Question

How do you perform acid base reactions?

Answer 1

Some context is necessary to address the question...

Explanation:

We know that in aqueous solution under standard conditions, the following equilibrium operates...

`2H_2O(l)rightleftharpoonsH_3O^+ +HO^-`

And careful measurement has established the extent of this equilibrium...

`K_w=[H_3O^+][HO^-]=10^(-14)`...

And thus in aqueous solution, we invoke two quantities, ….

`underbrace(H_3O^+)_"the acid"`,

AND....

.. `underbrace(HO^-)_"the base"`

Equivalently, we could take logarithms of the expression...

`log_10(K_w)=log_10([H_3O^+][HO^-])=log_10(10^(-14))`...

And so ….

`log_10[H_3O^+]+log_10[HO^-]=-14`...else..

`+14=underbrace(-log_10[H_3O^+])_"pH"underbrace(-log_10[HO^-])_"+ pOH"`

And so...`14=pH+pOH`...the defining relationship....

I acknowledge that I may not have addressed the question you wanted answered... As to a specific reaction, you may refer to a titration reaction....where a known volume of titrant of known concentration is added to an unknown quantity of acid or base in solution….