Ksp Ca(OH)2 with Common Ion Effect Lab
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- เผยแพร่เมื่อ 13 ธ.ค. 2011
- Part of NCSSM CORE collection: This video shows the collection of data to determine the K sp of Ca(OH)2 in water and a solution of CaCl2. www.dlt.ncssm.edu
Please attribute this work as being created by the North Carolina School of Science and Mathematics. This work is licensed under Creative Commons CC-BY creativecommons.org/licenses/b...
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POV: You're doing an online lab for Chemistry and are looking to the comments for assistance
Yes it does. It shows that less acid is needed because less CaOH2 dissolved in the CaCL. So th common ion decreased the solubility
i did this in the lab and got the exact opposite results lmao i was like why did my solubility increase
Why is a titration better than using the initial pH to calculate [OH-]? Is it something about the accuracy? Using the pH, the molar solubility for calcium hydroxide would be the same in the first case, but slightly different in the second case (0.00912 M using the pH and 0.00934 M using the titration). Thanks for the video.
I got 4.45*10^-5 ksp value for the first one. very different from accepted value
does anyone know how to calculate Ksp from the given data?
Does anybody knows how to calculate Kps with the data obtained?
Yes, did you figure it out?
@@brothersbuildlego7400 Hey do you still know the answer?
sources of error?
Tarea de la profe Dioses. XD
Does anyone know how to calculate the ksp , please 😭😭
maybe the concentration of your HCl was less than the concentration of HCl used in this demonstration.
when i did this same experiment in the college i need 27ml of HCl 0,1M to finally get the yellow color
Maybe the initial amount of CaCl2 was too high
I am the 69th like. I have won the internet.
what's with this guy's voice?
SPOIL: This has absolutely nothing to do with common ion effect.