Chemistry by OpenStax (2015-05-04) 1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
1 Essential Ideas 2 Atoms, Molecules, And Ions 3 Composition Of Substances And Solutions 4 Stoichiometry Of Chemical Reactions 5 Thermochemistry 6 Electronic Structure And Periodic Properties Of Elements 7 Chemical Bonding And Molecular Geometry 8 Advanced Theories Of Covalent Bonding 9 Gases 10 Liquids And Solids 11 Solutions And Colloids 12 Kinetics 13 Fundamental Equilibrium Concepts 14 Acid-base Equilibria 15 Equilibria Of Other Reaction Classes 16 Thermodynamics 17 Electrochemistry 18 Representative Metals, Metalloids, And Nonmetals 19 Transition Metals And Coordination Chemistry 20 Organic Chemistry 21 Nuclear Chemistry Chapter14: Acid-base Equilibria
Chapter Questions Section: Chapter Questions
Problem 1E: Write equations that show NH3 as both a conjugate acid and a conjugate base. Problem 2E: Write equations that show H2PO4- acting both as an acid and as a base. Problem 3E: Show by suitable net ionic equations that each of the following species can act as a Br usted-Lowry... Problem 4E: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry... Problem 5E: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry... Problem 6E: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry... Problem 7E: What is the conjugate acid of each of the following? What is the conjugate base of each?. (a) OH-.... Problem 8E: What is the conjugate acid of each of the following? What is the conjugate base of each?. (a) H2S.... Problem 9E: Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted—Lowry base, and its... Problem 10E: Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its... Problem 11E: What are amphiprotic species? Illustrate with suitable equations. Problem 12E: State which of the following species are amphiprotic and write chemical equations illustrating the... Problem 13E: State which of the following species are amphiprotic and write chemical equations illustrating the... Problem 14E: Is the self-ionization of water endothermic or exothermic? The ionization constant for water (Kw) is... Problem 15E: Explain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at... Problem 16E: The ionization constant for water (Kw) is 2.91014 at 40 C. Calculate [H3O+], [OH-], pH, and pOH for... Problem 17E: The ionization constant for water (Kw) is 9.3111014 at 60 C. Calculate [H3O+], [OH-], pH, and pOH... Problem 18E: Calculate the pH and the pOH of each of the following solutions at 25 C for which the substances... Problem 19E: Calculate the pH and the pOH of each of the following solutions at 25 C for which the substances... Problem 20E: What are the pH and pOH of a solution of 2.0 M HCl, which ionizes completely? Problem 21E: What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52? Problem 22E: Calculate the hydrogen ion concentration and the hydroxide ion concentration in wine from its pH,... Problem 23E: Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice from its... Problem 24E: The hydronium ion concentration in a sample of rainwater is found to be 1.7106M at 25 C. What is the... Problem 25E: The hydroxide ion concentration in household ammonia is 3.2103M at 25 C. What is the concentration... Problem 26E: Explain why the neutralization reaction of a strong acid and a weak base gives a weakly acidic... Problem 27E: Explain why the neutralization reaction of a weak acid and a strong base gives a weakly basic... Problem 28E: Use this list of important industrial compounds (and Figure 14.8) to answer the following questions... Problem 29E: The odor of vinegar is due to the presence of acetic acid, CH3CO2H, a weak acid. List, in order of... Problem 30E: Household ammonia is a solution of the weak base NH3 in water. List, in order of descending... Problem 31E: Explain why the ionization constant, Ka, for H2SO4 is larger than the ionization constant for H2SO3. Problem 32E: Explain why the ionization constant, Ka, for HI is larger than the ionization constant for HP. Problem 33E: Gastric juice, the digestive ?uid produced in the stomach, contains hydrochloric acid, HCl, Milk of... Problem 34E: Nitric acid reacts with insoluble copper (II) oxide to form soluble copper (II) nitrate, Cu(NO3)2, a... Problem 35E: What is the ionization constant at 25 C for the weak acid CH3 NH3+, the conjugate acid of the weak... Problem 36E: What is the ionization constant at 25 C for the weak acid (CH3)2 NH2+, the conjugate acid of the... Problem 37E: Which base, CH3NH2 or (CH3)2NH, is the stronger base? Which conjugate acid, (CH3)2NH2+ or... Problem 38E: Which is the stronger acid, NH4+ or HBrO? Problem 39E: Which is the stronger base, (CH3)3N or H2BO3-? Problem 40E: Predict which acid in each of the following pairs is the stronger and explain your reasoning for... Problem 41E: Predict which compound in each of the following pairs of compounds is more acidic and explain your... Problem 42E: Rank the compounds in each of the following groups in order of increasing acidity or basicity, as... Problem 43E: Rank the compounds in each of the following groups in order of increasing acidity or basicity, as... Problem 44E: Both HF and HCN ionize in water to a limited extent. Which of the conjugate bases. F“ or CN”, is the... Problem 45E: The active ingredient formed by aspirin in the body is salicylic acid, C6H4OH(CO2H). The carboxyl... Problem 46E: What do we represent when we write: CH3CO2H(aq)+H2O(l)H3O+(aq)+CH3CO2(aq)? Problem 47E: Explain why equilibrium calculations are not necessary to determine ionic concentrations in... Problem 48E: Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in... Problem 49E: What two common assumptions can simplify calculation of equilibrium concentrations in a solution of... Problem 50E: What two common assumptions can simplify calculation of equilibrium concentrations in a solution of... Problem 51E: Which of the following will increase the percent of NH3 that is converted to the ammonium ion in... Problem 52E: Which of the following will increase the percent of HF that is converted to the fluoride ion in... Problem 53E: What is the effect on the concentrations of NO2-, HNO2, and OH- when the following are added to a... Problem 54E: What is the effect on the concentration of hydro?uoric acid, hydronium ion, and fluoride ion when... Problem 55E: Why is the hydronium ion concentration in a solution that is 0.10 M in HCl and 0.10 M in HCOOH... Problem 56E: From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb, for each... Problem 57E: From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each... Problem 58E: Determine Kb for the nitrite ion, NO2-. In a 0.10-M solution this base is 0.0015% ionized. Problem 59E: Determine Ka for hydrogen sulfate ion, HSO4-. In a 0.10-M solution the acid is 29% ionized. Problem 60E: Calculate the ionization constant for each of the following acids or bases form the ionization... Problem 61E: Calculate the ionization constant for each of the following acids or bases from the ionization... Problem 62E: For which of the following solutions must we consider the ionization of water when calculating the... Problem 63E: Even though both NH3 and C6H5NH2 are weak bases, NH3 is a much stronger acid than C6H5NH2. Which of... Problem 64E: Calculate the equilibrium concentration of the non-ionized acids and all ions in a solution that is... Problem 65E: Calculate the equilibrium concentration of the non-ionized acids and all ions in a solution that is... Problem 66E: Calculate the equilibrium concentration of the nonionized bases and all ions in a solution that is... Problem 67E: Calculate the equilibrium concentration of the nonionized bases and all ions in a solution that is... Problem 68E: Using the Ka value of , place Al(H2O)63+ in the correct location in Figure 14.8.
Problem 69E: Calculate the concentration of all solute species in each of the following solutions of acids or... Problem 70E: Propionic acid, C2H5CO2H (Ka=1.34105), is used in the manufacture of calcium propionate, a food... Problem 71E: White vinegar is a 5.0% by mass solution of acetic acid in water. If the density of white vinegar is... Problem 72E: The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous... Problem 73E: Nicotine, C10H14N2, is a base that will accept two protons (K1=7107,K2=1.41011). What is the... Problem 74E: The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data. Problem 75E: The pH of a 0.15-M solution of HSO4- is 1.43. Determine Ka for HSO4- from these data. Problem 76E: The pH of a 0.10-M solution of caffeine is 11.16. Determine Kb for caffeine from these data:... Problem 77E: Tile pH of a solution of household ammonia, a 0.950 M solution of NH3 is 11.612. Determine Kb for... Problem 78E: Determine whether aqueous solutions of the following salts are acidic, basic, or neutral: (a)... Problem 79E: Determine whether aqueous solutions of the following salts are acidic, basic, or neutral: (a) FeCl3.... Problem 80E: Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization... Problem 81E: Which of the following concentrations would be practically equal in a calculation of the equilibrium... Problem 82E: Calculate the concentration of each species present in a 0.050-M solution of H2S. Problem 83E: Calculate the concentration of each species present in a 0.010-M solution of phthalic acid,... Problem 84E: Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time.... Problem 85E: The ion HTe- is an amphiprotic species; it can act as either an acid or a base.. (a) What is Ka for... Problem 86E: Explain why a buffer can be prepared from a mixture of NH4Cl and NaOH but not from NH3 and NaOH. Problem 87E: Explain why the pH does not change significantly when a small amount of an acid or a base is added... Problem 88E: Explain why the pH does not change significantly when a small amount of an acid or a base is added... Problem 89E: What is [H3O+] in a solution of 0.25 M CH3CO2H and 0.030 M NaCH3CO2?.... Problem 90E: What is [H3O+] in a solution of 0.075 M HNO2 and 0.030 M NaNO2?.... Problem 91E: What is [OH-] in a solution of 0.125 M CH3NH2 and 0.130 M CH3NH3Cl?.... Problem 92E: What is [OH-] in a solution of 1.25 M NH3 and 0.78 M NH4NO3?. NH3(aq)+H2O(l)NH4+(aq)+OH(aq)Kb=1.8105 Problem 93E: What concentration of NH4NO3 is required to make [OH]=1.0105 in a 0.200-M solution of NH3? Problem 94E: What concentration of NaF is required to make [H3O+]=2.3104 in a 0.300-M solution of HF? Problem 95E: What is the effect on the concentration of acetic acid, hydronium ion, and acetate ion when the... Problem 96E: What is the effect on the concentration of ammonia, hydroxide ion, and ammonium ion when the... Problem 97E: What will be the pH of a buffer solution prepared from 0.20 mol NH3, 0.40 mol NH4NO3, and just... Problem 98E: Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of... Problem 99E: How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a... Problem 100E: What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution... Problem 101E: A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate.... Problem 102E: A 5.36-g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to... Problem 103E: Which acid in Table 14.2 is most appropriate for preparation of a buffer solution with a pH of 3.1?... Problem 104E: Which acid in Table 14.2 is most appropriate for preparation of a buffer solution with a pH of 3.7?... Problem 105E: Which base in Table 14.3 is must appropriate for preparation of a buffer solution with a pH of... Problem 106E: Which base in Table 14.3 is most appropriate for preparation of a buffer solution with a pH of 9.20?... Problem 107E: Saccharin, C7H4NSO3H, is a weak acid (Ka=2.1102). If 0.250 L of diet cola with a buffered pH of 5.48... Problem 108E: What is the pH of 1.000 L of a solution of 100.0 g of glutamic acid (C5H9NO4, a diprotic acid;... Problem 109E: Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a... Problem 110E: Explain why an acid-base indicator changes color over a range of pH values rather than at a specific... Problem 111E: Why can we ignore the contribution of water to the concentrations of H3O+ in the solutions of... Problem 112E: Why can we ignore the contribution of water to the concentration of OH- in a solution of the... Problem 113E: Draw a curve for a series of solutions of HF. Plot [H3O+]total on the vertical axis and the total... Problem 114E: Draw a curve similar to that shown in Figure 14.23 for a series of solutions of NH3. Plot [OH-] on... Problem 115E: Calculate the pH at the following points in a titration of 40 mL (0.040 L) of 0.100 M barbituric... Problem 116E: The indicator dinitrophenol is an acid with a Ka of 1.1104. In a 1.0104 -M solution, it is colorless... Problem 27E: Explain why the neutralization reaction of a weak acid and a strong base gives a weakly basic...
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Analytical chemistry
Transcribed Image Text: The salt resulting from the reaction of HNO3 with NH3 would have an aclidic characteristics.
Select one:
O True
O False
Branch of chemistry that deals with the separation, identification, and quantification of chemical compounds. Instruments such as centrifuges, microscopes, and spectrometers are commonly used in analytical chemistry. Forensic science is well-known for being reliant on analytical chemistry techniques.
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