75 + Interview Questions in ELECTROLYSIS IN GENERAL AWARENESS Page 2 InterviewSolution

51.	Write down the words or phrases from the brackets that will correctly fill in the blanks in the following sentences:(a) Pure water consists entirely of ________________ (ions/ molecules).(b) We can expect that pure water ________________ (will / will not) normally conduct electricity.
Answer» (a) Molecules (b) Will not

51.

Write down the words or phrases from the brackets that will correctly fill in the blanks in the following sentences:(a) Pure water consists entirely of (ions/ molecules).(b) We can expect that pure water (will / will not) normally conduct electricity.

Answer»

(a) Molecules

(b) Will not

Discussion

52.	Select the correct answer from the list in brackets:1. An aqueous electrolyte consists of the ions. mentioned in the list, the ion which could be discharged most readily during electrolysis.[Fe2+ , Cu2+ , Pb2+ , H+].2. The metallic electrode which does not take part in an electrolytic reaction.[Cu, Ag, Pt, Ni].3. The ion which is discharged at the anode during the electrolysis of copper sulphate solutions using copper electrodes as anode and cathode.[Cu2+ , OH– , SO42- -, H+].4. When dilute sodium chloride is electrolysed using graphite electrodes, the cation is discharged at the cathode most readily.[Na+ , OH– , H+ , Cl–].5. During silver plating of an article using potassium argentocyanide as an electrolyte, the anode material should be [Cu, Ag, Pt, Fe].
Answer» (1) Cu²⁺ (2) Pt (3) Cu²⁺ (4) H¹⁺ (5) Ag

52.

Select the correct answer from the list in brackets:1. An aqueous electrolyte consists of the ions. mentioned in the list, the ion which could be discharged most readily during electrolysis.[Fe2+ , Cu2+ , Pb2+ , H+].2. The metallic electrode which does not take part in an electrolytic reaction.[Cu, Ag, Pt, Ni].3. The ion which is discharged at the anode during the electrolysis of copper sulphate solutions using copper electrodes as anode and cathode.[Cu2+ , OH– , SO42- -, H+].4. When dilute sodium chloride is electrolysed using graphite electrodes, the cation is discharged at the cathode most readily.[Na+ , OH– , H+ , Cl–].5. During silver plating of an article using potassium argentocyanide as an electrolyte, the anode material should be [Cu, Ag, Pt, Fe].

Answer»

(1) Cu²⁺

(2) Pt

(3) Cu²⁺

(4) H¹⁺

(5) Ag

Discussion

53.	State which from A to E fits the description ‘A pink metal is deposited at the cathode during the electrolysis of the soln. of this salt. (A) Sulphur(B) Silver chloride(C) Hydrogen chloride(D) Copper [II] sulphate(E) Graphite.
Answer» (D) Copper [II] sulphate

53.

State which from A to E fits the description ‘A pink metal is deposited at the cathode during the electrolysis of the soln. of this salt. (A) Sulphur(B) Silver chloride(C) Hydrogen chloride(D) Copper [II] sulphate(E) Graphite.

Answer»

(D) Copper [II] sulphate

Discussion

54.	A, B and C are three electrolytic cells, connected in different circuits. Cell ‘A’ contains NaCl soln., and the bulb in the circuit glows brightly, when the circuit is completed. Cell ‘B’ contains acetic acid and the bulb glows dimly. Cell ‘C’ contains sugar soln., and the bulb not glow. Give reasons for each observation.
Answer» Electrolytic cell A has completely ionised sodium chloride solution. Thus, the ions can easily migrate to oppositely charged poles and hence bulb glows brightly. To conclude sodium chloride solution is a strong electrolyte. Electrolytic cell B has a weak electrolyte as only 5% of the acetic acid molecules ionise. Thus, a weak current flows through it and hence the bulb glows dimly. Electrolytic cell C has a non-electrolyte. Sugar molecules do not ionise and hence no current flows through. Thus, the bulb does not glow.

54.

A, B and C are three electrolytic cells, connected in different circuits. Cell ‘A’ contains NaCl soln., and the bulb in the circuit glows brightly, when the circuit is completed. Cell ‘B’ contains acetic acid and the bulb glows dimly. Cell ‘C’ contains sugar soln., and the bulb not glow. Give reasons for each observation.

Answer»

Electrolytic cell A has completely ionised sodium chloride solution. Thus, the ions can easily migrate to oppositely charged poles and hence bulb glows brightly. To conclude sodium chloride solution is a strong electrolyte.

Electrolytic cell B has a weak electrolyte as only 5% of the acetic acid molecules ionise. Thus, a weak current flows through it and hence the bulb glows dimly.

Electrolytic cell C has a non-electrolyte. Sugar molecules do not ionise and hence no current flows through. Thus, the bulb does not glow.

Discussion

55.	Mr. Ramu wants to electroplate his key chain with nickel to prevent rusting. For this electroplating :(i) Name the electrolyte(ii) Name the cathode(iii) Name the anode(iv) Give the reaction at the cathode(v) Give the reaction at the anode.
Answer» (i) Nickel sulphate (ii) Key chain (iii) Pure nickel plate (iv) Ni²⁺ + 2e^– ⟶ Ni (v) Ni – 2^e– ⟶ Ni²⁺

55.

Mr. Ramu wants to electroplate his key chain with nickel to prevent rusting. For this electroplating :(i) Name the electrolyte(ii) Name the cathode(iii) Name the anode(iv) Give the reaction at the cathode(v) Give the reaction at the anode.

Answer»

(i) Nickel sulphate

(ii) Key chain

(iii) Pure nickel plate

(iv) Ni²⁺ + 2e^– ⟶ Ni

(v) Ni – 2^e– ⟶ Ni²⁺

Discussion

56.	Copper sulphate solution is electrolysed using copper electrodes. Study the diagram given below and answer the question that follows:(i) Which electrode to your left or right is known as the oxidising electrode and why ? (ii) Write the equation representing the reaction that occurs.(iii) State two appropriate observations for the above electrolysis reaction.
Answer» (i) Electrode on the left side is the oxidising electrode because copper atoms lose electrons at this electrode. (ii) Cu – 2e^– ⟶ Cu²⁺ (iii) Reddish brown copper metal is deposited at cathode and blue colour of aqueous copper (II) Sulphate solution remains unchanged.

56.

Copper sulphate solution is electrolysed using copper electrodes. Study the diagram given below and answer the question that follows:(i) Which electrode to your left or right is known as the oxidising electrode and why ? (ii) Write the equation representing the reaction that occurs.(iii) State two appropriate observations for the above electrolysis reaction.

Answer»

(i) Electrode on the left side is the oxidising electrode because copper atoms lose electrons at this electrode.

(ii) Cu – 2e^– ⟶ Cu²⁺

(iii) Reddish brown copper metal is deposited at cathode and blue colour of aqueous copper (II) Sulphate solution remains unchanged.

Discussion

57.	Three different electrolytic cells A, B and C are connected in separate circuits. Electrolytic cell A contains sodium chloride solution. When the circuit is completed a bulb in the circuit glows brightly. Electrolytic cell B contains acetic acid solution and in this case the bulb in the circuit glows dimly. The electrolytic cell C contains sugar solution and the bulb does not glow. Give a reason for each of these observations.
Answer» In Cell A : Sodium chloride being strong electrolyte dissociates completely and therefore current flows better. In Cell B : Acetic acid being weak electrolyte ionises only partially and therefore, only a weak current flows. In Cell C : Sugar being a covalent compound does not ionise at all and therefore, no current flows.

57.

Three different electrolytic cells A, B and C are connected in separate circuits. Electrolytic cell A contains sodium chloride solution. When the circuit is completed a bulb in the circuit glows brightly. Electrolytic cell B contains acetic acid solution and in this case the bulb in the circuit glows dimly. The electrolytic cell C contains sugar solution and the bulb does not glow. Give a reason for each of these observations.

Answer»

In Cell

A : Sodium chloride being strong electrolyte dissociates completely and therefore current flows better. In Cell

B : Acetic acid being weak electrolyte ionises only partially and therefore, only a weak current flows. In Cell

C : Sugar being a covalent compound does not ionise at all and therefore, no current flows.

Discussion

58.	During electroplating of an article with nickel – (1) Name1. The electrolyte2. The cathode(2) Give the reaction of the electrolysis at1. The cathode .2. The anode
Answer» (1) (a) Nickel sulphate (b) Article (c) Pure nickel plate / rod (2) (a) At Cathode: Ni²⁺ + 2e^–→ Ni(s) (b) At Anode: Ni(s) – 2e^–→ Ni²⁺

58.

During electroplating of an article with nickel – (1) Name1. The electrolyte2. The cathode(2) Give the reaction of the electrolysis at1. The cathode .2. The anode

Answer»

(1) (a) Nickel sulphate

(b) Article

(c) Pure nickel plate / rod

(2) (a) At Cathode: Ni²⁺ + 2e^–→ Ni(s)

(b) At Anode: Ni(s) – 2e^–→ Ni²⁺

Discussion

59.	A soln. of AgNO3 is a good electrolyte but it is not used for electroplating an article with silver. Why.
Answer» Migration of Ag¹⁺ ion from the complex salt solution silver cyanide is slow as compared to silver nitrate. That is why silver nitrate solution is not used.

Discussion

60.

What is the difference between:(a) Modern explanation and Arrhenius explanation for the theory of electrolysis:(b) electrolytic dissociation and ionization :(c) A cation and an anion,

Answer»

(a) Difference between Modern explanation and Arrhenius explanation for the theory of electrolysis: Arrhenius considered that water ionizes electrolytes but Modern theory explained that electrolytes are ionic even in solid state and their ions are held by strong electrostatic forces which make them immobile. Water renders these ions mobility by breaking the electrostatic forces.

(b) Difference between electrolytic dissociation and ionization :

Ionization	Dissociation
1. Formation of positively or negatively charged ions from molecules which are not initially in the ionic state.	1. Separation of ions which are already present in an ionic compound.
2. Polar covalent compounds show ionization. e.g. HCl, H₂CO₃, NH₄OH etc.	2. Electrovalent compounds show dissociation. e.g. Potassium chloride, lead bromide, etc.

(c) A cation and anion:

Cation	Anion
1. Are positively charged ions.	1. Are negatively charged ions.
2. Migrate to cathode during electrolysis.	2. Migrate to anode during electrolysis.
3. Gain electron from the cathode and get reduced to become a neutral atom.	3. Lose electrons to the anode and get oxidized to become a neutral atom.

(d) Electrolytic dissociation and thermal dissociation: Electrolytic dissociation is the dissociation of an electrovalent compound into ions in the fused state or in aqueous solution state. Thermal dissociation: Reversible breakdown of a chemical compound into simpler substances by heating it. The splitting of ammonium chloride into ammonia and hydrogen chloride is an example. On cooling, they recombine to form the salt.

Discussion

61.	Write equations to show the electrolytic dissociation of :(a) Two acids(b) Two bases.
Answer» (a) Acids: H₂SO₄ ⇌ 2H+ + SO₄^2- HNO₃ ⇌ H⁺ + NO₃ ^– (b) Bases: NaOH ⇌ Na⁺ + OH^– KOH ⇌ K+ + OH^–

61.

Write equations to show the electrolytic dissociation of :(a) Two acids(b) Two bases.

Answer»

(a) Acids:

H₂SO₄ ⇌ 2H+ + SO₄^2-

HNO₃ ⇌ H⁺ + NO₃ ^–

(b) Bases:

NaOH ⇌ Na⁺ + OH^–

KOH ⇌ K+ + OH^–

Discussion

62.	Electrolysis is a redox process. Explain.
Answer» Electrolysis is a redox process. The reaction at the cathode involves reduction of cations as they gain of electrons while the reaction at anode involves oxidation of anions as they loss of electrons to become neutral. Example: Dissociation of sodium chloride during electrolysis. NaCl ⇌ Na⁺ + Cl^- Cathode : Na⁺ + e^-⟶ Na (reduction) Cl^- − e^- ⟶ Cl(oxidation) Cl + Cl ⟶ Cl₂ Overall reaction : 2NaCl ⟶ 2Na + Cl₂

62.

Electrolysis is a redox process. Explain.

Answer»

Electrolysis is a redox process. The reaction at the cathode involves reduction of cations as they gain of electrons while the reaction at anode involves oxidation of anions as they loss of electrons to become neutral.

Example: Dissociation of sodium chloride during electrolysis.

NaCl ⇌ Na⁺ + Cl^-

Cathode : Na⁺ + e^-⟶ Na (reduction)

Cl^- − e^- ⟶ Cl(oxidation)

Cl + Cl ⟶ Cl₂

Overall reaction : 2NaCl ⟶ 2Na + Cl₂

Discussion

63.	Name two substances in each case:(a) Contain only molecules,(b) Contain only ions,(c) Contain ions as well as molecules.
Answer» (a) Glucose, Kerosene (b) NaCl and NaOH (c) CH₃COOH and NH₄OH

63.

Name two substances in each case:(a) Contain only molecules,(b) Contain only ions,(c) Contain ions as well as molecules.

Answer»

(a) Glucose, Kerosene

(b) NaCl and NaOH

(c) CH₃COOH and NH₄OH

Discussion

64.	Write two applications of electrolysis in which the anode diminishes in mass.
Answer» 1. Used in electroplating. 2. Purification of metals.

64.

Write two applications of electrolysis in which the anode diminishes in mass.

Answer»

1. Used in electroplating.

2. Purification of metals.

Discussion

65.	Select the ion in each case, that would get selectively discharged from the aqueous mixture of the ions listed below:(1) SO42- , NO–3 and OH– ;(2) Pb2- , Ag+ and Cu2+ .
Answer» 1. OH ion will get discharged in preference to SO₄^2- or NO₃^– ions. 2. Ag⁺ ions will get discharged in preference to Pb²⁺ or Cu²⁺ ions

65.

Select the ion in each case, that would get selectively discharged from the aqueous mixture of the ions listed below:(1) SO42- , NO–3 and OH– ;(2) Pb2- , Ag+ and Cu2+ .

Answer»

1. OH ion will get discharged in preference to SO₄^2- or NO₃^– ions.

2. Ag⁺ ions will get discharged in preference to Pb²⁺ or Cu²⁺ ions

Discussion

66.	State the observations at the anode & at the cathode during the electrolysis of –1. Fused lead bromide using graphite electrodes.2. Copper sulphate solution using copper electrodes.
Answer» 1. At cathode silvery droplets of molten lead appear. At anode reddish vapours of bromine are given out. 2. Brown metal copper is deposited at cathode. Cu²⁺ ion is liberated at anode. Colour of CuSO₄ solution (blue colour) does not fade.

66.

State the observations at the anode & at the cathode during the electrolysis of –1. Fused lead bromide using graphite electrodes.2. Copper sulphate solution using copper electrodes.

Answer»

1. At cathode silvery droplets of molten lead appear. At anode reddish vapours of bromine are given out.

2. Brown metal copper is deposited at cathode. Cu²⁺ ion is liberated at anode. Colour of CuSO₄ solution (blue colour) does not fade.

Discussion

67.	Write equations for the reactions taking place at cathode and at anode during the electrolysis of :1. Acidified nickel sulphate solution with nickel electrode2. Acidified copper sulphate solution with copper electrode.3. Acidified copper sulphate solution with platinum electrode.4. Acidulated water with inert electrode.5. Molten lead bromide with inert electrodes.6. Electroplating a spoon with silver.
Answer» 1. Cathode : Ni²⁺ + 2e^- → Ni Anode : Ni - 2e^- → Ni²⁺ 2. Cathode : Cu²⁺ + 2e^- → Cu Anode : Cu - 2e^- → Cu²⁺ 3. Cathode : Cu²⁺ + 2e^- → Cu Anode : OH^- - e^-→OH 4OH^- → 2H₂O + H₂ 4. Cathode : H⁺ + e^- → [H] 2[H] → H₂ OH^- - e^- → OH Anode : 4OH → 2H₂O + O₂ 5. Cathode : Pb²⁺ + 2e^- → Pb Anode : 2Br^- - 2e^- → 2 [Br] 2 [Br] → Br₂ 6. Cathode : AgNO₃→ Ag⁺+ NO₃^- Ag⁺ + e^- → Ag Anode : NO^-₃ - e^- → NO₃ Ag + NO₃ → AgNO₃

67.

Write equations for the reactions taking place at cathode and at anode during the electrolysis of :1. Acidified nickel sulphate solution with nickel electrode2. Acidified copper sulphate solution with copper electrode.3. Acidified copper sulphate solution with platinum electrode.4. Acidulated water with inert electrode.5. Molten lead bromide with inert electrodes.6. Electroplating a spoon with silver.

Answer»

1. Cathode : Ni²⁺ + 2e^- → Ni

Anode : Ni - 2e^- → Ni²⁺

2. Cathode : Cu²⁺ + 2e^- → Cu

Anode : Cu - 2e^- → Cu²⁺

3. Cathode : Cu²⁺ + 2e^- → Cu

Anode : OH^- - e^-→OH

4OH^- → 2H₂O + H₂

4. Cathode : H⁺ + e^- → [H]

2[H] → H₂

OH^- - e^- → OH

Anode : 4OH → 2H₂O + O₂

5. Cathode : Pb²⁺ + 2e^- → Pb

Anode : 2Br^- - 2e^- → 2 [Br]

2 [Br] → Br₂

6. Cathode : AgNO₃→ Ag⁺+ NO₃^-

Ag⁺ + e^- → Ag

Anode : NO^-₃ - e^- → NO₃

Ag + NO₃ → AgNO₃

Discussion

68.	Identify the substance underlined, in each of the following1. The elctrolvte used for electroplating an article with silver.2. The particles present in a liquid such as kerosene, that is a non-electrolyte.
Answer» 1. Sodium argentocyanide or Potassium argentocyanide solution. 2. Molecules

68.

Identify the substance underlined, in each of the following1. The elctrolvte used for electroplating an article with silver.2. The particles present in a liquid such as kerosene, that is a non-electrolyte.

Answer»

1. Sodium argentocyanide or Potassium argentocyanide solution.

2. Molecules

Discussion

69.	How is it possible to discharge Na+ ions in preference to H+ ions in electrolysis of NaCl solution ?
Answer» By using cathode made of moving mercury, Na⁺ ions are discharged in preference to H⁺ ions because of the nature of electrode. Mercury has strong tendency to form an amalgam with : sodium Na⁺ + e^– ⟶ Na Na + Hg ⟶ Na/Hg When the sodium amalgam dissolves in water, the reaction is 2Na/Hg + 2H₂O ⟶ 2NaOH + H₂ + Hg

69.

How is it possible to discharge Na+ ions in preference to H+ ions in electrolysis of NaCl solution ?

Answer»

By using cathode made of moving mercury, Na⁺ ions are discharged in preference to H⁺ ions because of the nature of electrode. Mercury has strong tendency to form an amalgam with : sodium

Na⁺ + e^– ⟶ Na

Na + Hg ⟶ Na/Hg

When the sodium amalgam dissolves in water, the reaction is

2Na/Hg + 2H₂O ⟶ 2NaOH + H₂ + Hg

Discussion

70.	Select from the list:Ammonia, Copper oxide, Copper sulphate, Hydrogen chloride, Hydrogen sulphide, Lead bromide.1. A solution of this compound is used as the electrolyte when copper is purified.2. When this compound is electrolysed in the molten state, lead is obtained at the cathode.
Answer» 1. Copper sulphate 2. Lead Bromide.

70.

Select from the list:Ammonia, Copper oxide, Copper sulphate, Hydrogen chloride, Hydrogen sulphide, Lead bromide.1. A solution of this compound is used as the electrolyte when copper is purified.2. When this compound is electrolysed in the molten state, lead is obtained at the cathode.

Answer»

1. Copper sulphate

2. Lead Bromide.

Discussion

71.	A certain metal, say M, does not liberate hydrogen from dilute sulphuric acid, but displaces copper from aqueous copper (II) sulphate. State the most likely place for the metal in electrochemical series.
Answer» The activity series is obtained, when we examine replacement of one metal ion from its solution by another metal. The metal (M) which displaces copper from aqueous copper (II) sulphate is placed at higher position as compared to copper in activity series.

Discussion

72.	M2O is the oxide of a metal ‘M’ which is the above hydrogen in the activity series. M2O when dissolved in water forms the corresponding hydroxide which-is a good conductor of electricity.1. State the reaction taking place at the cathode.2. Name the product at the anode.
Answer» 1. Reaction of cathode: M⁺ + e → M 2. Product at anode: O₂ + O^2-→ O₂ (Oxygen)

72.

M2O is the oxide of a metal ‘M’ which is the above hydrogen in the activity series. M2O when dissolved in water forms the corresponding hydroxide which-is a good conductor of electricity.1. State the reaction taking place at the cathode.2. Name the product at the anode.

Answer»

1. Reaction of cathode: M⁺ + e → M

2. Product at anode: O₂ + O^2-→ O₂ (Oxygen)

Discussion

73.	M is a metal above hydrogen in the activity series and its oxide has the formula M2O. This oxide when dissolved in water forms the corresponding hydroxide which is a good conductor of electricity. In the above context answer the following:(i) What kind of combination exists between M and O ?(ii) How many electrons are there in the outermost shell of M ?(iii) Name the group to which M belongs. (iv) State the reaction taking place at the cathode.(v) Name the product at the anode
Answer» (i) Electrovalent bond exists between M and O. (ii) One electron is there in the outermost shell. (iii) M belongs to First group. (iv) M⁺ + e^– ⟶ M (at cathode). M + M ⟶ M₂ (v) Oxygen gas is liberated at anode.

73.

M is a metal above hydrogen in the activity series and its oxide has the formula M2O. This oxide when dissolved in water forms the corresponding hydroxide which is a good conductor of electricity. In the above context answer the following:(i) What kind of combination exists between M and O ?(ii) How many electrons are there in the outermost shell of M ?(iii) Name the group to which M belongs. (iv) State the reaction taking place at the cathode.(v) Name the product at the anode

Answer»

(i) Electrovalent bond exists between M and O.

(ii) One electron is there in the outermost shell.

(iii) M belongs to First group.

(iv) M⁺ + e^– ⟶ M (at cathode).

M + M ⟶ M₂

(v) Oxygen gas is liberated at anode.

Discussion

74.	Hydroxyl (OH– ) ion is lower in the activity series, than chloride ion. Yet when a concentrated solution of hydrochloric acid is subjected to electrolysis, the hydroxyl ion does not get discharged.
Answer» If an electrolyte has a much higher concentration of ions that are higher in the electrochemical series than those that are lower, then the higher gets discharged in preference to the lower one. Concentrated hydrochloric acid being strong electrolyte gets fully dissociated furnishing H⁺ and Cl^– ion. Water is less dissociated into H⁺ and OH^– ion. Thus, concentration of chloride ion is more as compared to OH^– ion and hence, chloride ion are discharged in preference to the OH^– ion

Discussion

75.	A strip of copper is placed in four different colourless salt solutions. They are KNO3 , AgNO3 , Zn(NO3)2 , Ca(NO3)2 . Which one of the solutions will finally turn blue ?
Answer» AgNO₃ solution .

Discussion

Explore topic-wise InterviewSolutions in .

Write down the words or phrases from the brackets that will correctly fill in the blanks in the following sentences:(a) Pure water consists entirely of ________________ (ions/ molecules).(b) We can expect that pure water ________________ (will / will not) normally conduct electricity.

State which from A to E fits the description ‘A pink metal is deposited at the cathode during the electrolysis of the soln. of this salt. (A) Sulphur(B) Silver chloride(C) Hydrogen chloride(D) Copper [II] sulphate(E) Graphite.

Mr. Ramu wants to electroplate his key chain with nickel to prevent rusting. For this electroplating :(i) Name the electrolyte(ii) Name the cathode(iii) Name the anode(iv) Give the reaction at the cathode(v) Give the reaction at the anode.

During electroplating of an article with nickel – (1) Name1. The electrolyte2. The cathode(2) Give the reaction of the electrolysis at1. The cathode .2. The anode

A soln. of AgNO3 is a good electrolyte but it is not used for electroplating an article with silver. Why.

What is the difference between:(a) Modern explanation and Arrhenius explanation for the theory of electrolysis:(b) electrolytic dissociation and ionization :(c) A cation and an anion,

Write equations to show the electrolytic dissociation of :(a) Two acids(b) Two bases.

Electrolysis is a redox process. Explain.

Name two substances in each case:(a) Contain only molecules,(b) Contain only ions,(c) Contain ions as well as molecules.

Write two applications of electrolysis in which the anode diminishes in mass.

Select the ion in each case, that would get selectively discharged from the aqueous mixture of the ions listed below:(1) SO42- , NO–3 and OH– ;(2) Pb2- , Ag+ and Cu2+ .

State the observations at the anode &amp; at the cathode during the electrolysis of –1. Fused lead bromide using graphite electrodes.2. Copper sulphate solution using copper electrodes.

Identify the substance underlined, in each of the following1. The elctrolvte used for electroplating an article with silver.2. The particles present in a liquid such as kerosene, that is a non-electrolyte.

How is it possible to discharge Na+ ions in preference to H+ ions in electrolysis of NaCl solution ?

Select from the list:Ammonia, Copper oxide, Copper sulphate, Hydrogen chloride, Hydrogen sulphide, Lead bromide.1. A solution of this compound is used as the electrolyte when copper is purified.2. When this compound is electrolysed in the molten state, lead is obtained at the cathode.

A certain metal, say M, does not liberate hydrogen from dilute sulphuric acid, but displaces copper from aqueous copper (II) sulphate. State the most likely place for the metal in electrochemical series.

M2O is the oxide of a metal ‘M’ which is the above hydrogen in the activity series. M2O when dissolved in water forms the corresponding hydroxide which-is a good conductor of electricity.1. State the reaction taking place at the cathode.2. Name the product at the anode.

Hydroxyl (OH– ) ion is lower in the activity series, than chloride ion. Yet when a concentrated solution of hydrochloric acid is subjected to electrolysis, the hydroxyl ion does not get discharged.

A strip of copper is placed in four different colourless salt solutions. They are KNO3 , AgNO3 , Zn(NO3)2 , Ca(NO3)2 . Which one of the solutions will finally turn blue ?

Write down the words or phrases from the brackets that will correctly fill in the blanks in the following sentences:(a) Pure water consists entirely of (ions/ molecules).(b) We can expect that pure water (will / will not) normally conduct electricity.

State the observations at the anode & at the cathode during the electrolysis of –1. Fused lead bromide using graphite electrodes.2. Copper sulphate solution using copper electrodes.