Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 15

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IMPORTANT

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A solution contains $0.524 g$ of camphor $(molar mass = 152 g {mol}^{- 1})$ dissolved in $36.8 g$ of ether(boiling point $= 34 . 6^{0} C$ ). The molal elevation constant of ether is ${1.94 K kg mol}^{-1}$ . The boiling point of the solution is______

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Important Questions on Solutions

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IMPORTANT

Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 16

0.1 M

solution each of glucose, sodium chloride, sodium sulphate and sodium phosphate are taken; the ratio of depression in freezing point is______

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Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 17

The depression in freezing point of a

5 %

aqueous solution of a substance '

A

’ is equal to the depression in freezing point of a

3 %

aqueous solution of a substance '

B

’ If the molecular weight of

B

is

72 g {mol}^{- 1}

, then the molecular weight of

A

is______.

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Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 18

The depression of the freezing point of a solvent(boiling point

303 K

) for a particular solution is

0.153 K

. Calculate the molal elevation constant, if the boiling point of the solution is

304.52 K

.(

K_{f} {=1.68 K kg mol}^{-1}

)

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Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 19

A solution containing

3.56 g

of a polymer in

1

litre of a solvent was found to have an osmotic pressure of

{5.2×10}^{-4}

atmosphere at

300 K

. The molecular mass of the polymer is_____.

{(R=0.082 L atm mol}^{-1} K^{-1})

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Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 20

A solution of glucose containing

9.2 g L^{- 1}

(molecular weight :

180 g/mol

) is isotonic with

3 %

solution of a non-volatile solute. The molecular weight of the solute will be_____.

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Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 21

If density of a solvent is greater than

{1 kg dm}^{-3}

, then the molarity

(M)

and molality

(m)

are related as_____.

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Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 22

The solubility of nitrogen gas at

2

atm pressure at

25^{0} C

is

{13.6 × 10}^{-4} {, mol dm}^{-3}

. Calculate the solubility of

N_{2}

gas from atmosphere at

25^{0} C

, if atmospheric pressure is

2

atmosphere and the partial pressure of

N_{2}

gas at this temperature and pressure is

1.56

atm.

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IMPORTANT

Chemistry Crash Course NEET>Chapter 8 - Solutions>Level 3>Q 23

The solubility of oxygen gas at

25^{0} C

at atmospheric pressure is

{1.43×10}^{-4} {mol dm}^{-3}

. Calculate the partial pressure of oxygen, if the Henry's law constant for oxygen is

{0.65×10}^{-4} {mol dm}^{-3} {atm}^{-1}

.