Problem 1PE Problem 2PE: Practice Exercise 16.2
An aqueous solution of sodium bicarbonate, , has a molar concentration of... Problem 3PE: Practice Exercise 16.3
Water draining from old coal and mineral mines often has pH values of 4.0 or... Problem 4PE: Because rain washes pollutants out of the air, the lakes in many parts of the world have undergone... Problem 5PE: Practice Exercise 16.5
Find the values of and that correspond to each of the following values of... Problem 6PE: Practice Exercise 16.6
Calculate the . (Hint: is a strong acid.)
Problem 7PE: Practice Exercise 16.7
Calculate the , and pH in a solution made by weighing 1.20 g of and... Problem 8PE: For each of the following acids, write the equation for its ionization in water and the appropriate... Problem 9PE: For each of the following acids, write the equation for its ionization in water and the appropriate... Problem 10PE: Practice Exercise 16.10 Use Table 16.2 to find all the adds that arc stronger than acetic acid and... Problem 11PE: Practice Exercise 16.11 Two acids, H A and H B, have pKa values of 3.16 and 4.14, respectively.... Problem 12PE: Practice Exercise 16.12 For each of the following bases, write the equation for its ionization in... Problem 13PE: Practice Exercise 16.13 Write the ionization reaction, and the expression, when each of the... Problem 14PE: Practice Exercise 16.14 The base methylamine CH3NH2 has a Kbof4.510-4. What is the Ka for the... Problem 15PE: Practice Exercise 16.15
The value of for the
Problem 16PE: Practice Exercise 16.16 Salicylic acid reacts with acetic acid to form aspirin, acetyl salicylic... Problem 17PE: Practice Exercise 16.17 When butter turns rancid, its foul odor is mostly that of butanoic acid,... Problem 18PE: Practice Exercise 16.18 Few substances are more effective in relieving intense pain than morphine.... Problem 19PE: A student planned an experiment that would use 0.10 M propionic acid, HC3H5O2. Calculate the value... Problem 20PE: Benzoic acid, HC6H5CO2, is a monoprotic add (only one H+ ionizes) with a Ka=6.3105. Calculate [H+]... Problem 21PE: Nicotinic acid, HC6H4NO2, is a B vitamin. It is also a weak acid with Ka=1.4105. Calculate [H+] and... Problem 22PE: Aniline, C6H5NH2, is a precursor for many dyes used to color fabrics, known as aniline dyes. Aniline... Problem 23PE: Pyridine, C5H5N, is a bad-smelling liquid for which Kb=1.810. What is the pH of a 0.010M aqueous... Problem 24PE: Practice Exercise 16.24
Phenol is an acidic organic compound for which . What is the pH of a 0.15 M... Problem 25PE: Practice Exercise 16.25
Are solutions of acidic, basic, or neutral? (Him: Write the ions for these... Problem 26PE: Are solutions of (a)NaNO3,(b)KF,and(c)NH4NO3 acidic, basic, or neutral? Now that we have reinforced... Problem 27PE: Practice Exercise 16.27
What is the pH of a solution when 25.0 g of methylammonium chloride, , is... Problem 28PE: What is the pH of a 0.10 M solution of NaNO2? Problem 29PE: Practice Exercise 16.29
If 500.0 mL of a 0.20 M solution of ammonia is mixed with 500.0 mL of a 0.20... Problem 30PE: Practice Exercise 16.30
Will an aqueous solution of ammonium cyanide. , be acidic, basic, or... Problem 31PE: Will an aqueous solution of ammonium nitrite, NH4NO2, be acidic, basic, or neutral? Problem 32PE: Acetic acid, HC2H3O2, and sodium acetate, NaC2H3O2 (this provides the acetate ion C2H3O2-), can be... Problem 33PE: For a buffer composed of NH3 and NH4+ (from NH4Cl), write chemical equations that show what happens... Problem 34PE: Practice Exercise 16.34
Calculate the pH of the buffer solution in the preceding example by using... Problem 35PE: One liter of buffer is made by dissolving 100.0 grams of acetic acid, HC2H3O2, and 100.0 grams of... Problem 36PE: Practice Exercise 16.36
From Table 16.2 select an acid that, along with its sodium salt, can be used... Problem 37PE: A chemist needed an aqueous buffer with a pH of 3.90. Would formic acid and its salt, sodium... Problem 38PE: Practice Exercise 16.38
How much will the pH change if we add 0.15 mol to 1.00 L of a buffer that... Problem 39PE: Practice Exercise 16.39
A buffer is prepared by mixing of solution. What b the pH of this buffer,... Problem 40PE: Write the three ionization steps for phosphoric acid, H3PO4, and write the Ka expressions for each... Problem 41PE: Ascorbic acid (vitamin C) is a diprotic acid, H2C6H6O6. (See Table 16.4.) Calculate... Problem 42PE: Sodium bicarbonate gives solutions that are slightly alkaline (approximately pH 8.3), and similar... Problem 43PE: What is the pHofa0.20M solution of Na2SO3at25C? For the diprotic acid,... Problem 44PE: Reasoning by analogy from what you learned about solutions of weak polyprotic acids, what is the... Problem 45PE: When a weak acid such as acetic acid, HC2H3O2, is titrated with KOH what are ALL of the species in... Problem 46PE: Suppose we titrate 20.0 mL of 0.100 MHCHO2 with 0.100MNaOH. Calculate the pH (a) before any base is... Problem 47PE: Practice Exercise 16.47
Suppose 30.0 mL of is added to 50.0 mL of . What will be the pH of the... Problem 1RQ: Write the chemical equation for (a) the autoionization water and (b) the equilibrium law for KW. Problem 2RQ: How are acidic, basic, and neutral solutions in water defined (a) in terms of [ H+ ]and[ OH ] and... Problem 3RQ: At 25C, how are the pHandpOH of a solution related to each other? Problem 4RQ: Why do chemists use pH notation instead of the concentration of H+ ions? Problem 5RQ: Explain how acids and bases suppress the ionization of water, often called the common ion effect. Problem 6RQ Problem 7RQ: Could you use the p-notation for the concentration of a very dilute solution of chloride ion for a... Problem 8RQ: List the strong acids. Problem 9RQ: 16.9. What chemical property is central to our classifying an acid as a strong acid?
Problem 10RQ: 16.10. Explain the difference between strength and concentration of an acid.
Problem 11RQ: How are strong bases identified? Problem 12RQ: 16.12. Some strong bases can be used to safely reduce stomach acidity (heartburn). What... Problem 13RQ: Explain why we can ignore the autoionization of a 1.0 M solution of a strong acid. Problem 14RQ: 16.14 Write the general equation for the ionization of a weak acid, HA, in water. Give the... Problem 15RQ: Which diagram best represents a weak acid? A strong add? A nonelectrolyte? Problem 16RQ: Why do we use equilibrium constants, KaandKb, for weak acids and bases, but not for the strong acids... Problem 17RQ: 16.17 Write the chemical equation for the ionization of each of the following weak acids in water.... Problem 18RQ: For each of the acids in Review Question 16.17 write the appropriate Ka expression. Problem 19RQ: Write the general equation for the ionization of a weak base, B, in water. Give the equilibrium law... Problem 20RQ: 16.20 Write the chemical equation for the ionization of each of the following weak bases in... Problem 21RQ: 16.21 For each of the bases in Review Question 16.20, the appropriate expression.
Problem 22RQ: The pKa of HCN is 9.31 and that of HF is 3.46. Which is the stronger Brnsted base, CN-orF-? Problem 23RQ: Write the structural formulas for the conjugate acids of the following: Problem 24RQ: 16.24 Write the structural formulas for the conjugate bases of the following:
Problem 25RQ: 16.25 How is percentage ionization defined? Write the equation.
Problem 26RQ: What criterion do we use to determine whether or not the equilibrium concentration of an acid or... Problem 27RQ: For which of the following are we permitted to make the assumption that the equilibrium... Problem 28RQ: What is the quadratic formula? When is it appropriate to use it finding equilibrium concentrations? Problem 29RQ: Aspirin is acetylsalicylic acid, a monoprotic acid whose Kavalueis3.310-4. Does a solution of the... Problem 30RQ: The Kb value of the oxalate ion, C2O42,is1.610-10.IsasolutionofK2C2O4 acidic, basic, or neutral?... Problem 31RQ: Consider the following compounds and suppose that 0.5 M solutions are prepared of each:... Problem 32RQ: Will an aqueous solution of AICl3 turn litmus red or blue? Explain. Problem 33RQ: A solution of hydrazinium acetate is slightly acidic. Without looking at the tables of equilibrium... Problem 34RQ Problem 35RQ: To form a buffer, two substances are needed. How are these substances related? Problem 36RQ: Write ionic equations that illustrate how each pair of compounds can serve as a buffer pair. (a)... Problem 37RQ: 16.37. The hydrogen phosphate ion is able to act as a buffer all by itself. Write chemical equations... Problem 38RQ: 16.38. When sulfur dioxide, an air pollutant from the burning of sulfur-containing coal or oil,... Problem 39RQ: Which diagram best describes a diprotic acid with the first proton a strong acid and the second... Problem 40RQ: Citric acid, found in citrus fruits, is a triprotic acid, H3C6H5O7. Write chemical equations for the... Problem 41RQ: What simplifying assumptions do we usually make in working problems involving the ionization of... Problem 42RQ: 16.42. Write the equations for the chemical equilibria that exist in solutions of (a) (b) and (c)... Problem 43RQ: What simplifying assumptions do we usually make in working problems involving equilibria of salts of... Problem 44RQ: Define the terms equivalence point and end point as they apply to an acid-base titration. Problem 45RQ: Will the solution be acidic, neutral, or basic at the equivalence point for (a) a formic acid... Problem 46RQ: 16.46. Qualitatively, describe how an acid-base indicator works. Why do we want to use a minimum... Problem 47RQ: 16.47 If you use methyl orange in the titration of , will the end point of the titration correspond... Problem 48RQ: 16.48 Using the list of indicators in Table 16.7, choose the appropriate indicators for the... Problem 49RQ: 16.49 Calculate the in each of the following solutions in which the hydroxide ion concentrations... Problem 50RQ: Calculate the [OH-],pH,andpOH for each of the following solutions in which the H+ concentrations are... Problem 51RQ: Calculate the molar concentrations of H+andOH- in solutions that have the following pH values. (a)... Problem 52RQ: Calculate the molar concentrations of H+andOH- in solutions that have the following pH values. (a)... Problem 53RQ: Calculate the molar concentrations of H+andOH- in solutions that have the following pOH values. (a)... Problem 54RQ: Calculate the molar concentrations of H+andOH- in solutions that have the following pOH values. (a)... Problem 55RQ: A certain brand of beer had a H+ concentration equal to 1.910-5molL-1. What is the pH of the beer? Problem 56RQ: A soft drink was put on the market with [H+]=1.410-5molL-1. What is its pH? Problem 57RQ: A sample of Windex had a [OH-]=6.310-5molL-1. What is the pH of the sample? Problem 58RQ: 16.58 Bases tend to be used for cleaning. A solution of Tide laundry detergent had a . What is the... Problem 59RQ Problem 60RQ: At the temperature of the human body, 37C, the value of Kwis2.51014. Calculate [H+],[OH-],pH,andpOH... Problem 61RQ: 16.61 The interaction of water droplets in rain with carbon dioxide that is naturally present in the... Problem 62RQ: 16.62 Acid rain forms when rain falls through air polluted by oxides of sulfur and nitrogen. Trees... Problem 63RQ: 16.63 What is the concentration of ? What is the pH of this solution? What is the concentration in... Problem 64RQ: 16.64 What is the concentration of H+in0.031MHClO4? What is the pH of the solution? What is the OH-... Problem 65RQ: 16.65 A sodium hydroxide solution is prepared by dissolving 6.0 g in 1.00 L of solution. What is... Problem 66RQ: 16.66 A solution was made by dissolving 0.837 g Ba(OH)2 in 100 mL final volume. What is the molar... Problem 67RQ: 16.67 A solution of has a measured pH of 11.60. What is the molar concentration of the in the... Problem 68RQ: A solution of HCl has a pH of 2.50. How many grams of HCl are there in 0.250 L of this solution? How... Problem 69RQ: 16.69 In a 0.0020 M solution of , how many moles per liter of come from the ionization of water?
Problem 70RQ: 16.70 In a certain solution of HCl, the ionization of water contributes moles per liter to the ... Problem 71RQ: A solution was prepared with 2.64 micrograms of Ba(OH)2 in 1.00 liter of water. What is the pH of... Problem 72RQ: What is the pH of a 3.0107M solution of HCl? What concentration of hydrogen ions is provided by the... Problem 73RQ: 16.73 Rhododendrons are shrubs that produce beautiful flowers in the springtime. They only grow well... Problem 74RQ: 16.74 As eggs age, the pH of the egg white increases from about 7.9 to 9.3 as the carbon dioxide... Problem 75RQ Problem 76RQ: The barbiturate ion, C4H3N2O3,hasKb=1.010-10 What is the Ka for barbituric acid? Problem 77RQ: Iodic acid, HIO3, has a pKa of 0.77. (a) What arc the formula and the Kb of its conjugate base? (b)... Problem 78RQ: Lactic acid HC3H5O3, is responsible for the sour taste of old milk. At 25C, its Ka=1.4104. (a) What... Problem 79RQ: *16.79 A 1.0 M solution of acetic acid has a pH of 2.37. What percentage of the acetic acid is... Problem 80RQ: *16.80 A 0.250 M solution of NH3 has a pH of 11.32. What percentage of the ammonia is ionized in... Problem 81RQ: 16.81 A 0.20 M solution of a weak acid, HA, has a pH of 3.22. What is the percentage ionization of... Problem 82RQ: 16.82 A 0.15 M Absolution of an acid found in milk has a pH of 2.80. What is the percentage... Problem 83RQ: A 0.12 M solution of a weak base is 0.012% ionized. What is the pH of the solution? What is the... Problem 84RQ: 16.84 If a weak base is 0.030% ionized in 0.030 Absolution, what is the pH of the solution? What is... Problem 85RQ: Iodic acid, HIO3, is an important oxidizing agent and a moderately strong acid. In a 0.100 M... Problem 86RQ: 16.86 Chloroacetic acid, , is a stronger monoprotic add than acetic acid. In a 0.10 M solution, the... Problem 87RQ: 16.87 Ethylamine, , has a strong, pungent odor similar to that of ammonia. Like ammonia, it is a... Problem 88RQ: Hydroxylamine, HONH2, like ammonia, is a Brnsted base. A 0.15 M solution has a pH of 10.11. What are... Problem 89RQ: *16.89 What are the concentrations of all the solute species in 0.1 $0 M lactic acid, ? What is the... Problem 90RQ: What are the concentrations of all the solute species in a l.0 M solution of hydrogen peroxide,... Problem 91RQ: 16.91 Codeine, a cough suppressant extracted from crude opium, is a weak base with a of 5.80. What... Problem 92RQ: Pyridine, C5H5N, is a bad-smelling liquid that is a weak base in water. Its pKb, is 8.77. What is... Problem 93RQ: A solution of acetic acid has a pH of 2.54. What concentration of acetic acid in this solution? Problem 94RQ: How many moles of NH3 must be dissolved in water to give 500.0 mL of solution with a pH of 11.22? Problem 95RQ: * 16.95 What is the pH of a 0.0050 M solution of sodium cyanide?
Problem 96RQ: *16.96 What is the pH of a 0.020 M solution of chloroacetic acid, for which?
Problem 97RQ: The compound para-aminobenzoic acid (PABA) is a powerful sun-screening agent whose salts were once... Problem 98RQ: 16.98 Barbituric acid, (which we will abbreviate H-Bar), was discovered by the Nobel Prize-winning... Problem 99RQ: 16.99 Calculate the pH of . What is the centration of HCN in the solution?
Problem 100RQ: Calculate the pH of 0.40MKNO2. What is the concentration of HNO2 in the solution? Problem 101RQ: Calculate the pH of 0.15MCH3NH3Cl. For methylamine, CH3NH2,Kb=4.510-4. Problem 102RQ: Calculate the pH of 0.10 M hydrazinium chloride, N2H5Cl. Problem 103RQ: A 0.18 M solution of the sodium salt of nicotinic acid (also known pharmaceutically as niacin) has a... Problem 104RQ: 16.104 A weak base B forms the salt , composed of the ions and . A 0.15 M solution of the salt has... Problem 105RQ: Liquid chlorine bleach is really nothing more than a solution of sodium hypochlorite, NaOCl, in... Problem 106RQ: *16.106 The conjugate acid of a molecular base has the general formula . A solution of a salt of... Problem 107RQ: 16.107 What is the pH of a solution that contains .
Problem 108RQ: A buffer is prepared containing 0.25MNH3and0.45MNH4+. Calculate the pH of the buffer using the... Problem 109RQ: Rework Review Problem 16.107 using the Kb for the acetate ion. (Be sure to write the proper chemical... Problem 110RQ: 16.110 Calculate the pH of the buffer in Review Problem 16.108 using the .
Problem 111RQ: By how much will the pH change if 0.025 mol of HCl is added to 1.00 L of the buffer in Review... Problem 112RQ: 16.112 By how much will the pH change if 25.0 mL of 0.20 M NaOH is added to 0.500 L of the buffer in... Problem 113RQ: Certain proteolytic enzymes react in alkaline solutions. One of these enzymes produces 1.8... Problem 114RQ: *16.114 A hydrolytic enzyme consumes moles of hydrogen ions per minute in 2.50 L of a buffer that... Problem 115RQ: *16.115 What are the initial and final pH values for the buffer in Review Problem 16.113? What is... Problem 116RQ: *16.116 What are the initial and final pH values for the buffer in Review Problem 16.114? What is... Problem 117RQ: How many grams of sodium acetate, NaC2H3O2, would have to be added to 1.0 L of 0.15 M acetic acid... Problem 118RQ: 16.118 How many grams of sodium formate, , would have to be dissolved in 1.0 L of 0.12 M formic acid... Problem 119RQ: Suppose 30.00 mL of 0.100 M HCl is added to an acetate buffer prepared by dissolving 0.100 mol of... Problem 120RQ: 16.120 How many milliliters of 0.15 MHCl would have to be added to the original 0.100 L of the... Problem 121RQ: Calculate the concentrations of all the solute species in a 0.15 M solution of ascorbic acid... Problem 122RQ: *16.122 Tellurium, in the same family as sulfur, forms an acid analogous to sulfuric acid and called... Problem 123RQ: Calculate the concentrations of all of the solute species involved in the equilibria in a 2.0 M... Problem 124RQ: What is the pH of a 0.25 M solution of arsenic acid, H3ASO4? In this solution, what are the... Problem 125RQ: Phosphorous acid, H3PO3, is actually a diprotic acid for which Ka1=5.010-2andKa2=2.010-7. What are... Problem 126RQ: 16.126 What is the pH of a 0.20 M solution of oxalic acid, ?
Problem 127RQ: Calculate the pH of 0.24MNa2SO3. What are the concentrations of all ions and H2SO3 in the solution? Problem 128RQ: *16.128 Calculate the pH of . What are the concentrations of all ions and in the solution?
Problem 129RQ: 16.129 Sodium citrate, , is used as an anticoagulant in the collection of blood. What is the pH of a... Problem 130RQ: 16.130 What is the pH of a 0.25 M solution of sodium oxalate, ?
Problem 131RQ: 16.131 What is the pH of a 0.50 M solution of ? In this solution, what are the concentrations of , ... Problem 132RQ: *16.132 The pH of a solution is adjusted to 12.00 using a strong base. What is the concentration of... Problem 133RQ: What is the pH of a solution prepared by mixing 25.0 mL of 0.180MHC2H3O2 with 40.0 mL of 0.250 M... Problem 134RQ: *16.134 What is the pH of a solution prepared by mixing exactly 25.0 mL of with 15.0 mL of 0.400... Problem 135RQ: 16.135 When 50.0 mL of 0.050 M formic acid, , is titrated with 0.050 M sodium hydroxide, what is the... Problem 136RQ: 16.136 When 25 mL of 0.12 M aqueous ammonia is titrated with 0.12 M hydrobromic acid, what is the pH... Problem 137RQ: *16.137 For the titration of 75.00 mL of 0.1000 M acetic acid with 0.1000 MNaOH, calculate the pH... Problem 138RQ: For the titration of 50.00 mL of 0.1000 M ammonia with 0.1000 M HCl, calculate the pH (a) before the... Problem 139RQ: *16.139 Calculate the percentage ionization of acetic acid in solutions having concentrations of l... Problem 140RQ: *16.140 What is the pH of a solution that is and also ? What is the concentration of acetate ion in... Problem 141RQ: A solution is prepared by mixing 325 mL of 0.500MNH3 and 175 mL of 0.500MHCl. Assuming that the... Problem 142RQ: *16.142 A solution is prepared by dissolving 15.0 g of pure and 25.0 g of in 775 mL of solution... Problem 143RQ: For an experiment involving what happens to the growth of a particular fungus in a slightly acidic... Problem 144RQ: *16.144 Predict whether the pH of is greater than, less than, or equal to 7.00. Give your... Problem 145RQ: *16.145 What is the pH of a M solution of ammonium acetate. ?
Problem 146RQ: How many milliliters of ammonia gas measured at 25.2C and 745 torr must be dissolved in 0.250 L of... Problem 147RQ: HClO4 is a stronger proton donor than HNO3, but in water both acids appear to be of equal strength;... Problem 148RQ: 16.148 The hydrogen sulfate ion, , is a moderately strong
Brønsted acid with a
(a) Write the... Problem 149RQ: Some people who take megadoses of ascorbic acid will drink a solution containing as much as 6.0 g of... Problem 150RQ: 16.150 For the titration of 25.00 mL of 0. , calculate the pH of the reaction mixture after each of... Problem 151RQ: Below is a diagram illustrating a mixture HFandF- in an aqueous solution. For this mixture, does pH... Problem 152RQ: *16.152 How many milliliters of must be added to 0.200 L of to give a mixture with a pH of 3.00?
Problem 153RQ: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively... Problem 154RQ: 16.154 How many milliliters of are needed to completely neutralize the in 325 mL of a hydrochloric... Problem 155RQ: 16.155 It was found that 25.20 mL of an solution are needed to react completely with 30.0 mL of a ... Problem 156RQ: Suppose 38.0 mL of 0.000200MHCl is added to 40.0 mL of 0.000180MNaOH. What will be the pH of the... Problem 157RQ: *16.157 Suppose 10.0 mL of gas at and 734 torr is bubbled into 257 mL of pure water. What will be... Problem 158RQ: *16.158 Suppose the HCl described in the preceding problem is bubbled into 20.00 L of a solution of ... Problem 159RQ: *16.159 What is the approximate freezing point of a 0.50 M solution of dichloroacetic acid, ?... Problem 160RQ: 16.160 What happens to the pH of a solution as it is heated? Does that mean that the autoionization... Problem 161RQ: Can the pH of a solution ever have a negative value? Give an example of a situation where the pH has... Problem 162RQ: In simplifying our calculations, we were satisfied with a maximum error of 5% in the concentration... Problem 163RQ: In the 1950s it was discovered that lakes in the northeastern United States had declining fish... Problem 164RQ: 16.164 Where are buffers found in everyday consumer products? Propose reasons why a manufacturer... Problem 165RQ: Why must the acid used for a buffer have a pKa within one pH unit of the pH of the buffer? What... Problem 166RQ: What conjugate acid-base pairs are used to buffer (a) over-the-counter drugs, (b) foods, (c)... Problem 167RQ: Your blood at 37C needs to be maintained within a narrow pH range of 7.35 to 7.45 to maintain... Problem 168RQ: Develop a list of the uses of phosphoric acid in various consumer products. Problem 169RQ: What would our pH scale look like if Arrhenius decided that pH=ln[ H+ ]? What would the pH of a... format_list_bulleted