- Ch.1 - Matter, Measurement & Problem Solving106
- Ch.2 - Atoms & Elements97
- Ch.3 - Molecules, Compounds & Chemical Equations134
- Ch.4 - Chemical Quantities & Aqueous Reactions115
- Ch.5 - Gases98
- Ch.6 - Thermochemistry84
- Ch.7 - Quantum-Mechanical Model of the Atom49
- Ch.8 - Periodic Properties of the Elements81
- Ch.9 - Chemical Bonding I: The Lewis Model79
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory78
- Ch.11 - Liquids, Solids & Intermolecular Forces41
- Ch.12 - Solids and Modern Material35
- Ch.13 - Solutions66
- Ch.14 - Chemical Kinetics83
- Ch.15 - Chemical Equilibrium52
- Ch.16 - Acids and Bases107
- Ch.17 - Aqueous Ionic Equilibrium130
- Ch.18 - Free Energy and Thermodynamics74
- Ch.19 - Electrochemistry87
- Ch.20 - Radioactivity and Nuclear Chemistry50
- Ch.21 - Organic Chemistry143
Chapter 13, Problem 37
Silver nitrate has a lattice energy of -820 kJ/mol and a heat of solution of 22.6 kJ/mol. Calculate the heat of hydration for silver nitrate.
Video transcript
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. b. What can you conclude about the relative magnitudes of the lattice energy of lithium iodide and its heat of hydration?
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. c. Sketch a qualitative energy diagram similar to Figure 13.7 for the dissolution of LiI.
When lithium iodide (LiI) is dissolved in water, the solution becomes hotter. d. Why does the solution form? What drives the process?
Use the data to calculate the heats of hydration of lithium chloride and sodium chloride. Which of the two cations, lithium or sodium, has stronger ion–dipole interactions with water? Why?
Potassium nitrate has a lattice energy of -163.8 kcal/mol and a heat of hydration of -155.5 kcal/mol. How much potassium nitrate has to dissolve in water to absorb 1.00⨉102 kJ of heat?
A solution contains 25 g of NaCl per 100.0 g of water at 25 °C. Is the solution unsaturated, saturated, or supersaturated? (Use Figure 13.11.)