Question

The solubility product, Ksp, for cobalt(III) hydroxide, Co(OH)3, is 1.6X104 at 25°C. What is the molar solubility of cobalt(III) hydroxide in a solution containing 0.077 M KOH at 25°C? 125.82e-41 x M Did you remember that the molar solubility of a substance is reduced whenever a common ion is present? Supporting Materials Periodic Table Constants and Factors Supplemental Data Additional Materials Tutorial -/50 points FSUGenChem2L1 8.PRE.002. Complete the following table of data for Ce2(SO4)3 9 H20. (Assume the density of water is 1.00 g/mL.) kap (kJ/mol) T(°C)| Solubility Concentration (g/100. g) (M) 15.0 12. 2 012 27.0 9.27 39.0 6.89 51.0 5.03 63.01 3.72 4: 75.0 2.93 870 2.69 Use a graph of AG vs. T to determine the following. (Enter your answers to three significant figures.) What is the value of AH for the system? kJ/mol What is the value of AS for the system? J/mol K

Answer 1

KOH is a strong base it dissociates completely

KOH-----> K+ + OH-

hence 0.077 M KOH will give 0.077 M OH-

but Co(OH)3 is a weak electrolyte and it dissociates as

Co(OH)3(s) = Co^3+(aq) + 3OH^-(aq)

s - -

- s 3s+0.077 (from common ion)

where s is the solubility of Co(OH)3

using the expression of Ksp = [Co^3+][OH^-]^3

Ksp = [s][3s+0.077]^3

1.6*10^-44 = [s][3s+0.077]^3

on solving

s = 3.5 *10^-41

(you can get this value by neglecting 3s in 3s+0.077 since due to common ion solubility is ver y very less)

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