Exam 2 Flashcards
Is the solute normally lesser or greater?
lesser
Is the solvent normally lesser or greater?
greater
Under what conditions does a solute dissolve?
solute-solvent attraction > solute-solute attraction
hydrated ions
when positive and negative are separated and surrounded by water molecules
solvation
process of solute and solvent molecules interacting
hydration
when the solvent is water
water is a ___ molecule
polar
three characteristics of water
- uneven electron distribution
- bent molecular shape
- dissolves most substances
van der Waals forces
forces between neutral molecules
London dispersion forces
temporary attractive force that results from the electrons of two adjacent atoms occupying positions where the atoms form temporary ‘induced’ dipoles.
-weakest van deer waal force
dipole-dipole forces
between positive end of one polar molecule and the negative end of another polar molecule
-can be repulsive
hydrogen bond forces
H (partially positive) and lone pair
ion-dipole forces
attraction that results from the electrostatic attraction between an ion and a neutral molecule
molecules with similar intermolecular forces are most likely ____ to one another
soluble
immiscible
when liquids do not mix
water and ethanol are ____.
miscible
water and gasoline are ____.
immiscible
gasoline and CCl4 are ____.
miscible
is non polar covalent hydrophobic or hydrophilic?
hydrophobic
are polar covalent and ionic compounds hydrophilic or hydrophobic?
hydrophilic
Are hydrocarbons polar or non polar?
non polar
polar and ionic substances dissolve best in ____.
polar solvents
non polar substances dissolve best in _____.
non polar substances.
electrolyte
contain ions when in an aq solution
-conduct electricity
non electrolyte
does not form ions when in an aq solution.
strong acids and bases do what in water?
completely ionizes
HCl is a ___ and ___.
strong acid, strong electrolyte
acetic acid is a ___ and ____.
weak acid (ionizes slightly), weak electrolyte
ionic compounds are usually ____.
strong electrolytes
ionic compound
ions held together by ionic bonding.
Hbr is a ___.
strong acid
HI is a ___.
strong acid
HNO3 is a ___.
strong acid
H2SO4 is a ___.
strong acid
HClO3 is a ____.
strong acid
HClO4 is a ___.
strong acid
NaOH is a ___.
strong base
KOH is a ___.
strong base
Ca(OH)2 is a ____.
strong base
molecular (covalent) compounds, with the exception of acids and bases, are ___.
nonelectrolytes
dissociation
when ionic compounds dissolve in water and the anions and cations separate from each other.
When acids dissolve in water the molecule ionizes into __ and ____.
H+, anions
When something is highly soluble, the original compound can still be found in small amounts.
true
Does AgCl dissolve in water?
only slightly, leaves white powder.
unsaturated solution
when more solute can be added to the solvent and the solute will still dissolve
saturated solution
when more solute is added than will dissolve (solubility limit has been reached)
Solubility
maximum amount of solute that will dissolve in a specific amount of solvent at a given temp. (mol/L)
a compound is soluble than it ___.
dissolves in water.
> 0.1M
soluble
<0.01M
insoluble
> 0.01M but <0.1M
partially soluble
When two soluble solutions are mixed, they may form an insoluble compound and a ____.
precipitate
Nitrate (NO3-) and acetate (C2H3O2-) are ___.
soluble
Alkali metal (first row) and ammonium (NH4+) salts are ___.
soluble
Most Cl-,Br-, and I- salts are ___ except __,__, and ___.
soluble, Ag+,Pb2+,Hg2(2+)
most sulfates (SO42-) are ____ except __,___, and ___.
soluble, Ca2+,Sr2+, and Ba2+, Ag, Pb
Most hydroxides (OH-) are ___ except
insoluble, Na,K, Li, NH4+
What hydroxides are partially soluble?
Ba2+,Sr2+,Ca2+
S2- is ___, unless with ___.
insoluble, Li,Na,K,NH4+,Ca,Sr,Ba
CO32- is ___.
insoluble
CrO42- is ____.
insoluble
Cr2O72- is ____.
insoluble
PO43- is ____.
insoluble
-except with alkali metal cations, NH4+
soluble when combined with anions
Li+,Na+,K+,NH4+
Carbonate (CO32-) and phosphate ions (PO43-) ions are usually ____ unless with ____.
insoluble, Li,Na, K, NH4+
The solubility of one substance in another varies with ___ and ___.
temp, pressure
For most ionic substances, solubility in water ____ as temp ____.
increases, increases
The solubility of gases ___ with temperature
decreases
Even insoluble solids will dissociate a little.
true.
Acetic acid is a __ and ___.
weak electrolyte, very soluble.
Concentration
amount of solute in a total volume of solution
Molarity
amount of solute (mol)/volume of soln (L)
dilution equation
M1V1=M2V2
moles =
mass / molar mass
combustion reaction
substance and oxygen reacting
A reaction between ions in aq solution can form:
another solid, a gas, or a liquid
precipitation reactions are
double displacement reactions
molecular equation
complete chem formula with states.
total ionic equation
all soluble ionic substances are represented by the ions they form in solution.
net ionic equation
same as total ionic (ions) but has spectator ions removed.
binary acids
acid hydrogens attached to a nonmetal atom. Ex: HCl
oxyacids
acid hydrogens attached to an oxygen atom (H2SO4)
acid produces ___.
H+ (A)
bases produces ___.
OH- (A)
Acid is a ___.
H+ donor (B-L)
Base is a ___.
H+ acceptor (B-L)
pH < 7.0
acid
The molarity of H3O in the solution determines the ___.
pH
two arrows in an equation represents?
equilibrium
-usually a weak electrolyte
HF is a
weak acid
HNO2 is a
weak acid
HClO is a
weak acid
CH3COOH is a
weak acid
bases can be __ or ___
ionic or covalent
LiOH is a
strong base
NaOH is a
strong base
KOH is a
strong base
RbOH is a
strong base
CsOH is a
strong base
Ca(OH)2 is a
strong base
Sr(OH)2 is a
strong base
Ba(OH)2 is a
strong base
NH3 is a
weak base
Fe(OH)2 is a
weak base
amines are ___ and they are ____.
molecules with C-N in them, weak bases
pH =
-log[H3O+]
[H3O+]=
10^-pH
pOH=
-log[OH-]
pH + pOH =
14
when an acid and base are combined
water is formed and a salt (ionic) (neutralization reaction)
acid/base titrations are based on
the neutralization reaction
the titrant or standard solution
solution being added from buret
end point (titration)
point in titration where there is a physical change of the solution
indicator
changes physically near the equivalence point
equivalence point (titration)
