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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
(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.
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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