Chemistry Unit 7 Test

self-ionization of water

in a sample of water, a small number of water molecules dissociate

ion-product constant for water

K_w = [H₃O⁺] [OH⁻]=1.0 × 10⁻¹⁴

hydronium ion

H₃O⁺

neutral solution

[H⁺]=[OH⁻], pH=7

acidic solution

[H⁺]>[OH⁻], pH<7

basic solution

[H⁺]<[OH⁻], pH>7

acid (Arrhenius definition)

dissociates to produce H⁺ in a solution

acid (Brønsted-Lowry definition)

H⁺ donor

base (Arrhenius definition)

dissociates to produce OH⁻ in a solution

base (Brønsted-Lowry definition)

H⁺ reciever

pH

concentration of H+ in a solution

conjugate acid-base pair

present when weak acids + bases are in equilibrium

pH (calculation from strong acid concentration)

pH=-log[H+]

pH (calculation from strong base concentration)

pOH-=-log[OH-]

strong acid

dissociates completely to give H+ (HCl)

strong base

dissociates completely to give OH- (OH)

weak acid/weak base

does not dissociate completely

neutralization reaction

acid+base → salt+ water

titration

experimental technique in which a neutralization reaction is performed gradually, often to determine the concentration of an unknown solution

indicator

gives a visible sign of pH; example of chemical equilibrium

end point (titration)

pale pink solution; when the titrant and analyst are in perfect stoichiometry

titration calculation

M_AV_A=M_BV_B

buffer(by property)

solution resists changes in pH when a small amt of acid or base is added

buffer(by composition)

weak acid +salt of conj base