ONLINE TEST - Electrochemistry – I - EM

This Quiz is a Simple test for +2 Science group students which contain Questions asked from March - 2006 to Sept - 2016 in Electrochemistry – I. Just participate in it and test your skill.

1. Equivalent conductance of acetic acid at 25°C is 80 ohm^–1 cm² (gram equivalent)^–1 and at infinite dilution is 400 ohm^–1cm² (gram equivalent)^–1. The degree of dissociation is
1
0.2
0.1
0.3


2. Faraday's laws of electrolysis are related to
atomic number of the cation
atomic number of the anion
equivalent weight of the electrolyte
speed of the cation


3. The indicator suitable for the titration of oxalic acid against NaOH is
potassium permanganate
phenolphthalein
litmus
methyl orange


4. If 0.2 ampere can deposit 0.1978 g of copper in 50 minutes, how much of copper will be deposited by 600 coulombs?
19.78 g
1.978 g
0.1978 g
197.8 g


5. Ostwald’s dilution law is applicable to the solution of
CH3COOH
NaCl
NaOH
H2SO4


6. The Indicator used in the titration of ammonium hydroxide with hydrochloric acid is
KMnO4
Methyl orange
Phenolphthalein
Litmus


7. The pH of a solution containing 0.1N NaOH solution is
1
10–1
13
10–13


8. When 10^–6 mole of a monobasic strong acid is dissolved in 1 litre of solvent, the pH of the sol
6
7
4
less than 7


9. When one coulomb of electricity is passed through an electrolytic solution, the mass deposited on the electrode is equal to
equivalent weight
molecular weight
electrochemical equivalent
one gram


10. When pH of a solution is 2, the hydrogen ion concentration in moles litre^–l is
1 x 10–12
1 x 10–4
1 x 10–7
1 x 10–2


11. When sodium acetate is added to (a solution of) acetic acid, the degree of ionisation of acetic acid
increases
decreases
does not change
becomes zero


12. A solution which is resistant to changes of pH on addition of small amounts of an acid or a ba
buffer solution
true solution
isohydric solution
ideal solution


13. Indicators used in acid-base titrations are _______
strong organic acids
strong organic bases
weak organic acids or weak organic bases
non-electrolysis


14. NH4OH is a weak base because _______
it has low vapour pressure
it is only partially ionised
it is completely ionised
it has low density


15. The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salt is given by
[H+] = Ka[Salt]/[ Acid ]
[H+] = Ka[Salt]
[H+] = Ka[Acid]
[H+] = Ka[Salt]/[Acid]


16. The laws of electrolysis were enunciated first by ______
Dalton
Faraday
Kekule
Avogadro


17. The process in which chemical change occurs on passing electricity is termed as _______
neutralization
hydrolysis
electrolysis
ionisation


18. The specific conductance of a 0.01 M solution of KCl is 0.0014 ohm–1 cm–1 at 25^oC. Its equivalent conductance is ______
14 ohm–1 cm2 eq–1
140 ohm–1 cm2 eq–1
1.4 ohm–1 cm2 eq–1
0.14 ohm–1 cm2 eq–1


19. Which one of the following formulae represents Ostwald’s dilution law for a binary electrolyte whose degree of dissociation is α and concentration C?
K = (1– α)C/α
K = α2C/ 1–α
K = (1– α)C/α2
K = α2C/ (1–α)C


20. Which one of the following relationship is correct?
pH =1 / [H+]
pH = log10 [H+]
log10 pH = [H+]
pH = log10 1 / [H+]


21. The value of enthalpy of neutralisation of strong acid by strong base is
– 87.32 kJ equiv– 1
– 57.32 kJ equiv– 1
– 72.57 kJ equiv– 1
– 77.23 kJ equiv– 1


22. For the titration between HCl and sodium carbonate the indicator used is
potassium permanganate
phenolphthalein
litmus
methyl orange


23. The number of moles of electrons required to discharge one mole of Al+3 is
3
1
2
4


24. pH range of phenol red is
6.8 – 8.4
4.4 – 6.2
3.1 – 4.4
8.3 – 10

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