Introduction to General, Organic and Biochemistry 11th Edition
ISBN: 9781285869759
Author: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
1 Matter, Energy, And Measurement 2 Atoms 3 Chemical Bonds 4 Chemical Reactions 5 Gases, Liquids, And Solids 6 Solutions And Colloids 7 Reaction Rates And Chemical Equilibrium 8 Acids And Bases 9 Nuclear Chemistry 10 Organic Chemistry 11 Alkanes 12 Alkenes And Alkynes 13 Benzene And Its Derivatives 14 Alcohols, Ethers, And Thiols 15 Chirality: The Handedness Of Molecules 16 Amines 17 Aldehydes And Ketones 18 Carboxylic Acids 19 Carboxylic Anhydrides, Esters, And Amides 20 Carbohydrates 21 Lipids 22 Proteins 23 Enzymes 24 Chemical Communications: Neurotransmitters And Hormones 25 Nucleotides, Nucleic Acids, And Heredity 26 Gene Expression And Protein Synthesis 27 Bioenergetics: How The Body Converts Food To Energy 28 Specific Catabolic Pathways: Carbohydrate, Lipid, And Protein Metabolism 29 Biosynthetic Pathways 30 Nutrition 31 Immunochemistry Chapter8: Acids And Bases
8.1 What Are Acids And Bases? 8.2 How Do We Define The Strength Of Acids And Bases? 8.3 What Are Conjugate Acid.base Pairs? 8.4 How Can We Tell The Position Of Equilibrium In An Acid.base Reaction? 8.5 How Do We Use Acid Ionization Constants? 8.6 What Are The Properties Of Acids And Bases? 8.7 What Are The Acidic And Basic Properties Of Pure Water? 8.8 What Are Ph And Poh? 8.9 How Do We Use Titrations To Calculate Concentration? 8.10 What Are Buffers? 8.11 How Do We Calculate The Ph Of A Buffer? 8.12 What Are Tris, Hepes, And These Buffers With The Strange Names? Chapter Questions Section: Chapter Questions
Problem 8.13P: 8-13 Define (a) an Arrhenius acid and (b) an Arrhenius base. Problem 8.14P: 8-14 Write an equation for the reaction that takes place when each acid is added to water. (a) HNO3... Problem 8.15P: 8-15 Write an equation for the reaction that takes place when each base is added to water. (a) LiOH... Problem 8.16P: 8-16 For each of the following, tell whether the acid is strong or weak. (a) Acetic acid (b) HCI (c)... Problem 8.17P: 8-17 For each of the following, tell whether the base is strong or weak. (a) NaOH (b) Sodium acetate... Problem 8.18P: 8-18 Which of these acids are monoprotic, which are diprotic, and which are triprotic? Which are... Problem 8.19P: 8-19 Define (a) a Brønsted—Lowry acid and (b) a Brønsted—Lowry base. Problem 8.20P: 8-20 Write the formula for the conjugate base of each acid. (a) H2SO4 (b) H3BO3 (c) HI (d) H3O+ (e)... Problem 8.21P: 8-21 Write the formula for the conjugate base of each acid. (a) H2PO4- (b) H2S (c) HCO3- (d)... Problem 8.22P Problem 8.23P Problem 8.24P Problem 8.25P: 8-25 Draw the acid and base reactions for the amphiprotic ion HPO32-. Problem 8.26P Problem 8.27P Problem 8.28P: 8-28 Will carbon dioxide be evolved as a gas when sodium bicarbonate is added to an aqueous solution... Problem 8.29P Problem 8.30P Problem 8.31P Problem 8.32P Problem 8.33P: 8-33 Write an equation for the reaction of HCI with each compound. Which are acid—base reactions?... Problem 8.34P: 8-34 When a solution of sodium hydroxide is added to a solution of ammonium carbonate and then... Problem 8.35P: 8-35 Given the following values of [H3O+), calculate the corresponding value of [OH-] for each... Problem 8.36P: 8-36 Given the following values of [OH-], calculate the corresponding value of [H3O+] for each... Problem 8.37P: 8-37 What is the pH of each solution given the following values of [H3O+]? Which solutions are... Problem 8.38P: 8-38 What is the pH and pOH of each solution given the following values of [OH-)? Which solutions... Problem 8.39P: 8-39 What is the pH of each solution given the following values of [H3O+)? Which solutions are... Problem 8.40P Problem 8.41P: 8-41 What is the [OH-] and pOH of each solution? (a) 0.10 M KOH, (b) 0.10 M Na2CO3, (c) 0.10 M... Problem 8.42P Problem 8.43P: 8-43 What is the molarity of a solution made by dissolving 12.7 g of HCI in enough water to make... Problem 8.44P: 8-44 What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water to make... Problem 8.45P: 8-45 Describe how you would prepare each of the following solutions (in each case, assume that the... Problem 8.46P: 8-46 If 25.0 mL of an aqueous solution of H2SO4 requires 19.7 mL of 0.72 M NaOH to reach the end... Problem 8.47P: 8-47 A sample of 27.0 mL of 0.310 M NaOH is titrated with 0.740 M H2SO4. How many milliliters of the... Problem 8.48P: 8-48 A 0.300 M solution of H2SO4 was used to titrate 10.00 mL of NaOH; 15.00 mL of acid was required... Problem 8.49P: 8-49 A solution of NaOH base was titrated with 0.150 M HCI, and 22.0 mL of acid was needed to reach... Problem 8.50P: 8-50 The usual concentration of HCO3- ions in blood plasma is approximately 24 millimoles per liter... Problem 8.51P: 8-51 What is the end point of a titration? Problem 8.52P Problem 8.53P: 8-53 Write equations to show what happens when, to a buffer solution containing equimolar amounts of... Problem 8.54P: 8-54 Write equations to show what happens when, to a buffer solution containing equimolar amounts of... Problem 8.55P: 8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid... Problem 8.56P Problem 8.57P Problem 8.58P: 8-58 What is the connection between buffer action and Le Chatelier's principle? Problem 8.59P Problem 8.60P: 8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid? Problem 8.61P: 8-61 Can 100 of 0.1 M phosphate buffer at pH 7.2 act as an effective buffer against 20 mL of 1 M... Problem 8.62P: 8-62 What is the pH of a buffer solution made by dissolving 0.10 mol of formic acid, HCOOH, and 0.10... Problem 8.63P: 8-63 The pH of a solution made by dissolving 1.0 mol of propanoic acid and 1.0 mol of sodium... Problem 8.64P Problem 8.65P Problem 8.66P: 8-66 Calculate the pH of an aqueous solution containing the following: (a) 0.80 M lactic acid and... Problem 8.67P Problem 8.68P: 8-68 If you have 100 mL of a 0.1 M buffer made of NaH2PO4 and Na2HPO4 that is at pH 6.8 and you add... Problem 8.69P Problem 8.70P Problem 8.71P: 8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it. Problem 8.72P Problem 8.73P Problem 8.74P Problem 8.75P Problem 8.76P: 8-76 (Chemical Connections 8B) Name the most common bases used in over-the-counter antacids. Problem 8.77P Problem 8.78P Problem 8.79P: 8-79 (Chemical Connections 8D) Another form of the sprinter's trick is to drink a sodium bicarbonate... Problem 8.80P Problem 8.81P Problem 8.82P: 8-82 Assume that you have a dilute solution of HCI (0.10 M) and a concentrated solution of acetic... Problem 8.83P Problem 8.84P Problem 8.85P Problem 8.86P: 8-86 Following are three organic acids and the pKaof each: butanoic acid, 4.82; barbituric acid,... Problem 8.87P: 8-87 The pKavalue of barbituric acid is 5.0. If the H3O+ and barbiturate ion concentrations are each... Problem 8.88P Problem 8.89P Problem 8.90P Problem 8.91P Problem 8.92P Problem 8.93P: 8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to... Problem 8.94P: 8-94 Suppose you wish to make a buffer whose pH is 8.21. You have available 1 L of 0.100 M NaH2PO4... Problem 8.95P Problem 8.96P: 8-96 Suppose you want to make a CH3COOH/CH3COO- buffer solution with a pH of 5.60. The acetic acid... Problem 8.97P Problem 8.98P: 8-98 When a solution prepared by dissolving 4.00 g of an unknown monoprotic acid in 1.00 L of water... Problem 8.99P Problem 8.100P Problem 8.101P: 8-101 Suppose you have an aqueous solution prepared by dissolving 0.050 mol of NaH2PO4 in 1 L of... Problem 8.102P Problem 8.103P: 8-103 Suppose you have a phosphate buffer (H2PO4-/HPO42-) of pH 7.21. If you add more solid NaH2PO4... Problem 8.104P Problem 8.105P Problem 8.106P Problem 8.107P: 8-107 Following are pH ranges for several human biological materials. From the pH at the midpoint of... Problem 8.108P: 8-108 What is the ratio of HPO42-/H2PO4- in a phosphate buffer of pH 7.40 (the average pH of human... Problem 8.109P Problem 8.110P: 8-110 A concentrated hydrochloric acid solution contains 36.0% HCI (density 1.18 = g/mL). How many... Problem 8.111P: 8-111 The volume of an adult's stomach ranges from 50 mL when empty to 1 L when full. On a certain... Problem 8.112P: 8-112 Consider an initial 0.040 M hypobromous acid (HOBr) solution at a certain temperature. At... Problem 8.113P Problem 8.114P Problem 8.115P: 8-115 When a solution prepared by dissolving 0.125 g of an unknown diprotic acid in 25.0 mL of water... Problem 8.116P: 8-116 A railroad tank car derails and spills 26 tons of concentrated sulfuric acid (1 ton = 907.185... Problem 8.117P Problem 8.97P
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Transcribed Image Text: To which side are the following equilibria shifted? (Draw the appropriate arrows and state reasons):
CICH₂COOH + NH2-CH3
CICH₂COO + NH3-CH3
CH3COO- + Cl2CHCOOH
CH3COOH + Cl₂CHCOO-
CCl3COO- + Cl2CHCOOH
CC13COOH + Cl₂CHCOO-
Ph-OH + HCO3-
Ph-0- + HCO3-
Ph-0- + H₂CO3
Ph-OH + CO3²-
Branch of chemistry concerned with the study of carbon-based compounds, also known as organic compounds. These compounds form due to carbon's notable potential in forming chemical bonds. Due to the abundance of organic compounds on Earth, organic chemistry is crucial in other scientific disciplines, including materials science and pharmaceutical science.
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