Question # 1

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

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

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)

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 one increases by common ion effect except?

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Crystallization

Solubility

Association of ions

All 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

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

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6X(5)

36X(5)

64X(5)

108X(5)

Consider the reaction

PCI5 (g) <---------> PCl3 (g) +Cl2 (g) in a closed container at equilibrium. At a fixed temperature, what will be the effect of adding more PCl5 on the equilibrium constant

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It increases

It remains unaffected

It decreases

Can't be predicted without Ki

lonization of KCIO3. is suppressed by

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Increasing temperatuse

adding KCl

adding NaNO3

Decreasing temperature

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

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)

A basic buffer solution can be prepared by mixing

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Strong acid and its salt with weak base

Weak base and its salt with strong acid

Strong base and its salt with weak acid

Weak acid and its salt with strong base

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

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

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9X3

3X4

27X4

9X4

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 decomposition of N2O4 to NO2 is carried out at 280°C in chloroform. When quilibrium is reached. 0.2 moles of N2O4 and 0.02 mole of NO2 are present in 1:1 ratio The equilibrium constant for the reaction N2O4------> 2NO2 is

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0.01

0.001

0.02

0.002

The value of Kc for H2O at 25C° is

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1x10 (-14)mole dm-3

14 mol dm-3

1.86×10(-16) mol dm-3

1.0x10 (-7)moldm-3

A basic buffer solution can be prepared by mixing?

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Weak acid and its salt with strong base

Weak base and its salt with strong acid

Strong acid and its salt with weak base

Strong base and its salt with strong acid

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

The most suitable temperature for preparing ammonia gas is

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250℃

450℃

350℃

550℃

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

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