Explanation The pH range for acidic substances varies from 1 to 7. For neutral substances it is 7, and for basic substances the value of pH ranges from 7.1 to 14. Since the value of pH is less than 7, the nature of the substance would be acidic. Furthermore, the values of [ H 3 O + ] and [ OH − ] can be calculated as follows: pH = − log [ H 3 O + ] log [ H 3 O + ] = − pH 10 log [ H 3 O + ] = 10 − pH [ H 3 O + ] = 10 − pH For the p H = 3.15 , [ H 3 O + ] can be calculated as: [ H 3 O + ] = 10 − pH = 10 − 3 .15 = 7 .1 × 10 − 4 M The [ O H − ] can be calculated as: [ H 3 O + ] × [ OH − ] = 1 .0 × 10 − 14 [ OH − ] = 1 .0 × 10 − 14 7 .1 × 10 − 4 = 1.4 × 10 − 11 M In the next case, [ H 3 O + ] is given as 3.7 × 10 − 9 M . Thus, the values of [ OH − ] and pH and acidic or basic nature can be calculated as follows: [ H 3 O + ] × [ OH − ] = 1 .0 × 10 − 14 [ OH − ] = 1 .0 × 10 − 14 3

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Chapter 16, Problem 51E

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To determine: The values of [H3O+], [OH−], and pH (power of hydrogen), and whether the solution is acidic or basic in nature.

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Chapter 16, Problem 50E

Chapter 16, Problem 52E

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Chapter 16 Solutions

Chemistry: A Molecular Approach (4th Edition)

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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. 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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. 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The values of [ H 3 O + ] , [ OH − ] , and pH (power of hydrogen), and whether the solution is acidic or basic in nature.

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To determine: The values of [H3O+], [OH−], and pH (power of hydrogen), and whether the solution is acidic or basic in nature.

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Chapter 16 Solutions