Calculating Ksp of Thallium Chloride at 100 Degrees Celsius

[[aq]]

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...

 

[Astronuc]

K_sp = [Tl¹⁺][Cl^1-], 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.

 

[ravenprp]

A:

Calculating the Ksp of a compound involves determining the solubility product constant, which is a measure of how much of the compound can dissolve in water at a given temperature. In this case, we are looking at the solubility of Thallium Chloride at 100 degrees Celsius.

First, we need to write the balanced chemical equation for the dissolution of Thallium Chloride in water:

TlCl (s) --> Tl+ (aq) + Cl- (aq)

Next, we need to determine the molar solubility of Thallium Chloride at 100 degrees Celsius. This is given as 2.4g / 100 ml, which can be converted to 0.024 g / mL. Since the molar mass of TlCl is 239.84 g/mol, this means that the molar solubility is 0.0001 mol/L.

Now, we can use this molar solubility to calculate the Ksp:

Ksp = [Tl+][Cl-] = (0.0001 mol/L)(0.0001 mol/L) = 1 x 10^-8

Therefore, the Ksp of Thallium Chloride at 100 degrees Celsius is 1 x 10^-8. I hope this helps clarify the concept of Ksp for you.