Chemistry 9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Steven S. Zumdahl
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 12ALQ: Consider two solutions of the salts NaX(aq) and NaY(aq) at equal concentrations. What would you need... Problem 13ALQ: What is meant by pH? True or false: A strong acid solution always has a lower pH than a weak acid... Problem 14ALQ: Why is the pH of water at 25C equal to 7.00? Problem 15ALQ: Can the pH of a solution be negative? Explain. Problem 16ALQ: Is the conjugate base of a weak acid a strong base? Explain. Explain why Cl does not affect the pH... Problem 17ALQ: Match the following pH values: 1, 2, 5, 6, 6.5, 8, 11, 11, and 13 with the following chemicals (of... Problem 18ALQ: The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be... Problem 19Q: Anions containing hydrogen (for example, HCO3 and H2PO4) usually show amphoteric behavior. Write... Problem 20Q: Which of the following conditions indicate an acidic solution at 25C? a. pH = 3.04 b. [H+] 1.0 107... Problem 21Q: Which of the following conditions indicate a basic solution at 25C? a. pOH = 11.21 b. pH = 9.42 c.... Problem 22Q: Why is H3O+ the strongest acid and OH the strongest base that can exist in significant amounts in... Problem 23Q: How many significant figures are there in the following numbers: 10.78, 6.78, 0.78? If these were pH... Problem 24Q: In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act... Problem 25Q: Consider the autoionization of liquid ammonia: Label each of the species in the equation as an acid... Problem 26Q: The following are representations of acidbase reactions: a. Label each of the species in both... Problem 27Q: Give three example solutions that fit each of the following descriptions. a. a strong electrolyte... Problem 28Q Problem 29Q Problem 30Q: Which of the following statements is(are) true? Correct the false statements. a. When a base is... Problem 31Q: Consider the following mathematical expressions. a. [H+] = [HA]0 b. [H+] = (Ka [HA]0)1/2 c. [OH] =... Problem 32Q: Consider a 0.10-M H2CO3 solution and a 0.10-M H2SO4 solution. Without doing any detailed... Problem 33Q: Of the hydrogen halides, only HF is a weak acid. Give a possible explanation. Problem 34Q: Explain why the following are done, both of which are related to acidbase chemistry. a. Power plants... Problem 35E: Write balanced equations that describe the following reactions, a. the dissociation of perchloric... Problem 36E: Write the dissociation reaction and the corresponding Ka equilibrium expression for each of the... Problem 37E: For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and... Problem 38E: For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and... Problem 39E: Classify each of the following as a strong acid or a weak acid. Problem 40E: Consider the following illustrations: Which beaker best illustrates what happens when the following... Problem 41E: Use Table 13-2 to order the following from the strongest to the weakest acid. HClO2,H2O,NH4+,HClO4 Problem 42E: Use Table 13-2 to order the following from the strongest to the weakest base. ClO2,H2O,NH3,ClO4 Problem 43E: You may need Table 13-2 to answer the following questions. a. Which is the stronger acid, HCl or... Problem 44E: You may need Table 13-2 to answer the following questions. a. Which is the stronger base, Cl or H2O?... Problem 45E: Calculate the [OH] of each of the following solutions at 25C. Identify each solution as neutral,... Problem 46E: Calculate the [H+] of each of the following solutions at 25C. Identity each solution as neutral,... Problem 47E: Values of Kw as a function of temperature are as follows: Temperature(C) Kw 0 1.14 1015 25 1.00 ... Problem 48E: 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 49E: Calculate the [OH] of each of the following solutions at 25C. Identify each solution as neutral,... Problem 50E: Calculate [H+] and [OH] for each solution at 25C. Identify each solution as neutral, acidic, or... Problem 51E: Fill in the missing information in the following table. Problem 52E: Fill in the missing information in the following table. Problem 53E Problem 54E: The pOH of a sample of baking soda dissolved in water is 5.74 at 25C. Calculate the pH, [H+], and... Problem 55E: What are the major species present in 0.250 M solutions of each of the following acids? Calculate... Problem 56E: 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 57E: Calculate the pH of each of the following solutions of a strong acid in water. a. 0.10 M HCl b. 5.0... Problem 58E: Calculate the pH of each of the following solutions containing a strong acid in water. a. 2.0 102 M... Problem 59E: Calculate the concentration of an aqueous HI solution that has pH = 2.50. HI is a strong acid. Problem 60E: Calculate the concentration of an aqueous HBr solution that has pH = 4.25. HBr is a strong acid. Problem 61E: How would you prepare 1600 mL of a pH = 1.50 solution using concentrated (12 M) HCl? Problem 62E: A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated... Problem 63E: What are the major species present in 0.250 M solutions of each of the following acids? Calculate... Problem 64E: What are the major species present in 0.250 M solutions of each of the following acids? Calculate... Problem 65E: Calculate the concentration of all species present and the pH of a 0.020-M HF solution. Problem 67E: For propanoic acid (HC3H5O2, Ka = 1.3 105), determine the concentration of all species present, the... Problem 68E: A solution is prepared by dissolving 0.56 g benzoic acid (C6H5CO2H, Ka = 6.4 105) in enough water... Problem 69E: Monochloroacetic acid, HC2H2ClO2, is a skin irritant that is used in chemical peels intended to... Problem 70E: A typical aspirin tablet contains 325 mg acetylsalicylic acid (HC9H7O4). Calculate the pH of a... Problem 72E: A solution is made by adding 50.0 mL of 0.200 M acetic acid (K4 = 1.8 103) to 50.0 mL of 1.00 103... Problem 73E: Calculate the percent dissociation of the acid in each of the following solutions. a. 0.50 M acetic... Problem 74E: Using the Ka values in Table 14.2, calculate the percent dissociation in a 0.20-M solution of each... Problem 75E: A 0.15-M solution of a weak acid is 3.0% dissociated. Calculate Ka. Problem 76E: An acid HX is 25% dissociated in water. If the equilibrium concentration of HX is 0.30 M, calculate... Problem 77E: Trichloroacetic acid (CCl3CO2H) is a corrosive acid that is used to precipitate proteins. The pH of... Problem 78E: The pH of a 0.063-M solution of hypobromous acid (HOBr but usually written HBrO) is 4.95. Calculate... Problem 79E: A solution of formic acid (HCOOH, Ka = 1.8 104) has a pH of 2.70. Calculate the initial... Problem 80E: A typical sample of vinegar has a pH of 3.0. Assuming that vinegar is only an aqueous solution of... Problem 81E: One mole of a weak acid HA was dissolved in 2.0 L of solution. After the system had come to... Problem 82E: You have 100.0 g saccharin, a sugar substitute, and you want to prepare a pH = 5.75 solution. What... Problem 83E: Write the reaction and the corresponding Kb equilibrium expression for each of the following... Problem 84E: Write the reaction and the corresponding Kb equilibrium expression for each of the following... Problem 85E Problem 86E: Use Table 14.3 to help order the following acids from strongest to weakest HNO3,H2O,NH4+,C5H5NH+ Problem 87E: Use Table 14.3 to help answer the following questions. a. Which is the stronger base, ClO4 or... Problem 88E: Use Table 14.3 to help answer the following questions. a. Which is the stronger acid, HClO4 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 97E 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: Calculate the mass of HONH2 required to dissolve in enough water to make 250.0 mL of solution having... 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 147AE: Hemoglobin (abbreviated Hb) is a protein that is responsible for the transport of oxygen in the... Problem 148AE: A 0.25-g sample of lime (CaO) is dissolved in enough water to make 1500 mL of solution. Calculate... Problem 149AE: At 25C, a saturated solution of benzoic acid (Ka = 6.4 105) has a pH of 2.80. Calculate the water... Problem 150AE: Calculate the pH of an aqueous solution containing 1.0 102 M HCl, 1.0 102 M H2SO4.and 1.0 102... Problem 151AE: Acrylic acid (CH29CHCO2H) is a precursor for many important plastics. Ka for acrylic acid is 5.6 ... Problem 152AE: Classify each of the following as a strong acid, weak acid, strong base, or weak base in aqueous... Problem 153AE: The following illustration displays the relative number of species when an acid, HA, is added to... Problem 154AE: Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an... Problem 155AE: Codeine (C18H21NO3) is a derivative of morphine that is used as an analgesic, narcotic, or... Problem 156AE: A codeine-containing cough syrup lists codeine sulfate as a major ingredient instead of codeine. The... Problem 157AE Problem 158AE: Rank the following 0.10 M solutions in order of increasing pH. a. HI, HF, NaF, NaI b. NH4Br, HBr,... Problem 159AE: Is an aqueous solution of NaHSO4 acidic, basic, or neutral? What reaction occurs with water?... Problem 160AE: Calculate the value for the equilibrium constant for each of the following aqueous reactions. a.... Problem 161AE Problem 162CWP: For solutions of the same concentration, as acid strength increases, indicate what happens to each... Problem 163CWP Problem 164CWP: Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are... Problem 165CWP: Consider a 0.67-M solution of C2H5NH2 (Kb = 5.6 104). a. Which of the following are major species... Problem 166CWP: Rank the following 0.10 M solutions in order of increasing pH. a. NH3 b. KOH c. HC2H3O2 d. KCl e.... Problem 167CWP: Consider 0.25 M solutions of the following salts: NaCl, RbOCl, KI, Ba(ClO4)2, and NH4NO3. For each... Problem 168CWP: Calculate the pH of the following solutions: a. 1.2 M CaBr2 b. 0.84 M C6H5NH3NO3 (Kb for C6H5NH2 =... Problem 169CWP: Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these... Problem 170CP: The pH of 1.0 108 M hydrochloric acid is not 8.00. The correct pH can be calculated by considering... Problem 171CP: Calculate the pH of a 1.0 107-M solution of NaOH in water. Problem 172CP: Calculate [OH] in a 3.0 107-M solution of Ca(OH)2. Problem 173CP: Consider 50.0 mL of a solution of weak acid HA (Ka = 1.00 106), which has a pH of 4.000. What... Problem 174CP Problem 175CP: Calculate the pH of a 0.200-M solution of C5H5NHF. Hint: C5H5NHF is a salt composed of C5H5NH+ and F... Problem 176CP: Determine the pH of a 0.50-M solution of NH4OCl. (See Exercise 175.) Problem 177CP: Calculate [OH] in a solution obtained by adding 0.0100 mol solid NaOH to 1.00 L of 15.0 M NH3. Problem 178CP: 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 179CP: 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 180CP: Calculate the mass of sodium hydroxide that must be added to 1.00 L of 1.00-M HC2H3O2 to double the... Problem 181CP: Consider the species PO43, HPO42, and H2PO4. Each ion can act as a base in water. Determine the Kb... Problem 182CP: Calculate the pH of a 0.10-M solution of sodium phosphate. (See Exercise 181.) Problem 183CP: Will 0.10 M solutions of the following salts be acidic, basic, or neutral? See Appendix 5 for Ka... Problem 184CP: a. The principal equilibrium in a solution of NaHCO3 is HCO3(aq)+HCO3(aq)H2CO3(aq)+CO32(aq)... Problem 185CP: 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 186CP: A sample containing 0.0500 mole of Fe2(SO4)3 is dissolved in enough water to make 1.00 L of... Problem 187IP: A 2.14 g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution... Problem 188IP: Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid... Problem 189IP: A certain acid, HA, has a vapor density of 5.11 g/L when in the gas phase at a temperature of 25C... Problem 190MP: An aqueous solution contains a mixture of 0.0500 M HCOOH (Ka = 1.77 104) and 0.150 M CH3CH2COOH (Ka... Problem 191MP: For the following, mix equal volumes of one solution from Group I with one solution from Group II to... Problem 22Q: Why is H3O+ the strongest acid and OH the strongest base that can exist in significant amounts in...
Related questions
Concept explainers
1.
(True or False)
Part B. Water is not an Arrhenius acid but can be a Bronsted acid.
(True or False)
Part C. A 6 M NaOH (aq) solution has no protons ions (H+) in it.
Definition Definition Compound that can increase the concentration of H + ions when it is dissolved in water.
Expert Solution
Part A
The given statement is False as HClO4 is stronger acid than H3 PO4 . This is because HClO4 deprotonates or dissociates more in water than H3 PO4 . Strong acids have the tendency to fully dissociate in water while weak acid do not dissociate completely. Also the central atom of HClO4 has a higher oxidation number(Cl = +7) than the central atom of H3 PO4 (P = +5). Higher the oxidation number, stronger is the acid.
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