EBK CHEMISTRY
4th Edition
ISBN: 8220102797864
Author: Burdge
Publisher: YUZU
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Chapter 16, Problem 17QP
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Chapter 16 Solutions
EBK CHEMISTRY
Ch. 16.1 - Practice Problem ATTEMPT What is (a) the conjugate...Ch. 16.1 - Practice Problem BUILD HSO 3 − is the conjugate...Ch. 16.1 - Practice Problem CONCEPTUALIZE Which of the models...Ch. 16.1 - 16.1.1 Which of the following pairs of species are...Ch. 16.1 - Which of the following species does not have a...Ch. 16.2 - Practice Problem ATTEMPT Identify and label the...Ch. 16.2 - Practice Problem BUILD
(a) Write an equation in...Ch. 16.2 - Practice Problem CONCEPTUALIZE Write the formula...Ch. 16.2 - Calculate [ OH − ] in a solution in which [ H 3 O...Ch. 16.2 - Calculate [ H 3 O − ] in a solution in which [ OH...
Ch. 16.3 - Prob. 1PPACh. 16.3 - Practice Problem BUILD
The value of at normal...Ch. 16.3 - Prob. 1PPCCh. 16.3 - Determine the pH of a solution at 25°C in which [...Ch. 16.3 - 16.3.2 Determine in a solution at...Ch. 16.3 - Determine the pOH of a solution at 25°C in which [...Ch. 16.3 - Determine [ OH − ] in a solution at 25°C if pH =...Ch. 16.4 - Practice ProblemATTEMPT Determine the pH of a...Ch. 16.4 - Practice Problem BUILD
Determine the pH of a...Ch. 16.4 - Practice Problem CONCEPTUALIZE
Strong acid is...Ch. 16.4 - Calculate the pH of a 0.075–-M solution of...Ch. 16.4 - 16.4.2 What is the concentration of in a solution...Ch. 16.4 - 16.4.3 What is the of a solution at that is...Ch. 16.4 - What is the concentration of KOH in a solution at...Ch. 16.4 - What is the pH of a solution at 25°C that is...Ch. 16.4 - What is the concentration of Ca ( OH ) 2 in a...Ch. 16.4 - Which diagram best represents a solution of...Ch. 16.5 - Practice Problem ATTEMPT Calculate the hydronium...Ch. 16.5 - Practice Problem BUILD Calculate the hydroxide ion...Ch. 16.5 - Practice Problem CONCEPTUALIZE
What is the value...Ch. 16.5 - The K a of a weak acid is 5.5 × 10 − 4 . What is...Ch. 16.5 - A 0.042-M solution of a weak acid has pH 4.01 at...Ch. 16.5 - The diagrams show solutions of three different...Ch. 16.6 - Practice ProblemATTEMPT Determine the pOH of a...Ch. 16.6 - Practice Problem BUILD Determine the pH of a...Ch. 16.6 - Prob. 1PPCCh. 16.6 - What is the pH of a 0.63-M solution of weak base...Ch. 16.6 - A 0.12-M solution of a weak base has a pH of 10.76...Ch. 16.6 - The diagrams show solutions of three different...Ch. 16.7 - Practice Problem ATTEMPT
Calculate the hydroxide...Ch. 16.7 - Practice ProblemBUILD Calculate the hydronium ion...Ch. 16.7 - Practice ProblemCONCEPTUALIZE What is the value of...Ch. 16.7 - 16.7.1 Calculate the of the cyanide ion . (See...Ch. 16.7 - Which of the anions listed is the strongest base?...Ch. 16.7 - The diagrams show solutions of three different...Ch. 16.8 - Practice Problem ATTEMPT
Calculate the pH of an...Ch. 16.8 - Practice ProblemBUILD Calculate the pOH of an...Ch. 16.8 - Practice Problem CONCEPTUALIZE
Estimate the pH of...Ch. 16.8 - Calculate the equilibrium concentration of CO 3 2...Ch. 16.8 - What is the pH of a 0.40-M solution of phosphoric...Ch. 16.8 - List the molecular and ionic species in order of...Ch. 16.8 - Which is true for any polyprotic acid? a) K a2 > K...Ch. 16.9 - Practice Problem ATTEMPT Calculate the...Ch. 16.9 - Practice Problem BUILD Calculate the concentration...Ch. 16.9 - Practice Problem CONCEPTUALIZE
Which of the plots...Ch. 16.10 - Practice Problem ATTEMPT Calculate the pOH of the...Ch. 16.10 - Practice Problem BUILD Calculate the pH of the...Ch. 16.10 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 16.10 - Calculate the pH of a 0.075-M solution of...Ch. 16.10 - Calculate the pH of a 0.082-M solution of...Ch. 16.10 - Prob. 3CPCh. 16.10 - Prob. 4CPCh. 16.10 - The diagrams represent solutions of three salts...Ch. 16.11 - Practice Problem ATTEMPT An aqueous solution of a...Ch. 16.11 - Practice Problem BUILD An aqueous solution of a...Ch. 16.11 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 16.12 - Practice Problem ATTEMPT
Calculate the pH at of a...Ch. 16.12 - Practice ProblemBUILD Calculate the pH at 25°C of...Ch. 16.12 - Practice Problem CONCEPTUALIZE The diagrams show...Ch. 16.12 - 16.12.1 Which of the following cannot act as a...Ch. 16.12 - Which of the following is a Lewis acid but not a...Ch. 16.13 - Practice Problem ATTEMPT
Determine the pH and...Ch. 16.13 - Prob. 1PPBCh. 16.13 - Practice Problem CONCEPTUALIZE
Which of the...Ch. 16.14 - Practice Problem ATTEMPT
Calculate the of a weak...Ch. 16.14 - Practice Problem BUILD
Calculate the of a weak...Ch. 16.14 - Practice Problem CONCEPTUALIZE Calculate K a...Ch. 16.15 - Practice Problem ATTEMPT
Calculate the pH at of a...Ch. 16.15 - Practice ProblemBUILD Calculate the pH at 25°C of...Ch. 16.15 - Practice Problem CONCEPTUALIZE
The diagrams...Ch. 16.16 - Practice ProblemATTEMPT Determine the K b of a...Ch. 16.16 - Practice Problem BUILD
Determine the of a weak...Ch. 16.16 - Practice Problem CONCEPTUALIZE
Determine the...Ch. 16.17 - Practice Problem ATTEMPT Determine (a) K b of the...Ch. 16.17 - Practice ProblemBUILD Determine (a) K b of the...Ch. 16.17 - Practice problemCONCEPTUALIZE Fee each week acid...Ch. 16.18 - Practice Problem ATTEMPT
Calculate the...Ch. 16.18 - Practice Problem BUILD
Calculate the...Ch. 16.18 - Practice ProblemCONCEPTURALIZE Which of the...Ch. 16.19 - Practice ProblemATTEMPT Indicate which is the...Ch. 16.19 - Practice Problem BUILD
Based on the information in...Ch. 16.19 - Prob. 1PPCCh. 16.20 - Practice ProblemATTEMPT Determine the pH of a...Ch. 16.20 - Practice ProblemBUILD Determine the concentration...Ch. 16.20 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 16.21 - Practice ProblemATTEMPT Determine the pH of a...Ch. 16.21 - Practice ProblemBUILD Determine the concentration...Ch. 16.21 - Practice Problem CONCEPTUALIZE
Which of the...Ch. 16.22 - Practice Problem ATTEMPT
Predict whether a 0.10-M...Ch. 16.22 - Prob. 1PPBCh. 16.22 - Prob. 1PPCCh. 16.23 - Practice ProblemATTEMPT Identify the Lewis acid...Ch. 16.23 - Practice Problem BUILD
Write formulas for the...Ch. 16.23 - Practice Problem CONCEPTUALIZE
Which of the...Ch. 16 - Calculate the pH of a solution that is 0.22 M in...Ch. 16 - 16.2 Determine pH at the equivalence point in the...Ch. 16 - Calculate the pH of a solution that is 0.22 M in...Ch. 16 - 16.4 Determine pH at the equivalence point in the...Ch. 16 - Define Brønsted acids and bases. Give an example...Ch. 16 - For a species to act as a Brønsted base, an atom...Ch. 16 - 16.3 Classify each of the following species as a...Ch. 16 - Identify the acid-base conjugate pairs in each of...Ch. 16 - 16.5 Write the formulas of the conjugate bases of...Ch. 16 - Write the formula for the conjugate acid of each...Ch. 16 - Which of the following could represent a Brønsted...Ch. 16 - 16.8 Oxalic acid has the following structure:
An...Ch. 16 - Rite the equilibrium expression for the...Ch. 16 - 16.10 In Section 15.3 we learned that when we...Ch. 16 - 16.11 The equilibrium constant for the...Ch. 16 - 16.12 Define the term amphoteric.
Ch. 16 - 16.13 Compare the magnitudes of in aqueous...Ch. 16 - Calculate the OH - concentration in an aqueous...Ch. 16 - 16.15 Calculate the concentration in an aqueous...Ch. 16 - The value of K w at 50°C is 5.48 × 10 − 14 ....Ch. 16 - The value of K w at 100°C is 5.1 × 3 10 − 13 ....Ch. 16 - Prob. 18QPCh. 16 - Prob. 19QPCh. 16 - Prob. 20QPCh. 16 - Prob. 21QPCh. 16 - Prob. 22QPCh. 16 - Calculate the concentration of OH- ions in a 1 .4...Ch. 16 - Prob. 24QPCh. 16 - 16.25 Calculate the pH of each of the following...Ch. 16 - Calculate the pH of each of the following...Ch. 16 - Prob. 27QPCh. 16 - Prob. 28QPCh. 16 - 16.29 The pOH of a solution is 9.40 at . Calculate...Ch. 16 - Prob. 30QPCh. 16 - Prob. 31QPCh. 16 - 16.32 A solution is made by dissolving 18.4 g of ...Ch. 16 - Prob. 33QPCh. 16 - Prob. 34QPCh. 16 - Prob. 35QPCh. 16 - Prob. 36QPCh. 16 - Prob. 37QPCh. 16 - Prob. 38QPCh. 16 - Prob. 39QPCh. 16 - 16.40 Calculate the concentration of in a...Ch. 16 - Calculate the concentration of HNO 3 in a solution...Ch. 16 - Prob. 42QPCh. 16 - Prob. 43QPCh. 16 - Prob. 44QPCh. 16 - Prob. 45QPCh. 16 - Explain what is meant by the strength of an acid.Ch. 16 - Prob. 47QPCh. 16 - Prob. 48QPCh. 16 - Why do we normally not quote K a values for strong...Ch. 16 - Which of the following solutions has the highest...Ch. 16 - Without referring to the text, write the formulas...Ch. 16 - In biological and medical applications, it is...Ch. 16 - 16.53 The for benzoic acid is Calculate the pH...Ch. 16 - The K a for hydrofluoric acid is 7.1 × 10 − 4 ....Ch. 16 - Calculate the pH of an aqueous solution at 25°C...Ch. 16 - Calculate the pH of an aqueous solution at 25°C...Ch. 16 - 16.57 Determine the percent ionization of the...Ch. 16 - Prob. 58QPCh. 16 - Prob. 59QPCh. 16 - Prob. 60QPCh. 16 - Calculate the K a of a weak acid if a 0.19 − M...Ch. 16 - Prob. 62QPCh. 16 - What is the original molarity of a solution of...Ch. 16 - What is the original molarity of a solution of a...Ch. 16 - 16.65 Which of the following statements are true...Ch. 16 - Prob. 66QPCh. 16 - Prob. 67QPCh. 16 - Compare the pH values for 0.10 − M solutions of...Ch. 16 - Which of the following has a higher pH: (a) 1 .0 M...Ch. 16 - Prob. 70QPCh. 16 - The pH of a 0.30-M solution of a weak base is...Ch. 16 - What is the original molarity of an aqueous...Ch. 16 - Prob. 73QPCh. 16 - Prob. 74QPCh. 16 - Prob. 75QPCh. 16 - Prob. 76QPCh. 16 - Prob. 77QPCh. 16 - Prob. 78QPCh. 16 - 16.79 Calculate for each of the following ions: ...Ch. 16 - Prob. 80QPCh. 16 - Prob. 81QPCh. 16 - Prob. 82QPCh. 16 - Prob. 83QPCh. 16 - Prob. 84QPCh. 16 - Compare the pH of a 0 .040 M HCl solution with...Ch. 16 - What are the concentrations of HSO 4, – SO 2– 4 ,...Ch. 16 - 16.87 Calculate the concentrations of
Ch. 16 - Calculate the pH at 25°C of a 0.25 − M aqueous...Ch. 16 - 16.89 Calculate the pH at of a aqueous solution...Ch. 16 - The first and second ionization constants of a...Ch. 16 - Prob. 91QPCh. 16 - Prob. 92QPCh. 16 - Prob. 93QPCh. 16 - Prob. 94QPCh. 16 - Prob. 95QPCh. 16 - Prob. 96QPCh. 16 - Prob. 97QPCh. 16 - Define salt hydrolysis. Categorize salts according...Ch. 16 - 16.99 Explain why small, highly charged metal ions...Ch. 16 - Al 3+ is not a Brønsted acid, but Al( H 2 O ) 6 3+...Ch. 16 - Specify which of the following salts will undergo...Ch. 16 - Prob. 102QPCh. 16 - Calculate the pH of a 0 .42 M NH 4 Cl solution . (...Ch. 16 - Prob. 104QPCh. 16 - Prob. 105QPCh. 16 - Prob. 106QPCh. 16 - 16.107 Predict whether the following solutions are...Ch. 16 - A certain salt, MX (containing the M + and X -...Ch. 16 - Prob. 109QPCh. 16 - Predict whether a solution containing the salt K 2...Ch. 16 - Prob. 111QPCh. 16 - Prob. 112QPCh. 16 - Prob. 113QPCh. 16 - Prob. 114QPCh. 16 - Prob. 115QPCh. 16 - Prob. 116QPCh. 16 - Prob. 117QPCh. 16 - Prob. 118QPCh. 16 - Prob. 119QPCh. 16 - Prob. 120QPCh. 16 - Prob. 121QPCh. 16 - Prob. 122QPCh. 16 - Prob. 123QPCh. 16 - Prob. 124QPCh. 16 - Identity the Lewis acid and the Lewis base in the...Ch. 16 - Predict the direction that predominates in this...Ch. 16 - Prob. 127APCh. 16 - Prob. 128APCh. 16 - Calculate the pH and percent ionization of a 0 .88...Ch. 16 - 16.130 Calculate the pH of a 0.20 M ammonium...Ch. 16 - Prob. 131APCh. 16 - Prob. 132APCh. 16 - 16.133 Like water, liquid ammonia undergoes...Ch. 16 - Prob. 134APCh. 16 - A solution contains a weak monoprotic acid HA and...Ch. 16 - Prob. 136APCh. 16 - Prob. 137APCh. 16 - Prob. 138APCh. 16 - Prob. 139APCh. 16 - A 10.0-g sample of white phosphorus was burned in...Ch. 16 - Prob. 141APCh. 16 - Prob. 142APCh. 16 - Prob. 143APCh. 16 - Prob. 144APCh. 16 - 16.145 Give an example of (a) a weak acid that...Ch. 16 - Prob. 146APCh. 16 - Prob. 147APCh. 16 - Prob. 148APCh. 16 - When chlorine reacts with water, the resulting...Ch. 16 - Prob. 150APCh. 16 - Calculate the pH of a 2 .00 M NH 4 CN solution.Ch. 16 - Calculate the concentrations of all species in a 0...Ch. 16 - Prob. 153APCh. 16 - 16.154 Calculate the concentrations of all the...Ch. 16 - Prob. 155APCh. 16 - Calculate the pH of a solution that is 1.00 M HCN...Ch. 16 - How many grams of NaCN would you need to dissolve...Ch. 16 - A solution of formic acid ( HCOOH ) has a pH of...Ch. 16 - Calculate the pH of a 1-L solution containing...Ch. 16 - 16.160 A 1.87-g sample of Mg reacts with 80.0 mL...Ch. 16 - Prob. 161APCh. 16 - Prob. 162APCh. 16 - A 0.400 M formic acid ( HCOOH ) solution freezes...Ch. 16 - Prob. 164APCh. 16 - Prob. 165APCh. 16 - Prob. 166APCh. 16 - 16.167 Both the amide ion and the nitride ion ...Ch. 16 - Determine whether each of the following statements...Ch. 16 - Prob. 169APCh. 16 - Prob. 170APCh. 16 - Prob. 171APCh. 16 - 16.172 A typical reaction between an antacid and...Ch. 16 - Prob. 173APCh. 16 - 16.174 Hemoglobin is a blood protein that is...Ch. 16 - Tooth enamel is largely hydroxyapatite [ Ca 3 ( PO...Ch. 16 - Prob. 176APCh. 16 - Prob. 177APCh. 16 - About half of the hydrochloric acid produced...Ch. 16 - Prob. 179APCh. 16 - Prob. 180APCh. 16 - Prob. 181APCh. 16 - (a) Use VSEPR to predict the geometry of the...Ch. 16 - The following questions are not based on a...Ch. 16 - The following questions are not based on a...Ch. 16 - The following questions are not based on a...Ch. 16 - The following questions are not based on a...
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- Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forwardWrite the reaction and the corresponding Kb equilibrium expression for each of the following substances acting as bases in water. a. aniline, C6H5NH2 b. dimethylamine, (CH3)2NHarrow_forwardWrite an equation to describe the proton transfer that occurs when each of these acids is added to water. (a) HCO3 (b) HCl (c) CH3COOH (d) HCNarrow_forward
- Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.arrow_forwardEach of the following statements concerns a 0.10 M solution of a weak organic base, B. Briefly describe why each statement is either true or false. a [B] is approximately equal to 0.10 M. b [B] is much greater than [HB+]. c [H3O+] is greater than [HB+]. d The pH is 13. e [HB+] is approximately equal to [OH]. f [OH] equals 0.10 M.arrow_forwardConvert the pK values to K values for the ionization of HCl, HClO4, and H2SO4 in glacial acetic acid. Rank these acids in order from strongest to weakest.arrow_forward
- . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.arrow_forwardWrite the ionization equation and the Kb expression for each weak base. CH3NH2 Phosphine, PH3arrow_forwardStrong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.arrow_forward
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