Acids and Bases
Review
A game by Taylor Shupe and Mallory
Mac
Arrhenius
Acids
BronstedLowery
Color
Indictors
Percent
Ionization
pH
Neutralization
100
100
100
100
100
100
200
200
200
200
200
200
300
300
300
300
300
300
400
400
400
400
400
400
What produces H+ in a solution
What is an Acid
What type of solution has [OH-]> 10-7 and
[OH-]> [H+].
What is Alkaline Solutions
Fill in the blank:
H+
OH-
Type of
solution
1.0x 10 -3
?
?
H+
OH-
Type of solution
1.0x 10 -3
1.0x 10 -11
acidic
This particular case could not be an
Arrhenius base.
What is NH3 ammonia
What is a proton acceptor?
What is a base
When an acid loses a
hydrogen ion it becomes a...
What is a base
Fill in the blank:
Conjugate base
Some substances, such as water,
are amphoteric, what is another
name for amphoteric?
What is amphiprotic
Color indicators are organic
compounds that establish equilibrium
between their ________ form and
ionic form in solution.
What is molecular
The pH at which the color change
occurs is called the
?
.
What is the end point
What type of indicator is this...
What is phenolphthalein
A solution is tested:
methyl red= yellow and
bromothymol blue = yellow.
What is the concentration of the
sample?
What is six
HCl is a strong acid. In an aqueous
solution it will ionize
%
What is 100
H2SO4(aq) + HOH(l)  H3O+(aq) +HSO4-(aq)
How many ionisable hydrogen(s)
does this equation contain
What is two
Find the percent ionization of
0.100M solution of formic acid if
it’s [H +] = 4.22x10-3 M
What is 4.22x10-3 x 100 = 4.22%
0.1
A 0.40 M solution of HClO3 is 0.027%
ionized. Find the Ka for this acid.
[H+] = 0.027 • (0.40) = 1.08 x 10-4 M
100
HClO3(aq)  H+(aq) + ClO3-(aq)
Ka = [H+][ClO3-]
[HClO3]
Ka = (1.08 x 10-4)(1.08 x 10-4)
(0.3999)
Ka = 2.9 x 10-8
Acids taste sour, bases taste
What is bitter
?
An unknown acid has a H+
of 3.9x10-3, what is the OH-?
What is 2.6x10 -12
Find the pOH of a solution with a
+
-3
[H ] of 6.7x10
What is 11.8
Acid + Base 
What is salt
+ water
Calculate the volume of seawater
with a pH of 7.80 that contains 1.0
mol of hydroxide ions.
pH = 7.8
= pOH = 6.2
= [OH-] = 6.3 x 10-7 M
6.3 x 10-7 mol = 1 L
1 mol = ?L
= 1.58 x 106 L
A
is a technique for finding
an unknown concentration of one
chemical from the known
concentration of a second chemical.
What is titration
Find the concentration of an HF
solution if 15.0 mL of 0.200 M KOH
just neutralized 20.0 mL of HF.
HF + KOH → KF + H2O
Step 1
Step 2
Step 3
n = MV = (0.200 mol / L)(0.0150 L) = 0.00300 mol KOH
x mol HF = 0.00300 mol KOH x
1mol HF = 0.00300 mol HF
1 mol KOH
M = n = (0.00300 mol) = 0.150 mol = 0.150 M
V (0.0200 L)
L
A titration shows that 242 mL of 0.500 M
NaOH will just neutralize all of the acetic
acid that is present in 150.0 mL of
vinegar. Find the % by mass of acetic acid
in vinegar.
NaOH + HC2H3O → NaC2H3O2 + H2O
Step 1 n = MV = (0.500 mol) (0.242 L) = 0.121 mol NaOH
L
Step 2 x mol HC2H3O2 = 0.121 mol NaOH x 1 mol HC2H3O2 = 0.121 mol HC2H3O2
1 mol NaOH
Step 3 x g HC2H3O2 = 0.121 mol HC2H3O2 x 60 g HC2H3O2 = 7.26 g HC2H3O2
1 mol HC2H3O2
Step 4 % mass = 7.26 g x 100 = 4.84% acid
150.0 g assumed