WorksheetsACIDS AND BASES
Total questions: 15
Worksheet time: 19mins
What is the pH of HF solution if its molar concentration of OH- = 6.45 x 10-13?
1.81
1.78
12.19
12.190
What is [H3O+] of HCOOH solution if [OH-] = 7.46 x 10 — 12?
1.34 x 10 —3 M
6.71 x 10 — 4 M
5.57 x 10 — 9 M
9.00 x 10 — 7 M
What is the [H3O+] if the pH of fruit juice is 4.25?
1.0 x 10 —14 M
5.62 x 10 —5 M
2.5 x 10 —4 M
5.6 x 10 —4 M
What is the pH of a hypochlorous acid if the molar concentration of [OH-] ions in the solution is 1.7 x 10-10?
4.23
7.46
8.46
9.77
Identify the Bronsted-Lowry acid reactant in the given reaction:
OCl- (aq) + H2O (l) ↔ HOCl (aq) + OH- (aq)
OCl-
H2O
HOCl
OH-
Identify the Bronsted-Lowry base reactant in the given equation:
H2SO4 (aq) + F- (aq) ↔ HSO4- (aq) + HF (aq)
H2SO4
F-
HSO4-
HF
Identify the Bronsted-Lowry acid in the given equation:
NH4+ (aq) + H2O (l) ↔ NH3 + H3O+ (aq)
NH4+
H2O
NH3
H3O+
Identify the conjugate base of HOCl
OCl
OCl-
OCl2-
OCl+
Which of the following is amphoteric species?
CN-
H2O
SO42-
CO2
What do we mean when we say strong acid?
an acid containing more than one acidic hydrogen.
a substance that can act as either an acid or base.
an acid that ionizes or dissociates completely when dissolved in water.
an acid that does not completely ionize when dissolved in water.
In terms of Arrhenius concept of acids and bases, how does an acid behave when dissolved in water?
any substance that can produce OH-
any substance that produces H+
any substance that can donate an H+ ion to another substance
any substance that can accept H+ ion from another substance
Identify the Bronsted-Lowry base reactant in the given equation:
HCN (aq) + H2O (l) ↔ H3O+ (aq) + CN- (aq)
HCN
H2O
H3O+
CN-
Identify the Bronsted-Lowry acid in the given equation
C6H5OH (aq) + NaOH (aq) ↔ H2O (l) + C6H5O- (aq) + Na+ (aq)
C6H5OH
NaOH
H2O
C6H5O
Which of the following is generally not included when writing an equilibrium constant expression?
Pure liquids
Pure solids
Both A and B
Neither A nor B
What is the pH of a 0.0025 M NaOH solution?
2.25
2.60
11.40
11.75
