General Chemistry - Standalone book (MindTap Course List) 11th Edition
ISBN: 9781305580343
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
1 Chemistry And Measurement 2 Atoms, Molescules, And Ions 3 Calculations With Chemical Formulas And Equaitons 4 Chemical Reactions 5 The Gaseous State 6 Thermochemisty 7 Quantum Theory Of The Atom 8 Electron Configurations And Periodicity 9 Ionic And Covalent Bonding 10 Molecular Geometry And Chemical Bonding Theory 11 States Of Matter; Liquids And Solids 12 Solutions 13 Rates Of Reaction 14 Chemical Equilibirum 15 Acids And Bases 16 Acid-base Equilibria 17 Solubility And Complex-ion Equilibria 18 Thermodynamics And Equilibrium 19 Electrochemistry 20 Nuclear Chemistry 21 Chemistry Of The Main-group Elements 22 The Transition Elements And Coordination Compounds 23 Organic Chemistry 24 Polymer Materials: Synthetic And Biological A.1 Scientific (exponential) Notation A.2 Logarithms A.3 Algebraic Operations And Graphing Chapter16: Acid-base Equilibria
16.1 Acid-ionization Equilibria 16.2 Polyprotic Acids 16.3 Base-ionization Of Equilibria 16.4 Acid-base Properties Of Salt Solutions 16.5 Common-ion Effect 16.6 Buffers 16.7 Acid-base Titration Curves Chapter Questions Section: Chapter Questions
Problem 16.1QP: Write an equation for the ionization of hydrogen cyanide, HCN, in aqueous solution. What is the... Problem 16.2QP Problem 16.3QP: Briefly describe two methods for determining Ka for a weak acid. Problem 16.4QP: Describe how the degree of ionization of a weak acid changes as the concentration increases. Problem 16.5QP Problem 16.6QP: Phosphorous acid, H2PHO3, is a diprotic acid. Write equations for the acid ionizations. Write the... Problem 16.7QP Problem 16.8QP: Write the equation for the ionization of aniline, C6H5NH2, in aqueous solution. Write the expression... Problem 16.9QP: Which of the following is the strongest base: NH3, C6H5NH2, or CH3NH2? See Table 16.2. Problem 16.10QP: Do you expect a solution of anilinium chloride (aniline hydrochloride). C6H5NH3Cl, to be acidic or... Problem 16.11QP Problem 16.12QP: The pH of 0.10 M CH3NH2 (methylamine) is 11.8. When the chloride salt of methylamine, CH3NH3Cl, is... Problem 16.13QP: Define the term buffer. Give an example. Problem 16.14QP: What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer... Problem 16.15QP Problem 16.16QP: If the pH is 8.0 at the equivalence point for the titration of a certain weak acid with sodium... Problem 16.17QP: Which of the following salts would produce the most basic aqueous solution? a Ca(NO3)2 b Lil c KCl d... Problem 16.18QP: If you mix 0.10 mol of NH3 and 0.10 mol of HCl in a bucket of water, you would expect the resulting... Problem 16.19QP: Hydrogen sulfide, H2S, is a very weak diprotic acid. In a 0.10 M solution of this acid, which of the... Problem 16.20QP: If 20.0 mL of a 0.10 M NaOH solution is added to a 30.0-mL sample of a 0.10 M weak acid, HA, what is... Problem 16.21QP: Aqueous Solutions of Acids, Bases, and Salts a For each of the following salts, write the reaction... Problem 16.22QP: The pH of Mixtures of Acid, Base, and Salt Solutions a When 0.10 mol of the ionic solid NaX, where X... Problem 16.23QP: Which of the following beakers best represents a container of a weak acid, HA, in water? (Water... Problem 16.24QP: You have 0.10-mol samples of three acids identified simply as HX, HY, and HZ. For each acid, you... Problem 16.25QP Problem 16.26QP: You have the following solutions, all of the same molar concentration: KBr, HBr, CH3NH2, and NH4Cl.... Problem 16.27QP Problem 16.28QP: A chemist prepares dilute solutions of equal molar concentrations of NH3, NH4Br, NaF, and NaCl. Rank... Problem 16.29QP Problem 16.30QP Problem 16.31QP: You are given the following acidbase titration data, where each point on the graph represents the pH... Problem 16.32QP: The three flasks shown below depict the titration of an aqueous NaOH solution with HCl at different... Problem 16.33QP: Write chemical equations for the acid ionizations of each of the following weak acids (express these... Problem 16.34QP: Write chemical equations for the acid ionizations of each of the following weak acids (express these... Problem 16.35QP: Acrylic acid, whose formula is HC3H3O2 or HO2CCHCH2, is used in the manufacture of plastics. A 0.77... Problem 16.36QP: Heavy metal azides, which are salts of hydrazoic acid, HN3, are used as explosive detonators. A... Problem 16.37QP: Boric acid, B(OH)3, is used as a mild antiseptic. What is the pH of a 0.015 M aqueous solution of... Problem 16.38QP: Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate... Problem 16.39QP: C6H4NH2COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the... Problem 16.40QP: Barbituric acid. HC4H3N2O3, is used to prepare various barbiturate drugs (used as sedatives).... Problem 16.41QP: A solution of acetic acid, HC2H3O2, on a laboratory shelf was of undetermined concentration. If the... Problem 16.42QP: A chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found... Problem 16.43QP: Hydrofluoric acid, HF, unlike hydrochloric acid, is a weak electrolyte. What is the hydronium-ion... Problem 16.44QP: Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the... Problem 16.45QP: What is the hydronium-ion concentration of a 2.00 M solution of 2,6-dinitrobenzoic acid,... Problem 16.46QP: What is the hydronium-ion concentration of a 3.00 104 M solution of p-bromobenzoic acid,... Problem 16.47QP: Phthalic acid, H2C8H4O4, is a diprotic acid used in the synthesis of phenolphthalein indicator. Ka1... Problem 16.48QP: Carbonic acid, H2CO3, can be found in a wide variety of body fluids (from dissolved CO2). a... Problem 16.49QP: Write the chemical equation for the base ionization of methylamine, CH3NH2. Write the Kb expression... Problem 16.50QP: Write the chemical equation for the base ionization of aniline, C6H5NH2. Write the Kb expression for... Problem 16.51QP: Butylamine, C4H3NH2 is a weak base. A 0.47 M aqueous solution of butylamine has a pH of 12.13. What... Problem 16.52QP: Trimethylamine, (CH3)3N, is a gas with a fishy, ammonialike odor. An aqueous solution that is 0.25 M... Problem 16.53QP: What is the concentration of hydroxide ion in a 0.060 M aqueous solution of methylamine. CH3NH2?... Problem 16.54QP: What is the concentration of hydroxide ion in a 0.21 M aqueous solution of hydroxylamine, NH2OH?... Problem 16.55QP: Note whether hydrolysis occurs for each of the following ions. If hydrolysis docs occur, write the... Problem 16.56QP: Note whether hydrolysis occurs for each of the following ions. If hydrolysis doe occur, write the... Problem 16.57QP Problem 16.58QP Problem 16.59QP: For each of the following salts, indicate whether the aqueous solution will be acidic, basic, or... Problem 16.60QP: Note whether the aqueous solution of each of the following salts will be acidic, basic, or neutral.... Problem 16.61QP: Decide whether solutions of the following salts are acidic, neutral, or basic. a ammonium acetate b... Problem 16.62QP: Decide whether solutions of the following salts are acidic, neutral, or basic. a ammonium cyanate b... Problem 16.63QP: Obtain a the Kb value for NO2; b the Ka value for C5H5NH+ (pyridinium ion). Problem 16.64QP Problem 16.65QP: What is the pH of a 0.025 M aqueous solution of sodium propionate, NaC3H5O2? What is the... Problem 16.66QP: Calculate the OH concentration and pH of a 0.0025 M aqueous solution of sodium cyanide, NaCN.... Problem 16.67QP: Calculate the concentration of pyridine, C5H5N, in a solution that is 0.15 M pyridinium bromide,... Problem 16.68QP: What is the pH of a 0.30 M solution of methylammonium chloride, CH3NH3Cl? What is the concentration... Problem 16.69QP: Calculate the degree of ionization of a 0.75 M HF (hydrofluoric acid); b the same solution that is... Problem 16.70QP: Calculate the degree of ionization of a 0.22 M HCHO2 (formic acid); b the same solution that is also... Problem 16.71QP: What is the pH of a solution that is 0.600 M HCHO2 (formic acid) and 0.400 M NaCHO2? Problem 16.72QP: What is the pH of a solution that is 0.20 M KOCN and 0.10 M HOCN (cyanic acid)? Problem 16.73QP: What is the pH of a solution that is 0.10 M CH3NH2 (methylamine) and 0.15 M CH3NH3Cl (methylammonium... Problem 16.74QP: What is the pH of a solution that is 0.15 M C2H5NH2 (ethylamine) and 0.10 M C2H5NH3Br (ethylammonium... Problem 16.75QP: A buffer is prepared by adding 39.8 mL of 0.75 M NaF to 38.9 mL of 0.28 M HF. What is the pH of the... Problem 16.76QP: A buffer is prepared by adding 115 mL of 0.30 M NH3 to 135 mL of 0.15 M NH4NO3. What is the pH of... Problem 16.77QP: What is the pH of a buffer solution that is 0.10 M NH3 and 0.10 M NH4+? What is the pH if 12 mL of... Problem 16.78QP: A buffer is prepared by mixing 525 mL of 0.50 M formic acid, HCHO2, and 475 mL of 0.50 M sodium... Problem 16.79QP: What is the pH of a buffer solution that is 0.15 M chloroacetic acid and 0.10 M sodium... Problem 16.80QP: What is the pH of a buffer solution that is 0.10 M propionic acid and 0.20 M sodium propionate? Problem 16.81QP: What is the pH of a buffer solution that is 0.15 M pyridine and 0.10 M pyridinium bromide? Problem 16.82QP: What is the pH of a buffer solution that is 0.15 M methylamine and 0.20 M methylammonium chloride? Problem 16.83QP: How many moles of sodium acetate must be added to 2.0 L of 0.10 M acetic acid to give a solution... Problem 16.84QP: How many moles of hydrofluoric acid, HF, must be added to 250 mL of 0.25 M sodium fluoride to give a... Problem 16.85QP: What is the pH of a solution in which 15 mL of 0.10 M NaOH is added to 25 mL of 0.10 M HCl? Problem 16.86QP: What is the pH of a solution in which 35 mL of 0.10 M NaOH is added to 25 mL of 0.10 M HCl? Problem 16.87QP: A 1.24-g sample of benzoic acid was dissolved in water to give 50.0 mL or solution. This solution... Problem 16.88QP: A 0.400-g sample of propionic acid was dissolved in water to give 50.0 mL of solution. This solution... Problem 16.89QP: Find the pH of the solution obtained when 32 mL of 0.087 M ethylamine is titrated to the equivalence... Problem 16.90QP: What is the pH at the equivalence point when 22 mL of 0.20 M hydroxylamine is titrated with 0.10 M... Problem 16.91QP: A 50.0-mL sample of a 0.100 M solution of NaCN is titrated by 0.200 M HCl. Kb for CN is 2.0 105.... Problem 16.92QP: Sodium benzoate, NaC7H5O2, is used as a preservative in foods. Consider a 50.0-mL sample of 0.250 M... Problem 16.93QP: Calculate the pH of a solution obtained by mixing 25.00 mL of 0.19 M NH3 with 25.00 mL of 0.060 M... Problem 16.94QP: Calculate the pH of a solution obtained by mixing 35.0 mL of 0.15 M acetic acid with 27.0 mL of 0.10... Problem 16.95QP: Salicylic acid, C6H4OHCOOH, is used in the manufacture of acetylsalicylic acid (aspirin) and methyl... Problem 16.96QP: Cyanoacetic acid, CH2CNCOOH, is used in the manufacture of barbiturate drugs. An aqueous solution... Problem 16.97QP: A 0.050 M aqueous solution of sodium hydrogen sulfate, NaHSO4, has a pH of 1.73. Calculate Ka2 for... Problem 16.98QP: A 0.10 M aqueous solution of sodium dihydrogen phosphate, NaH2PO4, has a pH of 4.10. Calculate Ka2... Problem 16.99QP Problem 16.100QP: Calculate the base-ionization constants for PO43 and SO42. Which ion is the stronger base? Problem 16.101QP: Calculate the pH of a 0.072 M aqueous solution of aluminum chloride, AlCl3. The acid ionization of... Problem 16.102QP: Calculate the pH of a 0.10 M aqueous solution of zinc chloride, ZnCl2. The acid ionization of... Problem 16.103QP: An artificial fruit beverage contains 11.0 g of tartaric acid, H2C4H4O6, and 20.0 g of its salt,... Problem 16.104QP: A buffer is made by dissolving 12.5 g of sodium dihydrogen phosphate, NaH2PO4, and 15.0 g of... Problem 16.105QP: Blood contains several acid base systems that tend to keep its pH constant at about 7.4. One of the... Problem 16.106QP: Codeine, C23H21NO3, is an alkaloid (Kb = 6 2 109) used as a painkiller and cough suppressant. A... Problem 16.107QP: Calculate the pH of a solution obtained by mixing 456 mL of 0.10 M hydrochloric acid with 285 mL of... Problem 16.108QP: Calculate the pH of a solution made up from 2.0 g of potassium hydroxide dissolved in 115 mL of 0.19... Problem 16.109QP: Find the pH of the solution obtained when 25 mL of 0.065 M benzylamine, C7H7NH2, is titrated to the... Problem 16.110QP: What is the pH of the solution obtained by titrating 1.30 g of sodium hydrogen sulfate, NaHSO4,... Problem 16.111QP: Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization... Problem 16.112QP: Ionization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the... Problem 16.113QP: Methylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of... Problem 16.114QP: Sodium benzoate is a salt of benzoic acid, C6H5COOH. A 0.15 M solution of this salt has a pOH of... Problem 16.115QP: Each of the following statements concerns a 0.010 M solution of a weak acid, HA. Briefly describe... Problem 16.116QP: Each of the following statements concerns a 0.10 M solution of a weak organic base, B. Briefly... Problem 16.117QP: A 0.288-g sample of an unknown monoprotic organic acid is dissolved in water and titrated with a... Problem 16.118QP: A 0.239-g sample of unknown organic base is dissolved in water and titrated with a 0.135 M... Problem 16.119QP: a Draw a pH titration curve that represents the titration of 50.0 mL of 0.10 M NH3 by the addition... Problem 16.120QP: a Draw a pH titration curve that represents the titration of 25.0 mL of 0.15 M propionic acid.... Problem 16.121QP: The equilibrium equations and Ka values for three reaction systems are given below.... Problem 16.122QP Problem 16.123QP: A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl.... Problem 16.124QP: A 25.00-mL sample contains 0.562 g of NaHCO3. This sample is used to standardize an NaOH solution.... Problem 16.125QP: A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic... Problem 16.126QP: A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a... Problem 16.127QP: An important component of blood is the buffer combination of dihydrogen phosphate ion and the... Problem 16.128QP: An important component of blood is the buffer combination of bicarbonate ion and carbonic acid.... Problem 16.129QP: Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the... Problem 16.130QP: Malic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the... Problem 16.131QP: A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The... Problem 16.132QP: A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 mol of sodium acetate.... Problem 16.133QP Problem 16.134QP Problem 16.135QP: A 30.0-mL sample of 0.05 M HClO is titrated by a 0.0250 M KOH solution Ka for HClO is 3.5 108.... Problem 16.136QP Problem 16.137QP Problem 16.138QP: Calculate the pH of a solution made by mixing 0.62 L of 0.10 M NH4Cl with 0.50 L of 0.10 M NaOH. Kb... Problem 16.139QP: Cyanic acid, HOCN, is a weak acid with a Ka value of 3.5 104 at 25C. In a 0.293 M solution of the... Problem 16.140QP: The Kb for NH3 is 1.8 105 at 25C. Calculate the pH of a buffer solution made by mixing 65.1 mL of... Problem 16.141QP: Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid,... Problem 16.142QP: K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic... Problem 16.143QP Problem 16.144QP Problem 16.145QP Problem 16.146QP: Two samples of 1.00 M HCl of equivalent volumes are prepared. One sample is titrated to the... Problem 16.147QP Problem 16.148QP Problem 16.149QP: A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the... Problem 16.150QP: A buffer solution is prepared by mixing equal volumes of 0.10 M NaNO2 and 0.10 M HNO2 solutions. a... Problem 16.151QP: The pH of a white vinegar solution is 2.45. This vinegar is an aqueous solution of acetic acid with... Problem 16.152QP: The pH of a household cleaning solution is 11.50. This cleanser is an aqueous solution of ammonia... Problem 16.153QP: What is the freezing point of 0.92 M aqueous acetic acid? The density of this solution is 1.008... Problem 16.154QP Problem 16.155QP: A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049... Problem 16.156QP: A chemist needs a buffer with pH 3.50. How many milliliters of pure formic acid (density = 1.220... Problem 16.157QP: Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or... Problem 16.147QP
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Concept explainers
A buffer solution is made that is 0.488 M in H2CO3 and 0.488 M in KHCO3.
If Ka1 for H2CO3 is 4.20x10^-7, what is the pH of the buffer solution?
pH =
Write the net ionic equation for the reaction that occurs when 0.124 mol HNO3 is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use H3O^+ instead of H^+)
Definition Definition Substance that constitutes everything in the universe. Matter consists of atoms, which are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction: solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
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