Question # 1

ph of the buffer CH₃COOh + CH₃COONa is 3.76. If the mixture contains 1 molar acetic acid and 0.1 molar sodium acetate, then pKa of this buffer is

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3.76

4.76

5.76

6.76

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Increase in concentration of 1

Decrease in concentration of I₂

Increase in temperature

Increase in total pressure

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

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

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Shift reaction toward forward direction

Shift reaction backward

Lower the value of K_c

No change in reaction

On passing HCI gas through a saturated solution of commercial sodium chloride, pure crystals of NaCI are precipitated due to

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Increase in pH of the solution

Decrease in pH of the solution

Common ion effect

Increase in ionization of NaCl

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Moles per dm³

Partial pressures

Number of moles

Mole fractions

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

pH and pKa of the buffer are related by Henderson equation which is

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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.

For which system does the equilibrium constant. K_chas units of

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Le-chatlier's principle

Only adding catalyst

Decreasing pressure

Decreasing temperature

The solubility product of AgCl is 2.0 x 10^-10mol²dm^-6The maximum concentration of Ag⁺ions in the solution is

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2.0 x 10^-10mol dm^-3

1.41 x 10^-5mol dm^-3

1.0 x 10^-10mol dm^-3

4.0 x 10^-20mol dm^-3

The solubility product of AgCl is 2.0 x 10^-3 mol² dm^-6 , The maximum concentration of Ag ion in the solution is :

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2.0 x 10^-10 mol dm^-3

1.41 x 10^-10 mol dm^-3

1.0x 10^-10 mol dm^-3

4.0x 10^-10 mol dm^-3

Which of the following favours the reverse reaction in chemical equilibrium?

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Increasing the concentration of the reactant

Removal of the least one of the products at regular intervals

Increasing the concentration of one or more of the products

None of these

Which one of the following is a buffer

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HCI + NaCI solution

CH₃COOH + CH₃COONH₄solution

H₂SO₄+ CaSO₄solution

CH₃COOH + CH₃COONa

When a weak acid is dissolved in water or a weak base dissolved in water, then in both cases the conjugate acid base pair is produced. The ionization constants K_aand K_bof a pair are related with each other as

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K_a= K_b

K_a. K_b= K_w

K_a. K_w= K_b

K_b. K_w= K_a

What happens when reaction is at equilibrium and more reactant is added :

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Forward reaction rate is increased.

Forward reaction rate is decreased.

Backward reaction rate is increased.

Equilibrium remains unchanged.

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 concentration of reactants is increased by x, then equilibrium constant K becomes

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ln K/x

K/x

K + x

K

N₂ + 3H₂ ⇌2NH₃

The unit of K_c for tis reaction will be:

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mol² dm^-6

mol^-2 dm⁺⁶

mol dm^-3

mol^-1 dm⁺³

Le-chatlier's principle is applied on the reversible reaction in order to

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Determine the rate of reaction

Predict the direction of reaction

Determine the extent of reaction

Find best conditions for favorable shifting the position of equilibrium

The solubility of PbF₂is 2.6 x 10^-3mole dm^-3then its solubility product is

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2.6 x 10^-3

6.76 x 10^-6

5.2 x 10^-6

7.0 x 10^-8

Units of Kw are

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Mole dm^-3

Mole²dm^-3

Mole²dm^-6

Mole²dm^-3

H₂+ L₂----2Hl

In the above equilibrium system, if the concentration of reactants at 25°C is increased, the value K_C will :

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Remains Constant

Increases

Cecreases

Depends upon nature of reactans

pH of water is 7, if 0.01 M NaOH is added, than its pH is

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12

14

zero

10

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Shift reaction toward forward direction

Shift reaction backward

Lower the value of K_c

No change in reaction

1 mole of N₂and 2 moles of H₂are allowed to react in a 1 dm³vessel. At equilibrium 0.8 mole of NH₃is formed. The concentration of H₂in the vessel is

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0.6 mole

0.8 mole

0.2 mole

0.4 mole

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

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Increase in concentration of one of the reactants

Increase in concentration of one of the products

Removal of one of the products regularly

None of these

Reactions that proceed on both sides and never go to completion are called

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Irreversible reactions

Reversible reactions

Opposing reactions

Spontaneous reactions

Base buffer solution can be prepared by mixing

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Weak acid and its salt

Strong acid and its salt with weak base

Weak base and its salt with strong acid

Strong base and its salt with weak acid

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