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### Topic: Solubility of silver acetate  (Read 18823 times)

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#### UG

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##### Solubility of silver acetate
« Reply #15 on: April 12, 2010, 08:03:34 AM »
x is ethanoic acid

#### Borek

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##### Solubility of silver acetate
« Reply #16 on: April 12, 2010, 08:46:02 AM »
(3.88 x 10-4 - 3.88 x 10-3 x) / x = 1.75 x 10-5 x
Calculating gives x = 0.0999549 M which would give [H+] = 4.51 x 10-5 M and pH = 4.3
Does this mean the approximation is not valid?

I am afraid so. Unfortunately, that also means you should solve full 3rd degree equation. Correct result doesn't have to be far from what you have calculated, but it is hard to predict how far it is. From my calculations pH is around 3.3.
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#### UG

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##### Solubility of silver acetate
« Reply #17 on: April 12, 2010, 05:41:41 PM »
But the answer says that the solubility is 0.130 mol L-1 and pH is equal to 4.23

#### Borek

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##### Solubility of silver acetate
« Reply #18 on: April 13, 2010, 02:56:56 AM »
Unfortunatelty that most likely means they used wrong approximation and have not checked its validity later.

Try to use equations you already have and the answer given as real to calculate concentrations of all ions and check if all mass balances and reaction quotients have correct values. My bet is that you will find they are inconsistent with question data.
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#### UG

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##### Re: Solubility of silver acetate
« Reply #19 on: April 13, 2010, 03:45:39 AM »
Hmm... you're right, the answers come out all funny. So the way to solve this is to just try and find a way to express an equation using only one of the 4 variables?

#### Borek

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##### Re: Solubility of silver acetate
« Reply #20 on: April 13, 2010, 04:40:09 AM »
Yes. Unfortunately that leads to a 3rd degree polynomial.
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