Which of the following cannot act both as a Bronsted acid and as a Bronsted base?

A species acts as an amphiprotic substance if it can both donate a proton (acid) and accept a proton (base).${\text{HCO}}_3^{-}$: Can give ${\text{CO}}_3^{2-}$ or take ${\text{H}}^{+}$ to become ${\text{H}}_2{\text{CO}}_3$.${\text{NH}}_3$: Can give ${\text{NH}}_2^{-}$ (in strong conditions) or take ${\text{H}}^{+}$ to become ${\text{NH}}_4^{+}$.$\text{HCl}$: It is a strong acid and readily donates a proton. However, it cannot accept a proton to form ${\text{H}}_2{\text{Cl}}^{+}$ under standard conditions. Thus, it acts only as an acid.${\text{HSO}}_4^{-}$: Can give ${\text{SO}}_4^{2-}$ or take ${\text{H}}^{+}$ to become ${\text{H}}_2{\text{SO}}_4$.