What percentage of the Ba2+ in solution is precipitated as BaCO3(s) if equal volumes of 2.4*10^-3 M Na2CO3(aq) and 1.1*10^-3M BaCl2(aq) are mixed
I made the equation as Na2CO3(aq)+BaCl2(aq)=BaCO3(s)+2NaCl(aq)
Then im assuming you use an ice table to find the concentration of BaCO3. From there i'm not sure how to find the % of Ba2+
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is it 100% because the Ba is only seen in the BaCO3 which is precipitated?
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