Karteikarten
Exam 1 (Chapter 11)
Karten in diesem Stapel (65)
- 1Solubilitychemical property referring to the ability for a given substance, the solute, to dissolve in a solvent
- 2gases are not very soluble in liquids becausethere are weak solute-solvent interactions
- 3solubility of gaseous solutes in liquidsdecrease with increasing temperature AND
increases with decreasing temperature - 4solubility of gaseous solutes in liquidsincreases with increasing pressure AND
decreases with decreasing pressure - 5Henry's law is forun reactive gases in water
- 6Units for kHmol/L x atm
- 72 real world applications of solubility of gases in water1. carbonated drinks (effects of T and P)
2. thermal pollution of waterways - 8solubility of solid solutes in liquidsincreases with increasing temperature AND
decreases with decreasing temperature - 9solubility of solid solutes in liquidsno change with increased pressure AND
no change with decreased pressure - 10Particulate level changes that accompany dissolution of solute in a solventendothermic, add energy to overcome interactions
- 11Energy changes that accompany dissolution of a solute in a solvent includeexothermic, forming new interactions
- 12Enthalpy of solution (triangle H solution)overall energy change on dissolving a solute in a given solvent at a given T
(This can be done in a calorimeter) - 13Solutes with weaker IMF or lattice energy are more likelyto dissolve in an appropriate solvent
- 14Lattice energyenergy released when an ionic compound forms from gas phase ions
- 15Q1Q2 and dcharge on ions and distance between ions
- 16Enthalpy of hydrationtriangle Hhyrdation=
triangleH solvent-solvent + triangleH solute-solute - 17Higher ionic energy hashigher lattice energy and therefore has higher melting point
- 18Stronger lattice energy requiresmost energy input to separate
- 19Higher lattice energymore soluble in water
- 20Factors that affect vapor pressure includeT and intermolecular forces (vapor pressure)
- 21High TemperatureHigh Vapor Pressure
- 22High IMFLow Vapor Pressure
- 23If it says solidsits non volatile (ionic compounds)
- 24Vapor pressure loweringchange in the vapor pressure (decrease) due to adding/dissolving a non volatile solute
- 25Vapor pressure lowering depends on theamount of concentration of the non volatile solute not the solute identity
- 26Colligative propertyproperty that depends on the amount of dissolved solute (not its identity)
- 274 Colligative properties1. Vapor pressure lowering
2. Boiling point elevation
3. Freezing point depression
4. Osmotic pressure - 28Psolute, nonvolatile valueapprox. 0
- 29Ideal solution (with respect to Raoults law)solution that has the predicted vapor pressure
- 30Ideal solutions more likely whensolute and solvent are similar BECAUSE
solute-solute and solvent-solvent interactions are similar - 31Real (non-ideal) solution (with respect to Raoult's law)doesn't behave as predicted by Raoult's law
- 32Non ideal solutions with P total > predictedsolute-solvent interactions less/weaker than solvent-solvent and have a positive deviation
- 33Non ideal solutions with P total < predictedsolute-solvent interactions stronger than solvent-solvent and have a negative deviation
- 34solutions are less likely to behave ideally whenparticles are dissimilar, opposite of ideal
- 35In a solution composed of volatile solutes, the mole fraction in the vapor (gas phase) is different from the mole fraction in the liquidThe vapor is enriched with the more volatile component
- 36Fractional distillationseparation of a mixture by boiling point using a high surface are column that causes several boiling + condensation cycles.--At each cycle the vapor is enriched with the more volatile componenet
- 37Consequences of vapor pressure loweingfreezing point depression and boiling point elevation
- 38Molality (molal concentration)m, a unit for concentration based on # of particles and temperature independent
(mass does not change with temperature but volume does) - 39Boiling point happens whenvapor pressure = external pressure
- 40Van't Hoff factor (i)the effective number of particles that form per mole of dissolved solute
- 41Ion pairing in solution reducesi value
- 42Large i will havea low freezing point
- 43Limiting values of i are reached whenthe solution is infinitely dilute
- 44Raoult's law calculations must takei into account
- 45Boiling point elevationthe increase in boiling temperature of a solution containing a nonvolatile solute
- 46Freezing point depressionthe decrease in the freezing temperature of a solution due to containing a nonvolatile solute
- 47Freezing point depression or boiling point elevation can be used to determinemolar mass of nonelectrolyte solutes
- 48Osmosisthe flow of solvent across a semipermeable membrane due to a difference in concentration on either side of the membrane
- 49Semipermeable memberanethin material that allows solvent through but not solute
- 50osmotic pressure (pi)pressure that would be applied to stop osmosis
- 51osmolarityRTiM
- 52osmolalityRTim
- 53Solvent flows fromless concentrated to more concentrated until the concentrations are equal, if possible
- 54volume increases volume decreasesmore dilute
more concentrated - 55Isotonic (isosmotic)the same concentration of particles on both side of the membrane. Two solutions having same osmotic pressure.
- 56Hypertonic (hyperosmotic)having a relatively large osmotic pressure. one side has too much pressure.
- 57Hypotonic (hyposmotic)having a small osmotic pressure
- 58Osmosis stops whenboth sides are isotonic
- 59Most plant and animal cells aresemipermeable membranes, red blood cells are 0.3 osmolar = 0.9% NaCl 5% glucose
- 60Isotonic blood cell (normal)same solute concentration in solution matches inside the cell
- 61hypertonic blood cell (shriveled)H2O leaves the cell
- 62Hypotonic red blood cell (swelled)H2O flows into the cell, swells and can even burst (lysis)
- 63Reverse osmosisapplying pressure to a solution so solvent flows through the membrane, leaving solute behind (purifying the solvent)
- 64Desalinationwater purification from sea water to regular water
- 65Measuring colligative properties can allowestimates molar mass
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- Beschreibung
- Chemistry II Karteikarten am Exam 1 (Chapter 11), erstellt von Eddie Plata am 24/09/2017.
- Erstellt von
- Eddie Plata
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