The K sp of PbBr 2 is 6.60×10 −6 . What is the molar solubility of PbBr 2 in pure water?

Hello everyone today we are being asked to determine the mole ursula ability of silver iodide. I had died in pure water with the K. S. P. Of 8.51 times 10 to the negative 17th. So the first thing we do is we want to draw out this equation as if it was dissolving in water. And so we have silver iodide right here A. G. I. And we have it in a solid form and it's going to disassociate into silver ions. So we have silver plus in the acquis form and we have iodine or iodide here. Also in the acquis form, we're gonna draw our nice little ice table here to help set the numbers up. So we have an initial concentration of zero across the board for this sodium iodide. We also have 04 silver ions and iodide ions. And then we're gonna slowly add some in but we don't know how many. So we're going to say we have X. And for the last row this is just going to be the some of the I. And the C. And so we simply have R. K. S. P. Is equal to X squared where X. Represents the silver ions as well as the iodine ions. And so combined it's just X squared R. K. S. P. We said was 8.51 times 10 to the negative 17th is equal to X squared scoring both sides will give you X. Is equal to 9.225 times 10 to the negative nine moller. And this is our final answer. I hope this helped. and until next time.

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Solubility Product Constant: Ksp

General Chemistry

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

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The K_sp of PbBr₂ is 6.60×10⁻⁶. What is the molar solubility of PbBr₂ in pure water?

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The K_sp of PbBr₂ is 6.60×10⁻⁶. What is the molar solubility of PbBr₂ in pure water?