Timeline for Two salts in mutual saturation, which one will precipitate first? [closed]
Current License: CC BY-SA 4.0
11 events
| when toggle format | what | by | license | comment | |
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| May 4, 2020 at 15:28 | history | closed |
Mithoron Mathew Mahindaratne Todd Minehardt Buck Thorn♦ Jon Custer |
Needs details or clarity | |
| May 2, 2020 at 19:08 | comment | added | MaxW | A saturated solution of a mixture of the two salts would have such a large ionic strength that the notion of the Ksp being a constant just doesn't work, even using activities. | |
| May 2, 2020 at 18:30 | comment | added | Mathew Mahindaratne | Do not forget there is a common ion effect here as well. | |
| May 2, 2020 at 17:12 | comment | added | R. Wang | I guess I answered my own question lol. thanks all! | |
| May 2, 2020 at 17:11 | comment | added | R. Wang | @IvanNeretin My bad on mutual satuation. I'm aware of Ksp, and I mean the concentration of both solutes at which one is at its satuation. Mutual satuation is a thing tho, and can be estimated from Ksp. For KI/KCl it should probably be 7.43M/2.14 M | |
| May 2, 2020 at 16:40 | comment | added | R. Wang | @MathewMahindaratne I could have been clearer, I mean weight of KCl : weight of KI is 75% : 25% | |
| May 2, 2020 at 16:28 | comment | added | Mathew Mahindaratne | Good question would be this type: chemistry.stackexchange.com/questions/72700/…. You can learn about a thing or two of solubility in those answers. | |
| May 2, 2020 at 16:25 | comment | added | Mathew Mahindaratne | This question is unsolvable at this stage. For example, you said your saturated solution consists of 75% $\ce{KCl}$ by weight. Is that mean $\pu{75g}$ of $\ce{KCl}$ in $\pu{100g}$ of solution? If so, it is impossible. Maximum solubility of $\ce{KCl}$ in water cannot exceed 25.5% at $\pu{20 ^\circ C}$. That's right, you forgot to include temperature. Solubilities are highly depend on temperature of the solution. | |
| May 2, 2020 at 16:23 | comment | added | Ivan Neretin | Mutual saturation is not a thing. If one salt reaches its solubility product, it will precipitate. If another does, it will. If both do, both will. | |
| May 2, 2020 at 15:11 | review | Close votes | |||
| May 4, 2020 at 15:28 | |||||
| May 2, 2020 at 14:36 | history | asked | R. Wang | CC BY-SA 4.0 |