Textbook Question
A 1.00-L solution saturated at 25 C with calcium oxalate 1CaC2O42 contains 0.0061 g of CaC2O4. Calculate the solubility-product constant for this salt at 25 C.
1149
views
Ch.17 - Additional Aspects of Aqueous Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 17, Problem 53a
(a) I f t he molar solubility of CaF2 at 35°C i s 1.24 × 10–3 mol/L, what is Ksp at this temperature?
Verified step by step guidance1
Identify the dissolution equation for calcium fluoride: \( \text{CaF}_2 (s) \rightleftharpoons \text{Ca}^{2+} (aq) + 2\text{F}^- (aq) \).
Write the expression for the solubility product constant \( K_{sp} \) for the dissolution of \( \text{CaF}_2 \): \( K_{sp} = [\text{Ca}^{2+}][\text{F}^-]^2 \).
Recognize that the molar solubility of \( \text{CaF}_2 \) is given as \( 1.24 \times 10^{-3} \) mol/L, which represents the concentration of \( \text{Ca}^{2+} \) ions in solution.
Determine the concentration of \( \text{F}^- \) ions, which is twice the molar solubility of \( \text{CaF}_2 \), because each formula unit of \( \text{CaF}_2 \) produces two \( \text{F}^- \) ions.
Substitute the concentrations of \( \text{Ca}^{2+} \) and \( \text{F}^- \) into the \( K_{sp} \) expression and solve for \( K_{sp} \).
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Solubility
Molar solubility refers to the maximum amount of a solute that can dissolve in a given volume of solvent at a specific temperature, expressed in moles per liter (mol/L). In the case of CaF2, the molar solubility indicates how much calcium fluoride can dissolve in water before reaching saturation.
Recommended video:
Guided course
04:13
Molar Solubility Example
Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that quantifies the solubility of a sparingly soluble ionic compound. It is calculated from the concentrations of the ions in a saturated solution, raised to the power of their coefficients in the balanced dissolution equation. For CaF2, Ksp is derived from the concentrations of Ca²⁺ and F⁻ ions.
Recommended video:
Guided course
01:47Solubility Product Constant
Dissociation of Ionic Compounds
When ionic compounds like CaF2 dissolve in water, they dissociate into their constituent ions. For CaF2, the dissociation can be represented as CaF2(s) ⇌ Ca²⁺(aq) + 2F⁻(aq). Understanding this dissociation is crucial for calculating Ksp, as it directly relates the molar solubility to the concentrations of the ions produced in solution.
Recommended video:
Guided course
02:11Ionic Compounds Naming
Related Practice
Textbook Question
(b) Write the expression for the solubility-product constant for each of the following ionic compounds: MnCO3, Hg(OH)2, and Cu3(PO4)3.
713
views
Textbook Question
(b) If 0.0490 g of AgIO3 dissolves per liter of solution, calculate the solubility-product constant.
956
views
Textbook Question
(a) True or false: 'solubility' and 'solubility-product constant' are the same number for a given compound.
929
views
Textbook Question
(b) It is found that 1.1 × 10-2 g SrF2 dissolves per 100 mL of aqueous solution at 25°C. Calculate the solubility product for SrF2.
Textbook Question
The solubility of two slightly soluble salts of M2 + , MA and MZ2, is the same, 4 * 10-4 mol/L. (c) If you added an equal volume of a solution saturated in MA to one saturated in MZ2, what would be the equilibrium concentration of the cation, M2+?
857
views
1
rank