Notifications
Clear all
Equilibrium
1
Posts
2
Users
0
Likes
394
Views
0
20/10/2021 11:36 am
Topic starter
Solid Ba(NO3)2 is gradually dissolved in a 1.0 × 10-4 M Na2CO3 solution. At which concentration of Bar2+, precipitate of BaCO3 begins to form? (Ksp for BaCO3 = 5.1 × 10-9)
(a) 5.1 × 10-5 M
(b) 7.1 × 10-8 M
(c) 4.1 × 10-5 M
(d) 8.1 × 10-7 M
1 Answer
0
20/10/2021 11:42 am
Correct answer: (a) 5.1 × 10-5 M
Explanation:
Given Na2CO3 = 1.0 × 10-4 M
∴ [CO32-] = 1.0 × 10-4 M
i.e s = 1.0 × 10-4 M
At equilibrium
[Ba2+][CO32-] = Ksp of BaCO3
[Ba2+] = \(\frac{K_{sp}}{[CO_3^{2-}]}\)
= \(\frac{5.1 \times 10^{-9}}{1.0 \times 10^{-4}}\)
= 5.1 × 10-5 M