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

16th Edition

ISBN: 9781323463840

Author: Tro

Publisher: PEARSON C

See similar textbooks

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibri…

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Videos

Question

Chapter 16, Problem 52E

Interpretation Introduction

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

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 16, Problem 51E

Chapter 16, Problem 53E

Students have asked these similar questions

Correct each molecule in the drawing area below so that it has the skeletal ("line") structure it would have if it were dissolved in a 0.1 M aqueous solution of HCI. If there are no changes to be made, check the No changes box under the drawing area. No changes. HO Explanation Check NH, 2 W O :□ G ©2025 M unter Accessibility

An expression for the root mean square velocity, vrms, of a gas was derived. Using Maxwell’s velocity distribution, one can also calculate the mean velocity and the most probable velocity (mp) of a collection of molecules. The equations used for these two quantities are vmean=(8RT/πM)1/2 and vmp=(2RT/M)1/2 These values have a fixed relationship to each other.(a) Arrange these three quantities in order of increasing magnitude.(b) Show that the relative magnitudes are independent of the molar mass of the gas.(c) Use the smallest velocity as a reference for establishing the order of magnitude and determine the relationship between the larger and smaller values.

The reaction of solid dimethylhydrazine, (CH3)2N2H2, and liquefied dinitrogen tetroxide, N2O4, has been investigated for use as rocket fuel. The reaction produces the gases carbon dioxide (CO2), nitrogen (N2), and water vapor (H2O), which are ejected in the exhaust gases. In a controlled experiment, solid dimethylhydrazine was reacted with excess dinitrogen tetroxide, and the gases were collected in a closed balloon until a pressure of 2.50 atm and a temperature of 400.0 K were reached.(a) What are the partial pressures of CO2, N2, and H2O?(b) When the CO2 is removed by chemical reaction, what are the partial pressures of the remaining gases?

Chapter 16 Solutions

CHEMISTRY: MOLECULAR. W/ACCESS >IC<

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;...

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

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

Concept explainers

Videos

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

Want to see the full answer?

Chapter 16 Solutions