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11th Chemistry Monthly Test - 2 ( Solutions )

MABS Institution

11th Chemistry Monthly Test - 2 ( Solutions )-Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

Which of the following concentration terms is temperature independent?
I) Molarity
II) Molality
III) Normality
IV) Mole fraction

I& II
I & III
II only
II & IV

Normality of 1.25M sulphuric acid is

1.25 N
3.75 N
2.5 N
2.25 N

Correct statement among the following regarding osmosis is

Solvent flows from high concentration of solute to low concentration of solute
Solvent flows from low concentration of solute to high concentration of solute
Solute flows from high concentration to low concentration
Solute flows from low concentration to high concentration

Two liquids having vapour pressures \({ p }_{ 1 }^{ 0 }\) and \({ p }_{ 2 }^{ 0 }\) in pure state in the ratio of 2 : 1 are mixed in the molar ratio of 1 : 2. The ratio of their moles in the vapour state would be

1: 1
1: 2
2: 1
3: 2

According to Raoults law, the relative lowering of vapour pressure for a solution is equal to

mole fraction of solvent
mole fraction of solute
number of moles of solute
number of moles of solvent

200ml of an aqueous solution of a protein contains 1.26g of protein. At 300K, the osmotic pressure of this solution is found to be 2.52 × 10^–3 bar. The molar mass of protein will be (R = 0.083 L bar mol^–1 K^–1)

62.22 Kg mol^-1
12444 g mol^-1
300 g mol^-1
none of these

The molality of a solution containing 1.8g of glucose dissolved in 250g of water is

0.2 M
0.01 M
0.02 M
0.04 M

Arrange the following aqueous solutions in the order of their increasing boiling points
i) 10^-4 M NaCI
ii) 10^-3M Urea
iii) 10^-3M MgCl₂
iv) 10^-3M NaCI

(i) < (ii) < (iv) < (iii)
(ii) < (i) < (iii) < (iv)
(i) <(ii) < (iii) < (iv)
(iv) < (iii) < (i) < (ii)

In the case of osmosis, solvent molecules move from solution having

higher vapour pressure to lower vapour pressure
higher concentration to lower concentration
lower vapour pressure to higher vapour pressure
higher osmotic pressure to lower osmotic pressure

The freezing point depression constant for water is 1.86^o K Kg mol^-1. If 5g Na₂SO₄ is dissolved in 45g water, the depression in freezing point is 3.64^oC. The Vant Hoff factor for Na₂SO₄ is

2.50
2.63
3.64
5.50

Part - B

Generic 2 - Answer All Question

State Raoult law and obtain expression for lowering of vapour pressure when nonvolatile solute is dissolved in solvent.

State Raoult's law

What are ideal solution? Give example.

What is working standard?

Why is the freezing point depression of 0.1 M NaCl solution nearly twice that of 0.1M glucose solution?

Define solubility.

Solubility of a solid solute in a liquid solvent increases with increase in temperature. Justify this statement.

Part - C

Generic 3 - Answer All Question

What is the mass of glucose (C₆ H₁₂O₆) in it one litre solution which is isotonic with 6 g L^-1 of urea (NH₂ CO NH₂)?

2.82 g of glucose is dissolved in 30 g of water. Calculate the mole fraction of glucose and water.

The depression in freezing point is 0.24K obtained by dissolving 1g NaCl in 200g water. Calculate van’t-Hoff factor. The molal depression constant is 1.86 K Kg mol^-1.

What type of non-idealities are exhibited by cyclohexane-ethanol and acetone-chloroform mixture? Give reason for your answer.

Calculate the boiling point of a solution which is prepared by dissolving 68.4g of solute 8 in one kilogram of water. (Molar mass of solute 8 is 342 g mol¹, Tb= 373.1K and Kb( water) = 0.52 K kg mol¹.

Explain how non-ideal solutions shows positive deviation from Raoult's law.

What are solid solution? Give example.

Part - D

Generic 5 - Answer All Question

Explain how would you prepare the following dilute solutions from more concentrated solution
(a) 5L of 6.00 MH₂SO₄ from 18.0 MH₂SO₄
(b) 250mL of 0.5 M CaCl₂ from 3.0 M CaCl₂ solution
(c) 0.2N H₂S0₄ 500mL from 3.0 M H₂SO₄

A sample of 12 M Concentrated hydrochloric acid has a density 1.2 gL^–1 Calculate the molality

(I) Define solution.
(il) E plain the types of solutions with suitable example.

On dissolving 10.85 g of a non-electrolyte of (molar mass 97g mol^-1 ) in 87g of benzene the boiling point was elevated by 0.25K. Calculate the value of molal boiling point elevation constant of benzene.
Calculate the percent by mass of NaC lif 1.75 g of NaCI is dissolved in 7.85 g of water.

How would you determine the molar mass from osmotic pressure.

"Rate of vapourisation is reduced by presence of non-volatile solute"- Explain,

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