A saturated solution of Pbl2 (Ksp= 7.9*10-9) contains [I']=0.00055 M. Find [Pbl3] if theformation constant for Pbl3 (aka B3) is Kf = 8.3*10³.%3DO 2.0*10-11 M6.6*10-8 M3.6*10-8 MO 6.6*10-5 M

ANSWER : If we add iodine ions in to a lead ion solution , a solid PbI2 precipitate will form ,then…

Answered: A saturated solution of Pbl2 (Ksp=…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 8P

See similar textbooks

Related questions

Question

A saturated solution of Pbl2 (Ksp= 7.9*10-9) contains [I']=0.00055 M. Find [Pbl3] if the
formation constant for Pbl3 (aka B3) is Kf = 8.3*10³.
%3D
O 2.0*10-11 M
6.6*10-8 M
3.6*10-8 M
O 6.6*10-5 M

Expert Solution

Step 1

ANSWER :

If we add iodine ions in to a lead ion solution , a solid PbI₂ precipitate will form ,then if add more iodine ions , the solid form will dissolve due to the formation of complex ions.

This behavior of lead and iodine can be explained by the following reactions and its equilibrium constants :

$P b I_{2} + I^{-} \leftrightarrow P b I_{3}^{-} (a q); K_{f} o r β_{3} = 8.3 * 10^{3} = 8300.0 K_{f} = \frac{[P b I_{3}^{-}]}{[P b I_{2}] [I^{-}]} 8300 = \frac{[P b I_{3}^{-}]}{[7.9 * 10^{- 9}] [0.00055]} 8300 = \frac{[P b I_{3}^{-}]}{[0.004345 * 10^{- 9}]} [P b I_{3}^{-}] = 8300 x 0.004345 * 10^{- 9} [P b I_{3}^{-}] = 36.06 x 10^{- 9} H e n c e, [P b I_{3}^{-}] = 3.6 x 10^{- 8} M$

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions