Domanda del libro di testo
A particular saturated solution of Ca3(PO4)2 has [Ca2+] = [PO43-] = 2.9 x 10^-7 M.
(c) What is [PO43-] in a saturated solution that has [Ca2+] = 0.010 M?
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Ch.17 - Applications of Aqueous Equilibria
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 17, Problema 99
For each of the following compounds, write a balanced net ionic equation for the dissolution of the compound in water, and write the equilibrium-constant expression for Ksp. (d) Hg2Cl2
Guida verificata passo dopo passo1
Identify the compound: Hg2Cl2 is mercury(I) chloride, which is a sparingly soluble salt in water.
Write the dissolution equation: When Hg2Cl2 dissolves in water, it dissociates into its ions. The balanced equation is: Hg2Cl2(s) ⇌ Hg2^2+(aq) + 2Cl^-(aq).
Write the net ionic equation: Since Hg2Cl2 is a solid and does not appear in the net ionic equation, the net ionic equation is the same as the dissolution equation: Hg2Cl2(s) ⇌ Hg2^2+(aq) + 2Cl^-(aq).
Define the solubility product constant (Ksp): The Ksp expression is based on the concentrations of the ions in the solution at equilibrium.
Write the Ksp expression: For the dissolution of Hg2Cl2, the Ksp expression is Ksp = [Hg2^2+][Cl^-]^2, where [Hg2^2+] and [Cl^-] are the molar concentrations of the ions at equilibrium.
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Net Ionic Equations
A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions that do not participate in the reaction. In the context of dissolution, it shows the ions that form when a compound dissolves in water, highlighting the actual chemical change occurring in the solution.
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Percorso guidato
00:51
Net Ionic Equations
Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It quantifies the extent to which a compound can dissolve in water, expressed as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation.
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01:47Solubility Product Constant
Dissociation of Ionic Compounds
Dissociation refers to the process by which an ionic compound separates into its constituent ions when dissolved in water. For example, when mercurous chloride (Hg2Cl2) dissolves, it dissociates into mercury (I) ions and chloride ions, which is essential for writing the net ionic equation and determining the Ksp expression.
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02:11Ionic Compounds Naming
Pratica correlata
Domanda del libro di testo
The titration of 0.02500 L of a diprotic acid solution with 0.1000 M NaOH requires 34.72 mL of titrant to reach the second equivalence point. The pH is 3.95 at the first equiva-lence point and 9.27 at the second equivalence point. If the acid solution contained 0.2015 g of the acid, what is the molar mass, pKa1, and pKa2 of the acid?
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Domanda del libro di testo
Consider the titration of 50.0 mL of 1.00 M H3PO4 with 1.00 M KOH. Calculate the pH after the addition of each of the following volumes of base. (a) 25.0 mL (c) 75.0 mL
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Domanda del libro di testo
Consider the titration of 50.0 mL of 1.00 M H3PO4 with 1.00 M KOH. Calculate the pH after the addition of each of the following volumes of base. (b) 50.0 mL (d) 100.0 mL
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