Question # 1

Whenever a week base is dissolved in water, it give its conjugate acid. similarly a weak acid in water produces its conjugate base. This conjugate acid-base pair concept is stated by

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Law of mass action

Le-charlier's principle

Common ion effect

Lowery Bronsted concept

A solution has pH = 0, its H⁺ion concentration is

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1 x 10^-14

1 x 10¹⁴

1 x 10¹

1

The avtive mass of 64 g of HI in a two litre flask would be

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2

1

5

0.25

Two moles of HI was heated in a sealed tube at 440°C till the equilibrium was reached. HI was found to be 22% decomposed. The equilibrium constant for dissociation is

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0.282

0.0796

0.0199

1.99

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Increases

Decreases

Remains same

Cannot be predicted

pH of the human blood which is essentially maintained constant due to carbonates, biocarbonates, phosphates etc., is

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7.00

7.25

7.35

7.47

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Introduction of an inert gas at constant volume

Introduction of PCl₃(g) at constant

Introduction of PCl₅(g) at constant volume

Introduction of Cl₂at constant volume

A buffer of a 0.09 molar acetic acid and 0.11 molar sodium acetate has pH = 4.83. If 0.01 mole NaOH in 1 dm³of the buffer solution is added, then pH of the buffer becomes

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4.74

4.92

5.0

4.0

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High temperature and low pressure

Low temperature and low pressure

Low temperature and high pressure

High temperature and high pressure

The rate of forward reaction is two times that of the reverse reaction at a given temperature and identical concentration, K equilibrium is

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0.5

1.5

2.5

2.0

The rate of reaction :

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Remain same as reaction proceeds.

May decrease or increase as reaction proceeds .

Increase as reaction proceeds.

Decreases as reaction proceeds.

The pH of 10^-3mole dm^-3of an aqueous solution of H₂SO₄is

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3.0

2.7

2.0

1.5

Units of Kw are

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Mole dm^-3

Mole²dm^-3

Mole²dm^-6

Mole²dm^-3

When H₂and I₂are mixed and equilibrium is attained, then

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Amount of HI formed is equal to the amount of H₂dissociated

HI dissociation stops

The reaction stops completely

None of these

The relation between Kc and Kp is

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At certain temperature, 50% of HI is dissociated into H₂and I₂the equilibrium constant is

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1.0

3.0

0.5

0.25

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Which one of the following is not a buffer

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H₂CO₃+ NaHCO₃solution

H₃PO₄+ NaH₂PO₄solution

Hl + Nal solution

NH₄OH + NH₄CI solution

The rate of a chemical reaction is directly;y proportional to product of molar concentration of reaction substance it is called :

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Low of conservation of energy.

Law of mass action.

Rate law .

Active mass rule.

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At equilibrium there is no further change in the concentration of Hl

At equilibrium concentration of l₂remains constant

At equilibrium concentration of H₂remains unaltered

At equilibrium the rate of formation of Hl is equal to the rate of decomposition of Hl

The optimum conditions of temperature and pressure to get maximum NH₃form N₂and H₂gases is

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2000°C and 10 atmosphere

0°C and 1 atmosphere

400°C and 200-300 atmosphere

200°C and 100 atmosphere

In 1000 molecules of 0.001 M acetic acid the number of H⁺ions is 12.6, then its percentage of ionization is

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1.33%

1.26%

12.6

1%

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[A] = [B]

[A] < [B]

[B] = [C]

[A] > [B]

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Decrease in temperature favour more dissolution of the salt

Increase in temperature favour more dissolution of the salt

Lowering pressure favour more dissolution of the salt

Increasing pressure favour more dissolution of the salt

Which one of the following is a buffer

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HCI + NaCI solution

CH₃COOH + CH₃COONH₄solution

H₂SO₄+ CaSO₄solution

CH₃COOH + CH₃COONa

The solubility product of Ca(OH)₂is 6.5 x 10^-6. The concentration of OH^-ions is

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1.175 x 10^-2

2.35 x 10^-2

3.25 x 10^-3

3.25 x 10^-4

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Initial concentration of acetic acid

Initial concentration of ethyl acetate

Equilibrium concentration of acetic acid

Equilibrium concentration of ethyl acetate

I a chemical reaction equilibrium is said to have been established when :

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Rate of opposing reactions are equal.

Rate constants of opposing reactions are equal.

Opposing reactions stop.

Concentration of reactants and products are equal

Law of mass action was given by :

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Guldberg and Waage.

Berkeley and Hartly.

Ramsay and Reyleigh.

Berthelot.

pH of 1 molar NaOH is

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7

zero

14

10

Which statement about the following equilibrium in correct?

2SO_{2 (g)}+ O_2(g)---------------2sO_3(g)H= - 188.3 KJ mol-1

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T value of K_{p falls witha rise in temperate.}

The value of K_{p falls withincreasing pressure}

Adding V_2O₅catalyst increase the equilibrium yield of sulfur trioxide

The value of K_{p is equal to}K_p

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