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Concentration required to begin precipitate pbcl2 for pbcl2 ksp=1. 17×10−5

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The concentration required to begin to precipitate PbCl2 for PbCl2 is 0.0216 M.

What is molarity?

Molarity is the measure of the concentration of any solute in per unit volume of the solution.

The reaction is [tex]\rm Pb^2^+(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s).[/tex]

The molarity of lead is 0.025 M

The ksp is given 17×10⁻⁵

Now, calculating the concentration

[tex][Pb^2^+] = 0.025 M.\\Ksp = 1.17 \times 10^-^5\\Ksp = [Pb^2^+] \times [Cl^-]^2\\[Cl^-] = \dfrac{\sqrt{ Ksp}}{[Pb^2^+]} \\\\[Cl^-] = \dfrac{\sqrt{ 0.0000117}}{0.025} \\[Cl^-] = 2.16 \times 10^-^2M.[/tex]

Thus, the concentration required to begin to precipitate PbCl2 for PbCl2 is 0.0216 M.

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