Question

Including activity coefficients, calculate the concentration of Pb2+ in a 0.100 M aqueous solution of NaIO3...

Including activity coefficients, calculate the concentration of Pb2+ in a 0.100 M aqueous solution of NaIO3 saturated with Pb(IO3)2. (Hint: look up the Ksp value for Pb(IO3)2.

Homework Answers

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

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1)Suppose a solution contains 0.26 M Pb2 and 0.45 M Al3 . Calculate the pH range...
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....
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...
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...
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...
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...
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...
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...
(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...
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...
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
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT