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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

Correct Answer :

D. prevent the precipitation of hydroxides of subsequent groups


Related Questions

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4

In an aquous solution of silver bromide concentration of Ag+ is 1×10-6 mol lit-1. If Ksp for AgBr is
4 x 10-13 then concentration of Br in the solution is

A. 4 x 10-8 mole liter-1

B. 2 x 10-19 mole liter-1

C. 4 x 10-7 mole liter-1

D. 2 x 10-5 mole liter-1

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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

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

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

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

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

A. H3O+

B. H2O

C. CH3COOH

D. CH3COOH and H3O+

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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

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

For the reversible reaction
N2g+3H2g=2NH3gH is-93.7 Kj.
The equilibrium will shift in the forward direction if conc. of

A. NH3 is increased

B. N2 is decreased

C. N2 is increased

D. temperature is kept variable

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4

According to Bronsted Lowry an acid is

A. that gives cation in solution

B. one that gives H+ ions in solution

C. electron acceptor

D. proton donor

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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

On dissolving sodium carbonate in water pH of the solution

A. decreases

B. increases

C. remains unchanged

D. may increase or decrease

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4

 Molar concentration of Ag+ in an aqueous solution of Ag2CrO4 at 298K is 1.5 x 10-4 Ksp, for Ag2CrO4 is

A. 1.125 x 10-8

B. 2.5 x 10-4

C. 2.25 x10-8

D. 1.6875 x 10-12

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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

An aqueous solution of sodium acetate is

A. amphoteric

B. halogenic

C. alkaline

D. acidic

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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

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

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

Which of the following is not hydrolysed in water ?

A. HCOONa

B. KCN

C. K2CO3

D. KC1

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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

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

pH of 0.1 M monobasic acid is 4 then molar concentration of H+ per litre will be

A. 10-8

B. 20×105

C. 10-3

D. 10-4

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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

Conjugate base of HCO3-is

A. HCO32-

B. HCO3+

C. H2CO3-

D. CO32-

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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

A solution is said to be saturated w.r.t the electrolyte it contains if

A. ionic product < Ksp

B. ionic product > Ksp

C. [ionic product]2 = Ksp

D. ionic product = Ksp

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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

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

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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

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