Question # 1

A homogeneous mixture of two or more than two chemical substances is called

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Solute

Solution

Solvent

Salvation

Vant Hoff's factor of Ca(NO₃)₂is

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1

2

3

4

Water shows maximum density at

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4°C

0°C

100°C

-4°C

0.5 M of H₂SO₄is diluted from 1 litre to 10 litre, normality of resulting solution is

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1 N

0.1 N

10 N

11 N

50 mL of 10 N H₂SO₄. 25mL of 12 N Hcl and 40 mL of 5N HNO₃are mixed and the volume of the mixture is made 100 mL by adding water. The normality of resulting will be

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1 N

2 N

3 N

9 N

Mixture of alcohol and water can be separated by

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Solvent extraction techniques

Crystallization

Precipitation and filtration

Fractional distillation

The osmotic pressure of solution increases if

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Temperature is decreased

Solution constant is increased

Number of solute molecules are increased

Volume is increased

Which is independent of temperature

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Molarity

Molality

Normality

Mole fraction

The vant Hoff factor (1) accounts for

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Degree of solubilisation of solute

The extent of dissolution of solute

The degree of decomposition of solution

Which one of the following is used as antifreeze in the radiator

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Methanol

Ethanol

Ethylene glycol

Glycerin

Isotonic solutions have same

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Molar concentration

Molality

Normality

None of these

The number of moles of solute in 1000g (1 Kg) of the solvent is called :

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Molarity

Normality

Mole fraction

Which one of the following has discontinuous solubility curve

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CaCI₂6H₂O

NaCI

KCI

NaNO₃

Compared to a 1.0M aqueous solution of calcium chloride will have

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The same freezing and boiling point

A lower freezing point and lower boiling point

A lower freezing point and higher boiling point

A higher freezing point and higher boiling point

Elevation of boiling point is measured by

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Beckmann's apparatus

Lands Berger's method

Antifreeze apparatus

None of these above

Hydrochloric acid available in the laboratory is 36% w/w. The density of HCl solution is 1.19 g cm^-3. The molarity of HCl solution is

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10.23 moles dm^-3

11.55 moles dm^-3

11.73 moles dm^-3

12.67 moles dm^-3

The solutions of NaCl and KCl are prepared separately by dissolving same amount of solute in water, which of the following statements is true fro these solutions ?

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KCl solution will have higher boiling point than NaCl solution.

Both the solutions have same boiling points.

KCl and NaCl solutions possess same vapour pressure.

KCl solution possesses lower freezing point than NaCl solution.

According to Raoult's law

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Relative lowering of V.P. is equal to mole fraction of solute

The lowering of V.P. is directly proportional to mole fraction of solute

V.P. of solvent above solution is equal to product of V.P. of pure solvent and mole fraction of solvent ins solution

All of the above

What mass of NaOH is required to prepare 2.5 dm³of 1.5 M NaOH solution

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130 g

140 g

150 g

160 g

A one thousand dm³sample of water contains one gram of iron (iii) ions what is the concentration in parts per million of Fe^3f(eq) in parts per million

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0.001

0.01

0.1

1.0

The weight of pure NaOH required to prepare 250 cm³of 0.1 N solution is

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4 g

1 g

2 g

5 g

Aqueous solution of glucose C₆H₁₂O₆, boils at 100.052°C. The solution contains

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180 grams glucose in 1 kg water

18 grams glucose in 1 kg water

1.8 grams glucose in 1 kg water

3.6 grams glucose in 1 kg

Precipitation will occur until the ionic product becomes

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Equal to K_sp

Lesser than K_sp

Greater than K_sp

None of these

Which of the following half molar solutions will have lowest freezing point

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Solution of non-volatile, none electrolyte

Solution of non volatile, weak electrolyte

Solution of non volatile strong electrolyte

Solution of volatile, non electrolyte

In azeotropic mixture showing negative deviation form Raoult's law show

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Higher b.p. than either

Lower b.p. than either

No change in b.p.

None of these

Molarity of pure water is :

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33.3

55.5

44.4

66.6

Hydrolysis of potassium acetate produces

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Acidic solution

Neutral solution

Basic solution

None of these

The molar boiling point constant is the ration of elevation in boiling point to :

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Molarity

Mole fraction of solvent

Mole fraction of solute.

If 5.85 of NaCI are dissolved in 90g of water the mole fraction of NaCI is

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0.1

0.01

0.2

0.0196

The weight of pure NaOH required to prepare 250 cm³of 0.1 N solution is

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4 g

1 g

2 g

5 g

Ifα us the degree of dissociation of Na₂SO₄the vant Hoff's factor (1) used for calculating the molecular mass is

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1 +α

1 -α

1 + 2α

1 - 2α

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