Textbook Question
From the value of Kf listed in Table 17.1, calculate the concentration of Ni2 +1aq2 and Ni1NH326 2+ that are present at equilibrium after dissolving 1.25 g NiCl2 in 100.0 mL of 0.20 M NH31aq2.
Ch.17 - Additional Aspects of Aqueous Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 17, Problem 64
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (a) MnS (b) PbF2 (c) AuCl3 (e) CuBr (d) Hg2C2O4.
Verified step by step guidance1
Identify the slightly soluble salt: Hg2C2O4 is mercury(I) oxalate.
Recognize that a strong acid will react with the anion of the salt. In this case, the oxalate ion (C2O4^2-) will react with the strong acid.
Write the dissociation equation for the slightly soluble salt: Hg2C2O4(s) ⇌ Hg2^2+(aq) + C2O4^2-(aq).
Consider the reaction of the oxalate ion with the strong acid (e.g., HCl): C2O4^2-(aq) + 2H+(aq) → H2C2O4(aq).
Combine the dissociation and the reaction with the strong acid to write the net ionic equation: Hg2C2O4(s) + 2H+(aq) → Hg2^2+(aq) + H2C2O4(aq).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Solubility and Slightly Soluble Salts
Solubility refers to the ability of a substance to dissolve in a solvent, typically water. Slightly soluble salts, like Hg2C2O4, do not dissolve significantly in water, leading to limited ionization. Understanding solubility is crucial for predicting how these salts will behave in reactions, particularly with acids.
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Net Ionic Equations
A net ionic equation represents the actual chemical species that are involved in a reaction, excluding spectator ions that do not participate. This simplification helps to focus on the essential changes occurring during the reaction, particularly in acid-base reactions where ions exchange or react to form new products.
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Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H+) from an acid to a base. In the case of slightly soluble salts reacting with strong acids, the acid can often protonate the anions of the salt, leading to the formation of soluble products. Understanding this interaction is key to writing accurate net ionic equations for such reactions.
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