Notifications
Clear all
Equilibrium
1
Posts
2
Users
0
Likes
359
Views
0
19/10/2021 10:05 am
Topic starter
In a saturated solution of the sparingly soluble strong electrolyte AgIO3 (molecular mass = 283) the equilibrium which sets is
AgIO3(s) ⇌ Ag+(aq) + IO3-(aq)
If the solubility product constant Ksp of AgIO3 at a given temperature is 1.0 × 10-8, what is the mass of AgIO3 contained in 100 mL of its saturated solution?
(a) 1.0 × 10-4 g
(b) 28.3 × 10-2 g
(c) 2.83 × 10-3 g
(d) 1.0 × 10-7 g
1 Answer
0
19/10/2021 10:23 am
Correct answer: (c) 2.83 × 10-3 g
Explanation:
Let s = solubility
AgIO3 ⇌ Ag+(aq) + IO3-(aq)
Ksp = [Ag+][IO3-] = s x s = s2
Given Ksp = 1 x 10-8
∴ s = \(\sqrt{K_{sp}}\) = \(\sqrt{1 \times 10^{-8}}\)
= 1.0 x 10-4 mol/lit = 1.0 x 10-4 x 283 g/lit
(∵ Molecular mass of AgIO3 = 283)
= \(\frac{1 \times 10^{-4} \times 283 \times 100}{1000}\) g/100 mL
= 2.83 x 10-3 g/100mL