Unit 13 Marker Board Review
Acids & Bases
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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 must contain _______ ions &
bases must contain _______ ions.
Answer:
hydrogen
hydroxide
Question #4
A Bronsted acid _____________ a
_______________ and a base
______________ a ____________.
Answer:
- donates
- hydrogen ion
- accepts
- hydrogen ion
Question #5
Label the Acid, Base, Conj Acid, Conj Base
• NH3 + H2O  NH4+ + OH• H2CO3 + H2O  H3O+ + HCO3Answer:
NH3 + H2O  NH4+ + OHB
A
CA
CB
H2CO3 + H2O  H3O+ + HCO3A
B
CA
CB
Question #6 (Acc Only)
Base anhydrides contain a
_________________ and oxygen.
Acid anhydrides contain a
_________________ and oxygen.
Answer: Metal
Nonmetal
Question #7
When an acid reacts with a base to
neutralize it, the products are a
_______________ & ___________.
Answer: Salt & Water
Question #8
Pure water has a pH of _________
because …
Answer: 7…Because it is
neutral!
Question #9
Acids have a pH ___________ than 7;
bases _____________ than 7.
Answer: Less
Greater
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
HCN
NH3
H2SO4
Mg(OH)2
H2CO3
HC2H3O2
Hydrobromic Acid—acid
Sodium Hydroxide—base
Nitrous Acid—acid
Hydrocyanic 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?
•Answer: pH = -log (0.0015) = 2.8
Question #21
• What is the pH of a solution with an pOH
of 10.5?
Answer: pH = 14 – pOH = 14 – 10.5 = 3.5
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?
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
Question #24
• What is the pOH of a solution with an
[OH-] of 7.81 x 10-3 M?
Answer: pOH = -log [OH-] =
-log (7.81x10-3) = 2.1
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?
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.
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
provided by Sam B.S for your benefit
• In a titration, 33.21 mL 0.3020M rubidium
hydroxide solution is required to exactly
neutralize 20.00 mL hydrofluoric acid
solution. What is the molarity of the
hydrofluoric acid solution?
• MHF = 0.5015M