   Chapter 25.8, Problem 25.9CYU

Chapter
Section
Textbook Problem

To measure the solubility for PbCrO4 you mix a small amount of a lead(ll) salt having radioactive 212Pb with a lead salt containing 0.0100 g of lead. To this mixture you add enough K2CrO4 to completely precipitate the lead(ll) ions as PbCrO4. The supernatant solution still contains a trace of lead, of course, and when you evaporate 10.00 mL of this solution to solid PbCrO4 you find a radioactivity that is 4.17 × 10–5 of what it is for the pure 212Pb salt. Calculate the solubility of PbCrO4 in mol/L (Adapted from C. E. Housecraft and A. G. Sharpe, Inorganic Chemistry, Pearson, 3rd edition, 2008, p. 84.)

Interpretation Introduction

Interpretation: In lead chromate lead has a +2 oxidation state. In lead +2 salts it has lead-212 radioactive isotope.

Concept introduction:

Solubility is the number of moles of solute per volume of a solution.

Radioactivity is the process in which a radioactive nucleus loses its energy by the emission of radiations namely, beta particle, alpha particle

Explanation

Given information as follows:

The amount of lead is 0.0100g.

The diluted volume is 10.00ml (The evaporated solution)

The activity of lead solution is 4.17×105.

Molar mass of lead is 207.20g/mol

The amount of Pb2+ is given below:

4.17×105×(0.0100gPb2+)=4.17×107gPb2+

Therefore,

Solubility of PbCrO4 can be calculated as:

Solubility=(4

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