December 04, 2022, 07:24:04 AM
Forum Rules: Read This Before Posting

### Topic: Precipatation of BaCO3  (Read 6558 times)

0 Members and 1 Guest are viewing this topic.

#### Tom

• Guest
##### 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 »

#### Donaldson Tan

• Editor, New Asia Republic
• Retired Staff
• Sr. Member
• Posts: 3177
• Mole Snacks: +261/-13
• Gender:
##### 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 »
"Say you're in a [chemical] plant and there's a snake on the floor. What are you going to do? Call a consultant? Get a meeting together to talk about which color is the snake? Employees should do one thing: walk over there and you step on the friggin� snake." - Jean-Pierre Garnier, CEO of Glaxosmithkline, June 2006

#### Tom

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

I appreciate it.

Tom