Textbook Question
A 100.0 mL sample of a solution that is 0.100 M in HCl and 0.100 M in HCN is titrated with 0.100 M NaOH. Calculate the pH after the addition of the following volumes of NaOH:
(a) 0.0 mL
120
views
Ch.16 - Aqueous Equilibria: Acids & Bases
McMurry8th EditionChemistryISBN: 9781292336145
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 16, Problem 39c
The following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have been omitted for clarity.
(c) Which acid, if any, is a strong acid?
Verified step by step guidance1
Identify the components in each diagram: red spheres represent hydrogen ions (H+), blue spheres represent anions (A-), and white spheres represent undissociated acid molecules (HA).
Recall that a strong acid completely dissociates in water, meaning it will produce a high concentration of H+ and A- ions with no undissociated HA molecules.
Examine each diagram to determine the extent of dissociation: look for the presence of H+ and A- ions versus undissociated HA molecules.
Compare the diagrams: the one with the highest number of H+ and A- ions and no undissociated HA molecules represents the strong acid.
Conclude which acid (X, Y, or Z) is the strong acid based on the diagram that shows complete dissociation.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Strong Acids
Strong acids are substances that completely dissociate into their ions in aqueous solution. This means that when a strong acid is added to water, it releases all of its hydrogen ions (H+) into the solution, resulting in a high concentration of H+ ions. Common examples include hydrochloric acid (HCl) and sulfuric acid (H2SO4). Identifying strong acids is crucial for understanding their behavior in chemical reactions and their impact on pH levels.
Recommended video:
Guided course
01:09
Strong Acid-Strong Base Titration
Dissociation in Aqueous Solutions
Dissociation refers to the process by which an acid separates into its constituent ions when dissolved in water. For strong acids, this process is complete, while weak acids only partially dissociate. The extent of dissociation affects the acidity of the solution, which can be visualized in diagrams showing the distribution of ions in the solution. Understanding dissociation is essential for predicting the properties and reactivity of acids in solution.
Recommended video:
Guided course
01:11Types of Aqueous Solutions
Acid-Base Theory
Acid-base theory encompasses various models that explain the behavior of acids and bases. The Brønsted-Lowry theory defines acids as proton donors and bases as proton acceptors. This framework helps in understanding how acids interact with water and other substances, influencing the pH and chemical equilibrium in solutions. Recognizing these interactions is vital for identifying strong acids and predicting their effects in chemical reactions.
Recommended video:
Guided course
02:08Bronsted-Lowry Acid-Base Theory
Related Practice
Textbook Question
Locate sulfur, selenium, chlorine, and bromine in the periodictable:(a) Which binary acid 1H2S, H2Se, HCl, or HBr2 is the strongest?Which is the weakest? Explain.
277
views
Textbook Question
What is the pH and the principal source of H3O+ ions in 1.0 * 10-10 M HCl? (Hint: The pH of an acid solution can’t exceed 7.) What is the pH of 1.0 * 10-7 M HCl?
107
views
Textbook Question
The following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have been omitted for clarity.
(e) What is the percent dissociation in the solution of HZ?
487
views
Textbook Question
Which of the following pictures represents a solution of a weak diprotic acid, H2A? (Water molecules have been omitted for clarity.) Which pictures represent an impossible situation? Explain.
(a) (b) (c) (d)
570
views
Textbook Question
A 40.0 mL sample of a mixture of HCl and H3PO4 was titrated with 0.100 M NaOH. The first equivalence point was reached after 88.0 mL of base, and the second equivalence point was reached after 126.4 mL of base.
(e) Sketch the pH titration curve, and label the buffer regions and equivalence points.
90
views