This document contains a chemistry worksheet with 20 multiple choice questions about acids and bases. The questions cover various acid-base chemistry concepts such as: calculating molarity from mass and volume of solutions, determining volumes and masses in chemical reactions involving acids and bases, and identifying products of acid-base reactions. The answers to each question are provided at the end.

1. Sekolah Menengah Kebangsaan St. Michael
Chemistry Form 4 – Acids and Bases
Drilling Exercise – Set 2
Objective Questions
1. When 2.0 g of sodium hydroxide are present in 500 cm
3
of its solution,what is its molarity?
[ Relative atomic mass : Na, 23 ; O, 16; H , 1 ]
A 0.001 moldm
-3
B 0.01 moldm
-3
C 0.1 moldm
-3
D 1.0 mol dm
-3
2. Calculate the number of moles of sulphuric acid in 100 cm
3
0.2 moldm
-3
of its solution ?
[ Relative atomic mass : H,1 ; S, 32 ; O, 16 ]
A 0.01 B 0.02 C 0.10 D 0.20
3. What is the concentration of hydroxide ions when 8.55 g of barium hydroxide is dissolved
in water to produce 250 cm
3
of solution ?
[ Relative atomic mass : Ba, 137 ; O, 16 ; H, 1 ]
A 0.01 B 0.05 C 0.20 D 0.40
4. 200 cm
3
of 0.5 moldm
-3
of hydrochloric acid was prepared from a standard solution of
2 moldm
-3
hydrochloric acid. Calculate the volume of the standard solution needed to be
dilute with acid ?
A 50 cm
3
B 75 cm
3
C 100 cm
3
D 150 cm
3
5. What is the mass of potassium hydroxide powder used to produce 100 cm
3
of 0.5 moldm
-3
potassium hydroxide solution ?
[ Relative atomic mass : O, 16; K, 39, H,1 ]
A 1.4 B 2.8 C 4.2 D 5.6
6 Calculate the volume of water needed to be added to 40 cm
3
of 2.0 moldm
-3
sulphuric acid
to obtain 80 cm
3
of 1 moldm
-3
sulphuric acid .
1

2. A 20 cm
3
B 40 cm
3
C 60 cm
3
D 80 cm
3
Questions 7 and 8 are based on the information below :
Zinc powder reacts with hydrochloric acid to produce zinc chloride and hydrogen gas,
according to the equation :
Zn(s) + 2 HCl(aq) → ZnCl2 (aq) + H2 (g)
7. Calculate the mass of zinc chloride that is formed when 1.3 g of zinc powder reacts with
excess hydrochloric acid.
[ Relative atomic mass : Zn, 65; Cl, 35.5 ]
A 1.36 B 2.72 C 3.48 D 6.72
8 Calculate the volume of the hydrogen gas released at room conditions when 1.3 g of zinc
powder reacts with excess hydrochloric acid.
[ Molar volume : 24 dm
3
mol
-1
at room conditions ]
A 120 cm
3
B 240 cm
3
C 360 cm
3
D 480 dm
3
9.
2 HNO3 + Ba(OH)2
→ Ba(NO3)2 + 2 H2O
25 cm
3
of 0.5 mol dm
-3
nitric acid reacts with 25 cm
3
of barium hydroxide solution. What is
the concentration of barium hydroxide solution ?
A 0.25 moldm
-3
B 0.5 moldm
-3
C 1.0 moldm
-3
D 2.0 moldm
-3
10.
H2SO4 + 2 LiOH → Li2SO4 + 2 H2O
50 cm
3
of 0.1 moldm
-3
sulphuric acid is neutralized by 100 cm
3
of lithium hydroxide solution.
What is the concentration of lithium hydroxide solution used in the reaction ?
A 0.005 moldm
-3
B 0.1 moldm
-3
C 0.2 moldm
-3
D 0.025 moldm
-3
11. Na2CO3 + 2 HCl → 2 NaCl + CO2 + H2O
Based on the equation above, what is the volume of gas released at room condition if
2

3. 25 cm
3
of 0.5 moldm
-3
hydrochloric acid reacts with sodium carbonate ?
[ Relative atomic mass : H, 1; C, 12; O, 16; Na,23; Cl 35.5; 1 mol of gas occupies 24dm
3
at
room condition ]
A 0.15 B 0.30 C 0.24 D 0.50
12. The equation below represents the reaction between hydrogen sulphide and nitric acid.
3 H2S + 2 HNO3
→ 3 S + 2 NO + 4 H2O
What is the mass of nitrogen monoxide gas released if 240 cm
3
of hydrogen sulphide gas
completely reacts with nitric acid at room condition ?
[ Relative atomic mass : N, 14; O, 16; 1 mol of gas occupies 24 dm
3
at room condition ]
A 0.2 B 0. 23 C 0.3 D 0.34
13. In the reaction below, 50 cm
3
of hydrochloric acid completely reacts with magnesium ribbon
to produce 120 cm
3
of hydrogen gas at room condition.
Mg + 2 HCl → Mg Cl2 + H2
What is the concentration of the hydrochloric acid used ?
[ 1 mol of gas occupies 24 dm
3
at room condition ]
A 0.005 B 0.01 C 0.1 D 0.2
14.
H2SO4 + Pb(NO3)2
→ PbSO4 + 2 HNO3
Calculate the volume of 0.2 moldm
-3
sulphuric acid, H2SO4 that is needed to react
completely with 10 cm
3
of 0.5 moldm
-3
of lead(II) nitrate, Pb(NO3)2 solution.
A 5 cm
3
B 10 cm
3
C 15 cm
3
D 25 cm
3
15. Calcium carbonate reacts with hydrochloric acid according to the chemical equation:
CaCO3 + 2 HCl → CaCl2 + CO2 + H2O
3

4. What is the mass of calcium carbonate that is required to produce 600 cm
3
of carbon
dioxide gas at room conditions when it reacts with excess hydrochloric acid ?
[ Relative atomic mass : Ca, 40; C, 12 , O, 16. Molar volume : 24 dm
3
mol
-1
at room
conditions ]
A 2.5 g B 3.5 g C 6.5 g D 25 g
16. 5 cm
3
of lead (II) nitrate solution requires 20 cm
3
of 0.3 moldm
-3
potassium iodide solution
to react completely according to the ionic equation below :
Pb
2+
(aq) + 2 I
-
(aq) → PbI2 (s)
What is the concentration of the lead(II) nitrate solution in moldm
-3
?
A 0.3 B 0.6 C 0.9 D 1.2
CuO + 2 HNO3
→ Cu(NO3)2 + H2O
17. Copper (II) oxide powder reacts with excess nitric acid to produre copper(II) nitrate and
water .If 11.28 g of copper(II) nitrate is formed, calculate the mass of copper (II) oxide
used in the reaction.
[ Relative atomic mass; Cu, 64; N, 14; O, 16 ]
A 2.4 g B 4.8 g C 6.0 g D 14.4 g
AgNO3 + KI → AgI + KNO3
18. Calculate the mass of silver iodide, AgI produced when 25 cm
3
of 1.5 moldm-
3
silver nitrate,
AgNO3 is mixed with 50 cm
3
of 0.5 moldm
-3
potassium iodide, KI solution.
[ Relative atomic mass : Ag ,108; I, 127 ]
A 2.5 g B 3.75 g C 5.875 g D 8.813 g
19. Nitric acid reacts with metal X to produce a salt according to the chemical equation below:
X + 2 HNO3
→ X ( NO3)2 + H2
Calculate the volume of 1.5 moldm
-3
nitric acid that is needed to completely react with
0.54 g of metal X.
4

5. [ Relative atomic mass : X, 24 ]
A 15 cm
3
B 20 cm
3
C 30 cm
3
D 45 cm
3
20. 10 cm
3
of 0.25 moldm
-3
T(OH)x solution is neutralized by 5 cm
3
of 1.0 moldm
-3
HxU solution.
The salt produced from the reaction is
A TU B T2U C TU2 D T3U2
Sekolah Menengah Kebangsaan St. Michael
Chemistry Form 4 – Acids and Bases
Drilling Exercise – Set 2
Answer :
1. C
2. B
3. D
4. A
5. B
6. B
7. B
8. D
9. A
10. B
11. A
12. A
13. D
14. D
15. A
16. B
17. B
5

6. 18. C
19. C
20. B
6

7. 18. C
19. C
20. B
6