Question # 1

If the difference of pKa values of the two acids is 2, then

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Acid with smaller pKa is 10 times stronger acid

Acid with greater pKa is 10 times stronger acid

Acid with smaller pKa is 100 times stronger acid

Acid with greater pKa is 100 times stronger acid

N₂+3H₂⇌ 2NH_{3 + Heat for above equation, themaximum product will be obtained at :}

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Low temperature at high pressure.

High temperature and low pressure.

High temperature and high pressure.

Low temperature at low pressure.

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

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3.0

2.7

2.0

1.5

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Forward reaction is favoured

Backward reaction is favoured

No effect

None of the above

Which of the following is a characteristic of a reversible reaction?

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It never proceeds to completion

It can be influenced by a catalyst

It proceeds only in the forward direction

Number of moles of reactants and products are equal

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.

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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

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450°C

250°C

850°C

1000°C

1.1 mol of A is mixed with 2.2 mol of B and the mixture is kept in on litre flask till the equilibrium is reached. At equilibrium, 0.2 mol of C is formed. If the equilibrium reaction is A+2B 2C+D, the value of equilibrium constant is

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0.002

0.004

0.001

0.003

In which of the following cases, the reaction goes farthest to completion

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K = 10³

K = 10^-2

K = 10

K = 10⁰

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

The best buffer is prepared when molar concentrations of the salt and acid are equal, then its pH and pKa value are related

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pH = pKa

pH < pKa

pH > pKa

pH x pKa = 14

The state of equilibrium refers to

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State of rest

Dynamic state

Stationary state

State of inertness

In exothermic reversible reaction increase in temperature shift the equilibrium to :

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Remains unchanged.

Product side.

Reactant side.

None of above.

Addition of solid NaHCO₃in water causes ionization of NaCHO₃its K_a= 4.7 x 10^-1. Then this solution has character

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Acidic

Very weakly basic

Alkaline

Neutral

Which one of the following has no units of its K_cvalue

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The value of K_pfalls with rise in temperature

The value of K_pfalls with increasing pressure

Addition of V₂O₅catalyst increase the concentration of SO₃

The value of K_pis equal to K_c

Product of concentration of ions raised to the power equal to the co-efficient of ions in balanced equation for saturated solution of a salt is called

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Ionic product

Equilibrium constant K_c

K_w

Solubility product (K_sp)

An aqueous solution is neutral when its

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pH = 14

pH = zero

pH = 7

Kw = 10^-7

In a reversible chemical reaction having two reactants in equilibrium, if the concentration of the reactants are doubled then the equilibrium constant will

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Also be doubled

Be halved

Becomes one fourth

Remains the same

Extent to H₂ + L₂à2Hl can be increased by :

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Increasing temperature.

Increasing product.

Increasing pressure.

Adding a catalyst.

Law of mass action was given by :

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Guldberg and Waage.

Berkeley and Hartly.

Ramsay and Reyleigh.

Berthelot.

The value of K_pis greater than K_cfor a gaseous reaction when

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Number of molecules of products is greater than the reactants

Number of molecules of reactants is greater than those of products

Number of molecules of reactants and products equal

Catalyst is added

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Moles^-2dm⁺⁶

No units

Mole dm^-3

Mole^-1dm^-3

The ph of 10-3 mole dm-3 of an aqueous solution of H₂SO₄ is :

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3.0

2.7

2.0

1.5

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Total pressure

Amount of A₂and B₂

Temperature

Catalyst

Acetic acid is 1.33% ionized, In 1000 molecules of 0.1 M acetic acid the number of H⁺ions is

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1.33

13.3

1.33

1

Ifk_cof a reaction productis verylarge, it indicates that equilibrium occurs :

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With the help of a catalyst.

With no forward reaction.

At a low product concentration.

At a high product concentration.

0.1 MHCI has pH = 1.0, it is about 100 times stronger than acetic acid. Then pH of acetic acid will be

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0.1

2.0

1.3

3.0

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