Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. c. 0.20 M Na₂X

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Hello everyone today we are being asked to find the Mueller sociability of the ionic compound A two X in 20.15 Mueller of sodium X solution were given the case P value of this A. Two X. Which is 2.62 times 10 to the negative 18. So the first thing we want to do when dealing with these kinds of problems is draw this as if it was dissociating. So if we have in a two X. In the acquis form, this would form two moles of sodium plus Aquarius As well as one X 2 -1. We did note that since we have 0.15 of this sodium X compound, we must therefore have 0.15 of this molar of this X. Two minus as well. And so we have a two X. As a solid, it's going to dissociate into two A plus ions because there's two of them and only one X. Or X two minus ions. And when we set up our ice table I. C. E. For solids we aren't concerned with them for our initial concentration of A. We have zero but for X we have 00.15 as we stated earlier since we have two A's for the A. Plus ion we have two X. For our change but for our X two minus we only have one. So it's just X. And so when we add these up, I plus C. Gives us E. We have two X. And then we only have 20.15 since X in this situation is negligible. And so the K. S. P. For our a two X. Is going to be equal to 2.62 times to the negative 18th. And so we set up our K. S. P. Equation. We have our concentration of a two plus since there are two of them as denoted by that coefficient. We have the exponent of two and we multiply that concentration by X two minus, plugging in our values. We have a K. S. P. Which is 2.62 times 10 to the negative 18 is equal to our concentration of A two plus which is two X. And since we spread that we're gonna add the exponents and then we're gonna add the concentration of our X two minus which is 20.15. This is going to simplify to R K. S. P value equal to 0. X squared. We're going to divide both sides by 0.6 and then take the square root of it. Giving us X. Is equal to 2.9 times 10 to the negative ninth. And that is going to be our final answer. I hope this helped until next time

Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. c. 0.20 M Na₂X

Verified Solution

Key Concepts

Molar Solubility

Solubility Product Constant (Ksp)

Common Ion Effect

Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. c. 0.20 M Na2X

Verified Solution

Key Concepts

Molar Solubility

Solubility Product Constant (Ksp)

Common Ion Effect

Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. c. 0.20 M Na₂X