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89 Cards in this Set
- Front
- Back
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solutions
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homogeneous mixtures of two or more substances that combine to form a single phase, usually a liquid phase
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gases can be dissolved in __
liquids can be dissolved in ____ solids can be dissolved in ____ |
liquids
liquids solids (metal alloys) |
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mixtures
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2+ substances that do not interact too much
ex) gas dissolved in gas |
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all solutions are considered mixtures but not all mixtures are considered solutions
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know this
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solution consists of a ____ and a ____
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solute; solvent
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solvent is the one whose ____ remains the same after mixing
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phase
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the solvent is usually in ____ quantity
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larger
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solute particles interact with solvent particles through ____ forces
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interparticle
ex) 1. ion-dipole 2. dipole-dipole 3. hydrogen bonding |
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solvation/dissolution
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electrostatic interaction between solute/solvent
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hydration
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when water is the solvent
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solvation involves ___ intermolecular bonds/interactions
and ____ new intermolecular bonds/interactions |
breaking; forming
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when the new bonds formed from solvation are stronger, the process is ______ and is favored at ____ temperartures
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exothermic; lower
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when the new bonds formed from solvation are weaker, the process is ____ and favored at ___ temperatures
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endothermic; higher
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what is an example of an exothermic solvation process?
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gas dissolved in a liquid
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most dissolutions are ____ in nature
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endothermic; create weaker bonds
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what is an example of an endothermic solvation process?
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dissolving sugar in water
-requires heat |
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when the enthalpy change in a solvation process occurs, it forms an ____ solution
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ideal
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the spontaneity is ___ only dependent upon the enthalpy change, but also on the _____
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NOT; ENTROPY
hence /\G = /\H - T/\S |
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spontaneity can occur with both ____ and ____ rxns
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endo/exothermic
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entropy ____ increases with dissolution and constant K + P
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ALWAYS
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spontaneous process results in a ___ in free energy while a non spontaneous process results in a ___ in free energy
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decrease (-/\G)
increase (+/\G) |
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solubility
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the maximum amount of that substance that can be dissolved in a particular solvent at a particular temperature
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saturated solution
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dissolved state = undissolved state; max amount added
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precipitants
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if solute added to already saturated solution; will not dissolve
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dilute
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low solute to solvent ratio
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concentrated
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high solute to solvent ratio
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when the change in the Gibbs function is ____ at a given temperature for the dissolution, the process is ___ and the solute will be soluble
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negative; spontaneous
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when the change in the Gibbs function is ____ at a given temperature for the dissolution, the process is ___ and the solute will be insoluble
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positive; non-spontaneous
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the spontaneity is directly proportional to the negativity of the gibbs function
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know this
a larger negative /\G will be more spontaneous than a smaller -/\G value |
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aqueous solution
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water = solvent
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all salts of alkali(I) metals are water soluble
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know this
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all salts of ammonium are water soluble
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know this
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all chlorides/bromides/iodides are water soluble EXCEPT....
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know this
when coupled with... Ag/Pb/Hg |
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all salts of sulfate are water soluble EXCEPT....
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know this
when coupled with Sr/Ca/Ba/Pb |
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all metal oxides are INSOLUBLE unless coupled WITH...
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know this
Ca/Sr/Ba and group I metals |
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ALL hydroxides are insoluble EXCEPT...
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know this
when coupled with Sr/Ba/Ca |
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ALL carbonates, phosphates, sulfides and sulfites are INSOLUBLE except....
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know this
when coupled with alkali metals and NH4+ |
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all sodium salts are completely soluble
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know this
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all nitrates are completely soluble
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know this
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Iron has 2 charges...
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+2/+3 = Fe
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Copper has 2 charges...
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+/+2 = Cu
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Fe names
+2 = +3 = |
ferrous
ferric |
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Cu names
+ = +2 = |
cuprous
cupric |
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monatomic anions (-ide)
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H-
F- O2- S2- N3- P3- |
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NO2- =
NO3- = |
Nitrite
Nitrate |
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SO3^2- =
SO4^2- = |
Sulfite
Sulfate |
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Chlorine
ClO- ClO2- ClO3- ClO4- |
hypochlorite
chlorite chlorate perchlorate |
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HCO3- =
HSO4- = H2PO4- = |
bicarbonate
bisulfate dihydrogen phosphate |
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cations have a ____ charge and anions have a ____ charge
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positive; negative
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electrolytes
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solutes that enable their solution to carry currents
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ionic compounds, when placed in water can act as ____ because the ions _____
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electrolytes; dissociate
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the electrical conductivity of a solution is governed by the ____ and the ____ of the ions in the solution
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presence; concentration
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strong electrolyte
example |
complete dissociation in water
-ionic compounds --KCl, NaCl -highly polar covalent bonds that dissociate --HCl |
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weak electrolyte
example |
ionizes or hydrolyzes incompletely in aqueous solution
-Hg2I2, acetic acid, ammonia |
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nonelectrolytes
example |
retain molecular structure in solution; do not ionize in aqueous solution
-nonpolar and organic compounds ex) O2, CO2, glucose |
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concentration
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the amount of solute dissolved in solvent
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percent composition
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(mass solute) / (mass solution) * 100
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mole fraction
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(number of moles of compound) /
(total moles of system) |
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molarity
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(moles of solute) / (liters of soln)
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molality
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(moles of solute) / (kg solvent)
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normality
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the number of equivalents of solute per liter of solution
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an equivalent = 1 mol of charge
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know this
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normality and acid base rxns
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concentrate on H+ ions
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normality and oxid-reduction rxns
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concentrate on electrons
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dilution
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MiVi =MfVf
m = molarity V = volume used to calculate new ratio with solvents... |
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dilution and EQ tip...
if asks how much is needed to be added to a solution to dilute a solution to a new molarity, the Vf you solve for is the final volume...you must subtract Vf - Vi to get what is needed to be added... |
know this
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practice: what volume of water needed to dilute 50mL of 3M H2SO4 to .75M H2SO4?
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MV =MV
= (3M)(50mL) = (.75M)(XmL) X = 200mL 200mL - 50mL = 150mL needed to dilute to get .75M H2SO4 |
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sparingly soluble salts are ionic compounds that have very low solubility in aqueous solutions
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know this
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the degree of solubility depends on the enthalpy, and entropy associated with the dissolution of the ionic solute
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know this
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common sparingly soluble compound
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AgCl
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solubility product constants are _____ dependent
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temperature
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value of constant for gas is dependent upon the _____
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pressure
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solubility product constant ____ with increasing temperature for nongas solutes and ____ for gas solutes
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increases
decreases |
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____ pressure for gas solutes leads to an _____ in the solubility product constant
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higher
increase |
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Q > K = supersaturation...
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precipitation occurs
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Q<K = unsaturated...
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still dissolve
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Q = K = saturation
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equilibrium
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slightly soluble salt of AB3 will have a Ksp value of...
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27X^4
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slightly soluble salt of AB2 will have a Ksp value of...
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4X^3
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slightly soluble salt of AB will have a Ksp value of...
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X^2
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solubility is ____ depending on the temperature
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variable
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solubility is dependent upon ____
for gas molecules |
pressure
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What is platelet aggregation?
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Step 3 in platelet plug formation
bridges form by fibrinogen |
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solubility is affected by other ____ added to the solution
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things/substances
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solubility of salt greatly reduced when it is dissolved in a soln that contains one of its constituent ions
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common ion effect
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presence of a common ion has ____ effect on the constant Ksp
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NO
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example: CaF2 is dissolved into CaCL2 solution...
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the solubility is decreased due to common ion effect
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breaking a bond is _____
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endothermic
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creating a bond is _____
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exothermic
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