WorksheetsAcid and Bases Revision
Total questions: 12
Worksheet time: 21mins
Which one of the following represents a concentrated
solution of a weak acid?
6.0 M CH3COOH
0.01 M CH3COOH
6.0 M HCl
0.01 M HCl
Which one of the following can act as either a
Brønsted–Lowry acid or base in aqueous solutions?
HS–
NH4+
CO32–
CH4
Which of the following acids can be classified as
polyprotic in water?
I - CH3COOH
II - H2SO3
III - NH4+
I only
II only
I and II only
I, II and III
A solution of NaOH has a pH of 13 at 25ºC. What mass,
in g, of sodium hydroxide is present in 500 mL of this
solution?
2.0
0.050
2.0 x 10–12
4.0
Which one of the following is the conjugate base of
OH–?
H2O
O2–
H3O+
NaOH
Which reactions can be classified as acid–
base reactions?
2Mg(s) + O2(g) → 2MgO(s)
Ca(s) + 2H+(aq) → Ca2+(aq) + H2(g)
HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq)
2Br–(aq) + Cl2(aq) → Br2(aq) + 2Cl–(aq)
Define the terms 'strong' and 'weak' acid
HCO3– is an amphiprotic ion. Write chemical
equations to show it acting in water as:
i a base
ii an acid.
Calculate the OH- concentration when the concentration of HNO3 is 0.20M
2.0 x 10-13 M
5.0 x 10-14 M
6.0 x 10-11 M
0.50M
Calculate the H30+ concentration when a solution of HCl has a concentration of 0.75M
0.55M
0.60M
0.75M
6.0 x 10-12 M
Calculate the pH of each of 100 mL solution of 0.050 M Ca(OH)2
11.58
13
14
12.82
65.0 mL solution of hydrochloric acid that was
prepared by dissolving 2.45 g of hydrogen
chloride in water. Calculate its pH
1.23
5.87
0.0139
0.0987
