Acids and Bases Homework
Name ________________________________
1. Identify what the general properties of an acid and base are.
2. First, define what an Arrhenius acid /base is and a Bronsted acid / base is and then
identify whether the following reactions would be classified as an Arrhenius acid / base
reaction, Bronsted acid / base reaction, both Arrhenius / Bronsted, or not an acid base
reaction
a. H2O + HCl  H3O+ + Clb. N2 + 3 H2  NH3
c. NH3 + H2O  NH4+ + OHd. NH3 + HCl  NH4+ + Cle. CH4 + 2 O2  CO2 + H2O
3. Identify the conjugate acid for the below bases
a. NH3
b. C2H5Oc. HSO4d. Fe. CO34. Identify the conjugate base for the below acids
a. HCl
b. HBr
c. H2O
d. HF
e. H2CO3
5. Determine the pH of the below solutions. M = Molarity. Identify the solution as either
being Acidic, basic, or neutral as well.
a. 1 x 10-3 M H+
b. 0.10 M OHc. 1 x 10-7 M H+
d. 1 x 10-10 M OHe. 1 x 10-18 M H+
f. 0.0025 M HCl
g. 0.055 M NaOH
h. 0.015 M Ba(OH)2 : Note that there are two OH’s generated
i. 0.0016 M HBr
j. 0.000000000000000001 M HCl
k. 0.000220 M HNO3
60 grams of NaOH is dissolved into 250 mL of water. What is the pH?
l.
m. 80 grams of HCl is dissolved into 500 mL of water. What is the pH?
n. 20 grams of KOH is dissolved into 200 mL of water. What is the pH?
o. 40 grams of HNO3 is dissolved into 1 L of water. What is the pH?
How many grams of NaOH should be dissolved into 500 mL of water to make a
solution have a pH of 13?
q. How many grams of HCl should be dissolved into 500 mL of water to make a
solution have a pH of 1.0?
6. Determine the pOH of the below solutions
a. a cup of coffee, pH 4.32
b. cow’s milk, pH 6.6
c. gastric juice, pH 1.5
d. tomato juice, pH 4.3
e. a coca cola drink, pH 2.8
f. Water, pH of 7.0
7. Determine the Hydronium and Hydroxide concentration of the below pH’s
a. a cup of coffee, pH 4.32
b. cow’s milk, pH 6.6
c. gastric juice, pH 1.5
d. tomato juice, pH 4.3
e. a coca cola drink, pH 2.8
f. Acid rain, pH of 5.2
g. Bleach, pOH of 1
h. Ammonia, pOH of 4.74
i. Vinegar, pH of 2.38
8. What is the difference between a strong acid and weak acid? Then identify the six strong
acids.
9. What is the difference between a strong base and a weak base? Then identify who are
strong bases.
10. Are the following salt solutions acidic, basic, or neutral?
a. KBr
b. Na2CO3
c. Fe(NO3)3
d. NH4NO3
e. CsF
f. LiC2H3O2
g. Na3PO4
h. Al(NO3)3
i. KCl
11. In the given scenarios, determine the relative strength of the acids given or bases given
a. HX, HY, and HZ are all acids. X- is a stronger base than Z- and Y- is a weaker
base than Z-. Rank HX, HY, and HZ in order of increasing acid strength.
b. A-, B-, and C- are all bases. A- is the largest atom and B- is the smallest atom.
Rank the bases in order of increasing base strength.
p.
c. As one moves across the periodic table, the strength of the acid _____? Ie NH3,
H2O, HF
d. As one moves down a column in the periodic table, the acid strength _____?
HCl, HBr, HI.
e. ClO4-, ClO3-, ClO2- are all bases. Rank the bases in order of increasing base
strength.
f. HX+, HY+, and HZ+ are the conjugate acids of the bases X, Y, and Z. If Z is the
strongest base, and Y is the weakest base, rank the conjugate acids in increasing
acid strength.
12. What is the approximate pH of the equivalence point for the following titrations (acidic /
basic / neutral)
a. NaOH + HCl
b. NH3 + HCl
c. NaOH + HF
d. KOH + HBr
e. NH2- + HClO4
13. Identify what type of titration is occurring below (what type is being added to what type)
for the four graphs
14. Determine how many mL of the (acid/ base) would be needed to neutralize the given
solution
a. 15 mL of 0.20 M NaOH being titrated with 0.10 M HCl
b. 30 mL of 0.35 M NaOH being titrated with 0.10 M HCl
c. 45 mL of 0.20 M Ba(OH)2 being titrated with 0.10 M HCl
d. 15 mL of 0.10 M HCl being titrated with 0.20 M NaOH
e. 30 mL of 0.10 M H2SO4 being titrated with 0.40 M NaOH
f. 60 mL of 0.10 M H3PO4 being titrated with 0.60 M NaOH
15. Identify the acid / base in the forward reaction
a. HCO3-1 (aq) + NH3 (aq)  CO3-2 (aq) + NH4+1 (aq)
b. HOCl (aq) + OH-1 (aq)  OCl-1 (aq) + H2O (l)
c. NH3 (aq) + KO(CH3)3 (aq)  NH2-1 (aq) + HO(CH3)3 (aq) + K+1 (aq)
16. Predict the products of the below reactions. The acid is listed first
a. HNO3 + OH- 
b. H2O + CH3NH2 
c. HPO4-2 + OH- 
d. HCl + NH3 
17. Given the H+ concentration, determine the OH- concentration (or vice versa)
a. 0.1 M H+
b. 1 x 10-5 M H+
c. 1 x 10-3 M H+
d. 1 x 10-9 M H+
e. 1 x 10-5 M OHf. 2 x 10-3 M OHg. 4 x 10-8 M OH18. Calculate the pH during the following titration after different amounts of acid have been
added. 50 mL of a 0.2 M NaOH solution is titrated with 0.4 M HCl solution. (Adding
Acid (HCl) to Base (NaOH).
a. 0 mL of acid has been added (what is the pH of the basic solution?)
b. 20 mL of acid has been added
c. 24 mL of acid has been added
d. 25 mL of acid has been added
e. 26 mL of acid has been added
19. Calculate the pH during the following titration after different amounts of base have been
added. 30 mL of a 0.3 M HBr solution is titrated with 0.1 M KOH solution. (Adding
Base (KOH) to Acid (HBr)
a. 0 mL of base has been added
b. 80 mL of base has been added
c. 89 mL of base has been added
d. 91 mL of base has been added
20. A 40 mL solution of 0.10 M HCl needs to be neutralized. How many grams of NaOH if
added to the solution would neutralize the solution?
21. How many mols of NaOH would be needed to neutralize the below acidic solutions?
a. 50 mL of 0.24 M HCl
b. 50 mL of 0.12 M H2SO4 which is a diprotic acid
c. 50 mL of 0.08 M H3PO4 which is a triprotic acic
22. Rainwater is naturally acidic. What molecules naturally and unnaturally (pollution) exist
in the air which makes rainwater acidic? Identify for one of the pollutants how it gets
into the air and what is being done to reduce the amount of pollution.