At a given temperature $P b I_{2}$ will be more soluble in

Question

At a given temperature $P b I_{2}$ will be more soluble in

A. water

Correct Answer :

A. water

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Comment

Which of the following is not hydrolysed in water ?

B. KCN

D. KC1

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

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pH of 0.001 M NaOH aqueous solution is

A. 2

B. 5

C. 11

D. 9

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If $N H_{3}$ is dissolved in water, pH of the solution

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Precipitation takes place when

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

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Ionisation constant of formic acid is 1.8 x $1.8 \times 10^{- 4}$ 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

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pH of a solution is 8.5. solution is

C. acids

D. basic

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On dissolving sodium chloride in water pH of the solution

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Dissociation constant of 0.01 M HCN is 4 x $10^{- 10}$ . The $H^{-}$ concentration in the solution is

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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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In an aquous solution of silver bromide concentration of $A g^{+} i s 1 \times 10^{- 6} m o l l i t^{- 1}$ . If $K_{s p}$ for AgBr is
4 x $10^{- 13}$ then concentration of Br in the solution is

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

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Which of the following is not hydrolysed in water ?

B. KCN

D. KC1

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Molar concentration of $A g^{+}$ in an aqueous solution of $A g_{2} C r O_{4}$ at 298K is 1.5 x $10^{- 4}$ $K_{s p}$ , for $A g_{2} C r O_{4}$ is

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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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Conjugate acid differs from its conjugate base by

A. proton

B. meson

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An aqueous solution of sodium acetate is

D. acidic

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An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

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$B a S O_{4}$ (Mol. wt 233) has solubility 0.009 gm $l i t^{- 1}$ at 298 K. Its solubility product is

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On dissolving copper sulphate in water pH of the solution

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In III gp of salt analysis for cations $N H_{4} C L$ and $N H_{4} O H$ are added as group reagents. Which of the following can be used instead of $N H_{4} C L$ ?

B. NaCL

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On dissolving sodium carbonate in water pH of the solution

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Which of the following is not a Lewis acid?

B. $B F_{3}$

C. $H_{2} O$

D. $A g^{+}$

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Conjugate base of $H C O_{3}^{-}$ is

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

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During salt analysis $N H_{4} O H$ is added before adding NH4OH for third gp., cation analysis so as to

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

B. 1.182

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

A. 0

B. 14

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Acetic acid is weak acid because it is

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Answer 1

B. 0.02 M Nal

Answer 2

C. O.4 M Pb

{(N O_{3})}_{2}

Answer 3

D. 0.02 MKI

Answer 4

A.

H C O O N a

Answer 5

C.

K_{2} C O_{3}

Answer 6

A. ionic product <

K_{s p}

Answer 7

B. ionic product >

K_{s p}

Answer 8

C.

[i o n i c p r o d u c t]^{2}

=

K_{s p}

Answer 9

D. ionic product =

K_{s p}

Answer 10

A. decreases

Answer 11

B. increases

Answer 12

C. remains unchanged

Answer 13

D. may increase or decrease

Answer 14

A. ionic product <

K_{s p}

Answer 15

B. ionic product >

K_{s p}

Answer 16

C.

{[i o n i c p r o d u c t]}^{2} = K_{s p}

Answer 17

D. ionic product =

K_{s p}

Answer 18

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

Answer 19

B. Decreasing the concentration of one of the products

Answer 20

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

Answer 21

D. None of the above

Answer 22

A. amphoteric

Answer 23

B. neutral

Answer 24

A. decreases

Answer 25

B. increases

Answer 26

C. remains unchanged

Answer 27

D. increase or decreases

Answer 28

A.

3 \times 10^{- 6} m o l e l i t^{- 1}

Answer 29

B.

2 \times 10^{- 6} m o l e l i t^{- 1}

Answer 30

C.

5 \times 10^{- 10} m o l e l i t^{- 1}

Answer 31

D.

5 \times 10^{- 8} m o l e l i t^{- 1}

Answer 32

A. 4 x

10^{- 8}

mole

l i t e r^{- 1}

Answer 33

B. 2 x

10^{- 19}

mole

l i t e r^{- 1}

Answer 34

C. 4 x

10^{- 7}

mole

l i t e r^{- 1}

Answer 35

D. 2 x

10^{- 5}

mole

l i t e r^{- 1}

Answer 36

A.

10^{- 8}

Answer 37

B.

20 \times 10^{5}

Answer 38

C.

10^{- 3}

Answer 39

D.

10^{- 4}

Answer 40

A.

H C O O N a

Answer 41

C.

K_{2} C O_{3}

Answer 42

A. 1.125 x

10^{- 8}

Answer 43

B. 2.5 x

10^{- 4}

Answer 44

C. 2.25 x

10^{- 8}

Answer 45

D. 1.6875 x

10^{- 12}

Answer 46

C. electron pair

Answer 47

D. positron

Answer 48

A. amphoteric

Answer 49

B. halogenic

Answer 50

C. alkaline

Answer 51

A. 16 x

10^{- 8}

Answer 52

B. 3.2 x 10

10^{- 11}

Answer 53

C. 3.2 x

10^{- 6}

Answer 54

D. 0.156 x

10^{- 2}

Answer 55

A. 1.521 x

10^{- 5}

Answer 56

B. 152.1 x

10^{- 19}

10"19

Answer 57

C. 1.9 x

10^{- 5}

Answer 58

D. 15.21 x

10^{- 9}

Answer 59

A. decreases

Answer 60

B. increases

Answer 61

C. remains unchanged

Answer 62

D. may increase or decrease

Answer 63

A.

N H_{4} N O_{3}

Answer 64

C.

{(N H_{4})}_{2} S O_{4}

Answer 65

D.

{(N H_{4})}_{2} C_{2} O_{4}

Answer 66

A. decreases

Answer 67

B. increases

Answer 68

C. remains unchanged

Answer 69

D. may increase or decrease

Answer 70

A.

Z n C L_{2}

Answer 71

A.

H C O_{3}^{2 -}

Answer 72

B.

H C O_{3}^{+}

Answer 73

C.

H_{2} C O_{3}^{-}

Answer 74

D.

C O_{3}^{2 -}

Answer 75

A.

10^{- 10}

gm eq.

Answer 76

B.

10^{- 4}

mole

l i t e r^{- 1}

Answer 77

C.

10^{- 4}

gm

l i t e r^{- 1}

Answer 78

D.

10^{- 3}

gm eq.

Answer 79

A. increase the concentration of

O H^{-}

ions

Answer 80

B. increase the concentration of ammonia

Answer 81

C. increase the concentration of chloride ions

Answer 82

D. prevent the precipitation of hydroxides of subsequent groups

Answer 83

A. 0.00134

Answer 84

C. 1.82 x

10^{- 5}

Answer 85

D. 2.8 x

10^{- 6}

1CF6

Answer 86

C. depends on pH of base

Answer 87

D. depends on pH of acid

Answer 88

A. organic acid

Answer 89

B. immiscible with water

Answer 90

C. slightly ionised

Answer 91

D. viscous

At a given temperature $P b I_{2}$ will be more soluble in

Correct Answer :

Show all ionic Equilibrium MCQ

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Precipitation takes place when

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

Ionisation constant of formic acid is 1.8 x $1.8 \times 10^{- 4}$ at 298 K. In 0.1 NHCOOH the percentage ionisation of HCOOH acid is

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On dissolving sodium chloride in water pH of the solution

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Conjugate acid differs from its conjugate base by

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Correct Answer :

Show all ionic Equilibrium MCQ

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pH of 0.001 M NaOH aqueous solution is

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

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

pH of a solution is 8.5. solution is

On dissolving sodium chloride in water pH of the solution

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

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

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

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