PS9 - PROBLEM
SET
#9
...

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Unformatted text preview: PROBLEM
SET
#9
 aka
LaDuca
textbook
remember
FAIL
 1)
Explain
why
a
solution
of
HNO3
and
NaNO3
is
not
a
buffer.
 2
a)
What
is
the
pH
of
a
250
mL
solution
that
contains
0.33
M
HCOOH
and
0.42
M
 NaHCOO?
 b)
What
is
the
pH
of
this
solution
if
4.00
mL
of
a
0.072
M
HNO3
solution
is
added
to
 this
solution?
 c)
10
mL
of
pure
water
is
now
added
to
the
solution.

What
is
the
pH
now?
 3
a)
What
is
the
pH
of
a
250
mL
solution
that
contains
3.42
g
NH3
and
7.33
g
NH4Br?
 b)
What
is
the
pH
of
this
solution
if
5.25
mL
of
a
0.085
M
Ba(OH)2
solution
is
added
 to
this
solution?
 4)
How
many
grams
of
a
weak
acid
and
the
potassium
salt
of
its
conjugate
base
are
 needed
to
prepare
500
mL
of
a
pH
4.92
buffer?

You
can
use
the
Ka
table
in
your
text
 to
pick
the
best
choice
of
weak
acid.
 5)
30.00
mL
of
a
0.250
M
benzoic
acid
(Ka
=
6.4
x
10‐5)
solution
is
titrated
with
0.500
 M
KOH.

Determine
the
pH:
 a)
before
any
base
solution
was
added.
 b)
after
7.50
mL
base
solution
was
added.
 c)
after
9.50
mL
base
solution
was
added.
 d)
after
15.00
mL
base
solution
was
added.
 e)
after
17.25
mL
base
solution
was
added.
 6)
30.00
mL
of
a
0.250
M
HClO4
solution
is
titrated
with
0.500
M
KOH.

Determine
 the
pH:
 a)
before
any
base
solution
was
added.
 b)
after
7.50
mL
base
solution
was
added.
 c)
after
9.50
mL
base
solution
was
added.
 d)
after
15.00
mL
base
solution
was
added.
 e)
after
17.25
mL
base
solution
was
added.
 
 
 7)
30.00
mL
of
a
0.250
M
CH3NH2
(Kb
=
4.4
x
10‐4)
solution
is
titrated
with
0.500
M
 HCl.

Determine
the
pH:
 a)
before
any
acid
solution
was
added.
 b)
after
7.50
mL
acid
solution
was
added.
 c)
after
9.50
mL
acid
solution
was
added.
 d)
after
15.00
mL
acid
solution
was
added.
 e)
after
17.25
mL
acid
solution
was
added.
 
 
 
 ...
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This note was uploaded on 04/15/2009 for the course LB 171L taught by Professor All during the Spring '08 term at Michigan State University.

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