Font size
WorksheetsCHM 101 Exam Practice Problems
Total questions: 20
Worksheet time: 33mins
1. The standard reduction potential of two half cell are: Zn++ + 2e- = Zn ; Eo = -0.76V 2Ag+ + 2e- = 2Ag Eo = +0.80V. The cell voltage for the electrochemical cell formed by connecting two half cell is ;
+0.04V
+1.56V
-2.36V
-1.50V
Hydrolysis is reverse of (a)
The ∆Eo for the reaction: Fe + Zn++ = Zn + Fe++ is -0.32. The equilibrium constant for the reaction is
1.4x10-11
2.8x10-11
1.5x10-4
1.8x10-12
If half reaction is multiplied by a positive number, its electrode potential:
Increases by two times
Increases by four times
Remains unchanged
Becomes half of its initial
In galvanic cell, which statement is not true?
Oxidation occurs at anode
Reduction occurs at cathode
Electrical energy produces the chemical reaction
Chemical reaction produces the electrical energy
Greater the reduction potential, greater is its tendency to be …………………and can be used as …… (a)
In the lead storage battery:
A reversible reaction can occur to recharge the battery
Lead is oxidized to create a flow of electrons
Lead forms the cathode when it is being reduced
All of the above
A concentration cell is constructed by placing identical Zn electrodes in two Zn2+ solutions. If the concentrations of the two Zn2+ solutions are 0.10 M and 0.00010 M, respectively, what is the potential of the cell?
+ 0.763 V
+ 0.089 V
+ 0.053 V
+ 0.24 V
Given the reaction: Pb(s) + Cu2+(aq) → Pb2+(aq) + Cu(s). What is the reducing agent?
Pb2+(aq)
Cu2+(aq)
Pb(s)
Cu(s)
In an electrolytic cell, the charge on the electrode that gives electrons to the species in solution is _____; the chemical change that occurs at this electrode is called _______.
(a)
Which of the following statements associated with corrosion is incorrect?
iron corrodes more readily than aluminium because iron is more active than aluminium
cathodic protection prevents corrosion by using a sacrificial anode
a corroding metal has both anodic and cathodic areas
corrosion involves both oxidation and reduction
The concentration of [H3O+] in the equilibrium with pure solution of NH4Cl whose chloride concentration is 0.1M, is [ Given, Kh = 5.6x10-10]
8.5x10-5M
1.2x10-6M
5.5x10-2M
7.5x10-6M
If the solubility of Ag2 CrO4 in pure water is 0.78 x 10-4 M then its solubility in 0.05 M AgNO3 is:
7.9 × 10-8 M
2.8 × 10-9 M
7.2 × 10-7 M
7.6 × 10-10 M
Which one of the following sets produces the precipitate of CaF2 (Ksp = 1.7x10-10), when equal volumes of followings are mixed?
10-4 M Ca2+ and 10-4 M F-
10-5 M Ca2+ and 10-3 M F-
10-2 M Ca2+ and 10-3 M F-
10-3 M Ca2+ and 10-5 M F-
Which of the following has pH above seven?
NH4Cl solution
NaCl solution
CuSO4 solution
CH3COONa solution
The pH of a buffer solution which contains 0.6 M NH4OH and 2 M NH4Cl is………… ………………. (Given, Kb for NH3 = 1.8x10-5)
(a)
The conjugate acid of the HPO4 - - is conjugate acid ……..
(a)
The best indicator for titrating HCl with NH4OH is
litmus
phenolphthalein
methyl orange
phenol red
All nucleophiles are
Arrhenius acid
Lowry-Bronsted bases
Lewis acids
Lewis bases
Weaker the acid, greater is the
ionic product
dissociation constant
hydrolysis constant
degree of ionization
