Acids and Bases – Review Exercise
1.
DAY 1, TABLE 1
CLASS SET
Write the formula for zinc hydroxide, barium hydroxide, ammonia, ammonium, and copper
(II) hydroxide.
Zn(OH)2, Ba(OH)2, NH3, NH4+, Cu(OH)2
2.
Write the formula for chlorous acid, hydrochloric acid, perchloric acid, and acetic acid.
HClO2, HCl, HClO4, HC2H3O2
3.
The pH of a solution is 5.66. What is the [OH-]?
10−5.66 = [𝐻+ ] = 2.188 𝑥 10−6 ,
4.
𝐾𝑤 = [𝐻+ ][𝑂𝐻− ],
[𝑂𝐻 − ] = 4.57 𝑥 10−9
An unknown 1M solution is tested to determine its contents. A student places a drop of the
substance on blue litmus paper, red litmus paper, a piece of zinc metal, and then places the
leads of a conductivity meter (light) into the solution. Make a table of the results you
would expect if the solution were a strong acid, weak acid, strong base, basic salt, or a
neutral salt.
Blue Litmus Red Litmus Zn
Conduct?

Red
Red
H2 derived
Strong Acid

Red
Red
Small amount of H2 derived
Weak Acid

Blue
Blue
-Strong Base

Blue
Blue
-Basic Salt

Blue
Red
-Neutral Salt
Acids and Bases – Review Exercise
5.
DAY 1, TABLE 2
CLASS SET
What must be considered when choosing an indicator for a titration?
Endpoint pH of indicator vs. equivalence pH for titration.
6.
56.33mL of benzoic acid, a weak monoprotic acid, is titrated with 28mL of a
0.5M potassium hydroxide solution. Draw the titration curve. Label the
approximate equivalence point.
7.
A 0.55 M solution of HCl is titrated using 35.2 mL of 0.62 M Ca(OH)2. What
volume of the acid was used?
2HCl + 1Ca(OH)2  2H2O + 1CaCl2
Now with 87% more answer!
0.0352 𝐿 𝐶𝑎 𝑂𝐻 2 𝑥
0.62 𝑚𝑜𝑙 𝐶𝑎 𝑂𝐻 2
1 𝐿 𝐶𝑎 𝑂𝐻 2
𝑥
2 𝑚𝑜𝑙 𝐻𝐶𝑙
1 𝑚𝑜𝑙 𝐶𝑎 𝑂𝐻 2
𝑥
1 𝐿 𝐻𝐶𝑙
0.55 𝑚𝑜𝑙 𝐻𝐶𝑙
79 mL HCl
8.
List the formulas and names for the seven strong acids.
HCl - hydrochloric, HBr - hydrobromic, HI – hydroiodic, HClO4 – perchloric,
HClO3 – chloric, HNO3 – nitric, H2SO4 - sulfuric
9.
If [OH-] = 4.8 x 10-5 M for a solution, what is the pH of the solution?
− log 4.8 𝑥 10−5 = 4.32 = 𝑝𝑂𝐻,
𝑝𝐻 = 9.68
Acids and Bases – Review Exercise
10.
DAY 1, TABLE 3
CLASS SET
Given the solubility curve at right, calculate
the pH of a solution made by bubbling 85g of
gaseous HCl into 100g water at 60.°C.
60𝑔 𝑑𝑖𝑠𝑠𝑜𝑙𝑣𝑒𝑠.
60. 𝑔𝐻𝐶𝑙
1𝑚𝑜𝑙
−
𝑥
𝑥
= 16.46𝑀
−
36.458 𝑔 0.1𝐿
𝑝𝐻 = −1.22
When [H+] > 1.00, pH is negative! Fluoroantimonic
acid has a pH of –27!
11.
19.3mL of citric acid, a triprotic acid with the
formula H3C6H5O7, is titrated with 0.75M
lithium hydroxide. 23mL of the base were used
to reach equivalence. What was the
concentration of the acid?
0.30M
12.
Write three amphoteric substances. Write both
dissociation reactions for one of them.
Variable. Similar Q in practice.
13.
Strong acids are always concentrated. Defend
or refute this statement with evidence. Use 2
to 3 sentences.
Strong or weak acids can be concentrated or dilute. We can dilute any
strong acid with water, reducing concentration.