Study your flashcards anywhere!

Download the official Cram app for free >

  • Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off

How to study your flashcards.

Right/Left arrow keys: Navigate between flashcards.right arrow keyleft arrow key

Up/Down arrow keys: Flip the card between the front and back.down keyup key

H key: Show hint (3rd side).h key

A key: Read text to speech.a key


Play button


Play button




Click to flip

29 Cards in this Set

  • Front
  • Back
Name the Properties of Acids
-gives a tart/sour taste (vinegar)
-conduct electricity when dissolved in water
-certain chemical dyes (indicators) cause change in color
-many metals react with to produce H2 gas
-reacts with compounds containing OH- to form H2O and salt
Name the Properties of Bases
-give a bitter taste and slippery feel (soap)
-can be strong/weak electrolyte
-change indicator specific color
-reacts with acid to form H2O and salt
Acid Definition
compound that produces H+ ions when dissolved in H2O
when substance ends with
-ide the acid name is (ex. Hydrogen and Cloride)
hydro______ic acid (ex. Hydrochloric acid)
when substance ends with
-ite the acid name is (ex. Hydrogen and Sulfite)
______ous acid (ex. sulforous acid)
when substance ends with
-ate the acid name is (ex. Hydrogen and Sulfate)
____ic acid (ex. sulfuric acid)
Base Definition
compound that produces OH- ions when dissolved in H2O
Naming of Bases
same as regular ionic compounds (ex. NaOH = Sodium Hydroxide)
Self Ionization Water
process of water splitting to produce 2 ions: H30+ and OH-

ex. H2O + H2O <> H3O+ and OH-
ex. H2O + H2O <> H+ and OH-
[H+] X [OH-]= 1 X 10^-14
acidic solution [H+] vs [OH-]
[H+] > [OH-]
basic solution [H+] vs [OH-]
[H+] < [OH-]
neutral solution [H+]vs[OH-]
[H+] = [OH-]
Definition of pH
-scale used to indicate the acidity or basicity; ranges from 0-14
-acid <7
-neutral = 7
-base >7
formulas for pH/pOH and concentrations
pOH= -log [OH-]
pH = -log [H+]
[OH-]= 10^-pOH
14=pH + pOH
arrhenius acid
compound that produces H+ ion when dissolved in H2O
arrhenius base
compound that produces OH- ion when dissolved in H2O
monoprotic acid
diprotic acid
triprotic acid
-acid with 1 ionizable H
-acid with 2 ionizable H
-acid with 3 ionizable H
bronsted-lowry acid
H+ ion proton donor
bronsted-lowry base
H+ ion proton acceptor
conjugate acid
product of base after accepting hydrogen ion
conjugate base
product of acid after donating hydrogen ion
conjugate acid/base pair
acid or base and its conjugate
substance that can act as either an acid or a base
lewis acid
e- pair acceptor
lewis base
e- pair donor
neutralization rxn
rxn of acid + base to produce H2O and salt compound
titration formulas
(use stoichiometry)
concentration (M)=

moles=concentration (M) X volume (L)
acid-base may react different ratios so...
balance the equation