Explain to me how to make a 1 molar solution of Copper II chloride. You should include the mass of the solid CuCl2, the volume of water needed, etc. Then, explain how you would use that solution to make a 0.5 molar solution (a dilution...how much water do you need to add?). Make sure to include:
all the relevant calculations
A visual representation of the solution (what are the ions present in the solution?) What is the solvent?

It is 4.92 e-4 sorry if i am wrong

The answer is 1.82 j/g°c                  

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.

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