Question

# Which of the following is used as a differentiating solvent for acids?A) ${\text{C}}{{\text{H}}_3}{\text{COOH}}$ B) ${{\text{H}}_2}{\text{O}}$ C) ${\text{HCl}}{{\text{O}}_4}$ D) None of these

$\Rightarrow {\text{HA + C}}{{\text{H}}_3}{\text{COOH}} \rightleftharpoons \left( {{\text{C}}{{\text{H}}_3}{\text{COOH}}_2^ + } \right) + {{\text{A}}^ - }$
Here if the acid HA is strong then the reaction will not lie very much to the right side of the equilibrium because the acetic acid (acts as a basic solvent) is poor acceptor of proton so the dissociated ${{\text{H}}^ + }$ ion will again form acid from which it was dissociated. Thus strong acid only slightly dissociates whereas weak acids completely dissociate. So the acids dissociate to different degrees in basic solvent which helps in differentiating the acids.