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Newbie

Joined: 29 Aug 2019
Posts: 1

# Need help with analytical chemistry Ques

I am trying to solve this question but in vain if anyone can explain it will be great.

Q: Calculate the solubility of the solutes Th(OH)4 for solution in which the cation concentration is 0.050M.

I found the Ksp which is 1.1*10^-15 and i solved it this way :-

[Th+]+[4OH-]=1.1x10^-15
4[OH]= 4√1.0*10^-15 = 1.8x10^-4
1/4(1.8*10^-4)
=4.5x10^-5 = Final Ans

but my answer is wrong since the answer is 1.5x10^-3 M

I have an exam and i am struck with this question pls tell me what is my mistake?

Distinguished Member

Joined: 27 Sep 2017
Posts: 301
Location: Berlin, Germany
 You have mistypings. Kl = [Th4+] * [(OH-)^4] Th = x , OH- = 4x Kl = x* (4x)^4 Kl = 256 * x^5 x =5√ (Kl/256) x = 5√(1.1 * 10^-15/256) x = 3,36 * 10^-4 OH- = 4*x OH- = 1,34 * 10^-3 mol/l
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