Chemistry 1126 PACE Self-Test
Study the MATH problems from the Self-Test.
Study the MATH problems from the Self-Test.
solvation
general term for the process of dissolving
Solubility depends on the _______ of the solution components and the existing conditions of _______ and _______.
identity ... pressure ... temperature
Scripture Verse
But if we hope that we see not, then do we with patience wait for it.
mole fraction X = moles of component/moles of solution
ratio of the number of moles of solution component to the number of moles of total solution
boiling-point elevation ∆Tb
increase in boiling point of a solvent caused by a solute
molaLity m = 1.00 mol solu/1.00 kg solv
indication of the number of moles of solute per kilogram of solvent
osmosis
transfer of solvent molecules into a solution through a semipermeable membrane
miscible
two substances in the same phase that are highly soluble in each other
immiscible
two substances in the same phase that are not soluble in each other
dissociation
formation of ions when an ionic compound dissolves
solubility
measure of how much solute will dissolve in a solvent
solute
substance dissolved in a solution
A solution consists of two or more components in a single _______.
phase
solution equilibrium
physical state in which solvation and crystallization occur at the same rate
hydrate MgBr2 * 6H2O
substance that holds a specific number of water molecules in its formula unit
hydrate
substance that holds a specific number of water molecules in its formula unit
molaRity M = 1.00 mol solu/1.00L soln
indication of the number of moles of solute per liter of solution
electrolyte
any substance which, when dissolved in water, produces a solution that conducts an electric current
molal boiling-point constant Kb
boiling-point constant of solvent in a 1.00-m solution of a nonvolatile, molecular solute
saturation
condition in which a solution contains the maximum amount of solute that may be dissolved
A solution is a _______ with a uniform consistency, but whose components do not ______ in definite proportions.
homogeneous combination ... chemically combine
Le Chatelier's principle
if any of the factors determining system equilibrium are changed, the system will adjust itself to counteract that change and reestablish equilibrium
heat of solution +∆Hsoln or -∆Hsoln
amount of heat absorbed or released when a solute dissolves in a specific amount of solvent
alloy
combination of a base metal and at least one other substance, which blend to form a solution with metallic properties
freezing-point depression ∆Tf
decrease in the freezing point of a solvent caused by a solute
solvent
dissolving medium of a solution
solute-solute solvent-solvent
endothermic interactions in the solution process
Zn⁺²(aq) + 2NO₃⁻(aq) + 2NH₄(aq) + S⁻²(aq) → 2NH₄⁺(aq) = 2NO₃⁻(aq) + ZnS(s) Zn⁺²(aq) + S⁻²(aq) → ZnS(s)
equations that show how dissociated ions react in aqueous solution
ionization
formation of ions when a molecular compound dissolves
spectator ions
ions that do not take part in the chemical reaction and are found in solution both before and after the chemical reaction
concentration
measurement of the amount of solute in a given amount of solvent
semipermeable membrane
thin material that permits only certain materials to pass through
Raoult's Law Psoln = Xsolv Psolv
vapor pressure of a solution is proportional to the mole fraction of the solvent
equilibrium vapor pressure
pressure exerted by vapor molecules of a system in equilibrium
hydration
process of dissolving a solute in water
colligative
properties that depend on the concentration of the solute in a solution but not on the identity of the solute
The components of a solution include in a _______ (substance dissolved) and a _______ (dissolving medium).
solute ... solution
Heat of solution is the total heat of three different energy changes caused by three types of interactions: _______ interactions, _______ interactions, and _______ interactions.
solute-solute ... solvent-solvent ... solute-solvent
supersaturated solution
solution that contains more solute than a normal saturated solution under the same conditions