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Topic: Precipatation of BaCO3  (Read 5543 times)

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Tom

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Precipatation of BaCO3
« on: June 03, 2004, 04:28:19 PM »
If a solution contains Ba+2 and Mg+2 each at a concentration of 1.0 x 10-3 M at 25º C.  Predict what will happen if the carbonate ion concentration is made 0.001 M (KspBaCO3= 8.1 x 10-9, Ksp MgCO3 = 4.0 x 10-5).

Would both MgCO3 and BaCO3 precipitate or neither will precipitate?
« Last Edit: April 09, 2005, 07:39:25 PM by Mitch »

Offline Donaldson Tan

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Re:T/F Questions
« Reply #1 on: June 03, 2004, 09:17:56 PM »
Tom: you can use the supscript (sup) and subscript(sub) button fyi.

Usually, the salt with the lower solubility product constant will precipitate preferentially.

Ba2+(aq) + CO32-(aq) <-> BaCO3(s)
Mg2+(aq) + CO32-(aq) <-> MgCO3(s)

when [ CO32- ] = 0.001,
Ionic Product for MgCO3
= (1.0X10^-3)(0.001)
= 1.0X10^-6 (< Ksp)
Ionic Product for BaCO3
= (1.0X10^-3)(0.001)
= 1.0X10^-6 (< Ksp)

Since in both cases, the respective ionic products are less than their respective Ksp, precipitation of neither carbonate occurs.


« Last Edit: June 03, 2004, 09:20:18 PM by geodome »
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Tom

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Re:Precipatation
« Reply #2 on: June 04, 2004, 09:19:02 AM »
Thankyou for explaining that Mana.

I appreciate it.

Tom

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