Question # 1

If Kc value is small then equilibrium position will shift

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Towards left

Remains unchanged

Towards right

lt is always constant value

What will be the pH of 1.0 mol dm-3 of NH4OH, which is 1% dissociated

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2

12

0

2.7

If the concentration of salt is greater than the acid in buffer solution, then the

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pH = pKa

pH = pKb

pH > pKa

pH < pKb

With increase in temperature, ionic product of H2O

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Decreases

Remains same

Increases

May increase or decrease

For what value of Kc almost forward reaction is complete

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Kc.=10(-30)

Kc.=1

Kc = 10(30)

Kc,=0

A certain buffer solution contains equal cone. of X- and HX. Ka for HX is 10(-8). The pH of buffer is

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3

11

8

14

Which Henderson equation is not correct?

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pH= pKa +log [ salt/acid]

pH = pKa - log [ salt/acid ]

pH= pKa - log[ acid/salt ]

Pka = pH - log [ salt/acid ]

Which one is very weak acid

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HF

HCI

H2CO3

H2O

In which of the following Equilibria will Kc and Kp have not the same value

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2HI <--------> H2+I2

2SO2 + O2 <--------> 2SO3

N2 + O2 <---------> 2NO

All of these

In the reaction A2 (g) + 4B2 (g) <-----------> 2AB4 (g) such that ∆H < 0, the formation of AB4(g) will be favoured at

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Low temperature and high pressure

Low temperature and low pressure

High temperature and low pressure

High temperature and high pressure

According to Lowery Bronsted concept, which of the following is considered as an acid?

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BF3

OH-

H3O+

Cl-

When HCI gas is passed through saturated solution of rock salt, the solubility of NaCl

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Increases

May increase or decrease

Decreases

None of these

The Kw. of water at 25 C° is given by

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10(-7)

10(-10)

10(-12)

10(-14)

The solubility of Fe(OH)3 is 'x' mole per dm3. Its Ksp would be

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9X3

3X4

27X4

9X4

Which one is correct about conjugate acid-base concept?

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Conjugate base of a very weak acid is relatively very strong

Conjugate base of a very weak acid is relatively very weak

Conjugate base of a very strong acid is relatively very weak

Both A and C

The pH of ideal buffer is

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10

7

Less than 7

0

The pH of neutral water is 6.8 then the temperature of H2O is

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25°C

More than 25°C

less than 25 C°

Not predicted

The most suitable temperature for preparing ammonia gas is

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250℃

450℃

350℃

550℃

At equilibrium, the concentration of reactants and products are

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Constant

Maximum

Different

Equal

The oxidation of SO2 to SO3 is exothermic reaction. The yield of SO3 will be maximum if

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Temperature is increased and pressure is kept constant

Temperature is reduced and pressure is increased

Both temperature and pressure are increased

For the reaction H2(g) +I2 (g) <---------> 2Hl(g). The equilibrium constant changes with

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Total pressure

Catalyst

Concentration of H2 and I2

Temperature

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