Question # 1

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

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

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)

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

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

An excess af silver nitrate is added to the aqueous barium chloride and the precipitate is removed by filtration. What are the main ions in the filtrate?

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Ag+ and NO3-, only

NO3- and Ba+2 only

Ag+ and NO-3, and Ba+2 only

CI- and NO-3, and Ba+2 only

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

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

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

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

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

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)

The pH of ideal buffer is

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10

7

Less than 7

0

The most suitable temperature for preparing ammonia gas is

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250℃

450℃

350℃

550℃

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

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)

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

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 best buffer those have

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pH = pKa

pH > pKa

pOH < pKb

pKa =0

For N2: +3H2<--------> 2NH3, if Kc is 1 than value of Kp at 273K would be

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1/22.414

1/(22.414)2

22.414

11.207

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