Question: the conversion of one precipitate to another by the addition of a suitable reagent is a process that involves heterogeneous equilibrium system. for example, silver chloride can be coverted to silver bromide by the additino of aqueous sodium bromide to a sample of silver chloride. the net conversion is AgCL(s) + Br goes <-> AgBr(s) +Cl(aq).

Question

How many grams of AgCl will be converted to AgBr by using 100.9ml of aqueous .100 M. NaBr?

Would you set up an ice table? How do you use the numbers given? Do you plug the .100 M of NaBr and than solve using x for Cl?

Answer 1

Notice in the reaction, each mole of Br converts one mole of Cl (not diatomic).

so if x is the amountof Br in AgBr, then x is also the amount of Cl on the right.

Yes, use x for this.

Answer 2

I can't find a Ksp value for this problem. I found a complex ion kf value for it though. How do i compute the molar solubility assuming hydrolysis occurs.

Answer 3

oops never mind it doesn't work that way

Answer 4

Please check my answer:

once i set up the ICE table i get this: the ksp= 1.8e-10= x/(.100-X)
x= 1.8e-9 M
1.8e-9 M * .1000L = 1.8e-10 mol (143.3212 g AgCl/ 1 mol)= 2.58e-8g AgCl.

Is this correct?