Answer:
B. Ksp = 1.7 × 10¯⁷
Explanation:
Hello there!
In this case, for this solubility equilibrium problem, we first need to set up the chemical reaction describing the dissolution of the involved salt, CuCl:
[tex]CuCl(s)\rightleftharpoons Cu^+(aq)+Cl^-(aq)[/tex]
Next, we write the corresponding equilibrium expression:
[tex]Ksp=[Cu^+][Cl^-][/tex]
Now, we need to calculate the concentrations of copper (I) and chloride ions at equilibrium; thus, given that 0.041 g of this solid is completely dissolved in 1.0 L of solution, we can firstly calculate the moles present in the solution:
[tex]n_{CuCl}=0.041gCuCl*\frac{1molCuCl}{99gCuCl} =4.14x10^-4mol[/tex]
Afterwards, since all the species in the reaction, CuCl, Cu+ and Cl- are in a 1:1:1 mole ratio, we realize that those moles correspond to ions in the solution, so their concentrations are:
[tex][Cu^+]=[Cl^-]=\frac{4.14x10^{-4}mol}{1.0L}= 4.14x10^{-4}M[/tex]
Then, we compute the Ksp by plug this value in the equilibrium expression:
[tex]Ksp=(4.14x10^{-4})(4.14x10^{-4})=1.7x10^{-7}[/tex]
Thus, the answer would be B. Ksp = 1.7 × 10¯⁷.
Regards!
