Unit 13
Marker Board
Review
Acids & Bases
You need a marker board, marker,
eraser, calculator, & periodic table.
Question #1
List 4 properties of acids.
Answer:
1 – Sour taste
2 – React with metals to form hydrogen gas
3 – React with metal carbonates to form CO2 gas
4 – Turn indicators red
Question #2
List 4 properties of bases.
Answer:
1 – Taste bitter
2 – Unreactive with metals and carbonates
3 – Feel slippery
4 – Turn indicator blue
Question #3
According to Arrhenius,
acids ionize to produce _______ ions &
bases ionize to produce _______ ions.
Answer:
hydrogen
hydroxide
Question #4
A Bronsted acid _____________ a
_______________ and a base
______________ a ____________.
___________ is a substance that can either
donate or accept a H+ ion.
Answer:
- donates, hydrogen ion
- accepts, hydrogen ion
- Amphoprotic/Amphoteric
Question #5
Label the Acid, Base, Conjugate Acid, &
Conjugate Base for each reaction below:
• NH3 + H2O  NH4+ + OH• H2CO3 + H2O  H3O+ + HCO3Answer:
NH3 + H2O  NH4+ + OHB
A
CA
CB
H2CO3 + H2O  H3O+ + HCO3A
B
CA
CB
Question #6
Strong acids ionize _______________ while
weak acids ionize ________________.
Which is the stronger acid?
Oxalic Acid: Ka = 5.1 x 10-5
Carbonic Acid: Ka = 4.8 x 10-11
Answer:
completely;
only partially;
Oxalic Acid (larger Ka value)
Question #7
When an acid reacts with a base to
neutralize it, the products are a
___________ & ___________.
Answer: Salt & Water
Question #8
List (write the formula for) the 6 strong acids.
Answer:
HCl
HI
HBr
HClO4
HNO3
H2SO4
Question #9
Acids have a pH ___________ than 7.
Bases have a pH __________ than 7.
Pure water has a pH of _____ because . . .?
Answer: Less
Greater
7 because it is neutral!
Question #10
Write the name for the following formulas. Is it an acid or base?
Check your answers after you’ve written ALL of them!
•
•
•
•
•
•
•
•
•
HBr
NaOH
HNO2
H3PO3
NH3
H2SO4
Mg(OH)2
H2CO3
HC2H3O2
Hydrobromic Acid—acid
Sodium Hydroxide—base
Nitrous Acid—acid
Phosphorous Acid - acid
Ammonia—base
Sulfuric Acid—acid
Magnesium Hydroxide - base
Carbonic Acid—acid
Acetic Acid—acid
Question #11
Write & balance the equation for the
neutralization of sulfuric acid with
potassium hydroxide.
Answer:
H2SO4 + 2 KOH  2 H2O + K2SO4
Question #12
Write & balance the neutralization reaction
of hydrobromic acid & calcium hydroxide.
Answer:
2 HBr + Ca(OH)2  2 H2O + CaBr2
Question #13
The formula for the hydronium ion is
____________________ & for the
hydroxide ion _______________.
Answer: H30+
&
OH-
Question #14
An H+ ion is really just a _______________
and cannot exist in solution.
Answer: Proton
Question #15
Write the equation for the
self-ionization of water.
Answer: H2O + H2O  OH- + H3O+
Question #16
The formula for calculating [H3O+] from pH is
______________________.
I type this into my calculator as: _________
Answer: [H3O+] = 10^(-pH)
2nd log (negative pH)
Question #17
The formula for calculating [H3O+] from [OH-]
is ______________________.
I type this into my calculator as: _______
Answer: Kw = [OH-][H3O+] = 1.0 x 10-14
[H3O+] = 1.0 x 10-14
[OH-]
1.0 E -14 / [OH-]
Question #18
• List the formulas for pH, H+ concentration,
pOH, & OH- concentration.
Answer:
pH = -log [H+] OR 14 - pOH
[H+] = 10^(- pH) OR 1.0 x 10-14 / [OH-]
pOH = -log [OH-] OR 14 - pH
[OH-] = 10^(- pOH) OR 1.0 x 10-14 / [H3O+]
Question #19
• pH + pOH = ___________
•Answer: 14
Question #20
What is the pH of an HCl solution with a
concentration of 0.0015 M? Acidic or
basic?
•Answer: pH = -log (0.0015) = 2.8
Acidic
Question #21
• What is the pH of a solution with an pOH
of 10.5? Acidic or basic?
Answer: pH = 14 – pOH = 14 – 10.5 = 3.5
Acidic
Question #22
• What is the [H+] of a solution with a pH of
4.51?
Answer: [H+] = 10^(-4.51) = 3.09 x 10-5 M
Question #23
• What is the pOH of a solution with a [H+]
of 9.99 x 10-9 M? Acidic or basic?
Answer: pOH = -log [OH-]
[OH-] = 1.0 x 10-14 / 9.99 x 10-9 = 1.0 x 10-6 M
pOH = -log(1.0 x 10-6) = 6.0
pH = 14 – 6.0 = 8.0  Basic
Question #24
• What is the pOH of a solution with an
[OH-] of 7.81 x 10-3 M? Acidic or basic?
Answer: pOH = -log [OH-] =
-log (7.81x10-3) = 2.1
pH = 14 – 2.1 = 11.9  Basic
Question #25
• Calculate the [OH-] if the pOH is 5.21.
Answer: [OH-] = 10^(-5.21) = 6.17 x 10-6 M.
Question #26
What is the purpose of a titration? What is
the role of an indicator in a titration? What
has been reached when acid and base
completely neutralize one another?
Answer: A titration enables you to determine the
concentration of a solution by reacting a known
volume of the solution with a solution of known
concentration.
An indicator changes color when the end point
of the titration has been reached.
The end point has been reached.
Question #27
• You add a substance to pure water and
the pH rises from 7 to 9. What has
happened to the concentration of H3O+?
Is the substance added an acid or a base?
Answer: The concentration of H3O+ has
decreased. The substance is a base.
Question #28
• In the titration of a strong acid with a
strong base, what pH range should the
indicator have?
Answer: 6-8
Question #29
• Write the balanced equation for the
reaction between nitric acid and
magnesium hydroxide.
Answer:
2 HNO3 + Mg(OH)2  Mg(NO3)2 + 2 H2O
Question #30
• What is the molarity of HNO3 if 15.0 mL is
completely neutralized by 38.5 mL of 0.15 M
Mg(OH)2?
Answer:
2 HNO3 + Mg(OH)2  Mg(NO3)2 + 2 H2O
MaVaCb = MbVbCa
Ma(15.0)( 1) = (0.15)(38.5)(2)
Ma = 0.77 M