Solutions: Equations Flashcards
Percent composition by mass = ?
Mass of solute / Mass of SOLUTION x 100
Molarity = M = ?
Moles of solute / Liters of SOLUTION
Molality = m = ?
Moles of solute / Mass of SOLVENT (kg)
When does m = M ?
For dilute aqueous solutions at 25 degree C
Dilution formula = ?
M1.V1 = M2.V2
Glucose molecular weight = ?
180 g/mol
MX: Ksp = ?
x^2
MX2: Ksp = ?
4x^3
MX3: Ksp = ?
27x^4
How to calculate the solubility when there is already a little of one of the ions in the solution?
Write down: Ksp = [M]^a . [X]^b = (x)^a . (x + [X from solution])^b
Note that x in the second parentheses is negligible; therefore rewrite: Ksp = [M]^a . [X]^b = (x)^a . ([X from solution])^b
Solve for x
Raoult’s Law = ?
Applies to?
Pa = Xa . Pa (in its pure state)
Ideal solutions
Boiling point of water in terms of pressure?
1 atm
Boiling point elevation equation = ?
Delta Tb = i.Kb.m
Freezing point depression equation = ?
Delta Tf = i.Kf.m
Osmotic pressure = ?
i.M.R.T
When given a list of Ksps, how do I find the compound that is most soluble in water?
- First compare compounds that have the “same” formula: MX, MX2, MX3…
- Then compare them to each other by calculating x
What is Kf?
The stability constant = opposite of Ksp = [complex ion]/[reactant 1].[reactant 2]