Question

Calculate the molar solubility of Al(OH)₃ in a buffer solution with 0.100 M NH₃ and 0.400 M

a) 0.002 M
b) 0.004 M
c) 0.006 M
d) 0.008 M

Answer 1

The calculation of Al(OH)3 molar solubility in a buffer requires knowledge of the solubility product constant (Ksp) and the equilibrium constants of the buffer components. Without these values, the precise molar solubility cannot be determined.

Step-by-step explanation:

The student has asked to calculate the molar solubility of Al(OH)3 in a buffer solution containing 0.100 M NH3 and 0.400 M NH4+.

To solve this problem, one would typically need the equilibrium constant for the dissolution of Al(OH)3 (Ksp) and the equilibrium constants for the NH3/NH4+ buffer system (Kb for NH3 and Ka for NH4+).

However, since we are not provided with these constants, the numerical answer cannot be calculated. In a real scenario, one would set up the equilibrium expression using Ksp and account for the common ion effect due to NH4+, which shifts the equilibrium and affects the solubility of Al(OH)3.