2006-11-25 19:01:53 · 5 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
The Ksp of BaSO4 at 25 C is Ksp=1.08*10^-10 according to
http://www.ktf-split.hr/periodni/en/abc/kpt.html
Therefore the solubility would be 1.04*10^-5 M
OK I just saw that you ask for the solubility of many compounds in other questions. At the link I gave you you will find the Ksp for a lot of compounds. Howto find solubility from that.
Let's assume that s is the solubility in mole/L of the salt AxBy then
.. .. .. .. .. .. AxBy <=> xA(+y) +yB(-x)
Dissolve .. ...s
Produce .. .. .. .. .. .. .. ..xs .. .. .. yx
Ksp=[A+y]^x *[B-x]^y = (xs)^x * (ys)^y = (x^x)(y^y)*s^(x+y) =>
s= [Ksp/(x^x*y^y)]^1/(x+y)
usually (like for BaSO4) x=y=1 so s=squareroot (Ksp)
2006-11-25 21:27:05 · answer #1 · answered by bellerophon 6 · 0⤊ 0⤋
The very low solubility of barium sulphate in water is used using fact the muse of the attempt for sulphate ions in answer. If soluble barium chloride is further to any soluble sulphate, a white precipitate of barium sulphate is seen. The barium chloride could desire to be acidified first with a sprint HCl.
2016-12-29 12:18:42 · answer #2 · answered by calvete 3 · 0⤊ 0⤋
The very low solubility of barium sulphate in water is used as the basis of the test for sulphate ions in solution. If soluble barium chloride is added to any soluble sulphate, a white precipitate of barium sulphate is seen. The barium chloride should be acidified first with a little HCl.
2006-11-25 19:52:40 · answer #3 · answered by Gervald F 7 · 0⤊ 0⤋
That make me happy in pants
2006-11-25 19:03:23 · answer #4 · answered by Devo 4 · 0⤊ 1⤋
should be high solubility
2006-11-25 19:09:22 · answer #5 · answered by tell me all!!! 4 · 0⤊ 1⤋