Download Intro to A/B Worksheet - ANSWER KEY

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Intro to Acids & Bases Review Worksheet
Naming Acids and Bases
Complete the table below –
Chemical Formula
HCl
NaOH
HNO3
Ca(OH)2
H2SO4
H2CO3
NH3
Acid/Base Name
Hydrochloric Acid
Sodium hydroxide
Nitric Acid
Calcium hydroxide
Sulfuric Acid
Carbonic acid
Ammonia
Acid or Base?
Acid
Base
Acid
Base
Acid
Acid
Base
Theories of Acids and Bases
1. We said that acids were any chemical that increased H+ in water, and bases were any chemical that increased
OH- in water. This was the Arrhenius/Bronsted-Lowry/Lewis (circle one) definition of acids and bases.
2. We also learned that substances that transfer protons are acids and substances that accept them are bases. This
was the Arrhenius/Bronsted-Lowry/Lewis (circle one) definition of acids and bases.
3. In addition we learned that substances that share electrons are bases and substances that accept electron pairs
are acids. This was the Arrhenius/Brownsted-Lowry/Lewis (circle one) definition of acids and bases.
Practice Problems-Who is Who?
DIRECTIONS: In the following reactions, identify which reactant in each reaction is the acid and which is
the base. In addition, identify each theory that can be applied and an explanation for why it can be applied
EXAMPLE:
HCl
+

H2O
H3O+1
Cl-1
+
HCl = acid and water is the base using Arrhenius Theory because HCl produces
Hydronium ion (=H+) in water. It could also be an acid by Bronsted Lowery because
HCl donates a H+ to water making water a BL base because it accepts the proton.
4.
HBr
+
H2O

H3O+1
+
Br-1
Answers may vary. HBr is an acid by Arrhenius.
5.
HI
+
H2O
H3O+1

I-1
+
Answers may vary. HI is an acid by Arrhenius.
6.
NH3
+
H2O

NH4+1
+
OH-1
Answers may vary. NH3 is a base by Arrhenius and a base by bronsted-lowry because it accepts a proton.
7.
HI
+
KOH

KI
+
Answers may vary. KOH is a base by lewis because it donates/shares an electron pair.
H2O
pH Problems:
pH formulas:
[H+1] = 10-pH
[OH-1] = 10-pOH
pH = -log [H+1]
pOH = -log [OH-1]
[H+1][OH-1] = 1 x 10-14
pH + pOH = 14
For each problem below write the equation you would use to solve it and then solve the problem
showing what you plugged in and where.
1.
Calculate the pH for the following [H+] concentrations:
a. 8.3 x 10-10 M
pH = -log [8.3 x 10-10 M] = 9.1
b. 2.6 x 10-3 M
pH = -log [2.6 x 10-3 M] = 2.6
2. Calculate the [H+] from the following pH values:
a. pH = 4.30
[H+] = 10-pH = 10-4.30 = 5.01 x 10-5 M
b. pH = 1.80
[H+] = 10-pH = 10-1.80 = 1.58 x 10-2 M
3. What would be the [OH-] of an aqueous solution given the [H+] = 2.0 x 10-4 M
[H+][OH-] = 1 x 10-14
[OH-] = 1 x 10-14 = 1 x 10-14 = 5.0 x 10-11
[H+]
2.0 x 10-4
4. What would be the pOH of an aqueous solution given the pH= 5.2
pH + pOH = 14
pOH = 14 – pH = 14 – 5.2 = 8.8
5. What would be the [OH-] of a solution whose pOH = 4.50
[OH-] = 10-pOH = 10-4.50 = 3.16 x 10-5
6. What would be the hydrogen ion concentration given a hydroxide concentration of 2.0 x 10-4 M
[H+][OH-] = 1 x 10-14
[H+] = 1 x 10-14 = 1 x 10-14 = 5.0 x 10-11
[OH-]
2.0 x 10-4