Enter your answer in the provided box. Ksp for Co(OH)2 at 25°C is 3.3 × 10?16. Using this and data from your textbook, calculate the value of ?G o f for Co(OH)2(s). kJ/mol

88 kJ/mol

Explanation:

Let's consider the solution of Co(OH)₂.

Co(OH)₂(s) ⇄ Co²⁺(aq) + 2 OH⁻(aq)

The solubility product (Ksp) is 3.3 × 10⁻¹⁶. We can find the Gibbs free energy change (ΔG°) using the following expression.

ΔG° = - R × T × lnKsp

where,

R: ideal gas constant

T: absolute temperature (25°C + 273.15 = 298 K)

ΔG° = - R × T × lnKsp

ΔG° = - (8.314 × 10⁻³ kJ/mol.K) × 298 K × ln 3.3 × 10⁻¹⁶

ΔG° = 88 kJ/mol

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