Ionic EquilibriumMedium
Question
Solid Ba (NO3)2 is gradually dissolved in a 1.0 × 10-4 M Na2CO3 solution. At what concentration ofBa2+ will a precipitate begin to form ?(Ksp for Ba CO3 = 5.1 × 10-9).
Options
A.4.1 × 10-5 M
B.5.1 × 10-5 M
C.8.1 × 10-8 M
D.8.1 × 10-7 M
Solution
Ba(NO3)2 + CaCO3 → BaCO3 + 2NaNO3
Here [CO3-2] = [Na2CO3] = 10-4 M
Ksp = [Ba+2][CO3-2 ⇒ 5.1 × 10-9 = [Ba2+] (10-4) ⇒ [Ba+2] = 5.1 × 10-5
this value, just precipitation starts.
Here [CO3-2] = [Na2CO3] = 10-4 M
Ksp = [Ba+2][CO3-2 ⇒ 5.1 × 10-9 = [Ba2+] (10-4) ⇒ [Ba+2] = 5.1 × 10-5
this value, just precipitation starts.
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