Chapter 12 Flashcards
Solubility
Amount of the substance that will dissolve in a given amount of solvent.
Aqueous Solutions
Water is the solvent. Gas, liquid, or solid are the solvent.
Entropy
A measure of energy randomization or energy dispersal in a system.
Miscible
Substances that are soluble in each other in all proportions
Enthalpy of Solution (∆Hsoln)
The sum of the changes in enthalpy for each step. (i) If the sum of endothermic terms is about equal in magnitude to the exothermic term, then ∆Hsoln is about zero. (ii) If the sum of endothermic terms is smaller in magnitude than the exothermic term, then ∆Hsoln is negative and the solution process is exothermic. (iii) If the sum of endothermic terms is greater in magnitude than the exothermic term, then ∆Hsoln is positive and the solution process is endothermic.
Heat of Hydration [∆H(hydration)]
The enthalpy change that occurs when 1 mol of gaseous solute ions are dissolved in water.
Dynamic Equilibrium
The point at which the rate of the reverse reaction equals the rate of the forward reaction.
Saturated Solution
A solution in which the dissolved solute is in dynamic equilibrium with any undissolved solute; any added solute will not dissolve.
Unsaturated Solution
A solution containing less than the equilibrium amount of solute; any added solute will dissolve until equilibrium is reached.
Supersaturated Solution
A solution containing more than the equilibrium amount of solute
Solubility of Gases
-Decreases with increasing temperature. -The higher the pressure of gas above a liquid, the more soluble the gas in the liquid.
Henry’s Law
Expresses the relationship between solubility of a gas and pressure: S(gas)=K(h)*P(gas)
Dilute Solution
Solution containing small quantities of solute relative to the amount of solvent.
Concentrated Solution
Solution containing large quantities of solute relative to the amount of solvent.
Molarity (M)
The amount of solute (moles) per volume of solution (L)
Molality (m)
The amount of solute (moles) per mass of solvent (kg)
ppm
(Mass Solute/Mass Solution) x 10^6
ppb
(Mass Solute/Mass Solution) x 10^9
Mole Fraction
Amount of Solute (moles) per total amount of solute + solvent (in moles).
Mole Percent
Mole Fraction x 100%
Colligative Property
-A property that depends on the number of particles dissolved in a solution, not on the particle type. -Four Types: (1) Vapor Pressure Lowering (2) Freezing Point Depression (3) Boiling Point Elevation (4) Osmotic Pressure
Vapor Pressure Lowering
The difference in vapor pressure between a pure solvent and a solution of the solvent. ∆P=P°(solvent) - P(solution)
Freezing Point Depression
The effect of a solute that causes a solution to have a lower melting point than the pure solvent.
Boiling Point Elevation
The effect of a solute that causes a solution to have a higher boiling point than the pure solvent. Note: BP of a solution containing nonvolatile solute is higher than the BP of the pure solvent.
Osmotic Pressure
The pressure required to stop osmotic flow.
π=MRT, T= 0.08206 L*atm/mol*K
Note:
*Osmosis: flow of solvent from a solution of lower concentration to one of higher concentration.
*Semipermeable Membrane: membrane that selectively allows select substances to pass through-separates two half of a cell.
van’t Hoff factor (i)
(moles of particles in solution) / (moles of formula units dissolved)
Henry’s Law
An equation that expresses the relationship between
solubility of a gas and pressure:
Sgas=KHPgas
Molarity (M)
M= Moles of Solute / Volume of Solution
Unites mol/L
Concentrations of Solutions
- Percent by Mass = (Mass of solute x 100%) / (Mass of Solution)
- ppm = (Mass of solute x 106) / (Mass of Solution)
- ppb = (Mass of solute x 109) / (Mass of Solution)
Mole Fraction (X)
Xsolute = (nsolute) / (nsolute + nsolvent)
Mole Percent
Mol % = X * 100%
Raoult’s Law
An equation used to determine the vapor pressure of a
solution:
Psolution = XsolventP°solvent
Vapor Pressure of a solution with volatile components
PA = XAP°A
PB = XBP°B
Ptotal = PA + PB
Molality (m)
(moles solute) / (mass solvent)
Units :mol / kg
Freezing Point Depression
(∆Tf) = m*Kf
Boiling Point Elevation
∆Tb = m*Kb