A 1.00-L solution saturated at 25 C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25 C.

Video transcript

Hello in this problem we are told at 25 degrees Celsius 0.787 g of iron to fluoride is contained in a one liter saturated iron to fluoride solution brass. To determine the scalability product constant of this compound at this temperature. Let's begin by finding the concentration of iron to fluoride. So we have 0.787 g. And one leader we can convert our mass to moles using the molar mass of iron to fluoride, Which is 93.842 g. Our mass of iron to fluoride cancels and we're left with moles per liter. So our concentration is 8.39 Times 10 to the -3 Molar. This then represents the Mueller scalability of iron to fluoride which will represent is S. We can then write the equation that describes equilibrium between are solid and its ions in solution. So the more scalability of iron to fluoride is s based on the story geometry for every one mole of iron to fluoride that goes into solution, you get one mole of iron too and we get two moles of Floridians. So that would be two S. We can then write our solid body product constant expression. This is equal to the concentration of iron too. Times the concentration of Floridians squared appear solid does not appear in our equilibrium constant expression. This then works out to s times two S squared. This then sympathized for s cubed. So we have four times s which is equal to 8.39 Times 10 to the -3. And so our scalability product constant works out to 2.36 times 10 to the -6. This then corresponds to answer B. Thanks for watching. Hope This helps.