Which equilibrium constant(s) or ratio of equilibrium contants should be used to calculate the `pH` of `1.00L` of each of the following solutions?
a. `KOH` b. `NH_(3)` c. `HC_(2)H_(3)O_(2)`
d. `HC_(2)H_(3)O_(2) +NaC_(2)H_(3)O_(2)` e. `KC_(2)H_(3)O_(2)`
f. `0.01 mol HC_(2)H_(3)O_(2) + 0.050 mol NaOh`
g. `H_(2)S` h. `0.01NH_(4)CI + 0.50mol NaOH`
i. `0.010 mol HC_(2)H_(3)O_(2) + 0.10mol NaOH`

Explanation

a. `K_(w)(S_(B))` b. `K_(b)` and `K_(W)(W_(B))`
c. `K_(a) (W_(A))` d. `K_(A)` (Acidic buffer)
e. `K_(h) = K_(W)//K_(a)` (Salt of `W_(A)//S_(B))`
f. `K_(a)` (The solution is the same as `0.05mol HC_(2)H_(3)O_(2) + 0.05 mol NaC_(2)H_(3)O_(2))` (It forms acidic buffer)
g. `K_(1)`
h. `K_(b)` and `K_(w)` (The reaction `NH_(4)^(o+) + overset(Θ)OH rarr H_(2)O + NH_(3)` produces a basic buffer solution of `NH_(3)` with the excess of `NH_(4)^(o+))`
i. `K_(h) = K_(w)//K_(a)` (The neutralised acid results in the formation of salt of `W_(A)//S_(B)`.