Acids and Bases

Question 1

Arrhenius acid

Answer 1

substance that dissociates in water to form hydrogen ions or protons
increases the number of H+ ions in the water

Question 2

Arrhenius base

Answer 2

dissociates in water to form hydroxide ions, OH-

Question 3

Brønsted-Lowry acid

Answer 3

proton donator

Question 4

Brønsted-Lowry base

Answer 4

proton acceptor
requires a lone pair of electrons to bond to the proton

Question 5

Water is amphoteric

Answer 5

can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base

Question 6

Strong acids and bases ionize

Answer 6

completely in aqueous solution

Question 7

weak acids and bases ionize

Answer 7

only partially

Question 8

conjugate base of a Brønsted-Lowry acid

Answer 8

species formed after an acid donates a proton

Question 9

conjugate acid of a Brønsted-Lowry base

Answer 9

species formed after a base accepts a proton

Question 10

two species in a conjugate acid-base pair molecular formula

Answer 10

same
acid has an extra proton compared to the conjugate base

Question 11

Acid or base “strength”

Answer 11

measure of how readily the molecule ionizes in water

Question 12

neutralization reaction

Answer 12

when an acid and a base react to form water and a salt and involves the combination of H+ ions and OH- ions to generate water, pH = 7

Question 13

Strong acids eg

Answer 13

HClO4
HCl
HBr
HI
HNO3
H2SO4

Question 14

Strong bases eg

Answer 14

LIOH
NaOH
KOH
Ca(OH)2
Sr(OH)2
Ba(OH)2

Question 15

acid + base

Answer 15

water + salt

Question 16

Self ionisation of water

Answer 16

conc of H+ and OH- ions is small because eqm lies on LHS
H2O = H+ + OH-
H2O + H2O = H3O+ + OH-

Question 17

Acids and Bases equations

Answer 17

pH + -log[H+]
pOH = -log [OH-]
[H+][OH-] = Kw = 10^-14
-log[H+] -log[OH-] = -log10^-14
pH + pOH = 14

Question 18

-ve exponent of [H3O] for concs with a coefficient of 1

Answer 18

H3O+ = 1x10-4, pH = 4.0
H3O- 1x10-11, pH = 11.0