From the Class Results, did the change significantly depending on the [K^-] conc

Question

From the Class Results, did the change significantly depending on the [K^-] concentration from KCl? Explain your answer. An experiment (similar to the one performed in this lab) involved dissolving lead (II) chloride, PbCl., in a 0.10 M solution of lead (II) nitrate, Pb(NO, ).. The chloride ion was then detected using Fajans Method. Fajans Method involves titrating CI against silver nitrate to make AgCl. The endpoint of the titration is observed when a dichlorofluorescein indicator changes from yellow to pink. a. Write the reaction for the dissociation of PbCl.(s). b. Write the^expression for the dissociation of PbCl_2.

Explanation / Answer

(3) Ksp, the solubility product constant is the equilibrium constant for a solid dissolving in an aqueous solution. The represents the maximum extent to which a solid can be dissolved in water. More soluble subtances have higher Ksp values.

KCl is an ionic compound and dissociates in water to form K+ and Cl- ions.

Ksp (for KCl) = [K+] x [Cl-]

Therefore, Ksp change significantly depends on [K+] concentration in the aqueous solution of KCl.

(4) (a) Reaction for the dissociation of PbCl2 (s) is:

PbCl2 (s) --------> Pb2+(aq) + 2Cl-(aq)

(b) Ksp expression for the dissociation of PbCl2 is:

Ksp = [Pb2+].[Cl-]2

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