Chapter 17: Problem 45
Write balanced equations and solubility product expressions for the solubility
equilibria of the following compounds:
(a)
Short Answer
Expert verified
Write dissociation equations for each compound and use their ions to construct Ksp expressions.
Step by step solution
01
Understand Solubility Product
The solubility product, represented as K_sp, is used to quantify the solubility of sparingly soluble ionic compounds. It describes the equilibrium between a solid and its constituent ions in a saturated solution. The equilibrium reaction is written for the dissociation of the ionic compound into ions, and K_sp is the product of the ion concentrations each raised to the power of their stoichiometric coefficients.
02
Write the Equilibrium Equation for CuBr
The compound CuBr dissociates as follows: The solubility product expression for CuBr is:
03
Write the Equilibrium Equation for ZnC2O4
The compound ZnC2O4 dissociates as follows: The solubility product expression for ZnC2O4 is:
04
Write the Equilibrium Equation for Ag2CrO4
The compound Ag2CrO4 dissociates as follows: The solubility product expression for Ag2CrO4 is:
05
Write the Equilibrium Equation for Hg2Cl2
The compound Hg2Cl2 can be thought of as dissociating partially due to its dimerization: The solubility product expression for Hg2Cl2 is:
06
Write the Equilibrium Equation for AuCl3
The compound AuCl3 dissociates as follows: The solubility product expression for AuCl3 is:
07
Write the Equilibrium Equation for Mn3(PO4)2
The compound Mn3(PO4)2 dissociates as follows: The solubility product expression for Mn3(PO4)2 is:
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Solubility Product (K_sp)
The solubility product constant, denoted as , is an important concept in understanding solubility equilibria. It helps predict the extent to which a sparingly soluble compound will dissolve in water. Unlike common soluble salts, sparingly soluble compounds only slightly dissociate into their ions when they dissolve.
The solubility product is calculated as the product of the concentrations of the ions, each raised to the power of their stoichiometric coefficients from the balanced equilibrium equation. For example, if you have a compound that dissolves into and , the solubility product expression is . allows chemists to predict the behavior of ions in solution.
The solubility product is calculated as the product of the concentrations of the ions, each raised to the power of their stoichiometric coefficients from the balanced equilibrium equation. For example, if you have a compound
helps determine whether a precipitate will form in a solution.- A small
value indicates low solubility and therefore, a higher likelihood of precipitation.
Ionic Dissociation
Ionic dissociation is a process where an ionic compound separates into its constituent ions when dissolved in water. For sparingly soluble compounds, the extent of dissociation into ions is minimal. When you write an equilibrium equation for a compound, you represent how it dissociates into its ions in an aqueous solution.
Consider : when it dissolves, it separates into and , demonstrating ionic dissociation. The equilibrium equation is:
This is crucial because it shows the formation of ions that affect the rates and extents of chemical reactions.
Consider
- Dissociation strength affects the solubility of the compound.
- Proper representation of dissociation is essential for calculating
.
Equilibrium Equations
Equilibrium equations represent the state where the dissolution of a sparingly soluble compound and the precipitation form a balanced dynamic system. At equilibrium, the rate at which the solid dissolves is equal to the rate at which ions precipitate back into the solid form.
For example, consider the dissolution of : it dissociates into and : This illustrates the balance of dissolution and precipitation at equilibrium.
For example, consider the dissolution of
- The coefficients from the balanced chemical equation become exponents in the
expression. - Understanding equilibrium helps in predicting the concentration of ions in a saturated solution.
Sparingly Soluble Compounds
Sparingly soluble compounds are compounds that dissolve in water to only a small extent. Unlike highly soluble salts that completely dissociate into ions, these compounds reach a point where no more solute can dissolve in the solution, known as the saturation point.
Some examples include and . Upon dissolution, they establish an equilibrium between the solid phase and its ionic components in the solution.
Some examples include
- They usually have very low
values. - In practice, these compounds slightly affect the ionic concentration in solutions, making them relevant in precipitation reactions.