Chem I – Acids/Bases/Salts
#1- Naming & Writing Acid - Review
Name____________________ Period_________
Name the following acids:
Acids are molecular compounds molecules that contain
hydrogen bonded to a nonmetal or to a group of
polyatomic ions. Acids can be either binary (consisting
of only two elements) or ternary (consisting of more
than two elements…usually polyatomic ions). Even
though acids are molecules that are covalently bonded,
they have properties of ionic compounds. Therefore the
rules for naming and writing ionic compounds apply.
1. HNO3
2. HCl
3. H2SO4
4. H2SO3
NAMING BINARY ACIDS

Hydro ______ ic acid.
Example: HCl = hydrochloric acid
5. HC2H3O2
NAMING TERNARY ACIDS:
1. Identify the polyatomic ion in the formula
2. Look for the ending and change:

“ate” changes to “ic”

“ite” changes to “ous”
6. HBr
7. HNO2
Example: HPO4 = phosphoric acid (PO4 is
phosphate therefore changed to “ic”)
8. H3PO4
3.
9. H2S
10. H2CO3
Look for polyatomic ions that contain four
oxygen possibilities (ClO3-1 and IO3-1)

Per_____ic
greatest # of oxygen atoms (ClO4-1)

_____ic
greater # of oxygen atoms (ClO3-1)

_____ous
smaller # of oxygen atoms (ClO2-1)
WRITING BINARY ACID FORMULAS:
1. Write H+1
2. Write the second element’s symbol &
oxidation number.
3. Criss Cross the charges to create a neutral
formula.
Example: Hydrochloric acid = H Cl- = HCl
Write the formulas of the following acids:
11. sulfuric acid
12. nitric acid
WRITING TERNARY ACID FORMULAS:
1. Write H+1
2. Identify the polyatomic ion.
3. Change the endings by:

“ic” changes to “ate”

“ous” changes to “ite”
4. Write the polyatomic ions & oxidation
number.
5. Criss Cross the charges to create a neutral
formula.
Example: sulfuric acid = H+ SO4-2 = H2S04
6. Look for prefixes such as “per” and “hypo”.
They indicate the actual number of oxygen
atoms in the compound.
Example: perchloric acid = H+ ClO4-1 = HCl04
13. hydrochloric acid
14. acetic acid
15. hydrofluoric acid
16. phosphorous acid
17. carbonic acid
18. nitrous acid
19. phosphoric acid
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20. hydrosulfuric acid
Chem I – Acids/Bases/Salts
Name_________________________ Period_______
Bronstead-Lowery Acids & Bases
PART A. According to the Bronstead-Lowry theory, an acid is a proton (H+) donor, and a base is a proton
acceptor.
H+
Example:
HCl +
acid
OH- →
Cl- +
base
H2O
Label the Bronsted-Lowrt acids and bases in the following reactions and show the direction of the proton
transfer. Notice that the reactions are reversible, therefore label the acid and base on each side of the
reaction.
H+
Example:
H2O +
acid
H+
Cl- ↔
base
OH- +
base
1. H2O + H2O ↔
2. H2SO4 + OH- ↔
acid
H3O+ + OH-
HSO4 + H2O
3. HSO4- + H2O ↔ SO4-2
4. OH-
HCl
+
H3O+
+ H3O+ ↔ H2O + H2O
5. NH3 + H2O ↔
2
NH4+ + OH-
PART B. According to Bronstead-Lowry theory, after an acid has given up its proton, it is capable of getting
back that proton and acting as a base. Conjugate base is what is left after an acid gives up a proton. The
stronger the acid, the weaker the conjugate base. The weaker the acid, the stronger the conjugate base.
Fill in the blanks in the table below.
ACID
BASE
1.
H2SO4
HSO4-
2.
H3PO4
ACID
11.
HClO
12.
Cl-1
NO2-1
3.
F-
13.
4.
NO3-
14.
H2SO3
HBr
5.
H2PO4-
15.
6.
H2O
16.
SO4-2
7.
17.
8.
HPO4-2
18.
9.
NH4+
19.
10.
H2O
BASE
20.
3
CO3-2
HCN
C2H3O2-1
H2CO3
HS-1
Chem I – Acids/Bases/Salts
#2- Neutralization Reactions

Perform the following neutralization reactions using: MAVA = MBVB *Remember to adjust the M
for H2SO4, Ca(OH)2, Ba(OH)2, and Sr(OH)2.
1. How many mL of a 0.50 M HCl acid is needed to neutralize a 500. mL 0.75 M KOH solution?
2. Calculate concentration of acid if 500. mL of HI is used to neutralize a 900. mL 1.50 M NaOH solution.
3. How many mL of a 6.0 M H2SO4 acid is needed to neutralize a 1500. mL 2.50 M KOH solution?
4. Find the concentration of acid if 25.0 mL of HClO4 is needed to neutralize a 35.5 mL 2.50 M LiOH
solution.
5. How many mL of a 0.500 M HNO3 acid is needed to neutralize a 575 mL 0.75 M Ca(OH)2 solution?
6. What is the concentration of base if 750 mL of NaOH is needed to neutralize a 1200. mL 1.25 M
H2SO4solution?
7. Find the mL of 0.350M Ba(OH)2 needed to completely react with 45.6 mL of 1.00M HBr acid.
8. What is the concentration of HClO3 if 55.5 mL is neutralized by 25.5 mL of 0.250M Sr(OH)2?
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Chem I – Acids/Bases/Salts
#3 - pH and pOH
PART A. The pH of a solution indicates how acidic or basic that solution is.
pH range of 0 - 7
7
7 - 14
acidic
neutral
basic
Since [H+] [OH] = 10-14 at 25O C. of [H+] is known, the [OH-] can be calculated and vice versa.
pH = -log [H+]
pOH = -log [OH-]
Together, pH + pOH = 14.
So if [H+] = 10-6 M, pH = 6.
So if [OH-] = 10-8 M, pOH = 8
Complete the flowing chart.
[H+]
1.
10-5 M
pH
5
10-9 M
10-2 M
11
5.
12
6.
10-5 M
7.
10-11 M
13
9.
10.
9
10-4 M
3.
8.
pOH
7
2.
4.
[OH-]
6
5
Acidic or Basic
Acidic
Calculate the pH of the solutions below.
1. 0.01 M HCl
2. 0.0010 M NaOH
3. 0.050 M Ca(OH)2
4. 0.030 M HBr
5. 0.150 M KOH
6. 2.0 HC2H3O2 (Assume 5.0% dissociation)
7. 3.0 M HF (Assume 10.0% dissociation)
8. 0.50 M HNO3
9. 2.50 M NH4OH (Assume 5.00% dissociation)
10. 5.0 M HNO2 (Assume 1.0% dissociation)
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Chem I – Acids/Bases/Salts
#4 – pH Table
*Formulas:
pH + pOH = 14
pH = -log[H+]
pOH = -log[OH-]
[H+] = antilog (-pH)
[OH-] = antilog (-pOH)
*Remember to adjust the M for H2SO4, Ca(OH)2, Ba(OH)2, and Sr(OH)2 (multiply by 2)
*Remember to adjust the M for weak acids and bases (multiply by the % disassociation)
PART A: Complete the following table:
Substance
Strong or
Weak Acid
or Base
[H+]
[OH-]
0.100 M HCl
0.250 M Ca(OH)2
0.750 M HNO2
(2.50%)
0.655 M KOH
0.200 M H2SO4
0.850 M HNO3
0.910 M HNO3
0.150 M HClO4
0.850 M HC2H3O2
(3.50%)
0.555 M NaOH
0.350 M Ba(OH)2
0.200 M HClO3
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pH
pOH
Acidic,
Basic or
Neutral
PART B: Solve each problem and show work.
1. Calculate pH of a 0.0150M HCl solution.
2. Find pOH of a 0.020M hydrobromic acid, HBr, solution.
3. What is the concentration of OH- if the pH of a solution is 4.45?
4. Calculate OH- concentration of a solution with a pOH of 7.85.
5. Find concentration of acid (H30+) if the pH is 3.50.
6. Hydrochloric acid in the stomach has a pH of about 2.00. Find the concentration of HCl.
7. Find concentration of base (OH-) given an acid concentration of 1.55 x 10-3M.
8. Find acid concentration given a base concentration of 6.35 x 10-2M.
9. Calculate pH of 1.44 x 10-1M of acetic acid. (2.50% dissociation)
10. Calculate concentration of acid given 0.250M of ammonia (base). (5.00% dissociation)
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Chemistry I
pH Scales of Indicators: #5

Use the following color codes for each of the following indicators and color in the pH scales
based on the indicator.
1. Phenolphthalein: pH: 0-9: colorless, 9-14: pink. Distinct division of color.
2. Malachite Green: pH: 0-2 yellow, 2-11.6 green, 11.6-13.8 blue, 13.8-14 colorless. Distinct
division.
3. Methyl Orange: pH: 3.0-4.4. Red to orange to yellow. Gradual division between colors.
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Chemistry I
Titration Problem Set #6
PART I: *MAVA = MBVB, *Calculate volume of base, *Calculate volume of acid, *Put in values and
solve
1. You conduct a titration using 0.500 M potassium hydroxide base (KOH) and an unknown
hydrochloric acid (HCl) solution. The buret had an initial reading of 0.35 mL and a final reading of
36.89 mL for the base and an initial reading of 0.89 mL and a final reading of 47.63 mL for the acid.
Calculate the molarity of the acid.
b. Calculate the pH of the acid solution.
c. Write an ionic and net ionic equation for the neutralization reaction.
2. You conduct a titration using 0.250 M nitric acid (HNO3) and an unknown sodium hydroxide (NaOH)
solution. The buret had an initial reading of 3.56 mL and a final reading of 24.82 mL for the acid and
an initial reading of 1.12 mL and a final reading of 33.56 mL for the base. Calculate the molarity of
the base.
b. Calculate the pH of the base solution.
c. Write an ionic and net ionic equation for the neutralization reaction.

Use the following titration curves to answer the question #3:
3. a. What is the pH of the equivalence point of this
titration?
b.
Is this solution acidic, basic, or neutral?
c. What is the approximate pH of the final solution?
d. Describe the strength of the acid and the strength
of the base that could have produced this titration
curve.
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PART II: *Strong acids + Strong bases = neutral salt water solution
*Strong acids + Weak bases = acidic salt water solution
*Weak acids + Strong bases = basic salt water solution
4. The following salts were created from titrating acids and bases. Determine the parent acid, parent base,
rank the strength of parent acids and bases, and determine whether the final salt solution is acidic,
basic, or neutral.
K2CO3
Parent Acid
(add H+1 to anion)
Parent Base
(add OH-1 to cation)
Type of Solution
H2CO3 (WA)
KOH (SB)
Basic
Na2SO4
Ca(C2H3O2)2
Zn(NO3)2
Mg(ClO3)2
Ba(ClO4)2
FeCl3
CsBr
5. When titrating the following acids and bases, write balanced equations and determine whether the final
solution would be neutral, acidic, or basic.
a. hydrochloric acid and zinc hydroxide yield water and zinc chloride
b. sodium hydroxide and hydrochloric acid yield water and sodium chloride
c. barium hydroxide and acetic acid yield water and barium acetate
d. sulfuric acid and magnesium hydroxide yield water and magnesium sulfate
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