SOLUTION CHEMISTRY AND PHASE EQUILIBRIA MCQs

SOLUTION CHEMISTRY AND PHASE EQUILIBRIA MCQs

Which concentration term is helpful and used in respect of standard solutions?

1. Normality
2. Formality
3. Molarity
4. All of A, B, and C

All of A, B, and C

A 10% solution of sucrose contains 10g of sucrose in how much volume of the solution?

1. 10 mL
2. 1 mL
3. 1000 mL
4. 100 mL

100 mL

The number of gram equivalents of the solute dissolved per dm³ of the solution is called

1. Formality
2. Molarity
3. Molality
4. Normality

Normality

Which is a not true criterion for an idea solution?

1. Free energy of mixing = 0
2. Volume of mixing = 0
3. Enthalpy of mixing = 0
4. Obeys Raoult’s law

Free energy of mixing = 0

The number of moles of solute dissolved in 1000 gram of the solvent is called

1. Molality
2. Formality
3. Mole fraction
4. Molarity

Molality

Which cation undergoes hydration with the least heat?

1. K⁺
2. Na⁺
3. Mg⁺⁺
4. Li⁺

K⁺

One ppm solution of NaOH contains 1.00 mg of the solute per how much of the volume of the solution?

1. 100 mL
2. 1000 mL
3. 10 mL
4. 1 mL

1000 mL

How much amount of NaOH is needed to prepare 100 mL of IN solution?

1. 4g
2. 80 g
3. 40 g
4. 0.4 g

4g

One litre solution of NaOH contains 4.0 g of it. What will be the difference between molarity and normality? (Molar mass = 40)

1. 0.10
2. 0.05
3. Zero0

D..02

Zero

The molarity of a solution containing 4g NaOH per 500 mL of solution is (Mol mass = 40)

1. 0.1
2. 0.4
3. 0.3
4. 0.2

0.2

Iso-osmotic solutions are those which have the same

1. Vapor pressure lowering
2. Boiling point elevation
3. Molality
4. Osmotic pressure

Osmotic pressure

Which solution has highest normality?

1. 6g NaOH 100 cm³
2. 0.5N H₂SO₄
3. 8g KOH per dm³
4. 1N H₃PO₄

6g NaOH 100 cm³

The number of moles of the solute dissolved per dm³ of the solution is called

1. Molarity
2. Formality
3. Normality
4. Molality

Molarity

Solutions with components which obeys Raoult’s law over the entire composition range are considered to be

1. Ideal solutions
2. Regular solutions
3. Dilute solutions
4. Real solutions

Ideal solutions

What systems perform effectively at the top solid temperature?

1. Triethylamine- water
2. Aniline water
3. Nicotine- water
4. Phenol-water

Nicotine- water

The temperature at which two conjugate solutions change into one homogeneous solution is called

1. Consolute temperature
2. Eutectic point
3. Critical temperature
4. Transition temperature

Consolute temperature

Which solutions of HCI will exactly neutralize 10 mL of 0.2 N NaOH?

1. 20 mL of 1.0 M solution
2. 20 mL of 0.2 M solution
3. 10 mL of 0.5 M solution
4. 20 mL of 0.1 M solution

20 mL of 0.1 M solution

The law which relates the solubility of a gas to its pressure is called

1. Hennery’s law
2. Nernst law
3. Ostwald’s law
4. Raoult’s law

Hennery’s law

The number of formula weight of the solute dissolved per dm³ of the solution is called.

1. Formality
2. Normality
3. Mole fraction
4. Molality

Formality

According to Henry’s law, the mole fraction of a gas (x) dissolved in a solvent is related to the pressure of the gas

1. x=k√P
2. P= kx
3. x=k/P
4. P= k/x

x=k√P

For dilute solutions colligative properties depend on

1. The number of the solute particles and irrespective of the nature of the solute and solvent
2. The number of the solute particles and on their nature

C The number of the solute particles and nature of solute and solvent

1. The number of the particles of the solute and nature of solvent

The number of the particles of the solute and nature of solvent

Which is not a colligative property?

1. Refractive index
2. Depression in F.P.
3. Elevation of B.P.
4. Lowering of V.P.

Refractive index

Which of following property does not depend upon the number of solute particles?

1. Elevation in B.P.
2. Boiling point of the solvent
3. Depression in F.P
4. Osmotic pressure

Boiling point of the solvent

Which will have the highest boiling point at one atmosphere?

1. 0.1 M solution of BaCl₂
2. 0.1 M solution of glucose
3. 0.1 M solution of common salt
4. Both A and B

0.1 M solution of BaCl₂

The freezing point of a solvent

1. Will increase on adding a solute
2. Will not change on adding solute
3. Will decrease on adding a solute
4. None of A, B, and C

Will decrease on adding a solute

If there are only two components in a solution with mole fraction X_A and X_B, then Which relation is true?

1. X_A = 1 – X_B
2. X_A + X_B > 1
3. X_A + X_B < 1
4. X_A + X_B = 0

X_A = 1 – X_B

Which solution would exhibit abnormal colligative properties?

1. 0.1 M glucose
2. 0.1 M urea
3. 0.1 M sucrose
4. 0.1 M NaCl

0.1 M NaCl

The osmotic pressure of a solution with definite composition

1. Varies inversely as the volume and as the temperature directly
2. Varies inversely as the temperature
3. Varies directly as the volume and temperature

D Independent of the temperature and varies inversely as the volume

Varies inversely as the volume and as the temperature directly

Which solution would have the largest depression in freezing point?

1. 1% AICI₃
2. 1% KC
3. 1% BaCl₂
4. 1% glucose

1% AICI₃

Which is not a colligative property?

1. Viscosity
2. Elevation in boiling point
3. Depression in freezing point
4. Lowering of vapor pressure

Viscosity

The flow of solvent into a solution when two are separated by a semi-permeable membrane is called

1. Osmosis
2. Effusion
3. Diffusion
4. Mixing

Osmosis

Sea water is converted into fresh water based upon the phenomenon of

1. Reverse osmosis
2. Sedimentation
3. Diffusion
4. Plasmolysis

Reverse osmosis

In dilute solutions the relative lowering of vapor pressure (Δp/p°) is related to osmotic pressure (π) by the relation

1. Δp/p° = πV/RT
2. Δp/p° = πRT
3. Δp/p° = π
4. Δp/p° = πRT/V

Δp/p° = πV/RT

Which is not affected by temperature change?

1. Molality
2. Formality
3. ppm
4. Molarity

Molality

At the same temperature, 0.1 M solution of urea is isotonic with

1. 0.1 M BaCl₂ solution
2. 0.1 M NaCl solution
3. 0.05 M urea solution
4. 0.1 M glucose solution

0.1 M glucose solution

Which expression is true?

1. RT = Cπ
2. C = RT/π
3. C = π/TR
4. Cπ = 1/RT

C = π/RT

The relative lowering of vapor pressure of a solution on the addition of non-volatile solute

1. Is equal to the sum of the mole fraction of the solute and solvent
2. Is equal to the mole fraction of solute
3. Depends upon the nature of the solute
4. Depends upon the nature of the solute and solvent

Is equal to the mole fraction of solute

What is the normality of 2.3M H₂SO₄ solution?

4. 4.6N
5. 0.23N
6. 2.3N
7. 0.46N

4.6N

Starting with pure NH₄Cl, the following is established NH₄CL ⇄ NH₃ + HCl. The number of components in the system is

1. Three
2. Two
3. One
4. May be two or three

One

The number of phases of a mixture of four gases enclosed in a container is

1. Zero
2. 4-1
3. 1
4. 4

1

In terms of number of phases (P), components (C) and degrees of freedom (F), the phase rule is expressed as

1. P + F = C + 2
2. F = P + C – 2
3. P + C = F + 2
4. P – F = C + 2

P + F = C + 2

The phase rule was deduced by which of the following?

1. Henry
2. Thomson
3. Friday
4. Gibbs

Gibbs

In a system, where the chemical potential of everycomponent is the same for all phases, the equilibrium is said to be in

1. Composition equilibrium
2. Thermal equilibrium
3. Metastable equilibrium
4. Mechanical equilibrium

Composition equilibrium

In a one-component system the maximum number of phases that can coexist in equilibrium is

1. 3
2. 2
3. 1
4. 4

3

The number of degrees of freedom and number of components for a system of sodium chloride solution in water containing undissolved salt, in equilibrium with water vapor, are

1. 1, 2
2. 4, 2
3. 1, 1
4. 3, 3

1,2

The maximum degree of freedom for a pure substance under equilibrium conditions is

A  Zero

1. 3
2. 2
3. 1

2

The temperature at which the vapor pressure becomes equal to external pressure is called

1. Boiling point
2. Critical temperature
3. Consolute temperature
4. Saturation point

Boiling point

30 mL of an acid solution is neutralized by 15 mL of 0.2N base. The strength of acid solution is

1. 0.4N
2. 0.15N
3. 0.3N
4. 0.1N

0.1N

What is the pH of aqueous solution of sodium acetate solution?

1. About 3
2. About 7
3. About 2
4. About 9

About 9

The pH of the blood is maintained by which buffers

1. NH₄Cl/NH₄OH
2. HCI/NACl
3. Tris/HC
4. H₂CO₃/HCO₃

H₂CO₃/HCO₃

For a single-component, maximum degree of freedom system is:

1. 1
2. Between 3 and 6
3. 3
4. 2

2

39. Which is the strongest acid?
40. HCI
41. HNO₃
42. H₂SO₄
43. HCIO₄

HCIO₄

Which concentration term is helpful and used for very dilute solutions?

1. mg/L
2. Normality
3. Molality
4. Molarity

mg/L

The number of degrees of freedom at the triple point for the water system is

1. Zero
2. Two
3. Three
4. One

Zero

Which is partially miscible?

1. Butanol and water
2. Ethanol and water
3. HCl and water
4. Benzene and toluene

Butanol and water

The molarity of 4% NaOH solution is (Mol wt=40)

3. 3.0
4. 1.0.
5. 2.0
6. 4.0

1.0

The property which do not depend on the amount of substance are called

1. Intensive Properties
2. Additive properties
3. Extensive properties
4. Colligative properties

Intensive Properties

40. Beckman thermometer reads up to
41. 0.01K
42. 0.1 K
43. 0.001 K
44. 1K

0.01K

Hydrolysis of sodium acetate produces

1. Basic solution
2. Neutral solution
3. Acidic solution
4. None of A, B, and C

Basic solution

A 10% solution of glucose freezes at

1. 0°C
2. More than 0°C
3. Less than 0 °C
4. None of A, B, and C

Less than 0 °C

Sulfur can exist in

1. One phase
2. Four phases
3. Three phases
4. Two phases

Four phases

A 10% solution of glucose contains 1 g per

1. 400 mL
2. 100 mL
3. 1 mL
4. 10 mL

10 mL

More Physical Chemistry MCQs

1. PHYSICAL CHEMISTRY MCQs
2. CHEMICAL AND IONIC EQUILIBRIA MCQs
3. NUCLEAR CHEMISTRY MCQs
4. CHEMICAL THERMODYNAMICS MCQs
5. NANOCHEMISTRY MCQs
6. CHEMICAL KINETICS MCQs
7. SURFACE CHEMISTRY MCQs
8. COLLOIDAL STATE MCQs
9. ELECTROCHEMISTRY MCQs
10. SPECTROSCOPY MCQs
11. SOLUTION CHEMISTRY AND PHASE EQUILIBRIA MCQs
12. PHOTOCHEMISTRY AND MOLECULAR SYMMETRY MCQs
13. CHEMISTRY MCQs From all subjects of  Chemistry