You have two buffer solutions 1) weak acid and its conjugate base 2)weak base and its conjugate acid. Write explicitly ( considering generic formula for acid and base) the equations of neutralization when you:
a) add strong acid and strong base 1)
b) add strong acid or strong base in 2)
HA = acid
A^- = conjugate base
HA + OH^- ==> H2O + A^-
A^- + H^+ ==> HA
You can do the other one.
I am trying to do the next one but I am still confused.
Would the next one simply be HA+OH^- ----> H2O + A^- ?
weak base = BH
conjugate acid = BH2^+
add strong acid:
BH + H^+ ==> BH^+
add strong base:
BH2^ + OH^- ==> BH + H2O
a) When you add a strong acid and a strong base to the first buffer solution (weak acid and its conjugate base), neutralization reactions occur. The generic formula for a weak acid is HA, and its conjugate base is A-.
The neutralization equation for adding a strong acid (H+) to the weak acid (HA) is:
H+ (aq) + A- (aq) → HA (aq)
Here, the strong acid donates its proton (H+) to the weak acid, forming the undissociated weak acid.
Next, if you add a strong base (OH-) to the conjugate base (A-) of the weak acid, the neutralization equation is:
OH- (aq) + HA (aq) → A- (aq) + H2O (l)
In this equation, the strong base accepts the proton from the weak acid, forming the conjugate base (A-) and water (H2O).
b) For the second buffer solution (weak base and its conjugate acid), when you add a strong acid to it, the neutralization equation is:
H+ (aq) + B (aq) → BH+ (aq)
Here, the strong acid donates its proton (H+) to the weak base, forming the conjugate acid (BH+).
Alternatively, if you add a strong base to the conjugate acid, the neutralization equation is:
OH- (aq) + BH+ (aq) → B (aq) + H2O (l)
In this equation, the strong base accepts the proton from the conjugate acid, forming the weak base (B) and water (H2O).