Question

At a certain temperature, a saturated solution of lead chromate (PbCrO4) has 4.33 x 10-6 g dissolved in 100 mL of water, a concentration of 1.34 x 10-7 M PbCrO4. What is the Ksp of lead chromate

Answer 1

This question is providing us with the concentration of a lead (II) chromate solution at its saturation point and asks for its solubility product. Thus, after the corresponding calculation, the result turns out to be 1.80x10⁻¹⁴.

Solubility products

In chemistry, solubility tells us how much solid is dissolved in a solvent before exhibiting a precipitate (undissolved solid). This can be calculated with the concept of solubility product based on the equilibrium the solid creates with its ions, which for this case looks like;

$PbCrO_4(s)\rightleftharpoons Pb^{2+}(aq)+CrO_4^{2-}(aq)$

Whose equilibrium expression is:

$Ksp=[Pb^{2+}][CrO_4^{2-}]$

Hence, since the solid and the ions are all in 1:1:1 mole ratios, we set the concentration of the ions equal to that of solid at equilibrium (saturation), in order to obtain the Ksp:

$Ksp=(1.34x10^{-7})(1.34x10^{-7})\\\\Ksp=1.80x10^{-14}$

Learn more about chemical equilibrium: brainly.com/question/26453983