Chapter 11
A solution that has above the normal amount of solute in it, causing special properties and precipitation if you are not careful
True or False: When a reaction reaches equilibrium, the reaction has finished and no forward or reverse reactions are observed
false: forward and reverse reactions are observed; they are equal and opposite meaning that no NET change is observed
If Q is higher than Ksp, what will happen?
Solute will precipitate
What phases are included in an ICE table
gas and aqueous
Molality is measured in
mols solute / kg solvent
Like dissolves like means what?
Molecules with the same or similar types of IMF will be able to dissolve in one another
What is the difference between Kc, Kp, and Q
Kc: concentration equilibrium constant
Kp: partial pressure equilibrium constant
Q: reaction quotient, for reactions not at equilibrium
The dissociation constant (Kd) for a complex ion is the _______ value of Kf
inverse/reciprocal
When would you calculate a Q value before starting an ICE table?
When you do not know which way the reaction will go (products and reactants all have initial values)
_____'s law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the solution
Henry's
What are the IMF ranked from strongest to weakest
Ion-dipole, hydrogen bonding, dipole-dipole, LDF
What is Le Châtelier’s Principle
On change of temperature, pressure, or concentration, chemical equilibrium will shift. The system shifts in equilibrium composition in a way that tends to counteract this change of variable
________ constant of a complex ion is the equilibrium constant for the formation of the complex ion from the aqueous metal ion and the ligands.
Formation constant, or stability constant, Kf,
When is the neglect x rule used? Why are we able to use it
It is used when we have a high starting concentration and a low Kc value. This indicates that the x value will not be very high and won't affect the large initial concentration that much, meaning we can neglect the change when solving.
What is Raoult's law and what is it used for?
P=P*X
it is used to calculate the change in vapor pressure in a solution with a nonvolatile solute
Name the colligative properties and if they are elevation or depression
- vapor pressure depression
- boiling point elevation
- freezing point depression
- osmotic pressure elevation
Say a reaction is at equilibrium, if you remove some reactant and add more product, what direction will the reaction shift?
it will shift in reverse to make more reactant
When dissolving AgCl in a solution of water vs a solution of table salt, you notice that more AgCl is able to dissolve in the water. What is this an application of?
common ion effect
Say you neglect x and get x = 1.3E-2. if you have an initial concentration of 0.02M. Would this x value be valid?
(1.3E-2 / 0.02) x 100% = 65% Nope! way above the 5% rule
When a salt dissolves in a solution, it breaks apart into multiple ions, effecting colligative properties. What is the name of this phenomenon and how does it affect the colligative properties.
Van't Hoff factor. It multiplies the colligative property changes by the number of ions produced by the salt.
A _______is a dispersion of particles of one substance (the dispersed phase) throughout another substance or solution (the continuous phase). They exhibit the ____ effect
Colloids; Tyndall effect
A reaction has a very high Kc, meaning at equilibrium there will be more _______(Reactants or products). If we have an even higher Q value, the reaction will shift and make more ________ (Reactants or products)
Products; reactants
__________ is the technique of separating two or more ions from a solution by adding a reactant that precipitates first one ion, then another ion, and so forth.
Fractional Precipitation
2NOCl (g) -> 2NO- (g) + Cl2 (g)
Say that the change is x (forward direction, no initial value) write an equation for the Kc
Kc = [x][2x]2 / [-2x]2
How do you convert Kc and Kp
Kp = Kc (RT)Δngas