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11th Chemistry Monthly Test - 1 ( Solutions )

MABS Institution

11th Chemistry Monthly Test - 1 ( Solutions )-Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

What would be the value of van't Hoff factor for a dilute solution of K₂SO₄ in water

3
2
1
4

In which of the following compound the solubility decreases with increase of temperature?

sodium chloride
ammonium nitrate
eerie sulphate
calcium chloride

Assertion: An ideal solution obeys Raoults Law
Reason: In an ideal solution, solvent-solvent, as well as solute-solute interactions, are similar to solute-solvent interactions.

both assertion and reason are true and reason is the correct explanation of assertion
both assertion and reason are true but reason is not the correct explanation of assertion
assertion is true but reason is false
both assertion and reason are false

Which of the following gas should have maximum value for k_H?

He
H₂
N₂
CO₂

An azeotropic solution of two liquids has a boiling point lower than either of the boiling points of the two liquids when it

shows negative deviation
shows positive deviation
shows no deviation
is unsaturated

If solute and solvent interactions are more than solute - solute and solvent - solvent interactions then

It is ideal solution
It is non-ideal solution with positive deviation
It is non-ideal solution with negative deviation
Can't be predicted

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

Two liquids X and Y on mixing gives a warm solution. The solution is

ideal
non-ideal and shows positive deviation from Raoults law
ideal and shows negative deviation from Raoults Law
non-ideal and shows negative deviation from Raoults Law

Which of the following aqueous solutions has the highest boiling point?

0.1 M KNO₃
0.1 M Na₃PO₄
0.1 BaCl₂
0.1 M K₂SO₄

Normality of 1.25M sulphuric acid is

1.25 N
3.75 N
2.5 N
2.25 N

Part - B

Generic 2 - Answer All Question

State Henry's law.

A 0.25 M glucose solution at 370.28 K has approximately the pressure as blood does what is the osmotic pressure of blood?

What is osmosis?

Show that the sum of mole fraction of a solution is equal to one.

The antiseptic solution of iodopovidone for the use of external application contains 10 % w/v of iodopovidone. Calculate the amount of iodopovidone present in a typical dose of 1.5 mL.
What are colligative properties? Give example.

Give the reason behind the lowering of vapour pressure in the dissolution of NaCI in water?

Define colligative properties.

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

Define (i) molality (ii) Normality.

Part - C

Generic 3 - Answer All Question

0.75 g of an unknown substance is dissolved in 200 g water. If the elevation of boiling point is 0.15 K and molal elevation constant is 7.5 K Kg mol^-1 then, calculate the molar mass of unknown substance

Write a brief note on ideal solutions.

What is meant by positive and negative deviations from Raoult's law and hoW is the sign of ΔH_mixrelated to positive and negative deviations from Raoult's law?

Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride

Define
(i) freezing point
(ii) Depression in freezing point. Explain with graph.
Explain the above variation in solubility with respect to temperature for selective compounds.

What volume of 4M HCl and 2M HCl should be mixed to get 500 mL of 2.5 M HCl?

Calculate the molarity of each of the following solutions

Answer the following.
(i) Define Van't Hoff factor
(ii) Write the i value for CH₃COOH and NaCI.
(iii) What does the following conditions reveal?
i =1, i < 1 and i > 1

NaOH and HCI react to form NaCI and H₂0 (a) What volume of 0.250 M NaOH solution contains 0.110 mol of NaOH (b) What of volume of 0.20 M NaOH is required to exactly react with 0.150mol HCI?

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

(I) Define Solubility
(ii) Explain about the factors that influences the solubility

Calculate the mass of acetic acid to be dissolved in 50g of water to lower its melting point by 1.5° C. (K_f = 1.86 K kg mol^-1).

Write note on reverse osmosis and explain its application in desalination of sea water.

How would you determine the molar mass from osmotic pressure.

Explain about the factors that are responsible for deviation from Raoult's law.
(i) What is Osmotic pressure and how is it related to the molecular mass of a non volatile substances?
(ii) What advantage the osmotic pressure method has over the elevation of boiling point method for determining the molecular mass?

Calculate the mole fractions of benzene and naphthalene in the vapour phase when an ideal liquid solution is formed by mixing 128 g of naphthalene with 39 g of benzene. It is given that the vapour pressure of pure benzene is 50.71 mmHg and the vapour pressure of pure naphthalene is 32.06 mmHg at 300 K.

Calculate the percent by mass of NaC lif 1.75 g of NaCI is dissolved in 7.85 g of water.

2.56 g of Sulphur is dissolved in 100g of carbon disulphide. The solution boils at 319. 692 K. What is the molecular formula of Sulphur in solution The boiling point of CS₂ is 319. 450K. Given that K_b for CS₂ = 2.42 K Kg mol^-1.

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