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  2. AP Chemistry
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Compare strong acids and weak acids.

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

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Compare strong acids and weak acids.

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

Compare strong bases and weak bases.

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

Compare pH and pOH.

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

Compare KaK_aKa​ and KbK_bKb​.

KaK_aKa​: acid dissociation constant, measures acid strength | KbK_bKb​: 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)

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

pH = -log[H+][H^+][H+]

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

pOH = -log[OH−][OH^-][OH−]

How do you calculate KaK_aKa​ from pKapK_apKa​?

Ka=10−pKaK_a = 10^{-pK_a}Ka​=10−pKa​

How do you calculate KbK_bKb​ from pKbpK_bpKb​?

Kb=10−pKbK_b = 10^{-pK_b}Kb​=10−pKb​

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][A^-]/[HA][A−]/[HA], where [A−][A^-][A−] is the concentration of the conjugate base and [HA][HA][HA] is the concentration of the weak acid.

What is the effect of adding acid to a buffer solution?

The buffer resists the change in pH by reacting with the added acid.

What is the effect of adding base to a buffer solution?

The buffer resists the change in pH by reacting with the added base.

What happens to pH as [H+][H^+][H+] increases?

pH decreases (becomes more acidic).

What happens to pOH as [OH−][OH^-][OH−] increases?

pOH decreases (becomes more basic).

What happens to the pH at half equivalence point?

pH = pKa

What happens to the pH at equivalence point?

The number of moles of acid and base are equal, so the pH depends on the strength of the acid and base.