All Flashcards

How do you calculate pH from $[H^+]$ ?

pH = -log $[H^+]$

How do you calculate pOH from $[OH^-]$ ?

pOH = -log $[OH^-]$

How do you calculate $K_a$ from $pK_a$ ?

$K_a = 10^{-pK_a}$

How do you calculate $K_b$ from $pK_b$ ?

$K_b = 10^{-pK_b}$

Describe the process of titration.

A solution of known concentration (titrant) is added to a solution of unknown concentration (analyte) until the reaction is complete, usually indicated by a color change or pH meter.

How to determine pH using the Henderson-Hasselbalch equation?

pH = pKa + log $[A^-]/[HA]$ , where $[A^-]$ is the concentration of the conjugate base and $[HA]$ is the concentration of the weak acid.

Compare strong acids and weak acids.

Strong acids: completely dissociate in water, high $[H^+]$ | Weak acids: partially dissociate, lower $[H^+]$

Compare strong bases and weak bases.

Strong bases: completely dissociate in water, high $[OH^-]$ | Weak bases: partially dissociate, lower $[OH^-]$

Compare pH and pOH.

pH: measures acidity, pH = -log $[H^+]$ | pOH: measures basicity, pOH = -log $[OH^-]$

Compare $K_a$ and $K_b$ .

$K_a$ : acid dissociation constant, measures acid strength | $K_b$ : base dissociation constant, measures base strength

Compare equivalence point and half-equivalence point in a titration.

Equivalence point: acid and base have completely reacted | Half-equivalence point: pH = pKa (weak acid), pOH = pKb (weak base)

Define acid.

Substances with a pH less than 7 that donate H+ ions.

Define base.

Substances with a pH greater than 7 that accept H+ ions.

Define pH.

A measure of the concentration of free protons (H+) in a solution.

Define pOH.

A measure of the concentration of hydroxide ions (OH-) in a solution.

Define buffer.

A solution that resists changes in pH when small amounts of acid or base are added, composed of a weak acid/base and its conjugate.

Define $K_a$ .

Acid dissociation constant; measures the strength of a weak acid.

Define $K_b$ .

Base dissociation constant; measures the strength of a weak base.