Solutions Flashcards
How to differentiate b/w solute and solvent
Solvent’s phase doesn’t change after mixing or, if same phase, one of greater quantity
When is solvation endo/exothermic
If new attractions are stronger than solvent alone, exothermic. Otherwise endo
Describe ideal solution
Enthalpy of dissolution = 0
What are sparingly soluble salts?
Solutes that dissolve minimally in solvent
What are the second 2 general solubility rules
- All chlorides, bromides, iodides are water soluble, with exceptions of ones formed with Ag+, Pb2+, Hg.2 2+
- All salts of SO4 2- are water soluble, except those with Ca2+, Sr2+, Ba2+, Pb2+
What’s the one infallible solubility rule?
All sodium (Na+) salts and nitrate (NO3 2-) salts are completely soluble
What do suffixes -ous/-ic, -ide, and -ite/-ate mean?
- ous: lesser charge than -ic
- ide: monoatomic anion
- ite: polyatomic oxyanion with lesser charge than -ate
What do prefixes hypo and per mean?
When series of oxyanions contains 4, 1 = hypo...ite 2= ...ite 3 = ...ate 4 = per...ate
What does bi and dihydrogen prefix mean?
Bi = single H addition (HCO3- = bicarbonate = hydrogen carbonate) Dihydrogen = 2 H addition (H2PO4- = dihydrogen phosphate)
Differentiate b/w electrolytes and nonelctrolytes
Electrolytes dissociate into ions in solution so can conduct electricity. Nonelectrolytes ionize weakly in solution
Explain percent composition by mass
100% * Mass of solute / mass of sltn (solute + solvent)
Explain mole fraction
moles of compound / # total moles of all species
Explain molality
# mol solute / # kg solvent Usually = molarity for dilute aqueous soltn's at 25ºC
Explain normality
# mole equivalents solute / L solution "Molarity of the stuff of interest"
Calculate dilution
M1V1 = M2V2
Calculate the Ksp of an ionic solid A.mB.n
K.sp = [A]^m * [B^n]
What’s the ion product?
Equivalent to Q of the K.sp
Describe the common ion effect
When an ion of a salt is already dissolved in a solvent, the solubility of that salt will be reduced. Results in same Ksp.
What are the first 2 general solubility rules?
- All salts of alkali metals are water soluble
2. All salts of NH4+ are water soluble
What are the final 3 general solubility rules?
- All metal oxides insoluble, except those with alkali metals and CaO, SrO, BaO which form turn into metal hydroxides in solution (CaO ==> Ca(OH)2)
- All hydroxides are insoluble except those with alkali metals and Ca2+, Sr2+, Ba2+
- All CO3 2-, PO4 3-, S 2-, and SO3 2- are insoluble, except those with alkali metals and ammonium
