1. An ionic compound A2B3 has a Ksp value of 1. 0 x 10-36
An ionic compound A2B3 has a Ksp value of 1.0 x Determine the concentration of the A3+ ion and the B2- ion. Then determine the molar solubility of the compound A2B3 .
Chemistry:
A2B3(s) ↔ 2A B2-
+2x x
X = 2.5 x 10-8
Now [A3+] = 2x = 5.0 x 10-8
[B2-] = 3x = 7.5 x 10-8
Molar Solubility of A2B3 :
5.0 x 10-8 mole A3+ L
1 mol A2B3
2 mol A3+
= mol A2B3 L
2.5 x 10-8

2. An ionic compound A2B3 has a Ksp value of 1. 0 x 10-36
An ionic compound A2B3 has a Ksp value of 1.0 x Determine the concentration of the A3+ ion in a solution that is in the B2- ion.
Chemistry:
A2B3(s) ↔ 2A B2-
+2x x
Try dropping the +3x term
X = 5.0 x 10-16
Now [A3+] = 2x = 10. x 10-16
Molar Solubility of A2B3 :
10. x mole A3+ L
1 mol A2B3
2 mol A3+
= mol A2B3 L
5.0 x 10-16