Upload
caroline-carter
View
217
Download
1
Tags:
Embed Size (px)
Citation preview
Review of Solubility and Precipitation
Reactions
Aqueous Solutions
Compounds dissolved into water.
Can contain molecules or ions in a solution.
How do you distinguish between ion or molecule?
DISSOCIATION !!
The ability of a compound to breakdown in a solution into individual ions
Ionic Compounds Break down into cations and anions Electrical conductors—ions flow through solution
Molecular Compound Compound remains intact as “molecules,” no
breakdown Generally NOT electrical conductors
Solubility
How much solute dissolves in a solution to produce a saturated solution
Temperature and Pressure dependent Increase with increasing temperature Increases with decreasing temperature (ex. Water
in lake) Pressure increases, solubility increases (ex. Soda
can)
Which compounds are soluble in water?
1) BaCl22) Pb (NO3)2
3) Na2S
4) BaCO3
5) PbS
Precipitation Prediction
1) Write the reactants in ionic from breakdown into ionic form if compounds are soluble leave as molecules if insoluble
2) Determine the solubility of the products. Use solubility Rules
Precipitation Predictions (cont.)
3) Check to see if one product is insoluble in water. Product will fall out of solution, identified as precipitate
4) Write the net ionic equation Displays which ions are directly involved in the reaction, produce
the precipitate Ions existing on BOTH sides of the equation are “spectator ions”
(do NOT participate in precipitate formation) Spectator ions are eliminated
Example 1:
MgSO4 + KOH
Write the net ionic equation. Will a precipitate form?
Solubility Product Constant (Ksp)
Chemical Equilibrium so far-----
Gases
Acids and Bases
Slightly soluble Salts Many ionic compounds—only a small fraction
dissolves
Example 1:
BaSO4(s) Ba+2(aq) + SO4
-2(aq)
Indicates salt exists in “solubility equilibrium”—some dissolves, some does not
Solubility Product Constant (Ksp)
Equilibrium constant for slightly soluble salts
Indicates equilibrium between solid salt and the ions found in a solution when it dissociates Expression represents the product of the
concentrations of ions in equilibrium
Temperature dependent
Values found in table along with solubility equation (p. 678, Appendix C—p.A18)
Example 2:
Write a Ksp expression for an equilibrium in a saturated aqueous solution of iron (III) phosphate and for an equilibrium in a separate aqueous solution of chromium (III) hydroxide.
Ksp and Solution Molarity
Ksp is an equilibrium constant, NOT concentration
Molarity/concentration separate from Ksp
Ksp values Considered estimates due to ion attractions to
other ions in solution and Ksp values not exact Used only for slightly soluble salts
Increase concentration of ions, increase Ksp value
Example 3:
A saturated aqueous solution of silver carbonate contains 32 mg of Ag2CO3 per liter at 20°C. Calculate the Ksp for Ag2CO3 at 20°C.
Example 4:
Based on a Ksp value of 1.4 x 10-5 at 25°C for silver sulfate, calculate this compound’s molar solubility at 25°C. Ag2SO4(s) 2Ag+
(aq) + SO4-2
(aq)
Example 5:
Without any calculations, arrange the following in order of INCREASING molar solubility. MgF2, CaF2, PbCl2, PbI2
Homework
Ksp Practice Problem Set #1