What is the molar solubility in water of Ag2CrO4? (The Ksp for Ag2CrO4 is 8 x 10^-12)
-------------------------
What is the final concentration of barium ions, [Ba{2+}] in a solution when 100 mL of .10M BaCl2 is mixed with 100 mL of 0.050 M H2SO4?
---------------------------
When 100mL of 1.0M Na3PO4 is mixed with 100 mL of 1.0M AgNO3, a yellow precipitate forms and [Ag+] becomes negligibly small. Rank the ions renmaining in solution in order of increasing concentration. [Na{+}] [NO3{-}] [PO4{3-}]
------------------------
Could you be thorough with the explaination?
2007-01-15 07:43:19 · 3 answers · asked by Neodudeman 1 in Science & Mathematics ➔ Chemistry
Ag2CrO4 <===> 2Ag+ + CrO4= and Ksp = [Ag+]^2[CrO4=]
So the molar solubility is equal to [CrO4=]. Let molar solubility be x. Then [Ag+] = 2x and [CrO4=] = x.
(2x)^2(x) = 4x^3 = 8 x 10^-12
x^3 = 2 x 10^-12
x = (cuberootoftwo) x 10^-4M
If you combine the two 100-mL solutions, you'll get the same number of moles in 200 mL. Also, SO4= reacts with Ba2+ 1:1. So you'll have BaSO4(s) lying on the bottom, which counts by convention as "1." The excess [Ba2+] = 0.025. (Half of the original got precipitated, and whatever was left was halved by the 100mL ===> 200mL dilution.
2007-01-15 08:03:27 · answer #1 · answered by steve_geo1 7 · 0⤊ 0⤋
Can't answer this for you, but try this link. They claim to be the "complete online source for chemistry solutions".
2007-01-15 07:53:43 · answer #2 · answered by Dee 2 · 0⤊ 0⤋
i cant help you with all of them... i dont comprehend all of them. i comprehend some although... #10) molarity describes the quantity of solute in moles and the quantity of the answer in liters (the form of moles of solute in keeping with quantity of answer in liters) m=molarity= moles of solute / liters of answer = mol / l !5) water is dilute while hexane is centred?
2016-12-16 05:25:17 · answer #3 · answered by Anonymous · 0⤊ 0⤋