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44 Cards in this Set

  • Front
  • Back
acids produce
H+ ions
acids conduct ___ and form
electricity and electrolytes
acids react with metal by being
corrosive
acids turn litnus paper
red
acids with phenolphthaletin
is clear
acids usually begin with
H
bases produce
OH- hydroxide)
bases conduct
electricity--form electrolytes
bases are corosive T or F
True
bases turn litmus paper
blue
bases with phenolphthalein
turn it pink
bases end in
OH
strong bases
dissociate (break down)
strong bases dissociate in
water
strong acid
ionizes (forms ions)
strong acids ionize in
water
acids and bases ionize/dissociate by
breaking apart to form (+) (-) ions
strong bases/acids have more or less ions
more
strong acids/bases are better or worse electrolytes
better
strong acids/bases conduct more or less electricity
more
pH sclae shows
strength and concentration
the pH numbers
0-14 (7 neutral)
neutralization is
a reaction b/t an acid and base to form salt and water
Arrhenius theory says acids
ionize to give off hydrogen ions in aqueous solution
Arrhenius theory says bases
ionize to give off hydroxide in aqueous solution
monoprotic acids have
one ionizable H; di, tri, etc
not all compounds that contain H are___; it depends on
acids--electronegativity
Bronsted-Lowery theory says acids
are a H ion donor
Bronsted-Lowery theory says bases
are a H ion acceptor
Bronsted-Lowery theory follows what other theory
Arrhenius
conjugate acids are
compounds formed when a base gains a H ion
conjugate bases are
compounds formed when an acid has donated a H ion
amphoteric act as
an acid or base (water)
Lewis theory says acids
accept a pair of electrons to form a covalent bond
Lewis theory says bases
can donate a pair of electrons to form a covalent bond
strong acids do what in water
completely ionize
strong acids are any
Binary Acid (HCl, HF, HBr)
strong acids are any acid with
2 or more oxygen than Hydrogen (H2SO4, HNO3)
strong bases and any
group I or II Hydroxide (except Be)
titration is a process of
adding a known amount of solution of known concentration to determine the concentration of another solution
standard solution is one of
known concentration
an end point is the point
at which the indicator changes color
buffers are solutions in which the
pH remains relatively constant when small ammounts of acid or base are added
calculating molarity and concentration
moles/Liter
M1V1=M2V2