The preparations of two aqueous solutions are described in the table below. For

Question

The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other row. You will find it useful to keep in mind that NH3 is a weak base. O acids: bases: other: 0.50 mol of HNO3 is added to! O acids: bases: O other: ?,?, .. . 0.5 mol of HCl is added to 1.0 L of a 0.5 M NH3 solution. 1.0 L of a solution that is 1.3 M in both NH3 and NH4CI

Explanation / Answer

Solution 1:

Major species at equilibrium is NH4Cl      (or NH4+ and Cl-)

acids : HCl

bases : NH3              (try NH4OH if wrong)

Solution 2:

Major species at equilibrium is NH4NO3 , NH4OH and NH4Cl

acids : HNO3

bases : NH3       (try NH4OH if wrong)

others : NH4Cl

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