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 specles 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: ? bases: D other: [ 1.4 mol of HCI is added to 1.0L of a 1.4M NH solution 0.35 mol of KOH is added to 1.0 L of a solution that is 1.0 M in both NH, and NH,Br acids: bases: D a other:0

Explanation / Answer

1)   NH3 + HCl ----> NH4Cl(aq)

   1 mol NH3 = 1 mol HCl

NH4Cl formed = acidic

species present, at equilibrium major species

   acidic NH4+

2) NH3 + H3O <----> NH4+(aq) + OH-(aq)

    NH4Br(aq) ----> NH4+(aq) + Br-(aq)

after addition of KOH

     OH-(aq) + NH4+(aq) ---> NH3(aq) + H2O(l)

species present, at equilibrium

    basic OH-

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