Textbook Question
The AIDS drug zalcitabine (also known as ddC) is a weak base with a pKb of 9.8. What percentage of the base is protonated in an aqueous zalcitabine solution containing 565 mg/L?
Ch.16 - Acids and Bases
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Chapter 16, Problem 138
Determine the pH of each solution. a. 0.0650 M HNO3 b. 0.150 M HNO2 c. 0.0195 M KOH d. 0.245 M CH3NH3I e. 0.318 M KC6H5O
Verified step by step guidance1
Step 1: Identify the nature of each compound in the solutions. HNO_3 is a strong acid, HNO_2 is a weak acid, KOH is a strong base, CH_3NH_3I is a salt of a weak base (CH_3NH_2) and a strong acid (HI), and KC_6H_5O is a salt of a weak acid (C_6H_5OH) and a strong base (KOH).
Step 2: For the strong acid HNO_3, calculate the pH directly from its concentration. Since HNO_3 is a strong acid, it dissociates completely, so [H^+] = 0.0650 M. Use the formula pH = -log[H^+].
Step 3: For the weak acid HNO_2, use the acid dissociation constant (K_a) to find [H^+]. Set up the equilibrium expression for the dissociation of HNO_2: HNO_2 ⇌ H^+ + NO_2^-. Use the expression K_a = [H^+][NO_2^-]/[HNO_2] and solve for [H^+]. Then calculate pH = -log[H^+].
Step 4: For the strong base KOH, calculate the pOH from its concentration. Since KOH is a strong base, it dissociates completely, so [OH^-] = 0.0195 M. Use the formula pOH = -log[OH^-], and then find pH using pH = 14 - pOH.
Step 5: For the salt CH_3NH_3I, determine the pH by considering the hydrolysis of CH_3NH_3^+. Write the hydrolysis reaction: CH_3NH_3^+ + H_2O ⇌ CH_3NH_2 + H_3O^+. Use the K_b of CH_3NH_2 to find K_a of CH_3NH_3^+ using K_w = K_a * K_b, and then calculate [H^+] to find pH.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH less than 7 indicates an acidic solution, while a pH greater than 7 indicates a basic solution. A pH of 7 is considered neutral. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration.
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The pH Scale
Strong vs. Weak Acids and Bases
Strong acids, like HNO3, completely dissociate in water, contributing all their hydrogen ions to the solution, while weak acids, like HNO2, only partially dissociate. Similarly, strong bases, such as KOH, fully dissociate to provide hydroxide ions, whereas weak bases, like CH3NH3, do not fully dissociate. Understanding the strength of acids and bases is crucial for calculating pH accurately.
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Concentration and pH Relationship
The concentration of hydrogen ions in a solution directly affects its pH. For strong acids, the pH can be calculated directly from the molarity of the acid, while for weak acids, the pH requires the use of the acid dissociation constant (Ka) to determine the concentration of hydrogen ions. For bases, the pOH can be calculated first, and then converted to pH using the relationship pH + pOH = 14.
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