Domanda del libro di testo
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.
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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 17, Problema 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.
Guida verificata passo dopo passo1
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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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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Percorso guidato
00:28
Solubility Rules
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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00:51Net Ionic Equations
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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Percorso guidato
01:09Acid-Base Reaction