Write an equilibrium reaction equation for each of the following buffer mixtures:
a)NH3(aq) and NH4Cl(aq)
b)HC7H5O2(aq) and NaC7H5O2(aq)
To write the equilibrium reaction equation for a buffer mixture, you need to know the components of the buffer and their corresponding conjugate pairs. Let's go through each example:
a) NH3(aq) and NH4Cl(aq):
In this case, NH3 acts as the base, while NH4Cl acts as the acid. The acid NH4Cl will dissociate in water, forming NH4+ ions and Cl- ions. The base NH3 will react with the hydronium ions (H3O+) in water to form NH4+ ions and water.
The equilibrium equation for this buffer mixture can be written as:
NH3(aq) + H3O+(aq) ↔ NH4+(aq) + H2O(l) + Cl-(aq)
b) HC7H5O2(aq) and NaC7H5O2(aq):
In this case, HC7H5O2 (acetic acid) acts as the acid, while NaC7H5O2 (sodium acetate) acts as the conjugate base. When acetic acid dissolves in water, it donates a proton (H+) to water, forming hydronium ions (H3O+). The conjugate base, sodium acetate, dissociates to form sodium ions (Na+) and the acetate ion (C7H5O2-).
The equilibrium equation for this buffer mixture can be written as:
HC7H5O2(aq) + H2O(l) ↔ H3O+(aq) + C7H5O2-(aq) + Na+(aq)
These equations represent the dynamic equilibrium between the acid and base forms of the buffer, where the acid and base constantly interconvert, maintaining the buffer's pH.
I'm not sure what you want.
NH3 + H^+ ==> NH4^+ oe
NH4^+ ==> NH3 + H^+
Do the same kind of thing for the other one.