Question # 1

In a given system, water and ice are in equilibrium, if the pressure is applied to the above system then

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Morc ice is formed

Amount of ice and water will remain the same

more ice is melted

both A and B

lonization of KCIO3. is suppressed by

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Increasing temperatuse

adding KCl

adding NaNO3

Decreasing temperature

For what value of Kc almost forward reaction is complete

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Kc.=10(-30)

Kc.=1

Kc = 10(30)

Kc,=0

If the temperature is inereased of following reaction, then will go in N2 +3H2 <---------> .2NH3, ∆H= -Ve

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Forward direction

Reverse direction

Remain constant

Cannot be predicted

Which one of the following has the lowest pH values

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0.1 M HCI

0.01 M HCl

0.1 M KOH

0.01 M KOH

With increase in temperature, ionic product of H2O

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Decreases

Remains same

Increases

May increase or decrease

The solubility product is only applicable for those substance whose molar concentrations is

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0.01

Equal to 1

Less than 0.01

Greater than 10

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

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

pH of an aqueous solution is 3.0 at 25°C. The hydrogen ion concentration in the solution would be

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0.001

0.01

0.0001

10(-5)

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

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9X3

3X4

27X4

9X4

Which statement is incorrect

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pH and [OH-] are inversely related to cach other

pOH and [OH-] are inversely related to each other

pH and [OH-] are directly related to each other

pOH means potential of hydroxyl ion concentration

Buffer action can be explained by except

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Common ion effect

Le-Chatelier's principle

Law of mass action

Solubility product

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 solubility product of AgCl is
2.0 x 10(-10) mol2 dm(-6). The maximum concentration Ag+ ions in the solution is:

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1.41 × 10(-5) mol. dm(-3)

1.41 × 10(-10) mol. dm(-3)

2.0 × 10(-10) mol. dm(-3)

4.0 × 10(-20) mol. dm(-3)

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

Which one increases by common ion effect except?

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Crystallization

Solubility

Association of ions

All of these

pH of 10-4 mole dm-3 of HCl

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2

4

3

5

The Kw. of water at 25 C° is given by

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10(-7)

10(-10)

10(-12)

10(-14)

Which of the following is a base according to lowery Bronsted concept?

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I-1

HCl

H3O+

NH4+1

The solubility of A2B3 is X mole dm-3. Its Ksp is?

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6X(5)

36X(5)

64X(5)

108X(5)

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