Chemistry

posted by .

Determination of the solubility product of PbI2. From the experimental data we obtain [I-] directly. To obtain Ksp for PbI2, we must calculate [Pb2+] in each equilibrium system. This is most easily done by constructing an equilibrium table. We first find the initial amount of I- and Pb2+ ion in each system from the way the mixture were made up. Knowing I- and the formula of lead iodide allows us to calculate [Pb2+], Ksp then follows directly.
PbI2 gives Pb2+(aq) + 2I- (aq)
Ksp = [Pb2+] [I-]^2
Data:
Test tube no. 1 2 3 4 5
mL 0.12 M Pb(NO3)2 5 5 5 5 saturated soln of PbI2
mL 0.03 M KI 2 3 4 5
mL 0.2 M KNO3 3 2 1 0
total volume in mL 10 10 10 10
absorbance of solution 0.300 0.330 0.412 0.405 0.333
[I-] in moles/Liter at equilibrium?
____
(Calculate for each of the five solutions)

Calculations

for each of the five solutions

initial no. of Pb2+?
___X 10^-5


initial no. of I-?
___X 10^-5

(no. moles I- at equilibrium)?
___X 10^-5

(no. moles I- precipitated)?
___X 10^-5

(no. moles Pb2+ precipitated)
___X 10^-5

(no. moles Pb2+
at equilibrium)
___X 10^-5

[Pb2+] at equilibrium)
____

Ksp PbI2
____

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    What [I-] should be maintained in KI(aq) to produce a solubility of 1.4×10−5 mol PbI2/L when PbI2 is added?
  2. chemistry

    When 10.0 mL of 0.012 M Pb(No3)2 is mixed with 10.0 mL of 0.030M KI, a yellow precipitate of PbI2(s) forms. a. Calculate the molarity of [Pb2+] b. calculate the initial molarity of [I-] c. On measuring the equilibrium concentration …
  3. chem

    Determination of the solubility product of PbI2. From the experimental data we obtain [I-] directly. To obtain Ksp for PbI2, we must calculate [Pb2+] in each equilibrium system. This is most easily done by constructing an equilibrium …
  4. chemistry

    What pb2+ concentration should be maintained in PbNO3 to produce a solubility of 1.7×10−4 PbI2/L when PbI2 is added?
  5. chemistry

    A solution of PbI2 has [Pb2+] = 4.5 x 10-5 and [I-] = 6.5 x 10-4. PbI2 has Ksp = 8.7 x 10-9. Write down the reaction that is taking place. Calculate Q. Is Q larger or smaller than the Ksp?
  6. Chemistry

    A solution of PbI2 has [Pb2+] = 4.5 x 10-5 and [I-] = 6.5 x 10-4. PbI2 has Ksp = 8.7 x 10-9. Write down the reaction that is taking place. Calculate Q. Is Q larger or smaller than the Ksp?
  7. Chemistry

    What [PB2+] should be maintained in Pb(NO3) to produce solubility of 1.0*10^-4 mol PbI2/L when PbI2 (s) is added?
  8. Chemistry

    Calculate the value of the equilibrium constant for the following reaction: PbI2 (s) + 2I- (aq) <-> PbI4 ^ 2- (aq) The solubility product constant Ksp for PbI2 is 9.8e-9 and the formation constant Kf for PbI4^2- is 3.0e4 I have …
  9. chem 100

    Super confusing question im not sure how to approach a. Determine the concentration of lead ion in solution (the molar solubility) if PbI2(s) is in equilibrium with water. Ksp = 9.8*10-9 b. From part a, it should be clear that if Pb2+(aq) …
  10. Chemistry (Urgent)

    Ksp of PbI2 at 25 degrees celcius and 15 degrees celcius is 7.5×10^-8 and 7.5×10^-9 respectively. (Pb=207 I=127) 1) write an expression for the equilibrium of PbI2 2)write an equation for the Ksp of PbI2 3)calculate the solubility …

More Similar Questions