Class 10 FRANK Solutions Chemistry Chapter 6: Electrolysis

Improve your Chemistry skills with our Frank Solutions for ICSE Class 10 Chemistry Chapter 6 Electrolysis. Go through the definitions of cation, electro metallurgy, anion, electrolysis, electrolyte and non-electrolyte. Revise the steps to explain the purification of impure copper using the electrolysis method. Also, revisit the various applications of electrolysis.

In addition, relearn equations for reactions which occur during the electrolysis of lead bromide with our ICSE Class 10 Chemistry Frank Solutions. To learn further about electrolysis, practise TopperLearning’s Selina Solutions, sample question paper solutions etc.

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Electrolysis Exercise 145

Solution 1

Solution 2

Solution 3

Solution 4

Solution 5

Solution 6

Solution 7

Solution 8

Solution 9

Electrolysis Exercise 146

Solution 10

Solution 11

Solution 12

Solution 13

Solution 14

Solution 15

Solution 16

Solution 17

Solution 18

Solution 19

Solution 20

Solution 21

(i) CuSO₄

(ii) Au³⁺

(iii) OH^⁻

(iv) Graphite rod

(v) Hydrogen and oxygen

Electrolysis Exercise 147

Solution 1994-1

(a) The article to be plated must be made Cathode.
(b) The ions of the metal which is to be electroplated must be present in the electrolyte.
(c) The metal to be plated on the article must be made anode. It needs to be periodically replaced.

Solution 1994-2

The passage of electricity through an electrolyte occurs through ions furnished by the electrolyte where as the passage of electricity through a copper wire occurs through electrons.

Solution 1995-1

Solution 1995-2

It is the process of decomposition of an electrolyte in the molten or aqueous state by discharge of ions at the electrodes on the passage of an electric current.

Solution 1995-3

Pure water does not conduct electricity because the degree of ionization is low. Thus to make it a good conductor of electricity acid is added to it which will increase the degree of ionization.

Solution 1996-1

Substance which contain
(i) Ions only:- HCl
(ii) Molecules only:- Petrol
(iii) Both ions and molecules:- CH₃COOH

Solution 1996-2

(a) Electrolyte is a compound which either in aqueous solution or in molten state allows an electric current to pass through it and is accompanied by discharge of ions and finally into neutral atoms at the two electrodes.
(b) Non- electrolyte are substances which do not conduct electricity in fused or aqueous state. They contain only molecules and do not ionize. For example: petrol, alcohol.
(c) If the electrolyte is described as 'strong electrolyte' it means it completely dissociates into its constituting ions in aqueous solution.

Solution 1996-3

(a) As for every copper ion discharged at the cathode, an ion of copper is formed at the anode which goes into the solution .Since atoms of copper are deposited at the cathode, the cathode becomesthicker and as the atoms of copper from the anode change into ions of copper, the anode becomes thinner.
(b) When platinum rods are used as electrodes, then x the blue colour of copper sulphate solution fades and sulphuric acid is formed. This is because oxygen is liberated at anode and copper metal is deposited at cathode
(c) Practical application of electrolysis of copper sulphate solution: This is the basis for purification of copper.
Other metals like Zinc, Nickel, Silver .Lead can also be purified.

Electrolysis Exercise 148

Solution 1997-1

Lead Bromide should be in the molten state if it has to conduct electricity.

Solution 1997-2

Solution 1997-3

Solution 1998-1

(a) Electrolyte
(b) Nickel
(c) cathode
(d) anode
(e) Cations

Solution 1999-1

The electrolysis of lead bromide liberates lead at cathode and bromine at anode.

Solution 1999-2

When a fused metallic chloride is electrolyzed, the metal is obtained at cathode.

Solution 2000-1

(a) Strong electrolytes - dilute hydrochloric acid, dilute sulphuric acid, Ammonium chloride
(b) Weak electrolyte - Acetic acid, Ammonium hydroxide
(c) Non-electrolytes - Carbon tetrachloride

Solution 2002-1

(i) molecules.
(ii) will not

Solution 2002-2

(a) When sulphuric acid is added to water it becomes good conductor as addition of sulphuric acid causes dissociation of water molecules into H⁺ and OH^- ions which are then responsible for conduction of electricity by pure water. The water thus obtained is called acidified water.
(b) Cathode, Anode

Solution 2002-3

Solution 2003-1

electricity, chemical

Electrolysis Exercise 149

Solution 2004-1

Solution 2004-2

(a) Molecules are found in a liquid compound which is a non-electrolyte.
(b) Non ionized molecules; H⁺ and X^- particles will be present in dilute solution.
(c) Loss, Gain
(d) The ions of the metal which is to be electroplated on the article must be present in a solution.
(e) Redox reaction is one in which oxidation and reduction occurs simultaneously.
Similarly in case of electrolysis:
At cathode: The cations gain electron and become neutral. As the electrons are gained the ion is said to be reduced.
At anode: The anions lose electron to form neutral atoms. As the electrons are lost the ion is said to be oxidized.
Hence in electrolysis also the oxidation and reduction occurs hence it is an example of Redox reaction.

Solution 2005-1

(i) Copper metal is solid and has no mobile ions whereas an electrolyte should dissociate into oppositely charged ions to conduct the electric current.
(ii) Hydrogen is released at the cathode when acidulated water is electrolyzed.
(iii) In sodium chloride, Na⁺ and Cl^- ions are not free to carry the electric current.
(iv) (a) Reduced
(b) Higher

Solution 2006-1

Solution 2006-2

Solution 2007-1

(i) Molten ionic compound - Strong electrolyte
(ii) Carbon tetrachloride- Non-electrolyte
(iii) An aluminium wire- Metallic conductor
(iv) A solution containing solvent molecules, solute molecules and ions formed by the dissociation of solute molecules- weak electrolyte
(v) A sugar solution with sugar molecules and water molecules- Non-electrolyte

Electrolysis Exercise 150

Solution 2007-2

Solution 2008-1

(d) Lead is deposited at the cathode

Solution 2008-2

Solution 2008-3

(a) Electrode A is made of gas carbon and electrode B is made of Carbon rods.
(b) At electrode A.
(c) Two compounds in the electrolyte are Al₂O₃ and Na₃AlF₆
(d) As at electrode B the oxygen is liberated during the process. The oxygen liberated oxidizes the carbon anode producing CO and CO₂.Thus electrode B is to be replaced continuously.

Solution 2009-1

Electrolysis Exercise 151

Solution 2009-2

Mg(OH)₂ as it is basic while rest are amphoteric.

Solution 2009-3

Molten Lead bromide conducts electricity.

Solution 2009-4

(a) Nickel ions move towards cathode.
(b) Nickel ions.

Solution 2010-1

(i) Lead (II) bromide

(ii) Oxidation

Solution 2010-2

(i) Aqueous solution of nickel sulphate with few drops of dil. sulphuric acid

(ii) Article (e.g. key chain)

(iii) Pure nickel

(iv) Ni²⁺ + 2e^-→ Ni

(v) Ni → Ni²⁺+ 2e^-

Solution 2010-3

Cell A contains sodium chloride solution which is a strong

electrolyte and contains only ions. So, it conducts electricity

and the bulb glows brightly.

Cell B contains both ions and molecules. So, there are few

ions to conduct electricity and the bulb glows dimly.

Cell C contains sugar solution which is a non-electrolyte and

does not contain ions. So, it is a bad conductor of electricity

and the bulb does not glow.

Solution 2011-1

Dilute sulphuric acid catalyses dissociation, so electrolysis of acidified water is considered an example of catalysis.

Solution 2011-2

(i) In covalent compounds, the bond is formed due to the sharing of electrons.

(ii) Electro covalent compounds have a high boiling point.

(iii) A molecule of nitrogen contains a triple bond.

Solution 2011-3

Copper sulphate solution

Copper metal

Conduction of electricity is

due to the flow of ions.

Conduction of electricity is

due to the flow of electrons.

It is an aqueous solution of

an ionic compound.

It is a metal in the solid

state.

It undergoes a chemical

change.

It remains unchanged

chemically.

Solution 2011-4

(i) Red shiny metal is deposited at the cathode.

(ii) The colour of the electrolytes changes gradually from blue to colourless.

(iii) At the cathode:

Cu²⁺+ 2e^-→ Cu

Reaction at the anode:

OH^-→ OH + e^-

4OH → 2H₂O + O₂

Electrolysis Exercise 152

Solution 2013-1

(i) The right electrode is the anode and oxidising electrode Cu → Cu²⁺+ 2e^-losing electrode.

(ii) Reaction at the anode: Cu → Cu²⁺+ 2e^-

Reaction at the cathode: Cu²⁺+ 2e^-→ Cu

(iii) The anode dissolves and anode mud containing precious metal is recovered.

Solution 2013-2

(i) Liquid carbon tetrachloride

Solution 2013-3

Dark reddish brown fumes of bromine evolve at the anode and greyish white metal lead is formed on the cathode.

Solution 2014-1

(iii) A silver grey deposit at the cathode and reddish brown fumes at the anode.

Solution 2014-2

(iii) Sodium argentocyanide solution

Solution 2014-3

(i) Electrovalent or ionic compounds

(ii) One electron

(iii) Since it has valency 1, M belongs to Group 1.

(iv) At the cathode: M⁺+ 1e^-→ M

(v) At the anode: Oxygen gas

Solution 2015-1

(i) Zinc is lower in the reactivity series, so it is comparatively less reactive. Hence, it is reduced by using carbon monoxide. But aluminium is very reactive; hence, it cannot be reduced by using a reducing agent and it can be reduced only by electrolytic reduction.

(ii) Carbon tetrachloride is a liquid and does not conduct electricity because it is a covalent compound and there are no free ions present and it contains only molecules.

(iii) In electrolysis of molten lead bromide, reactive bromine is liberated at the anode. As bromine is very reactive, an inert electrode like graphite is preferred in the electrolysis of molten lead bromide.

(iv) Acetic acid is a weak acid and has fewer ions, so conductivity is less, whereas dilute sulphuric acid is a strong acid and has more ions, and therefore, its electrical conductivity is more.

(v) During electrolysis of lead bromide, there is loss of electrons at the anode by bromine and gain of electrons at the cathode by lead. Thus, oxidation and reduction occur side by side. So, it is a redox reaction.

PbBr₂⇌ Pb⁺²+ 2Br^-

Solution 2015-2

Strong Electrolytes	Weak Electrolytes
Electrolytes which allow a large amount of electricity to flow through them.	Electrolytes which allow small amounts of electricity to flow through them.
These are good conductors of electricity.	These are poor conductors of electricity.
These almost completely dissociate in the fused or aqueous solution state.	These are partially dissociated in the fused or aqueous solution state.
These solutions contain only free mobile ions.	These solutions contain ions as well as molecules.

Electrolysis Exercise 153

Solution 2015-3

Anode

Electrolyte

Purification of copper

Impure copper

Solution of

copper sulphate

and dilute

sulphuric acid

(i)

(ii) Ag - e^- → Ag⁺

Cu - e- → Cu²⁺

Cl^⁻‒ e^-→ Cl

Cl + Cl → Cl₂

Solution 2016-1

(i) Electrostatic forces of attraction between ions in the solid state are very strong. These forces weaken in the fused state or in the solution state. Hence, ions become mobile.

(ii) If silver nitrate solution is used directly instead of double cyanide of silver and sodium, the deposition of silver will be very fast and hence not very smooth and uniform.

(iii) Copper has no mobile electrons in the solid state and an electrolyte should dissociate into oppositely charged ions to conduct electricity.

Hence, copper is a non-electrolyte.

Solution 2016-2

(i) Oxygen is the product formed at the anode.

(ii) Ag⁺ and Na⁺

Solution 2016-3

(i) Electrodes:

Cathode: Copper

Anode: Platinum

Reaction at the cathode: Cu²⁺ + 2e^-→ Cu

Reaction at the anode: 4OH^- - 4e^-→ 4OH

2OH + 2OH →2H₂O + O₂

(ii) The cathode and anode are both made of graphite plates.

Reaction at the cathode: Pb²⁺ + 2e^-→Pb

Reaction at the anode: Br^- - e^-→Br

Br + Br →Br₂

Solution 2017-1

(i) The electrolyte used for electroplating an article with silver: Sodium argentocyanide or potassium argentocyanide

(ii) The particles present in a liquid such as kerosene that is a non-electrolyte: Molecules

Solution 2017-2

(i) Observations:

Anode: Dark reddish brown fumes of bromine evolve at the anode.

Cathode: Greyish white metal lead is formed on the cathode.

(ii) Observations:

Anode: Nothing gets deposited on the anode because the copper anode dissolves during the reaction as Cu²⁺ ions are formed.

Cathode: Reddish brown Cu is deposited.

Solution 2017-3

(a) OH^-

(b) Ag⁺

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