unit 10 - acids, bases, & salts Flashcards
electrolytes
Substances that can conduct electric current, because they dissociate into ions (charged
particles that can carry a current) in the liquid state.
- ALL acids, bases, and salts are electrolytes
Acids
Release Hydrogen Ions (H+) or form Hydronium Ions (H3O+) ions in solution.
- Watch out for “COOH” endings
they are organic acids (CH3COOH) - Watch out for CO2 (aq); carbon dioxide in
water becomes H2CO3
COOH endings are
organic acids (CH3COOH)
acids generally begin with
H or end in COOH
reading table k (acids)
as you go down, weaker the acid
HCl - strong
CH3COOH - weak
bases
Release Hydroxide Ions (OH-) in solution.
*Watch out for NH3 (aq); ammonia in water becomes NH4OH
bases end in
OH generally
salts
Substances that are not acids or
bases BUT ! dissociate into ions in
solution that are not H+ and OH-.
nonelectrolytes
Substances that are bad conductors of electricity because they do NOT dissociate into ions in solution.
Ex. Molecular Substances or Covalent
- C6H12O6, C12H22O11 (sugars)
- C2H5OH (alcohol) * Watch out for this* alcohols have C’s & H’s followed by OH thus they are not a base.
alcohols have…
C’s and H’s followed by OH thus they are not a base
characteristics of acids
- Acids have a sour taste.
Ex. Lemon contain Citric Acid. - Acids are electrolytes & conduct electric currents.
All Acids release H+ Ions/H3O+
(hydrogen)/(hydronium)
arhenius definition of an Acid
Acids are electrolytes & conduct electric currents. All Acids release H+ Ions/H3O+
(hydrogen)/(hydronium)
strong acids easily…
ionize
- release high [H+]
weak acids dont easily
ionize
- release low [H+]
characteristics of bases
- Bases have a Bitter taste.
- Bases are slippery to the touch.
- Bases are electrolytes & conduct Electric Currents. All Bases release
[OH-] Ions
arrhenius definition of Bases
- Bases are electrolytes & conduct Electric Currents. All Bases release
[OH-] Ions
strong bases release
high [OH-]
weak bases release
low [OH-]
What are the two major reaction that involve acids &/or bases?
1) Neutralization Reactions
- Acids + Bases
2) Special Single Replacement Rxns
- Acids + Strong!! Metals
Neutralization Reaction
** special double replacement
acid + base => salt + water
what is the reverse reaction of neutralization
- reverse reaction (opposite) is hydrolysis
- salt + water => acid + base
acids react with _______ metals to produce what
STRONG metals to produce hydrogen gas
**not all metals will do this because of their reactivity
acids reacting with metals
- Look it up on Table J
- ONLY!! metals listed above Hydrogen (H2) Are reactive enough that will react with acids to produce Hydrogen gas + a salt.
acids and bases affect the color of indicators based on the specific
pH
EX: Will Cu react with HCl? Why or why not?
No, Cu is not active enough
pH is based on the
- concentration of an acid
- pH scale expresses [H+] concentration as a # from 0-14
pH of 0
strong acid
pH of 7
neutral
pH of 14
strong base
DO NOT discuss pH range
- USE ONLY!!! The numbers to the right or left of \the range. Even for part 2 answers
- Never use number in the range because the indicator is just changing color.
the lower the pH the…
more acidic the substance is (the less basic it is)
more acidic = _____ H+ ions released
more H+ ions released
ex: pH of 3 more acidic than 4
the higher the pH the…
less acidic the substance is (the more basic it is)
less acidic = _____ H+ ions released
fewer H+ ions released
ex: pH of 9 is less acidic (more basic) than 7
water can dissociate
when pH 7 or pure water at 25°C
[H+] = 1 x 10^-7 & [OH-] = 1x 10^-7
concentration in acids
[H+] is Greater than [OH-]
concentration in bases
[OH-] is Greater than [H+]
concentration when neutral
[H+] is equal to [OH-]
pH formula
pH = -log [H+]
- to find the pH, you need H+ concentration
pH change
- each change in a single pH unit is a TEN fold change in the [H+]
- ex: [H+] is 10x greater in a solution with a pH of 5 as a solution with a pH of 6
if [H+] = 1x10^-9, pH is
9
pOH formula
pOH = -log [OH-]
other than neutral
[H+] X [OH-] = 1 X 10^-14 M
pH + pOH
= 14
titrations
The process of adding measured volumes of an Acid or Base of known concentration TO an Acid or Base of unknown concentration until neutralization occurs
when the NEUTRALIZATION point is reached it means the
[H+ ] = [OH- ]; pH is 7
- moles of H+ = moles of OH-
titration formula
Ma x Va = Mb x Vb
- look at this for sigfigs
when data table says “volume used”
use that in MaVa = MbVb
when data table says “initial or final volume”
subtract to find volume used
Bronsted/Lowry:”Alternate Theory”: Acids
acids lose protons (proton donors)
Bronsted/Lowry:”Alternate Theory”: Bases
bases gain protons (proton acceptors)
