To determine the percent of PdCl2 extracted from a 25.0 mL solution into 10.0 mL of tri-n-butylphosphate, we can use the distribution ratio and the initial concentration of PdCl2.

First, we need to calculate the initial moles of PdCl2 in the aqueous phase (25.0 mL of a 7x10^-4 M solution):

Initial moles of PdCl2 in the aqueous phase = (0.0007 mol/L) x (0.025 L) = 1.75 x 10^-5 moles of PdCl2

Now, we can use the distribution ratio (D) to find out how much PdCl2 will be extracted into the organic phase (tri-n-butylphosphate). The distribution ratio is defined as:

D = (moles of PdCl2 in the organic phase) / (moles of PdCl2 in the aqueous phase)

We are given that D = 2.3. So, we can set up the equation:

2.3 = (moles of PdCl2 in the organic phase) / (1.75 x 10^-5 moles of PdCl2 in the aqueous phase)

Now, solve for the moles of PdCl2 in the organic phase:

moles of PdCl2 in the organic phase = 2.3 x 1.75 x 10^-5 = 4.025 x 10^-5 moles

Finally, to find the percent of PdCl2 extracted into the organic phase, divide the moles in the organic phase by the total moles initially present and multiply by 100:

Percent extraction = (4.025 x 10^-5 moles / 1.75 x 10^-5 moles) x 100 ≈ 230%

So, approximately 230% of the PdCl2 will be extracted from the aqueous phase into the organic phase. This might seem counterintuitive, but it's a common result when dealing with distribution ratios and is often used to describe the efficiency of the extraction process.
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