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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?
Chemistry
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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You have 363 mL of a 1.25M potassium chloride solution, but you need to make a 0.50M potassium chloride solution. How many milli
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3 years ago
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