Question

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!

Answer #1

Part I

Pb(NO3)2--->Pb+2 + 2N03- meaning that the concentration of Pb+2 is equal to the concentration of Pb+2=Pb(NO3)2=9.05*10-3M.

In the other hand Pb(IO3)2 results on

Pb(IO3)2---> Pb+2 +2IO3-

Ksp= [Pb+2]*[IO3-]2=2.5*10-13

As the problem says that the only source of Pb+2 comes from the other reaction, the concentration of [Pb+2] is the same above [Pb+2]=9.05*10-3

Clearing [IO3-]= sq(2.5*10-13/9.05*10-3)=5.26*10-6

Part II

Pb(IO3)2---> Pb+2 +2IO3- and Ksp= [Pb+2]*[IO3-]2=2.5*10-13

Being now [Pb+2]=3.80*10-6, we can clear [IO-3] in solution that is 2-56*10-4

Only comming from NaIO3 dissociation the substract of the total [IO3-] minus the amounto produced by PbIO3 dissociation that is 2*3.80*10-6

So, NaIO3---> Na+ + IO3-

[NaIO3]=2.56*10-4- 2*3.86*10-6= 2.46*10-4

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...

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.

3) Find the concentration of Ca2+ and IO-3 in a saturated
Ca(IO3)2 solution prepared by adding Ca(IO3)2 to a 0.015 M solution
of KIO3. Ksp of Ca(IO3)¬2(s) is 4.4x10-7M3.

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.

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.

Calculate the molar solubility of Ca(IO3)2
in each solution below. The Ksp of calcium
iodate is
7.1
×
10−7.
(a) 0.070 M Ca(NO3)2
(b) 0.070 M NaIO3

(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?

Calculate the molar solubility of Ba(IO3)2 in a solution that is
also 0.0600 M in Ba(NO3)2. (Ksp (Ba(IO3)2) = 1.57 x 10-9 )

A particular saturated solution of PbI2 has [Pb2+]=5.0×10−3M and
[I−]=1.3×10−3M.
Part A
What is the value of Ksp for PbI2?
Express your answer using two significant figures.
Part B
What is [I−] in a saturated solution of PbI2 that has [Pb2+] =
2.5×10−4 M ?
Express your answer using two significant figures.
Part C
What is [Pb2+] in a saturated solution that has [I−] =
2.4×10−4 M ?
Express your answer using two significant figures.

If 550 mL of some Pb(NO3)2 solution is mixed with 400 mL of 6.70
x 10−2 M NaCl solution, what is the maximum concentration of the
Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00
x 10−5 M at this temperature.) Enter the concentration in M.

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