Question # 1

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

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

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BF3

OH-

H3O+

Cl-

Buffer action can be explained by except

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Common ion effect

Le-Chatelier's principle

Law of mass action

Solubility product

pH of 10-4 mole dm-3 of HCl

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2

4

3

5

In a saturated solution of AgCl, the molar concentration of Ag+ and Cl- is 1.0x10(-5)M each. What is the value of Ksp

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1.0x10(-5)

1.0x10(-15)

0.1x10(-5)

1.0x10(-10)

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

Which one increases by common ion effect except?

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Crystallization

Solubility

Association of ions

All of these

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

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

Buffer solutions are used in except

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Clinical analysis

Nutrition

Soil science

Qualitative analysis

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

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

At equilibrium, the concentration of reactants and products are

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Constant

Maximum

Different

Equal

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

Correct relationship b/w Kc and Kp can be written as

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Kp=, Kc(R)∆n

Kc=Kp (RT)∆n

Kp.= Kc.(RT)∆n

Kp=Kc (R/N)∆n

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

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9X3

3X4

27X4

9X4

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

lonization of KCIO3. is suppressed by

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Increasing temperatuse

adding KCl

adding NaNO3

Decreasing temperature

What will be the pH of 1.0 mol dm -3 of H2X, which is only 50% dissociated

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1

0

2

Less than 0

Which one is best buffer those have

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pH = pKa

pH > pKa

pOH < pKb

pKa =0

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