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(1) The solubility of Salt AB2(S) IS 5mol/dm^3.
a. Obtain an expression for the solubility product of AB2(S),in terms of s.
b. Calculate the Ksp of AB2,given that solubility is 2.4x10^3mol/dm^3

Respuesta :

Answer:

a. Ksp = 4s³

b. 5.53 Ɨ 10⁓ mol³/dm⁹

Explanation:

a. Obtain an expression for the solubility product of AB2(S),in terms of s.

ABā‚‚ dissociates to give

ABā‚‚ ⇄ A²⁺ + 2B⁻

Since 1 mole of ABā‚‚ gives 1 mole of A and 2 moles of B, we have the mole ratio as

ABā‚‚ ⇄ A²⁺ + 2B⁻

1 : 1 : 2

Since the solubility of ABā‚‚ is s, then the solubility of A is s and that of B is 2s

So, we have

ABā‚‚ ⇄ A²⁺ + 2B⁻

[s] Ā  Ā  Ā  Ā [s] Ā  Ā [2s]

So, the solubility product Ksp = [A²⁺][B⁻]²

= (s)(2s)²

= s(4s²)

= 4s³

b. Calculate the Ksp of ABā‚‚, given that solubility is 2.4 Ɨ 10³ mol/dm³

Given that the solubility of AB is 2.4 Ɨ 10³ mol/dm³ and the solubility product Ksp = [A²⁺][B⁻]² = 4s³ where s = solubility of AB = 2.4 Ɨ 10³ mol/dm³

Substituting the value of s into the equation, we have

Ksp = 4s³

= 4(2.4 Ɨ 10³ mol/dm³)³

= 4(13.824 Ɨ 10³ mol³/dm⁹)

= 55.296 Ɨ 10³ mol³/dm⁹

= 5.5296 Ɨ 10⁓ mol³/dm⁹

≅ 5.53 Ɨ 10⁓ mol³/dm⁹

Ksp = 5.53 Ɨ 10⁓ mol³/dm⁹