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. In the given case, the value of [ H 3 O + ] is given as 3.5 × 10 − 3 M ; thus, the values of [ OH − ] and pH can be calculated as follows: [ H 3 O + ] × [ OH − ] = 1 .0 × 10 − 14 [ OH − ] = 1 .0 × 10 − 14 3.5 × 10 − 3 = 2.8 × 10 − 12 M pH = − log [ H 3 O + ] = − log ( 3.5 × 10 − 3 ) = 2.45 Since the value of pH is less than 7, the nature of the substance would be acidic. In the next case, the value of [ OH − ] is given as 3.8 × 10 − 7 M . Therefore, the values of [ H 3 O + ] and pH can be calculated as follows: [ H 3 O + ] × [ OH − ] = 1 .0 × 10 − 14 [ H 3 O + ] = 1 .0 × 10 − 14 3.8 × 10 − 7 = 2.6 × 10 − 8 M pH = − log [ H 3 O + ] = − log ( 2.6 × 10 − 8 M ) = 7.58 Since the value of pH is more than 7, the given substance is basic in nature

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Chapter 15, Problem 52E

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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 15, Problem 51E

Chapter 15, Problem 53E

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Chapter 15 Solutions

Chemistry: A Molecular Approach & Student Solutions Manual for Chemistry: A Molecular Approach, Books a la Carte Edition Package

Ch. 15 - Prob. 1SAQ Ch. 15 - Q2. Which pair is a Brønsted–Lowry conjugate...Ch. 15 - Prob. 3SAQ Ch. 15 - Prob. 4SAQ Ch. 15 - Q5. An HNO3(aq) solution has a pH of 1.75. What is...Ch. 15 - Q6. Find the pH of a 0.350 M aqueous benzoic acid...Ch. 15 - Q7. Find the pH of a 0.155 M HClO2(aq) solution....Ch. 15 - Prob. 8SAQ Ch. 15 - Prob. 9SAQ Ch. 15 - Prob. 10SAQ

Ch. 15 - Prob. 11SAQ Ch. 15 - Prob. 12SAQ Ch. 15 - Prob. 13SAQ Ch. 15 - Prob. 14SAQ Ch. 15 - Q15. Which acid has the largest Ka: HClO2(aq),...Ch. 15 - 1. What causes heartburn? What are some possible...Ch. 15 - 2. What are the general physical and chemical...Ch. 15 - Prob. 3E Ch. 15 - Prob. 4E Ch. 15 - Prob. 5E Ch. 15 - Prob. 6E Ch. 15 - Prob. 7E Ch. 15 - Prob. 8E Ch. 15 - Prob. 9E Ch. 15 - Prob. 10E Ch. 15 - 11. What are diprotic and triprotic acids? List an...Ch. 15 - 12. Define the acid ionization constant and...Ch. 15 - 13. Write an equation for the autoionization of...Ch. 15 - 14. What happens to the [OH–] of a solution when...Ch. 15 - Prob. 15E Ch. 15 - Prob. 16E Ch. 15 - Prob. 17E Ch. 15 - Prob. 18E Ch. 15 - Prob. 19E Ch. 15 - Prob. 20E Ch. 15 - Prob. 21E Ch. 15 - 22. How can you determine if an anion will act as...Ch. 15 - 23. What is the relationship between the acid...Ch. 15 - 24. What kinds of cations act as weak acids? List...Ch. 15 - 25. When calculating the [H3O+] for a polyprotic...Ch. 15 - Prob. 26E Ch. 15 - Prob. 27E Ch. 15 - Prob. 28E Ch. 15 - Prob. 29E Ch. 15 - Prob. 30E Ch. 15 - 31. What is acid rain? What causes it, and where...Ch. 15 - Prob. 32E Ch. 15 - 33. Identify each substance as an acid or a base...Ch. 15 - 34. Identify each substance as an acid or a base...Ch. 15 - 35. In each reaction, identify the Brønsted–Lowry...Ch. 15 - Prob. 36E Ch. 15 - 37. Write the formula for the conjugate base of...Ch. 15 - 38. Write the formula for the conjugate acid of...Ch. 15 - 39. Both H2O and H2PO4– are amphoteric. Write an...Ch. 15 - 40. Both HCO3– and HS– are amphoteric. Write an...Ch. 15 - Prob. 41E Ch. 15 - Prob. 42E Ch. 15 - Prob. 43E Ch. 15 - Prob. 44E Ch. 15 - Prob. 45E Ch. 15 - Prob. 46E Ch. 15 - 47. Calculate [OH–] in each aqueous solution at 25...Ch. 15 - Prob. 48E Ch. 15 - Prob. 49E Ch. 15 - 50. Calculate [H3O+] and [OH–] for each solution...Ch. 15 - Prob. 51E Ch. 15 - Prob. 52E Ch. 15 - 53. 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Calculate the [H3O+] and pH of each...Ch. 15 - 113. Calculate the concentration of all species in...Ch. 15 - 114. Calculate the concentration of all species in...Ch. 15 - 115. Calculate the [H3O+] and pH of each H2SO4...Ch. 15 - Prob. 116E Ch. 15 - Prob. 117E Ch. 15 - Prob. 118E Ch. 15 - 119. Based on their molecular structure, pick the...Ch. 15 - Prob. 120E Ch. 15 - Prob. 121E Ch. 15 - 122. Which is a stronger base, PO43– or AsO43–?...Ch. 15 - 123. Classify each species as either a Lewis acid...Ch. 15 - 124. Classify each species as either a Lewis acid...Ch. 15 - Prob. 125E Ch. 15 - Prob. 126E Ch. 15 - Prob. 127E Ch. 15 - Prob. 128E Ch. 15 - Prob. 129E Ch. 15 - Prob. 130E Ch. 15 - Prob. 131E Ch. 15 - Prob. 132E Ch. 15 - 133. Acid rain over the Great Lakes has a pH of...Ch. 15 - 134. White wines tend to be more acidic than red...Ch. 15 - 135. Common aspirin is acetylsalicylic acid, which...Ch. 15 - Prob. 136E Ch. 15 - Prob. 137E Ch. 15 - Prob. 138E Ch. 15 - Prob. 139E Ch. 15 - 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 15 Solutions