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 acids: D bases: O D.D 2.6 mol of HBr is added to 1.0 L of a 1.4 MNH3 solution other: 0.13 mol of NaOH is added toacids: bases: 1.0 L of a solution that is 1.4 M in both NH and NH4Br oth

Explanation / Answer

In the solution containing HBr and NH3:

Acid : HBr

Base : NH3

Other: NH4Br

This is because HBr is a strong acid , NH3 is a weak base and NH4Br is a neutral salt.

In the other solution containing NaOH and NH3, NH4Br buffer:

Acid : NH4+

Base : OH-

Other: NH3, NaBr

NH4+ acts as the acid, OH- from the strong base NaOH acts as the base and NH3 ( being a weak base) and NaBr are other species.

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