Quiz 2 - Acids and Bases | Acids and Bases

A conjugate acid-base pair HA/A^- differ only by the presence or absence of a proton.
An acid donates a proton H⁺ to a base ⇒ a base is converted to its conjugate acid by adding a proton.

A pH value greater than 7 means that the solution is basic.

In a neutral solution: [H₃O⁺] = [HO^-] = 1.0 x 10^-7 M

The dissociation of water, known as the self-ionization of water, is described by the equilibrium reaction: 2 H₂O (l) ⇌ H₃O⁺ (aq) + HO^- (aq)

In the dissociation of water, the forward and reverse reactions happen rapidly. However, the equilibrium lies far to the left, meaning that only a small fraction of water molecules are dissociated at any given moment.

pH + pOH = 14 ⇒ a solution with a pOH = 11 has a pH = 3
[H₃O⁺] = 10^-pH ⇒ [H₃O⁺] = 1.0 x 10^-3 M

Amphoteric compound: compound that can act as both a Bronsted acid and base
Polyprotic acid: acid that donate more than one acidic proton

The conjugate base of an acid is formed by removing one proton (H⁺) from the acid. Removing an H⁺ from HCO₃⁻​ gives CO₃²⁻​.

The acid ionization constant (K_a​) for acetic acid is the ratio of the concentrations of the dissociated products CH₃COO⁻ and H⁺ to the concentration of the undissociated acid CH₃COOH.

NaOH is a strong base and fully dissociates in water, producing a high concentration of hydroxide ions, which results in the highest pH.

HCl is a strong acid and fully dissociates in water. The pH is calculated as pH = − log⁡ [H⁺]. For a 0.001 M solution of HCl, [H⁺] = 0.001 M, the pH is 3.