A solution of ammonia NH3(aq) is at equilibrium. How would the equilibrium change if NH4+ were added to the solution? A. The equilibrium would shift to produce more NH4+.

B. The equilibrium would shift to produce less NH4+.

C. The equilibrium would shift to produce more NH3.

D. The equilibrium would shift to produce more H+.​

C. The equilibrium would shift to produce more NH₃(g)

Explanation:

NH₃(aq) + H₂O(l) ⇄ NH₄⁺(aq) + OH⁻(aq)

Adding NH₄⁺ to the equilibrium would result in an excess on the product side of the equation and initiate shift to the left until the new equilibrium is established.

Note: Think of the reaction as being on a seesaw, that is ...

NH₃(aq) + H₂O(l) ⇄ NH₄⁺(aq) + OH⁻(aq)

                           Δ

At equilibrium the seesaw is balanced, but when NH₄⁺ is added, the seesaw is tilted to the right b/c of excess NH₄⁺ and, by natural action, shifts left forming more NH₃ & H₂O in order to form a new balanced equilibrium. :-)

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.

for points guys