17 Questions
What is the equilibrium constant expression for the reaction between Ca2+ and 2F-?
[Ca2+][F-]
In the solubility calculations of CaF2, what is the Ksp value at 25 °C?
4.0x10-11
For the reaction of Ag+ and Br-, what is the balanced equilibrium equation?
Ag+ + Br- -> AgBr
What does the Ksp value represent in a solubility product constant expression?
Product of ion concentrations at equilibrium
What is the solubility of AgBr calculated to be in the sample problem at 25 °C?
7.07 x 10^-7 M
What table is used in solubility calculations to track initial, change, and equilibrium values?
ICE (Initial, Change, Equilibrium) table
Calculate the solubility of PbSO4 if the Ksp value is 1.8x10-8.
4.2x10-7 M
What is the solubility of FeCO3 with a Ksp value of 3.5x10-12?
2.6x10-5 M
Determine the solubility of Ag+ and SO42- if the Ksp value is 1.8x10-10.
1.4x10-9 M
What is the solubility of CaF2 given a Ksp value of 1.6x10-9?
8.0x10-5 M
Compute the solubility of Ca3(PO4)2 if the Ksp value is 2.5x10-27.
1.25x10-18 M
What is the equilibrium constant expression, Ksp, for the reaction involving barium sulfate?
Ksp = [Ba2+][SO4 2-]
If the concentration of barium ions in a solution of barium sulfate is 2.0 x 10^-5 M, what is the concentration of sulfate ions?
1.0 x 10^-5 M
In the context of solubility equilibria, what does it mean if a compound is described as 'practically insoluble'?
It forms a precipitate in water
Which of the following statements best describes the technique of gravimetric analysis in relation to insoluble compounds?
It relies on measuring the weight of pure precipitates
What is the significance of the equilibrium constant, Kf, in the context of complexation equilibria?
It quantifies the stability of the complex formed
If a compound has a high solubility product constant (Ksp) value, what can be inferred about its solubility?
It is highly soluble in water
Study Notes
Solubility Equilibrium
- Solubility is the equilibrium amount of solute that dissolves in a given amount of solvent at a given temperature and pressure.
- Solubility can be mathematically expressed using the solubility product constant (Ksp).
Ksp Expression
- The Ksp expression is written as: Ksp = [A+] [B-]^n, where [A+] is the concentration of the cation and [B-]^n is the concentration of the anion raised to the power of its stoichiometric coefficient.
Calculations Involving Solubility Equilibria
- To compute the solubility of a reaction, follow these steps:
- Write the balanced equilibrium reaction.
- Write the Ksp expression.
- Make an ICE (Initial, Change, and Equilibrium) table.
- Substitute the values into the Ksp equation and solve for x.
Sample Problems
- Compute the solubility of the reaction of Ag+ and Br-: Ksp = 5.0x10^-13, x = 7.07 x10^-7 M.
- Compute the solubility of the reaction of Ca2+ and F-: Ksp = 4.0x10^-11, x = 2.15 x10^-4 M.
Assessment Task
- Enumerate and describe the different concepts in solubility.
- Write the solubility product expression for PbSO4, Ca3(PO4)2, and Fe(OH)3.
- Compute the solubility of the reaction of PbCl2, Fe2+ and CO32-, and Ca2+ and F-.
- Compute the solubility of the reaction of Ag+ and SO42-.
Complexation Equilibria
- The reaction between an acceptor metal ion M and a ligand L is characterized by an equilibrium constant (Kf).
- Example: The copper-EDTA complex at 25°C: Kf = 6.3 x 10^18.
Solubility Equilibria in Analysis
- Solubility equilibria can be used analytically to separate and determine the concentration of insoluble compounds.
- Example: Gravimetric analysis of sulfate ions using barium chloride (BaCl2).
- The solubility product (Ksp) is an equilibrium constant for the reaction: BaSO4 (s) = Ba2+ + SO4 2-.
This quiz covers the concepts of solubility including Ksp calculations. It includes topics such as making ICE tables, determining equilibrium concentrations, and using the solubility product expression. Test your understanding of Ksp calculations and solubility concepts with this assessment.
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