Explanation Justification for the correct option: The pH and percent ionization of solution A can be calculated as follows: The reaction showing ionization of HNO 2 can be written as follows: HNO 2 ( a q ) + H 2 O ( l ) → H 3 O + ( a q ) + NO 2 − ( a q ) Let the concentration of hydronium ion be x . The ICE table can be written as follows: HNO 2 ( a q ) + H 2 O ( l ) → H 3 O + ( a q ) + NO 2 − ( a q ) Initial 0 .55 0 0 Change − x − x x Equilibrium 0.55 − x x x The expression for ionization constant K a can be written as follows: K a = [ H 3 O + ] [ NO 2 − ] [ HNO 2 ] The value of K a for HNO 2 is 4.6 × 10 − 4 . Substitute the values from the ICE table as follows: 4.6 × 10 − 4 = x . x ( 0.55 − x ) The value of x in ( 0.55 − x ) is small; thus; it can be neglected. 4.6 × 10 − 4 = x 2 0.55 4.6 × 10 − 4 × 0.55 = x 2 2.53 × 10 − 4 = x 2 2.53 × 10 − 4 = x Hence, x = 0.016 . The concentration of hydronium ion is 0.016. The pH can be calculated as follows: pH = − log [ H 3 O + ] = − log [ 0.016 ] = 1.79 The percent ionization can be calculated as follows: Percent ionization = Ionized acid Initial concentration of acid × 100 Percent ionization = [ H 3 O + ] equil [ H N O 2 ] equil × 100 = 0.016 0.55 × 100 = 2.90 % The pH and percent ionization of solution B can be calculated as follows: The reaction showing ionization of HNO 2 can be written as follows: HNO 2 ( a q ) + H 2 O ( l ) → H 3 O + ( a q ) + NO 2 − ( a q ) Let the concentration of hydronium ion be x

Chemistry: A Molecular Approach, Books a la Carte Edition; Modified MasteringChemistry with Pearson eText -- ValuePack Access Card -- for Chemistry: A Molecular Approach, 4/e

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ISBN: 9780134465654

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Chapter 16, Problem 9SAQ

Interpretation Introduction

Introduction: With a decrease in the degree of dissociation, the concentration increases. The percent ionization in case of a weak acid decreases on increasing the concentration of acid.

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Chapter 16, Problem 8SAQ

Chapter 16, Problem 10SAQ

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Chapter 16 Solutions

Chemistry: A Molecular Approach, Books a la Carte Edition; Modified MasteringChemistry with Pearson eText -- ValuePack Access Card -- for Chemistry: A Molecular Approach, 4/e

Ch. 16 - Prob. 1SAQ Ch. 16 - Q2. Which pair is a Brønsted–Lowry conjugate...Ch. 16 - Prob. 3SAQ Ch. 16 - Prob. 4SAQ Ch. 16 - Q5. An HNO3(aq) solution has a pH of 1.75. What is...Ch. 16 - Q6. Find the pH of a 0.350 M aqueous benzoic acid...Ch. 16 - Q7. Find the pH of a 0.155 M HClO2(aq) solution....Ch. 16 - Prob. 8SAQ Ch. 16 - Prob. 9SAQ Ch. 16 - Prob. 10SAQ

Ch. 16 - Prob. 11SAQ Ch. 16 - Prob. 12SAQ Ch. 16 - Prob. 13SAQ Ch. 16 - Prob. 14SAQ Ch. 16 - Q15. Which acid has the largest Ka: HClO2(aq),...Ch. 16 - 1. What causes heartburn? What are some possible...Ch. 16 - 2. What are the general physical and chemical...Ch. 16 - Prob. 3E Ch. 16 - Prob. 4E Ch. 16 - Prob. 5E Ch. 16 - Prob. 6E Ch. 16 - Prob. 7E Ch. 16 - Prob. 8E Ch. 16 - Prob. 9E Ch. 16 - Prob. 10E Ch. 16 - 11. What are diprotic and triprotic acids? List an...Ch. 16 - 12. Define the acid ionization constant and...Ch. 16 - 13. Write an equation for the autoionization of...Ch. 16 - 14. What happens to the [OH–] of a solution when...Ch. 16 - Prob. 15E Ch. 16 - Prob. 16E Ch. 16 - Prob. 17E Ch. 16 - Prob. 18E Ch. 16 - Prob. 19E Ch. 16 - Prob. 20E Ch. 16 - Prob. 21E Ch. 16 - 22. How can you determine if an anion will act as...Ch. 16 - 23. What is the relationship between the acid...Ch. 16 - 24. What kinds of cations act as weak acids? List...Ch. 16 - 25. When calculating the [H3O+] for a polyprotic...Ch. 16 - Prob. 26E Ch. 16 - Prob. 27E Ch. 16 - Prob. 28E Ch. 16 - Prob. 29E Ch. 16 - Prob. 30E Ch. 16 - 31. What is acid rain? What causes it, and where...Ch. 16 - Prob. 32E Ch. 16 - 33. Identify each substance as an acid or a base...Ch. 16 - 34. Identify each substance as an acid or a base...Ch. 16 - 35. In each reaction, identify the Brønsted–Lowry...Ch. 16 - Prob. 36E Ch. 16 - 37. Write the formula for the conjugate base of...Ch. 16 - 38. Write the formula for the conjugate acid of...Ch. 16 - 39. Both H2O and H2PO4– are amphoteric. Write an...Ch. 16 - 40. Both HCO3– and HS– are amphoteric. Write an...Ch. 16 - Prob. 41E Ch. 16 - Prob. 42E Ch. 16 - Prob. 43E Ch. 16 - Prob. 44E Ch. 16 - Prob. 45E Ch. 16 - Prob. 46E Ch. 16 - 47. Calculate [OH–] in each aqueous solution at 25...Ch. 16 - Prob. 48E Ch. 16 - Prob. 49E Ch. 16 - 50. Calculate [H3O+] and [OH–] for each solution...Ch. 16 - Prob. 51E Ch. 16 - Prob. 52E Ch. 16 - 53. Like all equilibrium constants, the value of...Ch. 16 - Prob. 54E Ch. 16 - 55. Calculate the pH of each acid solution....Ch. 16 - Prob. 56E Ch. 16 - Prob. 57E Ch. 16 - 58. Determine the pH of each solution. a. 0.048 M...Ch. 16 - Prob. 59E Ch. 16 - Prob. 60E Ch. 16 - 61. What is the pH of a solution in which 224 mL...Ch. 16 - Prob. 62E Ch. 16 - Prob. 63E Ch. 16 - 64. Determine the [H3O+] and pH of a 0.200 M...Ch. 16 - 65. Determine the pH of an HNO2 solution of each...Ch. 16 - 66. Determine the pH of an HF solution of each...Ch. 16 - Prob. 67E Ch. 16 - Prob. 68E Ch. 16 - Prob. 69E Ch. 16 - Prob. 70E Ch. 16 - 71. Determine the percent ionization of a 0.125 M...Ch. 16 - Prob. 72E Ch. 16 - Prob. 73E Ch. 16 - Prob. 74E Ch. 16 - Prob. 75E Ch. 16 - Prob. 76E Ch. 16 - Prob. 77E Ch. 16 - Prob. 78E Ch. 16 - Prob. 79E Ch. 16 - Prob. 80E Ch. 16 - Prob. 81E Ch. 16 - Prob. 82E Ch. 16 - Prob. 83E Ch. 16 - Prob. 84E Ch. 16 - Prob. 85E Ch. 16 - Prob. 86E Ch. 16 - Prob. 87E Ch. 16 - Prob. 88E Ch. 16 - Prob. 89E Ch. 16 - Prob. 90E Ch. 16 - Prob. 91E Ch. 16 - Prob. 92E Ch. 16 - Prob. 93E Ch. 16 - Prob. 94E Ch. 16 - Prob. 95E Ch. 16 - Prob. 96E Ch. 16 - 97. Determine the [OH–] and pH of a solution that...Ch. 16 - Prob. 98E Ch. 16 - Prob. 99E Ch. 16 - Prob. 100E Ch. 16 - Prob. 101E Ch. 16 - 102. Determine if each salt will form a solution...Ch. 16 - Prob. 103E Ch. 16 - Prob. 104E Ch. 16 - 105. Determine the pH of each solution. a. 0.10 M...Ch. 16 - 106. Determine the pH of each solution. a. 0.20 M...Ch. 16 - Prob. 107E Ch. 16 - Prob. 108E Ch. 16 - Prob. 109E Ch. 16 - Prob. 110E Ch. 16 - Prob. 111E Ch. 16 - 112. Calculate the [H3O+] and pH of each...Ch. 16 - 113. Calculate the concentration of all species in...Ch. 16 - 114. Calculate the concentration of all species in...Ch. 16 - 115. Calculate the [H3O+] and pH of each H2SO4...Ch. 16 - Prob. 116E Ch. 16 - Prob. 117E Ch. 16 - Prob. 118E Ch. 16 - 119. Based on their molecular structure, pick the...Ch. 16 - Prob. 120E Ch. 16 - Prob. 121E Ch. 16 - 122. Which is a stronger base, PO43– or AsO43–?...Ch. 16 - 123. Classify each species as either a Lewis acid...Ch. 16 - 124. Classify each species as either a Lewis acid...Ch. 16 - Prob. 125E Ch. 16 - Prob. 126E Ch. 16 - Prob. 127E Ch. 16 - Prob. 128E Ch. 16 - Prob. 129E Ch. 16 - Prob. 130E Ch. 16 - Prob. 131E Ch. 16 - Prob. 132E Ch. 16 - 133. Acid rain over the Great Lakes has a pH of...Ch. 16 - 134. White wines tend to be more acidic than red...Ch. 16 - 135. Common aspirin is acetylsalicylic acid, which...Ch. 16 - Prob. 136E Ch. 16 - Prob. 137E Ch. 16 - Prob. 138E Ch. 16 - Prob. 139E Ch. 16 - 140. Determine the pH of each two-component...Ch. 16 - Prob. 141E Ch. 16 - Prob. 142E Ch. 16 - 143. The pH of a 1.00 M solution of urea, a weak...Ch. 16 - 144. A solution is prepared by dissolving 0.10 mol...Ch. 16 - 145. Lactic acid is a weak acid found in milk. Its...Ch. 16 - Prob. 146E Ch. 16 - Prob. 147E Ch. 16 - Prob. 148E Ch. 16 - Prob. 149E Ch. 16 - 150. To what volume should you dilute 1 L of a...Ch. 16 - Prob. 151E Ch. 16 - Prob. 152E Ch. 16 - 153. Calculate the pH of a solution prepared from...Ch. 16 - 154. To 1.0 L of a 0.30 M solution of HClO2 is...Ch. 16 - 155. A mixture of Na2CO3 and NaHCO3 has a mass of...Ch. 16 - 156. A mixture of NaCN and NaHSO4 consists of a...Ch. 16 - 157. Without doing any calculations, determine...Ch. 16 - 158. Without doing any calculations, determine...Ch. 16 - Prob. 159E Ch. 16 - 160. Without using a calculator, determine the pH...Ch. 16 - Prob. 161QGW Ch. 16 - Prob. 162QGW Ch. 16 - Prob. 163QGW Ch. 16 - Prob. 164QGW Ch. 16 - Prob. 165QGW Ch. 16 - 166. Sulfur dioxide protects wine from spoiling;...

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