Consider two precipitation reactions that occurs in the solution when we add solid barium nitrate.
1) Ba 2+ (aq) + SO 42- (aq) BaSO4 (S)
2) Ba 2+ (aq) + CO 32- (aq) BaCO3 (S)
To identify which precipitate will starts forming first, we need to calculate minimum concentration of Ba 2+ required to start precipitation of two compounds.
We have, Ksp = [ Ba 2+] [SO 42- ] = 1.1 10 -10
[ Ba 2+] minimum = 1.1 10 -10 / [SO 42- ]
We have given [SO 42- ] = 6.23 10 -03 M
[ Ba 2+] minimum = 1.1 10 -10 / 6.23 10 -03 = 1.76 10 -08 M -------------> (1)
We have, Ksp = [ Ba 2+] [CO 3 2- ] = 5.0 10 -09
[ Ba 2+] minimum = 5.0 10 -09 / [CO 3 2- ]
We have given [CO 3 2- ] = 1.29 10 -02 M
[ Ba 2+] minimum = 5.0 10 -09 / 1.29 10 -02 = 3.88 10 -07 M ---------------->(1)
From equation 1 and 2 , we found that [ Ba 2+] required for precipitation of BaSO4 is lower than BaCO3.
Hence, BaSO4 will precipitate out first and [ Ba 2+] when this first precipitation begins is 1.76 10 -08 M.
ANSWER :
A) What is the formula of compound that precipitates out first
BaSO4 |
B) What is the concentration of Ba 2+ ions when this first precipitation begins?
[ Ba 2+] =
1.76 10 -08 M |
( Note : IF your values of K sp values are different result
value of second option may change slightly )
let me know if you need any values Review Topics) [References) Use the References to access...
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