Nootan Chemistry Class 12 Solutions

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Nootan Chemistry Class 12 Solutions. We covered all the ISC Nootan Chemistry Class 12 Solutions pdf free download file in this post for free so that you can practice well for the exam.

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Nootan Chemistry Class 12 Objective with Solutions

Total number of benzene rings and nitrogen atoms present in p-rosaniline hydrochloride are:

(A) 3 benzene rings, 3 nitrogen atoms

(B) 3 benzene rings, 2 nitrogen atoms

(C) 4 benzene rings, 4 nitrogen atoms

(D) 4 benzene rings, 3 nitrogen atoms

Option a – 3 benzene rings, 3 nitrogen atoms

Which of the following cannot reduce Fehling solution?

(A) Methanal

(B) Ethanal

(C) Ethanoic acid

(D) Methanoic acid

Option c – Ethanoic acid

Which of the following is oxidized by ammonical silver nitrate?

(A) Alkoxy alkanes

(B) Alkanes

(C) Alkanols

(D) Alkanals

Option d – Alkanals

Schiff’s reagent on reacting with aldehyde forms a magenta color because of:

(A) Oxidation of alkanal

(B) Reduction of alkanal

(C) Reduction of Schiff’s reagent

(D) Oxidation of Schiff’s reagent

Option c – Reduction of Schiff’s reagent

The pink or red color of p-rosaniline hydrochloride is decolorized by passing:

(A) Carbon monoxide

(B) Sulfur trioxide

(C) Sulfur dioxide

(D) Carbon dioxide

Option c – Sulfur dioxide

Schiff’s reagent gives a magenta color with:

(A) Methyl ethanoate

(B) Ethanoic acid

(C) Propanone

(D) Ethanal

Option d – Ethanal

According to Bronsted concept, the base is a substance that is

(A) a Proton doner

(B) a Proton accepter

(C) an Electron donor

(D) an Electron accepter

Option b – a Proton accepter

Lewis acids are

(A) Electrophiles

(B) Nucleophiles

(C) Electron pair doner

(D) Proton accepter

Option a – Electrophiles

Which of the following fluoro-compounds is most likely to behave as a Lewis base?

(A) BF3

(B) PF3

(C) CF4

(D) SiF4

Option b – PF3

What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

(A) 12.65

(B) 2.0

(C) 7.0

(D) 1.04

Option a – 12.65

Which one of the following pairs of solutions is not an acidic buffer?

(A) HCIO4 and NaClO4

(B) CH3COOH and CH3COONa

(C) H₂CO3 and Na2CO3

(D) H3PO4 and Na3PO4

Option a – HCIO4 and NaClO4

Which will make a basic buffer?

(A) 100 ml of 0.1 M CH3COOH + 100 ml of 0.1 M NaOH

(B) 100 ml of 0.1 HCI + 200 ml of 0.1 M M NH4OH

(C) 100 0.1 M ml of 0.1 M HCl + 100 ml of NaOH

(D) 50 ml of 0.1 M NaOH+ 25 ml of 0.1 M CH3COOH

Option b – 100 ml of 0.1 HCI + 200 ml of 0.1 M M NH4OH

HCl was passed through a solution of CaCl₂, MgCl₂, and NaCl. Which of the following compound(s) crystallize (s)?

(A) NaCl, MgCl₂ and CaCl₂

(B) Both MgCl₂ and CaCl₂

(C) Only NaCl

(D) Only MgCl₂

Option c – Only NaCl

Addition of NH4Cl into NH4OH. The dissociation of NH4OH decreases it is due to

(A) Hydrolysis

(B) Common ion effect

(C) Precipitation

(D) Reduction

Option b – Common ion effect

The addition of NaCl into AgCl decreases the solubility of AgCl, because

(A) Ksp of AgCl decreases

(B) Ksp of AgCl increases

(C) Solution becomes unsaturated

(D) I.P. exceeds the Ksp

Option a – Ksp of AgCl decreases

The solubility product is applicable for an

(A) Saturated solution of sparingly soluble salt.

(B) Unsaturated solution of normal salt.

(C) Any salt solution.

(D) Molar solution of the salt

Option b – Unsaturated solution of normal salt

The pH of a buffer solution was made by mixing 25 ml of 0.02 M NH4OH and 25 ml of 0.02 M NH4CI at 25°C. (pKb of NH4OH = 4.8)

(A) 5.8

(B) 9.2

(C) 4.8

(D) 3.8

Option b – 9.2

A basic buffer is prepared by mixing

(A) Acetic acid and sodium acetate

(B) Sodium hydroxide and sodium chloride

(C) Ammonium hydroxide and ammonium chloride

(D) Sodium sulfate and sulphuric acid

Option c – Ammonium hydroxide and ammonium chloride

When an ionic product, is greater than the solubility product the solution becomes

(A) Saturated

(B) Unsaturated

(C) Colloidal

(D) Supersaturated or precipitated

Option d – Supersaturated or precipitated

Which of the following sulfides has the lowest solubility product?

(A) FeS

(B) MnS

(C) PbS

(D) ZnS

Option c – PbS

Which of the following will suppress the ionization of acetic acid in aqueous solution?

(A) NaCl

(B) HCI

(C) KCI

(D) NH4Cl

Option b – HCl

The pair which shows the common ion effect is

(A) AgCN + KCN

(B) NaCl + HCI

(C) NH4OH + NH4Cl

(D) BaCl₂ + Ba(NO3)2

Option c – NH4OH + NH4Cl

Purification of common salt based on

(A) Buffer solution

(B) Le-chatelier’s Principle

(C) Hydrolysis

(D) Common ion effect

Option d – Common ion effect

For NH4OH and NH4Cl buffer solutions, the pH of the buffer can be increased

(A) By adding NH4Cl

(B) By removing NH4Cl

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(C) By adding NH4OH

(D) By adding H₂O

Option c – By adding NH4OH

Buffer solutions are solutions that resist the change in pH by the addition of

(A) a small amount of acid

(B) a small amount of base

(C) a small amount of acid or base

(D) a small amount of its salt.

Option c – a small amount of acid or base

Which can not act as a buffer?

(A) NH4Cl and NH4OH

(B) CH3COOH and CH3COONa

(C) 40 ml of 0.1 M NaCN + 20 ml of 0.1 MHCN

(D) CH3COOH and NaCl

Option d – CH3COOH and NaCl

In an aqueous CH3COOH solution of sodium acetate is added then the pH of the solution

(A) Decreases

(B) Increases

(C) Does not changes

(D) Can not be predicted

Option b – Increases

The strength of weak acids and weak base salts depends on

(A) Ka volume

(B) Kb value

(C) Both Ka and Kb values

(D) None of these

Option c – Both Ka and Kb values

Which will not be hydrolyzed?

(A) Potassium nitrate

(B) Potassium cyanide

(C) Potassium carbonate

(D) Potassium acetate

Option a – Potassium nitrate

Which salt gives a basic solution to hydrolysis?

(A) KCN

(B) KCI

(C) NH4Cl

(D) CH3COONH4

Option a – KCN

Hydrolysis of ammonium acetate involves

(A) Only cations

(B) Only anions

(C) Neither cation nor anion

(D) Both ions

Option d – Both ions

Aq. NaNO3 solution is

(A) Acidic

(B) Basic

(C) Neutral

(D) May be acidic or basic in nature

Option c – Neutral

CH3COONa is a salt of

(A) Strong acid and strong base

(B) Strong acid and weak base

(C) Weak acid and strong base

(D) Weak acid and weak base

Option c – Weak acid and strong base

Which salt does not undergoes hydrolysis?

(A) CuCl₂

(B) CH3COONH4

(C) KCN

(D) KCI

Option d – KCl

Hydrolysis reaction involves, salt containing

(A) Cations only

(B) Anions only

(C) May cations or anions or both ions.

(D) Neither cation nor anion

Option c – May cations or anions or both ions

Na₂SO4 is an example of

(A) Strong acid and weak base

(B) Strong base and weak acid

(C) Weak acid and weak base

(D) Strong acid and strong base

Option d – Strong acid and strong base

An aqueous solution of sodium carbonate is alkaline in nature due to

(A) Cation hydrolysis

(B) Anion hydrolysis

(C) Cation and anion hydrolysis

(D) Neither cation or anion hydrolysis

Option b – Anion hydrolysis

Aqueous copper sulfate solution is

(A) Acidic in nature

(B) Basic in nature

(C) Amphoteric

(D) Neutral solution

Option a – Acidic in nature

Ammonium cyanide salt is formed from

(A) Weak acid and strong base

(B) Weak acid and weak base

(C) Strong base and strong acid

(D) Weak base and strong acid

Option b – Weak acid and weak base

The pH of the solution is 3. The solution is diluted by 100 times. The pH of the resulting solution is

(A) 5

(B) 7

(C) 1

(D) 11

Option a – 5

The pH of a cenimolar Barium hydroxide solution is

(A) 2.0

(B) 12.3

(C) 12.0

(D) 11.7

Option b – 12.3

When the base is diluted, the pH of the solution is

(A) Increases

(B) Decreases

(C) Constant

(D) Changes but depends on base

Option a – Increases

Human blood has a pH

(A) 5.2

(B) 6.3

(C) 7.3

(D) 8.3

Option c – 7.3

Which of the following will decreases the pH of a 50 ml solution of 0.01 M HCI?

(A) Addition of 5 ml of 1 M HCI

(B) Addition of 50 ml of 0.01 M HCI

(C) Addition of 50 ml of 0.002 M HCI

(D) Addition of MG

Option a – Addition of 5 ml of 1 M HCl

As the temperature of the solution increases, the pH of the solution

(A) Increases

(B) Decreases

(C) Does not change

(D) Depends on solution increases or decreases

Option b – Decreases

At 25°C, the pH of the solution is 6.96, then the solution is

(A) Slightly acidic

(B) Slightly basic

(C) Strongly acidic

(D) Strongly basic

Option a – Slightly acidic

pKw of boiling water is

(A) pH – pOH

(B) 14

(C) >14

(D) <14

Option d –

pH of the solution is independent of

(A) Concentration

(B) Temperature

(C) Degree of ionization

(D) Amount of solution

Option d – Amount of solution

At any temperature, pH + pOH is equal to

(A) 14

(B) 12

(C) 13

(D) pkw

Option d – pkw

The Bronsted acid gives the weakest conjugate! the base is

(A) HF

(B) H₂S

(C) HCI

(D) H₂O

Option c – HCl

Arrhenius’s theory does not explain the acidic nature of

(A) HCI

(B) HOOH

(C) CO₂

(D) H₂CO3

Option c – CO₂

The strength of acids and bases depends on ( Nootan chemistry class 12 solutions )

(A) the Concentration of the solution

(B) the Degree of dissociation

(C) Pressure

(D) Both ‘A’ and ‘B’

Option d – Both ‘A’ and ‘B’

Equimolal solution of A and B shows the depression in F.P. in the ratio 2 : 1. A remains in a normal state in solution B will be in the solution

(A) Normal

(B) Dissociated

(C) Associated

(D) Hydrolysed

Option c – Associated

In aq. solution of glucose is allowed to freeze then crystals of which will be separated out first?

(A) Glucose

(B) Water

(C) Both

(D) Neither water nor glucose

Option a – Glucose

If the solution boils at temperature T₁ and the solvent at temperature T₂. The elevation in boiling point given by

(A) T₁+T₂

(B) T₁ – T₂

(C) T₂-T₁

(D) Both (A) and (B)

Option b – T₁ – T₂

Maximum elevation in boiling point is for ( Nootan chemistry class 12 solutions )

(A) 1 M NaCl

(B) 1 M CaCl₂

(C) 1 M BaCl₂

(D) 1 M FeCl3

Option d – 1 M FeCl3

A solution that has higher osmotic pressure as compared to the other solution is known as

(A) Hypotonic

(B) Hypertonic

(C) Isotonic

(D) Abnormal

Option b – Hypertonic

A solution which lower osmotic pressure than that of the other solution is known as

(A) Hypotonic

(B) Hypertonic

(C) Normal

(D) Isotonic

Option a – Hypertonic

(A) 0.1 M glucose, (B) 0.05 M NaCl, (C) 0.05 M BaCl2, and (D) 0.1 M AlCl3 solutions. Which one of the following pairs is the isotonic solution?

(A) A and B

(B) B and C

(C) A and D

(D) A and C

Option a – A and B

If the amount of a nonelectrolyte dissolved is double but the solvent is quadrupled. The elevation in B.P. of the solution will be

(A) Double

(B) Halved

(C) Four times

(D) Unchanged

Option b – Halved

Raoult’s law is applicable for (i) Dilute solutions only (ii) When a solute is nonvolatile (iii) When the solute does not dissociate or associate (iv) When the solution behaves as an ideal. The correct statement is

(A) i, ii

(B) ii, iii

(C) iii, iv

(D) i, ii, iii, iv

Option d – i, ii, iii, iv

12 g urea dissolved in one-liter water and 68.4 g sucrose dissolved in the same volume of water, lowering the vapor pressure

(A) Urea solution equal to sucrose solution

(B) Urea solution less than sucrose solution.

(C) Urea solution greater than sucrose solution.

(D) Urea solution has half of the sucrose solution.

Option a – Urea solution equal to sucrose solution

Phenol dimerizes in benzene having Van’t Hoff factor 0.54. The degree of association is

(A) 0.46

(B) 0.27

(C) 0.54

(D) 0.92

Option d – 0.92

The freezing point of 0.1 M glucose is -1.86°C. If an equal volume of 0.3 M glucose solution is added, F.P. of the mixture will be

(A) -7.44°C

(B) -5.58°C

(C) -3.72°C

(D) -2.79°C

Option c – -3.72°C

Dissociation of solute in solution

(A) Decreases the number of solute particles.

(B) Increases the number of solute particles.

(C) Solute particles are double.

(D) Solute particles remain the same.

Option b – Increases the number of solute particles

A super-saturated solution is a metastable solution whose concentration

(A) is Equal to the solubility of a substance in a solvent.

(B) Less than the solubility of a substance

(C) Exceeds the solubility

(D) Continuously changes

Option c – Exceeds the solubility

Van’t Hoff factor ‘i’ for dilute aq. solution of Barium hydroxide is

(A) 0

(B) 1

(C) 2

(D) 3

Option d – 3

The mass of urea that is to be dissolved in 100 g of water in order to decrease vapor pressure by 1.8% is

(A) 3.0

(B) 0.6

(C) 6.0

(D) 0.3

Option c – 6.0

A 5% by mass of an aqueous solution of A of molar mass 342 g is isotonic with 0.878% by mass of solution B. The molar mass of B is

(A) 120

(B) 180

(C) 60

(D) 90

Option c – 60

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