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4

Ionisation constant of formic acid is 1.8 x 1.8×10-4 at 298 K. In 0.1 NHCOOH the percentage ionisation of HCOOH acid is

A. 0.18

B. 42.4

C. 4.24

D. 2.89

Correct Answer :

C. 4.24


Related Questions

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4

Degree of ionisation depends on

A. temperature

B. nature of solvent

C. neither (a) nor (b)

D. both (a) and (b)

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4

pH of 0.001 M NaOH aqueous solution is

A. 2

B. 5

C. 11

D. 9

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4

At a given temperature PbI2 will be more soluble in

A. water

B. 0.02 M Nal

C.  O.4 M Pb NO32

D. 0.02 MKI

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4

Which of the following is not hydrolysed in water ?

A. HCOONa

B. KCN

C. K2CO3

D. KC1

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4

Conjugate acid differs from its conjugate base by

A. proton

B. meson

C. electron pair

D. positron

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4

Decinormal solution of acetic acid ionised to an extent of 1.3%. pH of this solution will be (log 1.3 = 0.11)

A. 3.89

B. 2.89

C. 4

D. 1.0

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4

Sum of pH and pOH of an acidic solution at 25°C is

A. 0

B. 14

C. depends on pH of base

D. depends on pH of acid

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4

Ostwald dilution law is applicable for :

A. weak electrolytes

B. strong electorate

C. basic

D. acids

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4

0.1 M acetic acid ionise to an extent of 1.34%. Ionisation constant of acetic acid is

A. 0.00134

B. 1.182

C. 1.82 x 10-5

D. 2.8 x 10-61CF6

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4

2 gm of NaOH is dissolved in one litre water. pH of the solution will be

A. 12.7

B. 11.7

C. 1.3

D. 17.7

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4

BaSO4(Mol. wt 233) has solubility 0.009 gmlit-1 at 298 K. Its solubility product is

A.  1.521 x 10-5

B. 152.1 x 10-1910"19

C. 1.9 x 10-5

D. 15.21 x 10-9

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4

CH3COOH+H2H3O++CH3COO-
In the above reaction acid is

A. H3O+

B. H2O

C. CH3COOH

D. CH3COOH and H3O+

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4

On dissolving sodium chloride in water pH of the solution

A. decreases

B. increases

C. remains unchanged

D. increase or decreases

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4

Precipitation takes place when

A. ionic product < Ksp

B. ionic product > Ksp

C. ionic product2=Ksp 

D. ionic product = Ksp

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4

Which of the following is not hydrolysed in water ?

A. HCOONa

B. KCN

C. K2CO3

D. KC1

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4

Kspfor AgCl (mol wt 143.5) is 17 x 10-11 at 298K. The molar solubility of AgCl at 298 Kis

A. 18.7 x10-5

B. 2.3 x 10-3

C. 9.90 x 10-3

D. 1.3 x 10-5

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4

An aqueous solution of sodium acetate is

A. amphoteric

B. halogenic

C. alkaline

D. acidic

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4

pH of 0.1 M monoprotic acid is 4. Then dissociation constant of the acid is :

A.  9

B. 10-7

C. 10-5

D. 1-3

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4

Solubility of calcium carbonate is 0.0305 gm/litre.Kspfor CaCO3 is

A. 0.000305

B. 193 x 10-8

C. 9.3 x10-8

D. 93.05 x1-5

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4

Conjugate base of HCO3-is

A. HCO32-

B. HCO3+

C. H2CO3-

D. CO32-

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4

Which of the following is not a Lewis acid?

A. ZnCL2

B. BF3

C. H2O

D. Ag+

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4

pH of a solution is 10. Hydroxide ion concentration in the solution is

A. 10-10 gm eq.

B. 10-4 mole liter-1

C. 10-4 gm liter-1

D. 10-3 gm eq.

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4

An aqueous solution CaF2 contains 2 x 10-4mole lit-1 of CaF2. Ksp for CaF2 is

A.  16 x 10-8

B. 3.2 x 1010-11

C. 3.2 x 10-6

D. 0.156 x 10-2

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4

Which of the following will favour the reverse reaction in a chemical equilibrium?

A. Increasing the concentration of one or more of the products

B. Decreasing the concentration of one of the products

C. Removal of at least one of the products at regular intervals

D. None of the above

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4

Acetic acid is weak acid because it is

A. organic acid

B. immiscible with water

C. slightly ionised

D. viscous

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4

pH of a solution is 8.5. solution is

A. amphoteric

B. neutral

C. acids

D. basic

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4

If NH3 is dissolved in water, pH of the solution

A. decreases

B. increases

C. remains unchanged

D. may increase or decrease

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4

During salt analysis NH4OH is added before adding NH4OH for third gp., cation analysis so as to

A. increase the concentration ofOH- ions

B. increase the concentration of ammonia

C. increase the concentration of chloride ions

D. prevent the precipitation of hydroxides of subsequent groups

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4

Strength of an acid depends on

A. hydrolysis

B. concentration of OH- ions

C. concentration ofH+ ions

D. no. of moles of base used for neutralisation

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4

Dissociation constant of 0.01 M HCN is 4 x10-10. The H- concentration in the solution is

A. 3×10-6 mole lit-1

B. 2×10-6 mole lit-1

C. 5×10-10 mole lit-1

D. 5×10-8mole lit-1