Chemistry & Chemical Reactivity 9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
1 Basic Concepts Of Chemistry 2 Atoms Molecules And Ions 3 Chemical Reactions 4 Stoichiometry: Quantitative Information About Chemical Reactions 5 Principles Of Chemical Reactivity: Energy And Chemical Reactions 6 The Structure Of Atoms 7 The Structure Of Atoms And Periodic Trends 8 Bonding And Molecular Structure 9 Bonding And Molecular Structure: Orbital Hybridization And Molecular Orbitals 10 Gases And Their Properties 11 Intermolecular Forces And Liquids 12 The Solid State 13 Solutions And Their Behavior 14 Chemical Kinetics: The Rates Of Chemical Reactions 15 Principles Of Chemical Reactivity: Equilibria 16 Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases 17 Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria 18 Principles Of Chemical Reactivity: Entropy And Free Energy 19 Principles Of Chemical Reactivity: Electron Transfer Reactions 20 Environmental Chemistry-earth's Environment, Energy, And Sustainability 21 The Chemistry Of The Main Group Elements 22 The Chemistry Of The Transistion Elements 23 Carbon: Not Just Another Element 24 Biochemistry 25 Nuclear Chemistry L Let's Review Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases
16.1 The Bronsted-lowry Concept Of Acids And Bases 16.2 Water And Ph Scale 16.3 Equilibrium Constants For Acids And Bases 16.4 Acid-base Properties Of Salts 16.5 Predicting The Direction Of Acid-base Reactions 16.6 Types Of Acid-base Reactions 16.7 Calculations With Equilibrium Constants 16.8 Polyprotic Acids And Bases 16.9 Molecular Structure, Bonding And Acid-base Behavior 16.10 The Lewis Concept Of Acids And Bases Chapter Questions Section: Chapter Questions
Problem 1PS: Write the formula and the give the name of the conjugate base of each of the following acids. a) HCN... Problem 2PS: Write the formula and give the name of the conjugate base of each of the following acids. a) NH3 b)... Problem 3PS: What are the products of each of the following acid-base reactions? Indicate the acid and its... Problem 4PS: What are the products of each of the following acid-base reactions? Indicate the acid and its... Problem 5PS: Write balanced equations showing how the hydrogen oxalate ion, HC2O4, can be both a Bronsted acid... Problem 6PS: Write a balanced equation showing how the HPO42 ion of sodium hydrogen phosphate Na2HPO4 can be a... Problem 7PS: In each of the following acid-base reactions, identify the Brnsted acid and base on the left and... Problem 8PS: In each of the following acid-base reactions, identify the Brnsted acid and base on the left and... Problem 9PS: An aqueous solution has a pH of 3.75. What is the hydronium ion concentration of the solution? Is it... Problem 10PS: A saturated solution of milk of magnesia. Mg(OH)2, has a pH of 10.52. What is the hydronium ion... Problem 11PS: What is the pH of a 0.0075 M solution of HCl? What is the hydroxide ion concentration of the... Problem 12PS: What is the pH of a 1.2 104 M solution of KOH? What is the hydronium ion concentration of the... Problem 13PS: What is the pH of a 0.0015 M solution of Ba(OH)2? Problem 14PS: The pH of a solution of Ba(OH)2 is 10.66 at 25 . What is the hydroxide ion concentration in the... Problem 15PS: Several acids are listed here with their respective equilibrium constants: C6H5OH(aq) + H2O() ... Problem 16PS: Several acids are listed here with their respective equilibrium constants: HF(aq) + H2O() H3O+(aq)... Problem 17PS: Which of the following ions or compounds has the strongest conjugate base? Briefly explain your... Problem 18PS: Which of the following compounds or ions has the weakest conjugate base? Briefly explain your... Problem 19PS: Which of the following compounds or ions has the weakest conjugate acid? Briefly explain your... Problem 20PS: Which of the following compounds or ion has the strongest conjugate acid? Briefly explain your... Problem 21PS: Dissolving K2CO3 in water gives a basic solution. Rite a balanced equation showing how this can... Problem 22PS: Dissolving ammonium bromide in water gives an acidic solution. Write a balanced equation showing... Problem 23PS: If each of the salts listed here were dissolved in water to give 0.10M solution, which solution... Problem 24PS: Which of the following common food additives gives a basic solution when dissolved in water? (a)... Problem 25PS Problem 26PS Problem 27PS Problem 28PS: An organic acid has pKa = 8.95. What is its Ka value? Where does the acid fit in Table 16.2? TABLE... Problem 29PS Problem 30PS: Which is the stronger of the following two acids? (a) acetic acid, CH3CO2H, Ka = 1.8 105 (b)... Problem 31PS: Chloroacetic acid (ClCH2CO2H) has Ka = 1.41 103. What is the value of Kb for the chloroacetate ion... Problem 32PS: A weak base has Kb = 1.5 109. What is the value of Ka for the conjugate acid? Problem 33PS: The trimethylammonium ion, (CH3)3NH+, is the conjugate acid of the weak base trimethylamine,... Problem 34PS: The chromium(III) ion in water, [Cr(H2O)6]3+. Is a weak acid with pKa = 3.95. What is the value of... Problem 35PS: Acetic acid and sodium hydrogen carbonate, NaHCO3, are mixed in water. Write a balanced equation for... Problem 36PS: Ammonium chloride and sodium dihydrogen phosphate, NaH2PO4, are mixed in water. Write a balanced... Problem 37PS: For each of the following reactions, predict whether the equilibrium lies predominantly to the left... Problem 38PS: For each of the following reactions, predict whether the equilibrium lies predominantly to the left... Problem 39PS: Equal molar quantities of sodium hydroxide and sodium hydrogen phosphate (Na2HPO4) are mixed. (a)... Problem 40PS: Equal molar quantities of hydrochloric acid and sodium hypochlorite (NaClO) are mixed. (a) Write the... Problem 41PS: Equal molar quantities of acetic acid and sodium hydrogen phosphate (Na2HPO4) are mixed. (a) Write a... Problem 42PS: Equal molar quantities of ammonia and sodium dihydrogen phosphate (NaH2PO4) are mixed. (a) Write a... Problem 43PS: A 0.015 M solution of hydrogen cyanate, HOCN, has a pH of 2.67. (a) What is the hydronium ion... Problem 44PS: A 0.10 M solution of chloroacetic acid, CICH2CO2H, has a pH of 1.95. Calculate Ka for the acid. Problem 45PS: A 0.025 M solution of hydroxyl amine has a pH of 9.11. What is the value of Kb for this weak base?... Problem 46PS: Methylamine, CH3NH2, is a weak base. CH3NH2(aq) + H2O() CH3NH3+(aq) + OH(aq) If the pH of a 0.065 M... Problem 47PS: A 2.5 103 M solution of an unknown acid has a pH of 3.80 at 25 C. (a) What is the hydronium ion... Problem 48PS: A 0.015M solution of a base has a pH of 10.09 a) What are the hydronium and hydroxide ion... Problem 49PS: What are the equilibrium concentrations of hydronium ion, acetate ion and acetic acid in a 0.20 M... Problem 50PS: The ionizations constant of a very weak acid, HA is 4.0109.Calculate the equilibrium concentrations... Problem 51PS: What are the equilibrium concentration of H3O+, CN and HCN in a 0.025 M solution of HCN? What is the... Problem 52PS: Phenol (C6H5OH) commonly called carbolic acid is a weak organic acid... Problem 53PS: What are the equilibrium concentrations of NH3,NH4+ and OH in a 0.15M solution of ammonia? What is... Problem 54PS: A hypothetical weak base has Kb=5.0104.Calculate the equilibrium concentrations of the base, its... Problem 55PS: The weak base methylamine, CH3NH2, has Kb=4.2104. It reacts with water according to the equation.... Problem 56PS: Calculate the pH of a 0.12 M aqueous solution of the base aniline, C6H5NH2(Kb=4.01010).... Problem 57PS: Calculate the pH of a 0.0010 M aqueous solution of HF. Problem 58PS: A solution of hydrofluoric acid, HF, has a pH of 2.30. Calculate the equilibrium concentration of... Problem 59PS: Calculate the hydronium ion concentration and pH in a 0.20 M solution of ammonium chloride NH4Cl. Problem 60PS: Calculate the hydronium ion concentration and pH for a 0.015M solution of sodium formate NaHCO3. Problem 61PS: Sodium cyanide is the salt of the weak acid HCN. Calculate the concentrations of H3O+,OH,HCN and Na+... Problem 62PS: The sodium salt of propionic acid, NaCH3CH2CO2 is used as an antifungal agent by veterinarians.... Problem 63PS: Calculate the hydronium ion concentration and pH of the solution that results when 22.0mL of 0.15M... Problem 64PS: Calculate the hydronium ion concentration and the pH when 50.0mL of 0.40M NH3 is mixed with 50.0mL... Problem 65PS: For each of the following cases, decide whether the pH is less than 7 equal to 7 or greater than 7.... Problem 66PS: For each of the following cases, decide whether the pH is less than 7, equal to 7 or greater than 7.... Problem 67PS: Oxalic acid, H2C2O4, is a diprotic acid. Write a chemical equilibrium expression for each ionization... Problem 68PS: Sodium carbonate is a diprotic base. Write a chemical equilibrium expression for each of the two... Problem 69PS: Prove that Ka1 Kb2 = Kw for oxalic acid H2C2O4, by adding the chemical equilibrium expressions that... Problem 70PS: Prove that Ka3 Kb1 = Kw for phosphoric acid, H3PO4, by adding the chemical equilibrium expressions... Problem 71PS: Sulphurous acid, H2SO3, is a weak acid capable of providing two H+ ions. (a) What is the pH of a... Problem 72PS: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 6.8 105 and Ka2 = 2.7 1012). What is... Problem 73PS: Hydrazine, N2H4, can interact with water in two steps. N2H4(aq) + H2O() N2H5+(aq) + OH(aq) Kb1 =... Problem 74PS: Ethylene diamine, H2NCH2CH2NH2, can interact with water in two steps, forming OH in each step... Problem 75PS: Which should be stronger acid, HOCN or HCN? Explain briefly. (In HOCN, the H+ ion is attached to the... Problem 76PS Problem 77PS: Explain why benzene sulfonic acid is a Brnsted acid. Problem 78PS: The structure of ethylene diamine is illustrated in study question 76. Is this compound a Brnsted... Problem 79PS: Decide whether each of the following substances should be classified as a Lewis acid or a Lewis... Problem 80PS: Decide whether each of the following substances should be classified as a Lewis acid or a Lewis... Problem 81PS: Carbon monoxide forms complexes with low-valent metals. For example, Ni(CO)4 and Fe(CO)5 are well... Problem 82PS: Trimethylamine, (CH3)3N, is a common reagent. It interacts readily with diborane gas, B2H6. The... Problem 83GQ: About this time, you may be wishing you had an aspirin. Aspirin is an organic acid with a Ka of 3.27... Problem 84GQ: Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an... Problem 85GQ: A 2.50 g sample of a solid that could be Ba(OH)2 or Sr(OH)2 was dissolved in enough water to make... Problem 86GQ: In a particular solution, acetic acid is 11% ionized at 25 C. Calculate the pH of the solution and... Problem 87GQ: Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced... Problem 88GQ: For each of the following reactions predict whether the equilibrium lies predominantly to the left... Problem 89GQ: A monoprotic acid HX has Ka = 1.3 103. Calculate the equilibrium concentration of HX and H3O+ and... Problem 90GQ: Arrange the following 0.10M solutions in order of increasing pH. (a) NaCl (b) NH4Cl (c) HCl (d)... Problem 91GQ: m-Nitrophenol, a weak acid, can be used as a pH indicator because it is yellow at pH above 8.6 and... Problem 92GQ: The butylammonium ion, C4H9NH3+, has a Ka of 2.3 1011. C4H9NH3+(aq) + H2O() H3O+(aq) + C4H9NH2(aq)... Problem 93GQ: The local anaesthetic novocaine is the hydrogen chloride salt of an organic base, procaine.... Problem 94GQ: Pyridine is weak organic base and readily forms a salt with hydrochloric acid.... Problem 95GQ: The base ethylamine (CH3CH2NH2) has a Kb of. A closely related base, ethanolamine(HOCH2CH2NH2), has... Problem 96GQ: Chloroacetic acid, ClCH2CO2H, is a moderately weak acid (Ka=1.40103). If you dissolve 94.5 mg of the... Problem 97GQ: Saccharin (HC7H4NO3S) is a weak acid with pKa = 2.32 at 25 C. It is used in the form of sodium... Problem 98GQ: Given the following solutions: (a) 0.1 M NH3 (b) 0.1 M Na2CO3 (c) 0.1 M NaCl (d) 0.1 M CH3CO2H (e)... Problem 99GQ: For each of the following salts, predict whether a 0.10 M solution has a pH less than, equal to, or... Problem 100GQ: Nicotine, C10H14N2, has two basic nitrogen atoms (Figure 16.12), and both can react with water.... Problem 101GQ Problem 102GQ: The equilibrium constant for the reaction of hydrochloric acid and ammonia is 1.8 109 (page 726).... Problem 103GQ: The equilibrium constant for the reaction of formic acid and sodium hydroxide is 1.8 1010 (page... Problem 104GQ: Calculate the pH of the solution that results from mixing 25.0 mL of 0.14 M formic acid and 50.0 mL... Problem 105GQ: To what volume should 1.00 102 mL of any weak acid, HA, with a concentration 0.20 M be diluted to... Problem 106GQ: The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106.... Problem 107GQ Problem 108GQ Problem 109IL Problem 110IL Problem 111IL Problem 112IL: A hydrogen atom in the organic base pyridine, C5H5N, can be substituted by various atoms or groups... Problem 113IL: Nicotinic acid, C6H5NO2, is found in minute amounts in all living cells, hut appreciable amounts... Problem 114IL Problem 115IL: Sulfanilic acid, which is used in making dyes, is made by reacting aniline with sulfuric acid. (a)... Problem 116IL: Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H)... Problem 117SCQ: How can water be both a Brnsied base and a Lewis base? Can water be a Brnsted acid? A Lewis acid? Problem 118SCQ: The nickel(II) ion exists as [Ni(H2O)4]2+ in aqueous solution. Why is this solution acidic? As part... Problem 119SCQ: The halogens form three stable, weak acids, HOX. (a) Which is the strongest of these acids? (b)... Problem 120SCQ: The acidity of the oxoacids was described in Section 16.9, and a larger number of acids are listed... Problem 121SCQ: Perchloric acid behaves as an acid, even when it is dissolved in sulfuric acid. (a) Write a balanced... Problem 122SCQ: You purchase a bottle of water. On checking its pH, you find that it is not neutral, as you might... Problem 123SCQ Problem 124SCQ Problem 125SCQ Problem 127SCQ: Consider a salt of a weak base and a weak acid such as ammonium cyanide. Both the NH4+ and CN ions... Problem 110IL
Related questions
Concept explainers
22- The RMN spectra of the two isomers of formula C10H14 are shown in problems 22a and 22b. Do not attempt to interpret the aromatic proton region between 7.1 and 7.3 ppm, except to determine the number of protons bound to the aromatic ring. Draw the structures of the isomers.
note: point out the structures on the chart for better understanding
Transcribed Image Text: 162 I INTRODUÇÃO À ESPECTROSCOPIA
C10H14
5,10
75
2,14
2,06
2.06
2,98
3.5
30
25
20
15
(b)
Transcribed Image Text: *22. Os espectros de RMN dos dois compostos isoméricos com fórmula C,H, são apresenta-
dos nos Problemas 22a e 22b. Não tente interpřêtar a região de prótons aromáticos entre
7,1 e 7,3 ppm, exceto para determinar o número de prótons ligados ao anel aromático.
Desenhe as estruturas dos isômeros.
114
C10H14
5,10
7,5
7,0
1,10
2,15
3,04
2,94
4,0
3,5
30
25
2,0
13
0,3
Definition Definition Organic compounds with a planar cyclic ring of atoms bonded through alternated single and double bonds. Aromatic organic compounds, also called arenes, are an important class of hydrocarbons under the branch of organic chemistry.
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