Calculate the pH at which the following conversion (reaction) will be at equilibrium in a basic medium: I 2 ( s ) ⇌ I − ( a q ) + I O 3 − ( a q ) When the equilibrium concentrations at 300 K are

Question

Calculate the pH at which the following conversion (reaction) will be at equilibrium in a basic medium:

$I_{2} (s) ⇌ I_{-} (a q) + I O_{3}^{-} (a q)$

When the equilibrium concentrations at 300 K are

$[I^{-}] = 0.10 M$ and $[I O_{3}^{-}] = 0.10 M$ .

Given the following standard Gibbs free energies of formation:

$Δ G_{f}^{\circ} (I^{-} (a q)) = - 50 k J / m o l$

$Δ G_{f}^{\circ} (I O_{3}^{-} (a q)) = - 123.5 k J / m o l$

$Δ G_{f}^{\circ} (H_{2} O (l)) = - 233 k J / m o l$

$Δ G_{f}^{\circ} (O H^{-} (a q)) = - 150 k J / m o l$

Gas constant $R = \frac{25}{3} J / (m o l \cdot K); ln x = 2.3 lo g_{10} x$ .

Given $p K_{w} = 14$ at 300 K.

Answer:

8

Solution:

TestHub · Accepted Answer

Correct answer: 8

Chemistry - Thermodynamics - II Question with Solution | TestHub