Question

If solutions of nh4cl(aq) and nh3(aq) are mixed, which ions in the resulting solution are spectator ions in any acid-base chemistry occurring in the solution?

Answer 1

If solutions of nh4cl(aq) and nh3(aq) are mixed, the ions in the resulting solution that would be the spectator ions in any acid-base chemistry occurring in the solution would be the chloride ions. The mixture is a common buffer of ammonia and ammonium chloride.  NH4Cl is a salt that is soluble in water dissociating into NH4+ and Cl-. The chloride ions are the spectator ions while NH4+ ions would be the conjugate acid for the buffer solution. Buffer solutions are solution which would resist change in pH when acid or a base is being added to the solution. The equilibrium reaction of the buffer solution in this problem would be

NH3 + H2O = OH– + NH4+

Answer 2

$\boxed{{\text{C}}{{\text{l}}^ - }}$ ionsact as spectator ions if solutions of ${\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl}}$ and ${\text{N}}{{\text{H}}_{\text{3}}}$ are mixed.

Further explanation:

Buffer solution offers resistance to any changes in their pH if strong acid or base is added to them. These are usually aqueous solution consisting of weak acid and its conjugate base.

Buffers can be acidic or basic as described below.

Acidic buffer:

These solutions have pH less than 7 and are formed by weak acid and its conjugate base.

Basic buffer:

These solutions have pH more than 7 and are formed by weak base and its conjugate acid.

Spectator ions are those ions that are present in same form on both sides of the chemical reaction. In other words, these ions do not participate in chemical reactions and cannot affect the reaction equilibrium. Since these are not involved in overall chemical reaction, spectator ions are not included while writing net ionic equations for any chemical reaction.

If solutions of ${\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl}}$ and ${\text{N}}{{\text{H}}_{\text{3}}}$ are mixed, it results in the formation of buffer ${\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl}}$. is a salt of weak acid and its dissociation occurs as follows:

 ${\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl}} \rightleftharpoons {\text{NH}}_4^ + + {\text{C}}{{\text{l}}^ - }$

The reaction of given buffer can be written as follows:

${\text{N}}{{\text{H}}_3} + {{\text{H}}_{\text{2}}}{\text{O}} \rightleftharpoons {\text{NH}}_4^ + + {\text{O}}{{\text{H}}^ - }$  

Since ${\text{C}}{{\text{l}}^ - }$  ions are not involved in net chemical reaction for buffer solution of ${\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl}}$ and ${\text{N}}{{\text{H}}_{\text{3}}}$ , these ions act as spectator ions.

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Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Buffer solutions

Keywords: buffer solution, NH4Cl, NH3, NH4+, Cl-, OH-, H2O, buffer, spectator ions.