Acids and Bases Flashcards
Characteristics of acids
sour, red on red litmus, red on blue litmus, electrolytic, form hydrogen when reacted with metal, watery, changes color dyes
characteristics of bases
bitter, blue on red litmus, blue on red litmus, electrolytic, slippery, changes color in dyes
Arrhenius Theory
acid- any compound that produces a hydrogen ion
base- a compound that produces a hydroxide ion
The Lewis Theory
acid- an electron pair accepter
base- an electron pair donor
Bronstead-Lowry
acid- a proton donor
base- a proton accpeter
amphiprotic
when a compound can act as either an acid or a base
conjugate acid base pairs
differ by one hydrogen ion (proton)
neutralizing reactions
acid + base → salt + water
Hx(aq) + MOH(aq) → Mx(aq) + H2O(aq)
monoprotic acids
acids that can donate one proton
monoprotic bases
bases that can accept one proton
polyprotic acids
acids that can donate two or more protons, donate protons one at a time
polyprotic bases
bases that can accept two or more protons
Ostwald Process
industrial synthesis of nitric acid (HNO), produces nitrogen dioxide which is highly poisonous
acid strength
proportional to the hydronium ion concentration (H3O+), weak acids establish equilibrium, strong acids dissociate 100% in water:
- hyperchloric acid (HClO4)
- hydroiodic acid (HI)
- hydrobromic acid (HBr)
- hydrochloric acid (HCl)
- nitric acid (HNO3)
- sulfuric acid (H2SO4)
- hydronium ion (H3O+)
base strength
proportional to hydroxide ion concentration (OH-), strong bases dissociates 100% in water
- hydroxides of group 1 metals
- heavy group 2 metals (Sr, Ba, Ra, Ca)
Dissociation of Water (Kw)
Kw = 1.0 x 10^-14 [H3O+][OH-] = 1.0 x 10^-14
equations for calculating pH and pOH
- pH = -log[H3O+]
- pOH = -log[OH-]
- pH + pOH = 14
- 1.0 x 10^-14 = [H3O+][OH-]
- Ka = [H3O+][OH-] / [HA-]
- Kb = [M+][OH-] / [MOH-]
- MaVa = MbVb
titration
indicator are used to determine the concentration of acids and bases: MaVa = MbVb
neutralization reactions (salt formation)
acid + base → salt + water
synthesis reactions
metal + nonmetal → salts
acid + metal → salt + hydrogen gas
acid anhydride + basic anhydride → salt
anhydride
without water - nonmetal oxide, metal oxide
acidic anhydride
compounds which contain oxygen and react with water to produce acidic solutions (ex: SO3(g) + H2O(l) → H2SO4(aq)
basic anhydrides
compounds which contain oxyge and react with water to produce basic solutions (ex: Na2O(s) + H2O(l) → 2NaOH(aq)
buffers
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
