17. Acid and Base Equilibrium

Which of the following equations correctly shows how the BrO⁻ ion acts as a Bronsted-Lowry base?

The following equation shows the equilibrium in an aqueous solution of ethylamine: C2H5NH2(aq) + H2O(l) ⇌ C2H5NH3+(aq) + OH−(aq) Which of the following represents a conjugate acid-base pair?

In the reaction C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH−(aq), which species acts as the Brønsted-Lowry base?

According to the Brønsted–Lowry definition, what is the conjugate acid of $H_{2}O$?

Which of the following is NOT a Brønsted–Lowry acid?

In the Brønsted–Lowry definition, what is the conjugate base of the ammonium ion $N_4^{+}$ (often written as $N_{4}H+$)?

In the Brønsted–Lowry model, what is the conjugate base of $N_4^{+}$ (ammonium)?

In the Brønsted–Lowry acid–base model, what is the conjugate acid of $N_1{H}_3$ (ammonia)?

According to the Brønsted–Lowry definition, what is a base?

In the Brønsted–Lowry model, what is the conjugate base of $HCN$?

In the Brønsted–Lowry model, what is the conjugate base of $HI$ after it donates a proton?

In the Brønsted–Lowry framework, what is the conjugate acid of $H^{-}S$ (HS⁻)?

Which of the following pairs is a Brønsted–Lowry conjugate acid–base pair?

Which of the following equations correctly shows NO₂⁻ acting as a Bronsted-Lowry base?