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... format_list_bulleted
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning