CHEMISTRY · Multi-part · CBSE · Chemistry · Metals and Non-metals · Metals and Non-metals
Problem
Solid aluminum hydroxide, Al(OH)₃, is added to a beaker containing excess 2.0 M NaOH solution, forming a clear, colorless solution. Carbon dioxide gas is then bubbled through the solution until precipitation is complete.
(a) Write the balanced net ionic equation for the dissolution of Al(OH)₃ in excess aqueous hydroxide.
(b) Identify the predominant aluminum-containing species present in solution after dissolution and explain its formation in terms of acid–base behavior.
(c) As CO₂ is bubbled through the solution, a white precipitate eventually forms. Write the balanced net ionic equation for the precipitation reaction that produces this solid.
(d) Explain, with reference to Le Châtelier’s principle, why the introduction of CO₂ gas drives the precipitation described in part (c).