...Problem 95AE:
4 95 Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers...Problem 96AE:
4 96 The commercial production of nitric acid involves the following chemical reactions
4 NH3(g) +...Problem 97AE:
Consider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution,...Problem 98AE:
98 Bronze is a solid solution of Cu(s) and Sn(s); solutions of metals like this that are solids are...Problem 101AE:
4.101 Hard water contains Ca2+ , Mg2 + , and Fe2+ , which Interfere with the action of soap and...Problem 102AE:
Tartaric acid. H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and a salt...Problem 104AE:
A solid sample of Zn(OH)2 is added to 0.350 L of 0.500 M aqueous HBr. The solution that remains is...Browse All Chapters of This Textbook
Chapter 1 - Introduction: Matter, Energy, And MeasurementChapter 1.2 - Classifications Of MatterChapter 1.5 - Units Of MeasurementChapter 1.6 - Uncertainty In MeasurementChapter 1.7 - Dimensional AnalysisChapter 2 - Atoms, Molecules, And IonsChapter 2.3 - The Modern View Of Atomic StructureChapter 2.4 - Atomic WeightsChapter 2.5 - The Periodic TableChapter 2.6 - Molecules And Molecular Compounds
Chapter 2.7 - Ions And Ionic CompoundsChapter 2.8 - Naming Inorganic CompoundsChapter 2.9 - Some Simple Organic CompoundsChapter 3 - Chemical Reactions And Reaction StoichiometryChapter 3.1 - Chemical EquationsChapter 3.2 - Simple Patterns Of Chemical ReactivityChapter 3.3 - Formula WeightsChapter 3.4 - Avogadro's Number And The MoleChapter 3.5 - Empirical Formulas From AnalysesChapter 3.6 - Quantitative Information From Balanced EquationsChapter 3.7 - Limiting ReactantsChapter 4 - Reactions In Aqueous SolutionChapter 4.1 - General Properties Of Aqueous SolutionsChapter 4.2 - Precipitation ReactionsChapter 4.3 - Acids, Bases, And Neutralization ReactionsChapter 4.4 - Oxidation-reduction ReactionsChapter 4.5 - Concentrations Of SolutionsChapter 4.6 - Solutions Stoichiometry And Chemical AnalysisChapter 5 - ThermochemistryChapter 5.2 - The First Law Of ThermodynamicsChapter 5.3 - EnthalpyChapter 5.4 - Enthalpies Of ReactionChapter 5.5 - CalorimetryChapter 5.6 - Hess's LawChapter 5.7 - Enthalpies Of FormationChapter 5.8 - Bond EnthalpiesChapter 5.9 - Foods And FuelsChapter 6 - Electronic Structure Of AtomsChapter 6.1 - The Wave Nature Of LightChapter 6.2 - Quantized Energy And PhotonsChapter 6.3 - Line Spectra And The Bohr ModelChapter 6.4 - The Wave Behavior Of MatterChapter 6.5 - Quantum Mechanics And Atomic OrbitalsChapter 6.8 - Electron ConfigurationsChapter 6.9 - Electron Configurations And The Periodic TableChapter 7 - Periodic Properties Of The ElementsChapter 7.3 - Sizes Of Atoms And IonsChapter 7.4 - Ionization EnergyChapter 7.6 - Metals, Nonmetals, And MetalloidsChapter 7.7 - Trends Of Group 1a And Group 2a MetalsChapter 8 - Basic Concepts Of Chemical BondingChapter 8.2 - Ionic BondingChapter 8.3 - Covalent BondingChapter 8.4 - Bond Polarity And ElectronegativityChapter 8.5 - Drawing Lewis StructuresChapter 8.6 - Resonance StructuresChapter 8.7 - Exceptions Of The Octet RuleChapter 9 - Molecular Geometry And Bonding TheoriesChapter 9.2 - The Vsepr ModelChapter 9.3 - Molecular Shape And Molecular PolarityChapter 9.5 - Hybrid OrbitalsChapter 9.6 - Multiple BondsChapter 9.7 - Molecular OrbitalsChapter 9.8 - Bonding In Period 2 Diatomic MoleculesChapter 10 - GasesChapter 10.2 - PressureChapter 10.3 - The Gas LawsChapter 10.4 - The Ideal-gas EquationChapter 10.5 - Further Applications Of The Ideal-gas EquationChapter 10.6 - Gas Mixtures And Partial PressuresChapter 10.7 - The Kinetic-molecular Theory Of GasesChapter 10.8 - Molecular Effusion And DiffusionChapter 10.9 - Real Gases: Deviations From Ideal BehaviorChapter 11 - Liquids And Intermolecular ForcesChapter 11.2 - Intermolecular ForcesChapter 11.3 - Select Properties Of LiquidsChapter 11.4 - Phase ChangesChapter 11.5 - Vapor PressureChapter 11.6 - Phase DiagramChapter 11.7 - Liquid CrystalsChapter 12 - Solids And Modern MaterialsChapter 12.3 - Metallic SolidsChapter 12.5 - Ionic SolidChapter 12.7 - Covalent-network SolidsChapter 13 - Properties Of SolutionsChapter 13.3 - Factor Affecting SolubilityChapter 13.4 - Expressing Solution ConcentrationChapter 13.5 - Colligative PropertiesChapter 14 - Chemical KineticsChapter 14.2 - Reaction RatesChapter 14.3 - Concentration And Rate LawsChapter 14.4 - The Change Of Concentration With TimeChapter 14.5 - Temperature And RateChapter 14.6 - Reaction MechanismsChapter 15 - Chemical EquilibriumChapter 15.2 - The Equilibrium ConstantChapter 15.3 - Understanding And Working With Equilibrium ConstantChapter 15.4 - Heterogeneous EquilibriumChapter 15.5 - Calculating Equilibrium ConstantsChapter 15.6 - Applications Equilibrium ConstantsChapter 15.7 - Le Chatelier's PrincipleChapter 16 - Acid—base EquilibriumChapter 16.2 - Bronsted-lowery Acids And BasesChapter 16.3 - The Autoionization Of WaterChapter 16.4 - The Ph ScaleChapter 16.5 - Strong Acids And BasesChapter 16.6 - Weak AcidsChapter 16.7 - Weak BasesChapter 16.8 - Relation Between Ka And KbChapter 16.9 - Acid-base Properties Of Salt SolutionChapter 16.10 - Acid-base Behavior And Chemical StructureChapter 17 - Additional Aspects Of Aqueous EquilibriumChapter 17.1 - The Common Ion EffectChapter 17.2 - BuffersChapter 17.3 - Acid-base TitrationsChapter 17.4 - Solubility EquilibriaChapter 17.5 - Factor That Affect SolubilityChapter 17.6 - Precipitation And Separation Of IonsChapter 18 - Chemistry Of The EnvironmentChapter 18.1 - Earth's AtmosphereChapter 18.2 - Human Activities And Earth AtmosphereChapter 19 - Chemical ThermodynamicsChapter 19.1 - Spontaneous ProcessesChapter 19.2 - Entropy And Second Law Of ThermodynamicsChapter 19.3 - The Molecular Interpretation Of Entropy And The Third Law Of ThermodynamicsChapter 19.4 - Entropy Changes In Chemical ReactionsChapter 19.5 - Gibbs Free EnergyChapter 19.6 - Free Energy And TemperatureChapter 19.7 - Free Energy And Equilibrium ConstantChapter 20 - ElectrochemistryChapter 20.1 - Oxidation States And Oxidation-reduction ReactionsChapter 20.2 - Balancing Redox EquationsChapter 20.3 - Voltaic CellsChapter 20.4 - Cell Potentials Under Standard ConditionsChapter 20.5 - Free Energy And Redox ReactionsChapter 20.6 - Cell Potentials Under Nonstandard ConditionsChapter 20.9 - ElectrolysisChapter 21 - Nuclear ChemistryChapter 21.1 - Radioactivity And Nuclear EquationsChapter 21.2 - Patterns Of Nuclear StabilityChapter 21.3 - Nuclear TransmutationsChapter 21.4 - Rates Of Radioactive DecayChapter 21.6 - Energy Changes In Nuclear ReactionsChapter 22 - Chemistry Of The NonmetalsChapter 22.1 - Periodic Trends And Chemical ReactionsChapter 22.3 - Group 8a:the Noble GasesChapter 22.4 - Group 7a:the HalogensChapter 22.7 - NitrogenChapter 22.10 - The Other Group 4a:elements:si,ge,sn And PbChapter 23 - Transition Metals And Coordination ChemistryChapter 23.2 - Transition-metals ComplexesChapter 23.4 - Nomenclature And Isomerism In Coordination ChemistryChapter 23.5 - Color And Magnetism In Coordination ChemistryChapter 23.6 - Crystal-field TheoryChapter 24 - The Chemistry Of Life: Organic And Biological ChemistryChapter 24.2 - Introduction To HydrocarbonsChapter 24.3 - Alkenes,alkynes,and Aromatic HydrocarbonsChapter 24.4 - Organic Functional GroupsChapter 24.7 - Proteins
Sample Solutions for this Textbook
We offer sample solutions for CHM 101 VOL 1 2014 >IC< homework problems. See examples below:
The figure (i) represents the space filling molecular models of two spheres attached to each other...The sign of the electric charge on the particle is negative in the given diagram. This experiment...Chapter 3, Problem 1EGiven The three salts are named as sodium sulfide, sodium bicarbonate and sodium chloride. The...Chapter 5, Problem 1DEChapter 6, Problem 1DEThe alkali metals such as rubidium and cesium which has lower first ionization energies can be used...The heat of hydrogenation of acetylene is −1299.53 kJ/mol and the fuel value of 3.0 mol acetylene is...The energy absorbed by the given compound is calculated by the formula, Energy=Plank's...
The given unknown gas is a noble gas and the difference in molar masses of noble gases is much...The force of attraction between the hydrogen and an electronegative atom is called hydrogen bonding....Explanation: The given polymer is first dissolved in the buffer solution. The experiment is...According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole...Given The chemical equation for the given hypothetical reaction is, aA+bB→cC+dD The reactants...Explanation: The spectrometer is a device which splits light into the array of separate colors which...If the solution is acidic, it changes blue litmus paper into red and there is no change in color for...Explanation: The concentration of NaOH solution is calculated by considering the small volume of the...Explanation: The chemicals involved in fracking operations are hydrochloric acid, sodium chloride,...The relation between the standard free energy change, standard entropy change and standard enthalpy...GivenThe electrical potential output of the cell is 1.50 V . The external device draws the current...Explanation: Pitchblende is a uranium ore with excess amount of UO2 , on oxidation UO2 leads to the...The physical state of the substance depends upon the size of the substance. The size of the atoms...The reaction of the given coordination compound with the solution of AgNO3 solution gives the...Explanation: The buffer solution of hemoglobin is prepared first. This buffer solution of hemoglobin...
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