Acids and Bases

Question 1

Characteristics of acids

Answer 1

sour, red on red litmus, red on blue litmus, electrolytic, form hydrogen when reacted with metal, watery, changes color dyes

Question 2

characteristics of bases

Answer 2

bitter, blue on red litmus, blue on red litmus, electrolytic, slippery, changes color in dyes

Question 3

Arrhenius Theory

Answer 3

acid- any compound that produces a hydrogen ion

base- a compound that produces a hydroxide ion

Question 4

The Lewis Theory

Answer 4

acid- an electron pair accepter

base- an electron pair donor

Question 5

Bronstead-Lowry

Answer 5

acid- a proton donor

base- a proton accpeter

Question 6

amphiprotic

Answer 6

when a compound can act as either an acid or a base

Question 7

conjugate acid base pairs

Answer 7

differ by one hydrogen ion (proton)

Question 8

neutralizing reactions

Answer 8

acid + base → salt + water

Hx(aq) + MOH(aq) → Mx(aq) + H2O(aq)

Question 9

monoprotic acids

Answer 9

acids that can donate one proton

Question 10

monoprotic bases

Answer 10

bases that can accept one proton

Question 11

polyprotic acids

Answer 11

acids that can donate two or more protons, donate protons one at a time

Question 12

polyprotic bases

Answer 12

bases that can accept two or more protons

Question 13

Ostwald Process

Answer 13

industrial synthesis of nitric acid (HNO), produces nitrogen dioxide which is highly poisonous

Question 14

acid strength

Answer 14

proportional to the hydronium ion concentration (H3O+), weak acids establish equilibrium, strong acids dissociate 100% in water:

1. hyperchloric acid (HClO4)
2. hydroiodic acid (HI)
3. hydrobromic acid (HBr)
4. hydrochloric acid (HCl)
5. nitric acid (HNO3)
6. sulfuric acid (H2SO4)
7. hydronium ion (H3O+)

Question 15

base strength

Answer 15

proportional to hydroxide ion concentration (OH-), strong bases dissociates 100% in water

1. hydroxides of group 1 metals
2. heavy group 2 metals (Sr, Ba, Ra, Ca)

Question 16

Dissociation of Water (Kw)

Answer 16

Kw = 1.0 x 10^-14
[H3O+][OH-] = 1.0 x 10^-14

Question 17

equations for calculating pH and pOH

Answer 17

1. pH = -log[H3O+]
2. pOH = -log[OH-]
3. pH + pOH = 14
4. 1.0 x 10^-14 = [H3O+][OH-]
5. Ka = [H3O+][OH-] / [HA-]
6. Kb = [M+][OH-] / [MOH-]
7. MaVa = MbVb

Question 18

titration

Answer 18

indicator are used to determine the concentration of acids and bases: MaVa = MbVb

Question 19

neutralization reactions (salt formation)

Answer 19

acid + base → salt + water

Question 20

synthesis reactions

Answer 20

metal + nonmetal → salts
acid + metal → salt + hydrogen gas
acid anhydride + basic anhydride → salt

Question 21

anhydride

Answer 21

without water - nonmetal oxide, metal oxide

Question 22

acidic anhydride

Answer 22

compounds which contain oxygen and react with water to produce acidic solutions (ex: SO3(g) + H2O(l) → H2SO4(aq)

Question 23

basic anhydrides

Answer 23

compounds which contain oxyge and react with water to produce basic solutions (ex: Na2O(s) + H2O(l) → 2NaOH(aq)

Question 24

buffers

Answer 24

used to maintain the pH of any solution when small amounts of acid or base are added, formed by weak acid + salt of conjugate base