Question

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

Write 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?

Answer 1

Basically I need help coming up with the equation, I have no idea what reactants to use or what the products are.

Answer 2

First you need to write down the balanced chemical equation
In this case that's AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)

Then you write down the complete ionic equation. To to that you need to separate all the aqueous compounds (the ones with (aq)) into ions. The solid compound in this case (AgCl) is left unseparated.
The complete ionic equation is:
Ag+ + NO3- + Na+ + Cl- --> AgCl(s) + Na+ + NO3-

Then you cancel out all the spectator ions. Those are the ones that are on both sides of the equation.

Whats left is : Ag+ + Cl- --> AgCl(s)

Answer 3

Okay so that's part i, I would do the same for part ii then?

Answer 4

(the last one is the net ionic equation)

Answer 5

The balanced equation will be Pb(NO3)2(aq) + 2NaCl(aq) --> PbCl2(s) + 2NaNO3

Answer 6

okay sorry, the Ksp expression for AgCl would be

Ksp = [products]/[reactants]
Ksp = [AgCl]/[Ag][Cl]

?

Answer 7

or do you not include the AgCl because it's solid, so it becomes 1/[Ag][Cl]

Answer 8

for the net ionic equation of ii I got Pb 2+ + 2Cl- --> PbCl2 (s)

Answer 9

and Ksp PbCl2 = 1/[Pb]^2[Cl]^2

Answer 10

oops I mean 1/[Pb 2+][Cl-]^2

Answer 11

Solids are not included when you calculate an equilibrium constant

Answer 12

Thanks for your help ^^

There's another part to the question, i made a new question for it. If you could help me I would really appreciate it :D

Answer 13

But isn't the NaCl solid? "Solid NaCl is added slowly..."

Answer 14

@Banterman
During the reaction the NaCl is not solid anymore.
When you add NaCl to water it will fall apart into Na+ and Cl- ions.