Calculating Ksp of Thallium Chloride at 100 Degrees Celsius

AI Thread Summary
The discussion centers on calculating the solubility product constant (Ksp) for Thallium(I) Chloride at 100 degrees Celsius, given a saturated solution concentration of 2.4 g per 100 ml. The conversion of this mass to molarity yields a concentration of 0.677 mol/L for chloride ions (Cl-). The Ksp expression is established as Ksp = [Tl+][Cl-]. It is clarified that since one mole of TlCl produces one mole of Tl+ and one mole of Cl-, the molar concentration of Thallium(I) ions (Tl+) is equal to that of chloride ions (Cl-). Thus, both species have a concentration of 0.677 mol/L, leading to the calculation of Ksp as (0.677)(0.677).
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I am having a tough time with getting my heard around what Ksp is; this question isbugging the heck out of me:

Q:
Calculate the Ksp of Thallium(1) Chloride at 100 Degrease celcius. The concentration of saturated solution of salt at this temperature is 2.4g / 100 ml .

Me:
As far as i got...

The Ksp of Thallium = [TI][Cl]

and

2.4 g / 100 ml is 0.677 mol / L of Cl ?


But beyond that I don't understand what i should be doing...
 
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Ksp = [Tl1+][Cl1-], which you wrote correctly.

So what is the molar concentration of each species? Tl and Cl must have the same concentration, and one mole of TlCl, yields one mole of each species.
 

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