Chemistry 10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
1 Chemical Foundations 2 Atoms, Molecules, And Ions 3 Stoichiometry 4 Types Of Chemical Reactions And Solution Stoichiometry 5 Gases 6 Thermochemistry 7 Atomic Structure And Periodicity 8 Bonding: General Concepts 9 Covalent Bonding: Orbitals 10 Liquids And Solids 11 Properties Of Solutions 12 Chemical Kinetics 13 Chemical Equilibrium 14 Acids And Bases 15 Acid-base Equilibria 16 Solubility And Complex Ion Equilibria 17 Spontaneity, Entropy, And Free Energy 18 Electrochemistry 19 The Nucleus: A Chemist's View 20 The Representative Elements 21 Transition Metals And Coordination Chemistry 22 Organic And Biological Molecules Chapter14: Acids And Bases
Chapter Questions Section: Chapter Questions
Problem 1RQ: Define each of the following: a. Arrhenius acid b. BronstedLowry acid c. Lewis acid Which of the... Problem 2RQ: Define or illustrate the meaning of the following terms: a. Ka reaction b. Ka equilibrium constant... Problem 3RQ: Define or illustrate the meaning of the following terms: a. amphoteric b. Kw reaction c. Kw... Problem 4RQ: How is acid strength related to the value of Ka? What is the difference between strong acids and... Problem 5RQ: Two strategies are followed when solving for the pH of an acid in water. What is the strategy for... Problem 6RQ: Two strategies are also followed when solving for the pH of a base in water. What is the strategy... Problem 7RQ: Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a... Problem 8RQ: For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in... Problem 9RQ: What is a salt? List some anions that behave as weak bases in water. List some anions that have no... Problem 10RQ: For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen... Problem 1ALQ: Consider two beakers of pure water at different temperatures. How do their pH values compare? Which... Problem 2ALQ: Differentiate between the terms strength and concentration as they apply to acids and bases. When is... Problem 3ALQ: Sketch two graphs: (a) percent dissociation for weak acid HA versus the initial concentration of HA... Problem 4ALQ: Consider a solution prepared by mixing a weak acid HA and HCl. What are the major species? Explain... Problem 5ALQ Problem 6ALQ: Consider two separate aqueous solutions: one of a weak acid HA and one of HCl. Assuming you started... Problem 7ALQ: You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide... Problem 8ALQ: Consider a solution prepared by mixing a weak acid HA. HCl, and NaA. Which of the following... Problem 9ALQ: Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA.... Problem 10ALQ: A certain sodium compound is dissolved in water to liberate Na+ ions and a certain negative ion.... Problem 11ALQ: Acids and bases can be thought of as chemical opposites (acids are proton donors, and bases are... Problem 13ALQ: You mix a solution of a strong acid with a pH = 4.0 and an equal volume of another strong acid... Problem 14ALQ: Consider two solutions of the salts NaX(aq) and NaY(aq) at equal concentrations. What would you need... Problem 15ALQ: What is meant by pH? True or false: A strong acid solution always has a lower pH than a weak acid... Problem 16ALQ: Why is the pH of water at 25C equal to 7.00? Problem 17ALQ: Can the pH of a solution be negative? Explain. Problem 18ALQ: Is the conjugate base of a weak acid a strong base? Explain. Explain why Cl does not affect the pH... Problem 19ALQ: Match the following pH values: 1, 2, 5, 6, 6.5, 8, 11, 11, and 13 with the following chemicals (of... Problem 20ALQ: The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be... Problem 21Q: Anions containing hydrogen (for example, HCO3 and H2PO4) usually show amphoteric behavior. Write... Problem 22Q: Which of the following conditions indicate an acidic solution at 25C? a. pH = 3.04 b. [H+] 1.0 107... Problem 23Q: Which of the following conditions indicate a basic solution at 25C? a. pOH = 11.21 b. pH = 9.42 c.... Problem 24Q: Why is H3O+ the strongest acid and OH the strongest base that can exist in significant amounts in... Problem 25Q: How many significant figures are there in the following numbers: 10.78, 6.78, 0.78? If these were pH... Problem 26Q: In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act... Problem 27Q: Consider the autoionization of liquid ammonia: Label each of the species in the equation as an acid... Problem 28Q: The following are representations of acidbase reactions: a. Label each of the species in both... Problem 29Q: Give three example solutions that fit each of the following descriptions. a. a strong electrolyte... Problem 30Q Problem 31Q: Consider the following statements. Write out an example reaction and K expression that is associated... Problem 32Q: The structures of adrenaline and aspirin are shown below: Label adrenaline and aspirin as a weak... Problem 33Q: Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups.... Problem 34Q: Which of the following statements is(are) true? Correct the false statements. a. When a base is... Problem 35Q: Consider the following mathematical expressions. a. [H+] = [HA]0 b. [H+] = (Ka [HA]0)1/2 c. [OH] =... Problem 36Q: Consider a 0.10-M H2CO3 solution and a 0.10-M H2SO4 solution. Without doing any detailed... Problem 37Q: Of the hydrogen halides, only HF is a weak acid. Give a possible explanation. Problem 38Q: Explain why the following are done, both of which are related to acidbase chemistry. a. Power plants... Problem 39E: Write balanced equations that describe the following reactions, a. the dissociation of perchloric... Problem 40E: Write the dissociation reaction and the corresponding Ka equilibrium expression for each of the... Problem 41E: For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and... Problem 42E: For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and... Problem 43E: Classify each of the following as a strong acid or a weak acid. Problem 44E: Consider the following illustrations: Which beaker best illustrates what happens when the following... Problem 45E: Use Table 13-2 to order the following from the strongest to the weakest acid. HClO2,H2O,NH4+,HClO4 Problem 46E: Use Table 13-2 to order the following from the strongest to the weakest base. ClO2,H2O,NH3,ClO4 Problem 47E: You may need Table 13-2 to answer the following questions. a. Which is the stronger acid, HCl or... Problem 48E: You may need Table 13-2 to answer the following questions. a. Which is the stronger base, Cl or H2O?... Problem 49E: Calculate the [OH] of each of the following solutions at 25C. Identify each solution as neutral,... Problem 50E: Calculate the [H+] of each of the following solutions at 25C. Identity each solution as neutral,... Problem 51E: Values of Kw as a function of temperature are as follows: Temperature(C) Kw 0 1.14 1015 25 1.00 ... Problem 52E: At 40.C the value of Kw is 2.92 1014. a. Calculate the [H+] and [OH] in pure water at 40.C. b. What... Problem 53E: Calculate [H+] and [OH] for each solution at 25C. Identify each solution as neutral, acidic, or... Problem 54E: Fill in the missing information in the following table. Problem 55E: The pH of a sample of gastric juice in a persons stomach is 2.1. Calculate the pOH, [H+], and [OH]... Problem 56E: An antacid purchased at a local drug store has a pOH of 2.3. Calculate the pH, [H], and [OH] of this... Problem 57E: What are the major species present in 0.250 M solutions of each of the following acids? Calculate... Problem 58E: A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H+I and... Problem 59E: Calculate the pH of each of the following solutions of a strong acid in water. a. 0.10 M HCl b. 5.0... Problem 60E: Calculate the pH of each of the following solutions containing a strong acid in water. a. 2.0 102 M... Problem 61E: Calculate the concentration of an aqueous HBr solution that has pH = 4.25. HBr is a strong acid. Problem 63E: How would you prepare 1600 mL of a pH = 1.50 solution using concentrated (12 M) HCl? Problem 64E: A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated... Problem 65E: What are the major species present in 0.250 M solutions of each of the following acids? Calculate... Problem 66E: What are the major species present in 0.250 M solutions of each of the following acids? Calculate... Problem 67E: Calculate the concentration of all species present and the pH of a 0.020-M HF solution. Problem 68E: Monochloroacetic acid, HC2H2ClO2, is a skin irritant that is used in chemical peels intended to... Problem 69E: For propanoic acid (HC3H5O2, Ka = 1.3 105), determine the concentration of all species present, the... Problem 70E: A solution is prepared by dissolving 0.56 g benzoic acid (C6H5CO2H, Ka = 6.4 105) in enough water... Problem 71E: A typical aspirin tablet contains 325 mg acetylsalicylic acid (HC9H7O4). Calculate the pH of a... Problem 74E: A solution contains a mixture of acids: 0.50 M HA (Ka = 1 103), 0.20 M HB (Ka = 1.0 1010), and... Problem 75E: Calculate the percent dissociation of the acid in each of the following solutions. a. 0.50 M acetic... Problem 76E: Calculate the percent dissociation for a 0.22-M solution of chlorous acid (HClO2, Ka = 1.2 102). Problem 77E: A 0.15-M solution of a weak acid is 3.0% dissociated. Calculate Ka. Problem 78E: A 1.0 102 -M solution of cyanic acid (HOCN) is 17% dissociated. Calculate Ka for cyanic acid. Problem 79E: Trichloroacetic acid (CCl3CO2H) is a corrosive acid that is used to precipitate proteins. The pH of... Problem 80E: The pH of a 0.063-M solution of hypobromous acid (HOBr but usually written HBrO) is 4.95. Calculate... Problem 81E: A solution of formic acid (HCOOH, Ka = 1.8 104) has a pH of 2.70. Calculate the initial... Problem 82E: A typical sample of vinegar has a pH of 3.0. Assuming that vinegar is only an aqueous solution of... Problem 83E: One mole of a weak acid HA was dissolved in 2.0 L of solution. After the system had come to... Problem 84E: An acid HX is 25% dissociated in water. If the equilibrium concentration of HX is 0.30 M, calculate... Problem 85E: Write the reaction and the corresponding Kb equilibrium expression for each of the following... Problem 86E: Write the reaction and the corresponding Kb equilibrium expression for each of the following... Problem 87E: Use Table 13-3 to help order the following acids from strongest to weakest. HNO3,H2O,NH4+,C5H5NH+ Problem 88E: Use Table 13-3 to help answer the following questions. a. Which is the stronger base, ClO4 or... Problem 89E: Calculate the pH of the following solutions. a. 0.10 M NaOH b. 1.0 1010 M NaOH c. 2.0 M NaOH Problem 90E: Calculate [OH], pOH, and pH for each of the following. a. 0.00040 M Ca(OH)2 b. a solution containing... Problem 91E: What are the major species present in 0.015 M solutions of each of the following bases? a. KOH b.... Problem 92E: What are the major species present in the following mixtures of bases? a. 0.050 M NaOH and 0.050 M... Problem 93E: What mass of KOH is necessary to prepare 800.0 mL of a solution having a pH = 11.56? Problem 94E: Calculate the concentration of an aqueous Sr(OH)2 that has pH =10.50. Problem 95E: What are the major species present in a 0.150-M NH3 solution? Calculate the [OH] and the pH of this... Problem 96E: For the reaction of hydrazine (N2H4) in water, H2NNH2(aq)+H2O(l)H2NNH3+(aq)+OH(aq) Kb is 3.0 106.... Problem 98E: Calculate [OH], [H+], and the pH of 0.40 M solutions of each of the following amines (the Kb values... Problem 99E: Calculate the pH of a 0.20-M C2H5NH2 solution (Kb = 5.6 104). Problem 100E: Calculate the pH of a 0.050-M (C2H5)2NH solution(Kb = 1.3 103). Problem 101E: What is the percent ionization in each of the following solutions? a. 0.10 M NH3 b. 0.010 M NH3 c.... Problem 102E: Calculate the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H5NH+, in a 0.10-M aqueous... Problem 103E: The pH of a 0.016-M aqueous solution of p-toluidine (CH3C6H4NH2) is 8.60. Calculate Kb. Problem 104E: Codeine (C18H21NO3) is a derivative of morphine that is used as an analgesic, narcotic, or... Problem 105E: Write out the stepwise Ka reactions for the diprotic acid H2SO3. Problem 106E: Write out the stepwise Ka reactions for citric acid (H3C6H5O7), a triprotic acid. Problem 107E: A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500. mg. One vitamin C... Problem 108E: Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5.5 103, Ka2 = 1.7 107, and Ka3 = 5.1 1012.... Problem 109E: Calculate the pH and [S2] in a 0.10-M H2S solution. Assume Ka1 = 1.0 107; Ka2 = 1.0 1019. Problem 110E: Calculate [CO32] in a 0.010-M solution of CO2 in water (usually written as H2CO3). If all the CO32... Problem 111E: Calculate the pH of a 2.0-M H2SO4 solution. Problem 112E: Calculate the pH of a 5.0 103-M solution of H2SO4. Problem 113E: Arrange the following 0.10 M solutions in order of most acidic to most basic. KOH,KNO3,KCN,NH4Cl,HCl Problem 114E: Arrange the following 0.10 M solutions in order from most acidic to most basic. See Appendix 5 for... Problem 115E: Given that the Ka value for acetic acid is 1.8 105 and the Ka value for hypochlorous acid is 3.5 ... Problem 116E: The Kb values for ammonia and methylamine are 1.8 105 and 4.4 104, respectively. Which is the... Problem 117E: Determine [OH], [H+], and the pH of each of the following solutions. a. 1.0 M KCl b. 1.0 M KC2H3O2 Problem 118E: Calculate the concentrations of all species present in a 0.25-M solution of ethylammonium chloride... Problem 119E: Calculate the pH of each of the following solutions. a. 0.10 M CH3NH3Cl b. 0.050 M NaCN Problem 120E: Calculate the pH of each of the following solutions. a. 0.12 M KNO2 b. 0.45 M NaOCl c. 0.40 M... Problem 121E: Sodium azide (NaN3) is sometimes added to water to kill bacteria. Calculate the concentration of all... Problem 122E: Papaverine hydrochloride (abbreviated papH+Cl; molar mass = 378.85 g/mol) is a drug that belongs to... Problem 123E: An unknown salt is either NaCN, NaC2H3O2, NaF, NaCl, or NaOCl. When 0.100 mole of the salt is... Problem 124E: Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak... Problem 125E: A 0.050-M solution of the salt NaB has a pH of 9.00. Calculate the pH of a 0.010-M solution of HB. Problem 126E: A 0.20-M sodium chlorobenzoate (NaC7H4ClO2) solution has a pH of 8.65. Calculate the pH of a 0.20-M... Problem 127E Problem 128E Problem 129E: Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral,... Problem 130E: Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral,... Problem 131E: Place the species in each of the following groups in order of increasing acid strength. Explain the... Problem 132E: Place the species in each of the following groups in order of increasing base strength. Give your... Problem 133E: Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S,... Problem 134E: Using your results from Exercise 133, place the species in each of the following groups in order of... Problem 135E: Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write... Problem 136E: Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write... Problem 137E: Identify the Lewis acid and the Lewis base in each of the following reactions. a.... Problem 138E: Identify the Lewis acid and the Lewis base in each of the following reactions. a.... Problem 139E: Aluminum hydroxide is an amphoteric substance. It can act as either a Brnsted-Lowry base or a Lewis... Problem 140E: Zinc hydroxide is an amphoteric substance. Write equations that describe Zn(OH)2 acting as a... Problem 141E: Would you expect Fe3+ or Fe2+ to be the stronger Lewis acid? Explain. Problem 142E Problem 143AE: A 10.0-mL sample of an HCl solution has a pH of 2.000. What volume of water must be added to change... Problem 144AE: Which of the following represent conjugate acidbase pairs? For those pairs that are not conjugates,... Problem 145AE: A solution is tested for pH and conductivity as pictured below: The solution contains one of the... Problem 146AE: The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium... Problem 148AE: When someone hyperventilates, a condition known as respiratory alkalosis can occur. Explain the... Problem 149AE: Hemoglobin (abbreviated Hb) is a protein that is responsible for the transport of oxygen in the... Problem 150AE: A 0.25-g sample of lime (CaO) is dissolved in enough water to make 1500 mL of solution. Calculate... Problem 151AE: At 25C, a saturated solution of benzoic acid (Ka = 6.4 105) has a pH of 2.80. Calculate the water... Problem 152AE: Calculate the pH of an aqueous solution containing 1.0 102 M HCl, 1.0 102 M H2SO4.and 1.0 102... Problem 153AE: Acrylic acid (CH29CHCO2H) is a precursor for many important plastics. Ka for acrylic acid is 5.6 ... Problem 154AE: Classify each of the following as a strong acid, weak acid, strong base, or weak base in aqueous... Problem 155AE: The following illustration displays the relative number of species when an acid, HA, is added to... Problem 156AE: Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an... Problem 157AE: Calculate the mass of HONH2 required to dissolve in enough water to make 250.0 mL of solution having... Problem 158AE: A codeine-containing cough syrup lists codeine sulfate as a major ingredient instead of codeine. The... Problem 159AE Problem 160AE: Rank the following 0.10 M solutions in order of increasing pH. a. HI, HF, NaF, NaI b. NH4Br, HBr,... Problem 161AE: Is an aqueous solution of NaHSO4 acidic, basic, or neutral? What reaction occurs with water?... Problem 162AE: Calculate the value for the equilibrium constant for each of the following aqueous reactions. a.... Problem 163AE: A solution is made by adding 50.0 mL of 0.200 M acetic acid (Ka = 1.8 105) to 50.0 mL of 1.00 103... Problem 164AE: Calculate the pH of a 0.010-M solution of iodic acid (HIO3, Ka = 0.17). Problem 167AE: Phosphoric acid is a common ingredient in traditional cola drinks. It is added to provide the drinks... Problem 168CWP: For solutions of the same concentration, as acid strength increases, indicate what happens to each... Problem 169CWP Problem 170CWP: Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are... Problem 171CWP: Consider a 0.67-M solution of C2H5NH2 (Kb = 5.6 104). a. Which of the following are major species... Problem 172CWP: Rank the following 0.10 M solutions in order of increasing pH. a. NH3 b. KOH c. HC2H3O2 d. KCl e.... Problem 173CWP: Consider 0.25 M solutions of the following salts: NaCl, RbOCl, KI, Ba(ClO4)2, and NH4NO3. For each... Problem 174CWP: Calculate the pH of the following solutions: a. 1.2 M CaBr2 b. 0.84 M C6H5NH3NO3 (Kb for C6H5NH2 =... Problem 175CWP: Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these... Problem 176CP: The pH of 1.0 108 M hydrochloric acid is not 8.00. The correct pH can be calculated by considering... Problem 177CP: Calculate the pH of a 1.0 107-M solution of NaOH in water. Problem 178CP: Calculate [OH] in a 3.0 107-M solution of Ca(OH)2. Problem 179CP: Consider 50.0 mL of a solution of weak acid HA (Ka = 1.00 106), which has a pH of 4.000. What... Problem 180CP Problem 181CP: Calculate the pH of a 0.200-M solution of C5H5NHF. Hint: C5H5NHF is a salt composed of C5H5NH+ and F... Problem 182CP: Determine the pH of a 0.50-M solution of NH4OCl. (See Exercise 175.) Problem 183CP: Calculate [OH] in a solution obtained by adding 0.0100 mol solid NaOH to 1.00 L of 15.0 M NH3. Problem 184CP: What mass of NaOH(s) must be added to 1.0 L of 0.050 M NH3 to ensure that the percent ionization of... Problem 185CP: Consider 1000. mL of a 1.00 104-M solution of a certain acid HA that has a Ka value equal to 1.00 ... Problem 186CP: Calculate the mass of sodium hydroxide that must be added to 1.00 L of 1.00-M HC2H3O2 to double the... Problem 187CP: Consider the species PO43, HPO42, and H2PO4. Each ion can act as a base in water. Determine the Kb... Problem 188CP: Calculate the pH of a 0.10-M solution of sodium phosphate. (See Exercise 181.) Problem 189CP: Will 0.10 M solutions of the following salts be acidic, basic, or neutral? See Appendix 5 for Ka... Problem 190CP: a. The principal equilibrium in a solution of NaHCO3 is HCO3(aq)+HCO3(aq)H2CO3(aq)+CO32(aq)... Problem 191CP: A 0.100-g sample of the weak acid HA (molar mass = 100.0 g/mol) is dissolved in 500.0 g water. The... Problem 192CP: A sample containing 0.0500 mole of Fe2(SO4)3 is dissolved in enough water to make 1.00 L of... Problem 193IP: A 2.14 g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution... Problem 194IP: Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid... Problem 195IP: A certain acid, HA, has a vapor density of 5.11 g/L when in the gas phase at a temperature of 25C... Problem 196MP: An aqueous solution contains a mixture of 0.0500 M HCOOH (Ka = 1.77 104) and 0.150 M CH3CH2COOH (Ka... Problem 197MP: For the following, mix equal volumes of one solution from Group I with one solution from Group II to... Problem 168CWP: For solutions of the same concentration, as acid strength increases, indicate what happens to each...
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Hello, my Organic Chemistry 1 question is shown in the attached image.
Transcribed Image Text: Draw the conjugate base for the acid (CH,),C=OH+. Remember to include charges and non-bonding electrons where
necessary.
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C
H
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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