Question # 1

Which substances are mixed to form a buffer solution?

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A strong acid and its salt of a strong base

Strong acid and its salt of weak base

Weak acid and its salt of strong base

Weak acid and its salt of weak base

A solution can be

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Dilute and concentrated

Saturated and dilute

Saturated and unsaturated

Supersaturated and saturated

Two solutions of NaCl and KCl are prepared separately by dissolving 0.1 M of the solute in water. Which of the following statements is not true for these solution

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KCl solution will have higher boiling point than NaCl solution

Both the solutions have same boiling

KCl and NaCl solution possess same vapour pressure

KCl solution possess same freezing point at NaCl solution

The molarity of solution containing 14.5 grams urea (N₂H₄CO) dissolved in 100 cm³of the solution is

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1 molar

0.1 molar

0.2 molar

0.25 molar

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

The concentration units independent of temperature would be

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Normality

Mass-volume precent

Molality

Molarity

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

The molarity of the solution containing x grams (NH₄)₂SO₄in 500 cm³of the solution is 0.6 what is x

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39.6

45.1

40.5

42.7

A solutiion of 0.5 mole camphor in 100 grmas chloroform (K_b= 0.322) has rise in boiling point than that of chloroform by

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0.81°C

1.61°C

1.81°C

0.61°C

Which of the following solution has the highest boiling point

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5.85% solution of sodium chloride

18.0% solution of glucose

6.0% solution of urea

All have the same 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

The process in which solvent particles surround solute particles is called

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Hydrolysis

Hydration

Solvation

Dissolution

Maximum freezing point falls in

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Camphor

Naphthalene

Benzene

Water

A solution contains 1.2046 x 10²⁴hydrochloric acid molecules in one dm³of the solution. The strength of the solution is

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6 N

2 N

4 N

8 N

Azeotropic mixture of HCl and water has

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48% HCl

22.2% HCl

36% HCl

20.2% HCl

What is the molarity of a solution containing 15.0 g urea in 500 cm³of solution

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0.5 M

1 M

1.5 M

2 M

A solution sucrose is 34.2%. The volume of solution containing one mole of solute :

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342cm³

1000cm³

500cm³

242cm³

Saturated solution of NaCl on heating becomes

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Super saturated

Unsaturated

Remains saturated

None

What will be the molarity of solution if 103 g (NH₄)₂SO₄is dissolved per 600 cm³of water

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2.32 M

3.32 M

4.32 M

1.30 M

The ratio of moles of a particular component of solution to total moles of all components of solution is :

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Mole fraction.

Molality.

Molarity.

Normality.

Number of moles of solute dissolved in 1 Kg of solvent is knowns as

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Molarity

Formality

Molality

Mole fraction

10% aqueous solution of NaCI has molarity

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1.7 M

2.7 M

0.17 M

3.7 M

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

10g Of NaOH Has Been Dissolved Perdm³of solution. The morality of solution is :

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0.025 M

1.5 M

0.1 M

.25 M

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

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

Mixture of alcohol and water can be separated by

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Solvent extraction techniques

Crystallization

Precipitation and filtration

Fractional distillation

The molarity of toluene solution in benzene is 0.22 if 5 grams of toluene dissolved, then mass of benzene is grams is

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267

260

240

247

Which inorganic precipitate acts as semipermeable membrane?

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Calcium sulphate

Barium oxalate

Nickel phosphate

Copper ferrocyanide

The process in which the solvent molecules are surrounded and interact with solute ions or molecules is called

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Solvation

Hydration

Hydrogenation

None

Cane sugar is not soluble in benzene but soluble in water because

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Cane sugar is a macro molecule

Cane sugar is an ionic compound

Can sugar has hydrogen bonding

Can sugar is an organic molecule

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