Mastering Chemistry with Pearson eText ...4th EditionNivaldo J. Tro Publisher: PEARSONISBN: 9780134162485
Mastering Chemistry with Pearson eText ...
Solutions for Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)
Problem 2SAQ:
Q2. What is the pH of a buffer that is 0.120 M in formic acid (HCHO2) and 0.080 M in potassium...Problem 3SAQ:
Q3. A buffer with a pH of 9.85 contains CH3NH2 and CH3NH3Cl in water. What can you conclude about...Problem 4SAQ:
Q4. A 500.0-mL buffer solution is 0.10 M in benzoic acid and 0.10 M in sodium benzoate and has an...Problem 5SAQ:
Q5. Consider a buffer composed of the weak acid HA and its conjugate base A–. Which pair of...Problem 6SAQ:
Q6. Which combination is the best choice to prepare a buffer with a pH of 9.0?
a) NH3; NH4Cl (pKb...Problem 7SAQ:
Q7. A 25.0-mL sample of an unknown HBr solution is titrated with 0.100 M NaOH. The equivalence point...Problem 8SAQ:
Q8. A 10.0-mL sample of 0.200 M hydrocyanic acid (HCN) is titrated with 0.0998 M NaOH. What is the...Problem 9SAQ:
Q9. A 20.0-mL sample of 0.150 M ethylamine is titrated with 0.0981 M HCl. What is the pH after the...Problem 10SAQ:
Q10. Three 15.0-mL acid samples—0.10 M HA, 0.10 M HB, and 0.10 M H2C—are all titrated with 0.100 M...Problem 11SAQ:
Q11. A weak unknown monoprotic acid is titrated with a strong base. The titration curve is shown....Problem 12SAQ:
Q12. Calculate the molar solubility of lead(II) bromide (PbBr2). For lead(II) bromide, Ksp = 4.67 ×...Problem 13SAQ:
Q13. Calculate the molar solubility of magnesium fluoride (MgF2) in a solution that is 0.250 M in...Problem 14SAQ:
Q14. A solution is 0.025 M in Pb2 +. What minimum concentration of Cl– is required to begin to...Problem 15SAQ:
Q15. Which compound is more soluble in an acidic solution than in a neutral solution?
a) PbBr2
b)...Problem 2E:
2. What is a buffer? How does a buffer work? How does it neutralize added acid? Added base?
Problem 3E:
3. What is the common ion effect?
Problem 5E:
5. What is the pH of a buffer solution when the concentrations of both buffer components (the weak...Problem 6E:
6. Suppose that a buffer contains equal amounts of a weak acid and its conjugate base. What happens...Problem 7E:
7. How do you use the Henderson–Hasselbalch equation to calculate the pH of a buffer containing a...Problem 8E:
8. What factors influence the effectiveness of a buffer? What are the characteristics of an...Problem 9E:
9. What is the effective pH range of a buffer (relative to the pKa of the weak acid component)?
Problem 11E:
11. The pH at the equivalence point of the titration of a strong acid with a strong base is 7.0....Problem 12E:
12. The volume required to reach the equivalence point of an acid–base titration depends on the...Problem 13E:
13. In the titration of a strong acid with a strong base, how do you calculate these quantities?
a....Problem 14E:
14. In the titration of a weak acid with a strong base, how do you calculate these quantities?
a....Problem 15E:
15. The titration of a polyprotic acid with sufficiently different pKas displays two equivalence...Problem 16E:
16. In the titration of a polyprotic acid, the volume required to reach the first equivalence point...Problem 17E:
17. What is the difference between the endpoint and the equivalence point in a titration?
Problem 18E:
18. What is an indicator? How can an indicator signal the equivalence point of a titration?
Problem 19E:
19. What is the solubility product constant? Write a general expression for the solubility constant...Problem 20E:
20. What is molar solubility? How can you obtain the molar solubility of a compound from Ksp?
Problem 21E:
21. How does a common ion affect the solubility of a compound? More specifically, how is the...Problem 22E:
22. How is the solubility of an ionic compound with a basic anion affected by pH? Explain.
Problem 23E:
23. For a given solution containing an ionic compound, what is the relationship between Q, Ksp, and...Problem 24E:
24. What is selective precipitation? Under which conditions does selective precipitation occur?
Problem 25E:
25. What is qualitative analysis? How does qualitative analysis differ from quantitative analysis?
Problem 26E:
26. What are the main groups in the general qualitative analysis scheme described in this chapter?...Problem 27E:
27. In which of these solutions will HNO2 ionize less than it does in pure water?
a. 0.10 M NaCl
b....Problem 28E:
28. A formic acid solution has a pH of 3.25. Which of these substances will raise the pH of the...Problem 29E:
29. Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution.
a. a...Problem 30E:
30. Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution.
a. a...Problem 31E:
31. Calculate the percent ionization of a 0.15 M benzoic acid solution in pure water and in a...Problem 32E:
32. Calculate the percent ionization of a 0.13 M formic acid solution in pure water and also in a...Problem 33E:
33. Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution.
a. 0.15...Problem 34E:
34. Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution.
a. 0.18...Problem 35E:
35. A buffer contains significant amounts of acetic acid and sodium acetate. Write equations showing...Problem 36E:
36. A buffer contains significant amounts of ammonia and ammonium chloride. Write equations showing...Problem 39E:
39. Use the Henderson–Hasselbalch equation to calculate the pH of each solution.
a. a solution that...Problem 40E:
40. Use the Henderson–Hasselbalch equation to calculate the pH of each solution.
a. a solution that...Problem 41E:
41. Calculate the pH of the solution that results from each mixture.
a. 50.0 mL of 0.15 M HCHO2 with...Problem 42E:
42. Calculate the pH of the solution that results from each mixture.
a. 150.0 mL of 0.25 M HF with...Problem 44E:
44. Calculate the ratio of CH3NH2 to CH3NH3Cl concentration required to create a buffer with pH =...Problem 46E:
46. What mass of ammonium chloride should you add to 2.55 L of a 0.155 M NH3 to obtain a buffer with...Problem 47E:
47. A 250.0-mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium acetate.
a. What is...Problem 48E:
48. A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO.
a. What is the initial pH of...Problem 50E:
50. For each solution, calculate the initial and final pH after adding 0.010 mol of NaOH.
a. 250.0...Problem 52E:
52. A 100.0-mL buffer solution is 0.100 M in NH3 and 0.125 M in NH4Br. What mass of HCl can this...Problem 53E:
53. Determine whether or not the mixing of each pair of solutions results in a buffer.
a. 100.0 mL...Problem 54E:
54. Determine whether or not the mixing of each pair of solutions results in a buffer.
a. 75.0 mL of...Problem 55E:
55. Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in...Problem 56E:
56. The fluids within cells are buffered by H2PO4– and HPO42–.
a. Calculate the ratio of HPO42– to...Problem 57E:
57. Which buffer system is the best choice to create a buffer with pH = 7.20? For the best system,...Problem 59E:
59. A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition...Problem 62E:
62. Two 25.0-mL samples, one 0.100 M HCl and the other 0.100 M HF, are titrated with 0.200 M KOH.
a....Problem 63E:
63. Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH3NH2, are titrated with 0.100 M...Problem 64E:
64. The graphs labeled (a) and (b) show the titration curves for two equal-volume samples of bases,...Problem 65E:
65. Consider the curve shown here for the titration of a weak monoprotic acid with a strong base and...Problem 66E:
66. Consider the curve shown here for the titration of a weak base with a strong acid and answer...Problem 67E:
67. Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each...Problem 69E:
69. Consider the titration of a 25.0-mL sample of 0.115 M RbOH with 0.100 M HCl. Determine each...Problem 71E:
71. Consider the titration of a 20.0-mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine each...Problem 78E:
78. A 0.446-g sample of an unknown monoprotic acid is titrated with 0.105 M KOH. The resulting...Problem 84E:
84. Referring to Table 17.1, pick an indicator for use in the titration of each base with a strong...Problem 87E:
87. Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure...Problem 88E:
88. Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure...Problem 89E:
89. Use the given molar solubilities in pure water to calculate Ksp for each compound.
a. MX; molar...Problem 93E:
93. Refer to the Ksp value from Table 17.2 to calculate the solubility of iron(II) hydroxide in pure...Problem 95E:
95. Calculate the molar solubility of barium fluoride in each liquid or solution.
a. pure water
b....Problem 113E:
113. A 150.0-mL solution contains 2.05 g of sodium benzoate and 2.47 g of benzoic acid. Calculate...Problem 118E:
118. A 250.0-mL buffer solution initially contains 0.025 mol of HCHO2 and 0.025 mol of NaCHO2. In...Problem 119E:
119. In analytical chemistry, bases used for titrations must often be standardized; that is, their...Problem 131E:
131. The Kb of hydroxylamine, NH2OH, is 1.10 × 10–8. A buffer solution is prepared by mixing 100.0...Problem 132E:
132. A 0.867-g sample of an unknown acid requires 32.2 mL of a 0.182 M barium hydroxide solution for...Problem 135E:
135. What relative masses of dimethyl amine and dimethyl ammonium chloride do you need to prepare a...Problem 139E:
139. Since soap and detergent action is hindered by hard water, laundry formulations usually include...Problem 140E:
140. A 0.558-g sample of a diprotic acid with a molar mass of 255.8 g/mol is dissolved in water to a...Problem 141E:
141. When excess solid Mg(OH)2 is shaken with 1.00 L of 1.0 M NH4Cl solution, the resulting...Problem 148E:
148. What amount of HCl gas must be added to 1.00 L of a buffer solution that contains [acetic acid]...Problem 149E:
149. Without doing any calculations, determine if pH = pKa, pH > pKa, or pH < pKa. Assume that HA is...Problem 150E:
150. A buffer contains 0.10 mol of a weak acid and 0.20 mol of its conjugate base in 1.0 L of...Browse All Chapters of This Textbook
Chapter 1 - Matter, Measurement, And Problem SolvingChapter 2 - Atoms And ElementsChapter 3 - Molecules, Compounds, And Chemical EquationsChapter 4 - Chemical Quantities And Aqueous ReactionsChapter 5 - GasesChapter 6 - ThermochemistryChapter 7 - The Quantum-Mechanical Model Of The AtomChapter 8 - Periodic Properties Of The ElementsChapter 9 - Chemical Bonding I: The Lewis ModelChapter 10 - Chemical Bonding II: Molecular Shapes, Valence Bond Theory, And Molecular Orbital Theory
Chapter 11 - Liquids, Solids, And Intermolecular ForcesChapter 12 - Solids And Modern MaterialsChapter 13 - SolutionsChapter 14 - Chemical KineticsChapter 15 - Chemical EquilibriumChapter 16 - Acids And BasesChapter 17 - Aqueous Ionic EquilibriumChapter 18 - Free Energy And ThermodynamicsChapter 19 - ElectrochemistryChapter 20 - Radioactivity And Nuclear ChemistryChapter 21 - Organic ChemistryChapter 22 - BiochemistryChapter 23 - Chemistry Of The NonmentalsChapter 24 - Metals And MetallurgyChapter 25 - Transition Metals And Coordination Compounds
Sample Solutions for this Textbook
We offer sample solutions for Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition) homework problems. See examples below:
Chapter 1, Problem 1SAQChapter 2, Problem 1SAQChapter 3, Problem 1SAQExplanation: Molar mass of MnO2= 55 + 2 × 16 = 55 + 32 = 87 Number of moles of MnO2= 25.087 = 0.287...Given: Initial pressure, P1 = 547 mmHg Initial volume, V1 = 0.500 L Final volume, V2 = 225 mL =...Chapter 6, Problem 1SAQChapter 7, Problem 1SAQJustify reasons for the correct statement: Coulomb’s law states that the potential energy (E) of two...Explanation: Ionic bond is formed between a positive ion and a negative ion. Positive ion results...
Reason for correct option: Lewis structure of CBr4: CBr4 Has 25 valence electrons. The central atom...The molecules of gases are not rigid. They have large space between them, more as compared to...Justify reasons for the correct answer: Calculate the separation between the atomic layers in the...Justify reasons for the correct statement: Octane is a nonpolar solvent. A compound or solute that...Justify reasons for the correct statement: The average rate of the reaction is written as follows:...Justify reasons for correct statement: The given reaction is as follows: C(s)+2H2(g)⇌CH4(g) Here,...Justification for the correct option: When an acid donates its hydrogen ion, a conjugate base is...In the given buffer of 0.100 M in NH4Cl and 0.100 M in NH3, NH3 is weak base and NH4Cl is a...The phase transition is from solid to gas during the chemical reaction, so entropy increases and...The equation for this reaction as follows: VO2+(aq)+Sn(s)+H+(aq)→VO2+(aq)+Sn2+(aq)+H2O(l) Separate...The original atom is called parent nuclide, and the product of the decay is called the daughter...Justification for the correct statement: Carbon has a valency of 4. So, carbon can form covalent...The lipids are a diverse group of naturally occurring organic compounds and chemical components of...Justify reasons for the correct statement: The AlO2− units substitute for three-fourths of SiO2;...Justify reason for correct statement: Gold occurs in elemental state with some small particles and...When we write the electron configuration of Cu+ ion using the periodic table, we see that argon is...
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