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adelina 88 [10]

3 years ago

9

Solid NaCl is added slowly to a solution containing 0.10M AgNO3 and 0.20M Pb(NO3)2. Ksp AgCl = 1.8 E-10 Ksp PbCl2 = 1.6 E-5 Writ

e a net ionic equation and corresponding Ksp expression for the dissolution of solid i. Silver Chloride (AgCl) ii. lead (II) chloride (PbCl2) How do I do this?

1 answer:

ZanzabumX [31]3 years ago

8 0

Answer:

Ag+(aq) + Cl-(aq) <--->AgCl(s)

Ksp = [Ag+] [Cl-]

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

Ksp = [Pb+] [Cl-]^2

Explanation:

In this question, we are to write the net ionic equation and corresponding Ksp expression for the salts in the question.

We proceed as follows;

Ag+(aq) + Cl-(aq) <--->AgCl(s)

Ksp = [Ag+] [Cl-]

aii) Pb+2(aq) + 2Cl-(aq) <--->PbCl2(s)

Ksp = [Pb+] [Cl-]^2

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Complete Question

The complete question is shown on the first uploaded image

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