An ionic compound A2B3 has a Ksp value of 1. 0 x 10-36

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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 10-36. Determine the concentration of the A3+ ion and the B2- ion. Then determine the molar solubility of the compound A2B3 . Chemistry: A2B3(s) ↔ 2A3+ + 3B2- 0 0 +2x +3x 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

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 10-36. Determine the concentration of the A3+ ion in a solution that is 0.010 in the B2- ion. Chemistry: A2B3(s) ↔ 2A3+ + 3B2- 0 0.010 +2x 0.010+3x Try dropping the +3x term X = 5.0 x 10-16 Now [A3+] = 2x = 10. x 10-16 Molar Solubility of A2B3 : 10. x 10-16 mole A3+ L 1 mol A2B3 2 mol A3+ = mol A2B3 L 5.0 x 10-16