Ab2 has a molar solubility of 3.72×10−4 m. what is the value of the solubility product constant for ab2? express your answer numerically.

Answer is: Ksp for AB₂ is 2.06·10⁻¹⁰.
Chemical reaction: AB₂(s) → Aˣ⁺(aq) + 2Bⁿ⁻(aq).

s(AB₂) = 3,72·10⁻⁴ M.
s(AB₂) = s(Aˣ⁺).

s(Bⁿ⁻) = 2s(AB₂).

Ksp(AB₂) = s(Aˣ⁺) · (s(Bⁿ⁻))².
Ksp(AB₂) = 3,72·10⁻⁴ · (7,44·10⁻⁴)².

Ksp(AB₂)= 2,06·10⁻¹⁰.

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.