A strong acid
- ionizes completely in solution
- produces hydronium ions in solution
- reacts with metals that are more active than hydrogen
Which of the following substances is a weak base?
NH3
Which of the following is not a strong acid?
CH3COOH
An Arrhenius acid is a chemical compound that
increases the concentration of H+ ions in a solution
All Br�nsted-Lowry acids
- are aqueous solutions
- can act as Arrhenius acids
- donate protons
Which of the following is a polyprotic acid?
H2SO4
What is the conjugate base of the hydronium ion, H3O+?
H2O
The conjugate acid of the chloride ion, Cl, is
HCl
A conjugate acid is an acid that forms when
a base gains a proton
In an acid-base reaction, the conjugate base of the weaker acid is the
stronger base
An amphoteric species is one that reacts at 25�C as a(n)
acid or base
A conjugate base is the species that
remains after an acid has given up a proton
In the following reaction, which substance is the conjugate base of HClO4?
HClO4(aq) + H2O(l) H3O+(aq) + ClO(aq)
ClO4-
What is the concentration of hydronium ions in pure water?
- 1.0 3 1027M
- Kw
--------
[OH-]
- same as [OH-]
As the [H3O+] of a solution increases, the value of
- long [H3O+] increases
- -log [H3O+] deacreases
- the solution's pH decreases
The pH of a solution is defined as
- log [H3O+]
Which of the following is not a property of an acidic solution?
[HO2] geater than 1x10-7 M
A basic solution
has a lower concentration of hydronium ions than hydroxide ions
A solution that has a pH of 13 is a
string base
What is the pH of household ammonia in which the [H3O+] is 1.0 � 10-12 M?
12
What is the [OH] in a sample of lime juice with a pH of 2.0?
1.0x10-12
An acid-base indicator
- is either a weak acid or weak base
- has a different color at a different pH
- can be used to find the equivalence point
When performing the calculation for a titration experiment, you need to have the balanced equation for the neutralization reaction in order to determine
the chemically equivalency amount of acid and base
A titration always involves the
controlled addition of a standard solution
For any acid titrated with a base, the equivalence point occurs when the
acid and base are present in chemically equivalent amounts
What is monitored in an acid-base titration?
pH
During an acid-base titration, a rapid change in pH
occurs when the amount of H3O+ ions and OH- ions are nearly equal
The neutralization of any strong acid and strong base produces mostly
H2O molecules
Which of the symbols below denotes the acid ionization constant?
Ka
The acid ionization constant for weak acids
is much less than 1
A solution that can resist changes in pH is called a(n)
buffered solution
Hydrolysis is a reaction that occurs when water molecules
react with ions of a salt
Salts of weak acids and weak bases can produce
- acidic solutions
- basic solutions
- neutral solutions
An acid and the base that can combine to form the salt CaCl2 are
HCl and Ca(OH)2
What are the conjugate acid-base pairs for the reaction represented by the following equation?
B and BH+ ; H2O and OH-
Arrhenius acids and bases
acids: contain H+ ions (Hx)
bases: contain OH- ions (MOH)
Bronsted Lowery acids and bases
acids: H+ / proton donor
bases: H+ / proton acceptor
lewis acids and bases
acids: electron pair acceptor
bases: electron pair donor
properties of acids:
- sour
- pH < 7
- food
properties of bases:
- pH > 7
- bitter
- cleaning supplies
- slippery
amphoteric:
acts as acid or base
pH =
p = -log
H = hydrogen ions
organic acids =
COOH
what molecule is amphoteric
water
bases tend to have.....charge?
a negative or no charge
hydronium =
H3O+
strong acids
dissociate completely (always starts with H)
- HCl
- HBr
- HI
- HNO5
- HClO4
- H2SO4
strong bases
- LiOH
- NaOH
- KOH
- Ca(OH)2
- Sr (OH)2
- Ba (OH)2
weak acids
don't dissociate completely
Ka and Kb
HA <-> H+ + A- (Ka)
B + H2O <-> BH+ + OH- (Kb)
pH diamond
2.
pH----[pOH]
1. [ 5. ] 3.
[ 6. ]
[H+]----[OH-]
4.
1. pH = -log[H+]
2. pH+pOH = 14
3. pOH = -log[OH-]
4. [H+][OH-} = Kw = 1x10^-14
5. 10^-pH = [H+]
6. [OH-} = 1o^-pOH
titrations:
use reaction of a known concentration of an acid or base to determine the concentration of an unknown acid or base using stoichiometry
- stock solution (known concentration)
- unknown base or acid
- pH indicator
equivalence pount
mols [H+] added = mols [OH-] present (neutralization point) "vertical line
standard solution:
the known concentration used to determine unknown
end point:
when the indicator changes color
buffers:
changes colors at particular pH change