Chapter 20

Know the Following Terms

Complex ions Dissociation constant Fractional precipitation
Molar solubility Precipitate Solubility product constant
Work the Following Exercises

Write the solubility product constant:5, 6.

Calculate the value of Ksp form solubility data: 8a, b; 9c, d, 10 (use data from 8a, 8b, 8c); 12.

Uses of Ksp: 14, 15, 16d, 18, 20, 23, 25, 26, 29, 31, 33, 64, 65.

Fractional Precipitation: 34, 35, 37.

Simultaneous Equilibria: 42, 48, 49, 51,
53.

Dissolution of Precipitates and Complex Ions: 54, 55, 56, 58, 72.
Performance Objectives for Solubility Equilibrium and Complex Ion Equilibrium
Given the name of salt, write its chemical formula.

Given a specific salt, use the solubility rules to classify the salt as either water soluble or insoluble.

Given a specific salt, write the equation for the equilibrium occurring between the solid compound and its ion.

Given a specific salt, write the equilibrium expression represented by the solubility product constant.

Given the molar solubility or solubility in mass per volume of solution, calculate the value of the solubility product constant.

Knowing the value of Ksp of an insoluble salt, calculate the salts molar solubility and solubility expressed as grams of solute per 100 mL of solution.

Given a salt, look-up the value for its Ksp, in a table listing solubility product constants.

Given a slightly soluble salt, its Ksp and a solution containing a known concentration of the common ion, calculate the salt's molar solubility.

Given the molar solubility of a salt, express its solubility in grams per 100 mL of solution.

Given the concentration of a specific cation and anion, calculate the salt's reaction quotient.

Given a salt, write the reaction quotient.

Given the magnitude of the reaction quotient, predict the direction the reaction should proceed.

Given the concentration of ions in solution, predict whether precipitation will occur.

Given the volumes and the concentration of both anion and cation, predict if precipitation will occur.

Given the original concentrations of both the anion and cation, calculate the molar concentration of the ions left in solution after precipitation.

Given the concentration of two anions, calculate the concentration of the cation necessary to just begin precipitation of the least soluble salt.

Given a solution containing two anions and a common cation, using the values of Ksp, decide which salt would be least soluble.


Given the concentration of two anions, calculate the concentration of cation necessary to just begin to precipitate the more soluble of the two salts.

Given the concentration of two anions, calculate the percentage of the anion remaining for the least soluble salt.

Given an insoluble salt of a weak acid, write the equation demonstration the effect of lowering the pH.

Given the metal-ion concentrations in solution and all necessary Ksp's, calculate the range of pH required to separate a mixture of two
cations by precipitation as a metal sulfide.

Given a ligand, metal ion, and their complex-ion, write the equation representing the formation of the complex ion.

Given a ligand, metal ion, and their complex-ion, write the equation representing the dissociation of the complex-ion.

Given the equation of the formation of a complex-ion write the mass action expression for the formation constant (stability constant).

Given the equation for the dissociation of a complex-ion, write the mass action expression for the dissociation of the complex-ion.

Given the original concentration of the cation and ligand, calculate the concentration of the complex-ion, the cation, and the ligand at equilibrium.

Given the concentration of the ligand and knowing the Ksp and Kf for the complex-ion and the insoluble salt, respectively, calculate the solubility of the slightly soluble ionic compound.

Given the original concentration of a cation, anion, and ligand as well as knowing the necessary equilibrium constants, predict whether the cation and anion will form a precipitate.


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