C)
NaI here is Strong electrolyte
It will dissociate completely to give [I-] = 0.01 M
At equilibrium:
PbI2 <----> Pb2+ + 2 I-
s 1*10^-2 + 2s
Ksp = [Pb2+][I-]^2
1.4*10^-8=(s)*(1*10^-2+ 2s)^2
Since Ksp is small, s can be ignored as compared to 1*10^-2
Above expression thus becomes:
1.4*10^-8=(s)*(1*10^-2)^2
1.4*10^-8= (s) * 10^-4
s = 1.4*10^-4 M
Answer: 1.4*10^-4 M
need help with 40 c 40. The Ksp for lead iodide (PbI2) is 1.4 X 10-8....
The Ksp for lead iodide (PI) is 1.4 x 10-8. Calculate the solubility of lead iodide in each of the following. a. water Solubility = mol/L b. 0.18 M Pb(NO3)2 Solubility = mol/L c. 0.018 M Nal Numeric input field Solubility = mol/L
A saturated solution of lead (II) iodide, PbI2 has an iodide concentration of 3.0 × 10-3 mol/ L. Calculate the solubility constant, Ksp, for lead (II) iodide. PbI2 (s) ß---à Pb2+(aq) + 2I-(aq) A saturated solution of lead (II) iodide, Pbl2 has an iodide concentration of 3.0 x 10-3 mol/ L. Calculate the solubility constant, Ksp, for lead (II) iodide Pbl2 (s) 8 3.5 x 10-8 5.0 x 10-8 2.8 x 10-8 1.4 x 10-8 -à Pb2 (aq)+2I(aq)
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1/ The molar solubility of PbI2 is 1.5 x 10-3 M. a/ What is the molar concentration of iodide ion in a saturated PbI2 solution? b/ Determine the solubility constant, Ksp, for lead(II) iodide 2/ Calculate the molar solubility of PBI2 in the presence of 0.10 M NaI 3/ Compare the molar solubility given in problem 1 and the molar solubility calculated in problem 2. Explain the cause of the difference.
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help please and thanks Calculate the molar solubility of lead (II) iodide, Pbl2, in water at 25°C (Kp= 1.4 x 10) 2. 3. Caleulate the molar solubility of lead (II) iodide, Pbl, in 0.1M Nal solution at 25°C (K- 1.4 x 10)
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