Question

Including activity coefficients, calculate the concentration of
Pb^{2+} in a 0.100 M aqueous solution of NaIO_{3}
saturated with Pb(IO_{3})_{2}. (Hint: look up the
Ksp value for Pb(IO_{3})_{2}.

Answer #1

Ksp of Pb(IO3)2 = [Pb2+][IO3-]^2 = 2.5 x 10^-13

Using debye-huckel equation for activity coefficient

Y = inv.log.[(-0.51zi^2(sq.rt.(u))/(1+3.3r(sq.rt.(u))]

with,

zi = charge ; u = ionic strength ; r = radius

we get,

u = 1/2cizi^2

= 1/2(0.1 x 2^2 + 2 x 0.1 x 1^2)

= 0.3

So,

Y[Pb2+] = inv/log[(-0.51 x 2^2 x sq.rt.(0.3))/(1+3.3 x 0.45 x sq.rt.(0.3))]

= 0.242

Y[IO3-] = inv/log[(-0.51 x 1^2 x sq.rt.(0.3))/(1+3.3 x 0.45 x sq.rt.(0.3))]

= 0.701

so,

2.5 x 10^-13 = [Pb2+](0.242)(0.1 x 0.701)^2

[Pb2+] concentration = 2.10 x 10^-10 M

1)Suppose a solution contains 0.26 M Pb2 and 0.45 M Al3 .
Calculate the pH range that would allow Al(OH)3 to precipitate but
not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found
here
2a)Calculate the concentration of IO3– in a 3.89 mM Pb(NO3)2
solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 ×
10-13. Assume that Pb(IO3)2 is a negligible source of Pb2 compared
to Pb(NO3)2.
2b)A different solution contains dissolved NaIO3. What is the
concentration...

Part I: Calculate the concentration of IO3– in a 9.05 mM
Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is
2.5 × 10-13. Assume that Pb(IO3)2 is a negligible source of Pb2
compared to Pb(NO3)2.
Part II: A different solution contains dissolved NaIO3. What is
the concentration of NaIO3 if adding excess Pb(IO3)2(s) produces
[Pb2 ] = 3.80 × 10-6 M?
Please explain thoroughly. I am SO confused!! Thank you SO much
in advance!

Including activity coefficients, find the molar concentration of
Ba2+ in a 0.0500 M solution of tetramethylammonium
iodate (soluble salts which completely dissociates into
(CH3)4N+ and
IO3- ions in aqueous solution. Hint: the
[IO3- ] from the slightly soluble
BaIO3 in negligible.

Including activity coefficients, find the molar concentration of
Ba2+ in a 0.0500 M solution of tetramethylammonium iodate (soluble
salts which completely dissociates into (CH3)4N + and IO3 - ions in
aqueous solution. Hint: the [IO3 - ] from the slightly soluble
BaIO3 in negligible.

A saturated solution of Cu(IO3)2 was
prepared in 0.015 M KIO3. The copper concentration was
found to be 0.0010 M. Set up an ICE chart and calculate the
equilibrium [IO3-] and the
Ksp.

Find the concentration of I– in 0.050 M AgNO3 saturated with
AgI. Include activity coefficients in your solubility-product
expression. The Ksp of AgI is 8.3× 10–17. A table of activity
coefficients at various ionic strengths can be found
here.(https://sites.google.com/site/chempendix/activity-coefficients-for-aqueous-solutions-at-25-c)

a
saturated solution cu(io3)2 was prepared in 0.015 m klo3. The
copper concentration was found to be 0.0010 M. Set up an ice table
and caunlate the [IO3-] and the Ksp.

(Part A) The concentration of barium carbonate in a saturated
aqueous solution of the salt at 25°C is 7.07 x
10^-6 M. What is the
Ksp of this sparingly soluble
salt?
(Part B) After mixing an excess PbCl2
with a fixed amount of water, it is found that the equilibrium
concentration of Pb2+ is 1.6 ×
10–2M. What is
Ksp for PbCl2?

Find the concentration of Hg2^2+ in 0.10 M of KI saturated with
Hg2I2. Include activity coefficients in your solubility product
expression. The Ksp of Hg2I2 is 4.6x10^-29

Suppose a solution contains 0.26 M Pb2 and 0.49 M Al3 .
Calculate the pH range that would allow Al(OH)3 to precipitate but
not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found
here.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 10 minutes ago

asked 19 minutes ago

asked 28 minutes ago

asked 28 minutes ago

asked 40 minutes ago

asked 51 minutes ago

asked 54 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago