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