Answer Happy

10) a) The molar solubility of iron(III)
sulfide in
a 0.236 M iron(III)
acetate solution is M.
b) The molar solubility of barium
phosphate in
a 0.122 M sodium
phosphate solution is M.
12) Write a balanced net ionic equation to show why the
solubility
of Zn3(PO4)2 (s)
increases in the presence of a strong acid and calculate the
equilibrium constant for the reaction of this sparingly soluble
salt with acid.

Consider only the FIRST STEP in the reaction with strong acid. Be
sure to specify states such as (aq) or (s).
+
+
+
K =
13) a) When 18.0 mL of
a 8.29×10-4 M potassium
bromide solution is combined
with 22.0 mL of
a 2.29×10-4 M lead
acetate solution does a precipitate form? fill
in the blank 1 (yes or no)

For these conditions the Reaction Quotient, Q, is equal
to
b) When 12.0 mL of
a 2.34×10-4 M silver
nitrate solution is combined
with 12.0 mL of
a 4.69×10-4 M sodium
phosphate solution does a precipitate form? fill
in the blank 1 (yes or no)

For these conditions the Reaction Quotient, Q, is equal
to
14) a) Solid potassium
sulfide is slowly added
to 75.0 mL of
a 0.0571 M iron(III)
nitrate solution. The concentration
of sulfide ion required to just initiate
precipitation is M.
b) Solid nickel(II) acetate is
slowly added to 75.0 mL of
a 0.0344 M potassium
sulfide solution. The concentration
of nickel ion required to just initiate
precipitation is M.
15) a) Solid sodium sulfide is
slowly added to 125 mL of
a copper(II) chloride solution until the
concentration of sulfide ion
is 0.0582 M. The maximum amount
of copper(II) ion remaining in solution
is M.
b) Solid ammonium
sulfide is slowly added
to 125 mL of
a 0.488 M lead
acetate solution until the concentration
of sulfide ion
is 0.0281 M. The mass
of lead ion remaining in solution
is grams.