17. Acid and Base Equilibrium

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

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

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

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

In the chemical equation HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO₂⁻(aq), which species act as Bronsted-Lowry acids?

The equilibrium constant for the reaction below has the value Ka = 3.5 x 10^-4. In this reaction, the stronger Brønsted-Lowry acid is ________ and the weaker Brønsted-Lowry acid is ________. HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)

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?

Which of the following represents the reaction when a weak base, B, is dissolved in water?

Which of the following explains why HCO3^- is a stronger conjugate base than CO3^2^-?

What is the formula for the conjugate acid of the Brønsted-Lowry base CH3NH2?