Definition of solvent and solute with examples, in chemistry , many substances around us exist not as pure materials but as mixtures. One of the most important types of mixtures is a solution, and to understand solutions, it is essential to know the meaning of solute and solvent. These two terms form the foundation of solution chemistry and are frequently asked in school-level and competitive examinations.

In definination of solvent and solute with examples , a solute is the substance that gets dissolved in a solution. It is usually present in a smaller amount. A solvent is the substance that dissolves the solute and is present in a larger amount. When a solute dissolves completely in a solvent, a homogeneous solution is formed, meaning the mixture has the same composition throughout.

For example, when common salt is added to water, salt dissolves in water to form salt solution. In this case, salt is the solute and water is the solvent. Similarly, when sugar dissolves in water, sugar acts as the solute while water acts as the solvent. These are simple examples commonly used to explain the concept.

In definition of solvent and solute with examples, the most widely used solvent is water, which is often called the universal solvent because it can dissolve many substances such as salts, acids, bases, and sugars. However, not all solutes dissolve in water. For example, oil does not dissolve in water. Instead, oil dissolves in non-polar solvents like petrol or benzene. This shows that the nature of both solute and solvent plays an important role in dissolution.

Solvents are not always liquids. In alloys like brass, zinc is the solute and copper is the solvent, even though both are solids. In air, oxygen and carbon dioxide are solutes, while nitrogen acts as the solvent because it is present in the largest amount. These examples show that solutes and solvents can exist in solid, liquid, or gaseous states.

Understanding the difinition of  solvent and s with examples helps aspirants grasp more advanced topics such as concentration units, colligative properties, and chemical reactions in solutions.

 30 MCQs on Definition of Solvent and Solute with Examples:

1.

The density of NaOH solution is 1.2 g cm⁻³. The molality of this solution is ___ m. (Nearest integer)
[Na = 23, O = 16, H = 1; density of H₂O = 1.0 g cm⁻³]

a) 5
b) 25
c) 20
d) 2

Answer: a

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2.

100 mL of Na₃PO₄ solution contains 3.45 g of sodium. The molarity is ____ ×10⁻² mol L⁻¹. (Nearest integer)

a) 50
b) 25
c) 500
d) 250

Answer: a

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3.

Volumes of 1 M NaOH needed to neutralize 50 mL of 1 M H₃PO₃ and 100 mL of 2 M H₃PO₂ respectively are:

a) 100 mL and 100 mL
b) 100 mL and 50 mL
c) 100 mL and 200 mL
d) 50 mL and 50 mL

Answer: c

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4.

A 6.50 molal KOH solution has density 1.89 g cm⁻³. Molarity is ____ mol dm⁻³. (Nearest integer)

a) 9
b) 19
c) 0.9
d) 1.9

Answer: a

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5.

4.5 g of compound A (M = 90) in 250 mL aqueous solution. Molarity = x ×10⁻¹ M. x is:

a) 2
b) 4
c) 1
d) 3

Answer: a

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6.

AB dissociates 75%. A solution shows ΔTb = 2.5 K. Molality is ____ (Nearest integer).
[Kb = 0.52 K kg mol⁻¹]

a) 3
b) 4
c) 5
d) 6

Answer: a

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7.

1 molal electrolyte A₂B₃ is 60% ionised. Boiling point at 1 atm is ____ K (Nearest integer).
[Kb (H₂O) = 0.52]

a) 375 K
b) 400 K
c) 350 K
d) 300 K

Answer: a

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8.

Ideal solution A and B at 350 K: vapour pressures of pure A and B are 7×10³ Pa and 12×10³ Pa. Solution has 40 mol% A. Vapour composition is:

a) Xa = 0.37; Xb = 0.63
b) Xa = 0.28; Xb = 0.72
c) Xa = 0.40; Xb = 0.60
d) Xa = 0.76; Xb = 0.24

Answer: b

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9.

OH⁻ concentration in mixture of 5.0 mL of 0.0504 M NH₄Cl and 2.0 mL of 0.0210 M NH₃ is x ×10⁻⁶ M. x is (Nearest integer).
[Kw = 10⁻¹⁴, Kb = 1.8×10⁻⁵]

a) 3
b) 6
c) 4
d) 9

Answer: a

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10.

3.0 g ethanoic acid in 50 g benzene has ____ molality.
(Atomic masses: H=1, C=12, O=16)

a) 1
b) 0.1
c) 1.5
d) 0.06

Answer: a

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11.

In basic medium CrO₄²⁻ oxidizes S₂O₃²⁻ to SO₄²⁻ and becomes Cr(OH)₄⁻. Volume of 0.154 M CrO₄²⁻ required for 40 mL of 0.25 M S₂O₃²⁻ is ____ mL (Nearest integer):

a) 173
b) 100
c) 153
d) 133

Answer: a

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12.

Density of 2 M ethylene glycol solution is 1.11 g/mL. Molality is approximately:

a) 1.92
b) 1.57
c) 2.05
d) 2.15

Answer: c

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13.

A 6.50 molal KOH solution has density 1.89 g cm⁻³. Molarity is ____ mol dm⁻³. (Nearest integer)

a) 9
b) 3
c) 6
d) 2

Answer: a

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14.

AB dissociates 75%. A solution shows ΔTb = 2.5 K. Molality is ____ (Nearest integer).
[Kb = 0.52]

a) 3
b) 1
c) 6
d) 4

Answer: a

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15.

NaOH is titrated with 1.25 M oxalic acid. Titre values: 4.5, 4.5, 4.4, 4.4, 4.4 mL. Acid taken = 10.0 mL. Molarity of NaOH is ____ M (Nearest integer):

a) 6
b) 3
c) 1
d) 4

Answer: a

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16.

4.5 g compound A (MW=90) in 250 mL solution. Molarity = x ×10⁻¹ M. x is:

a) 2
b) 3
c) 1
d) 4

Answer: a

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17.

50 mL of 0.2 N HCl is titrated with 0.1 N NaOH. After adding 50 mL NaOH, remaining titration is completed using 0.5 N KOH. Volume of KOH required is:

a) 10 mL
b) 11 mL
c) 12 mL
d) 10.5 mL

Answer: a

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18.

Conc. HNO₃ is 63% by mass, density 1.4 g/mL. Volume needed to prepare 250 mL of 1.2 M HNO₃ is:

a) 18
b) 21.42
c) 20
d) 14.2

Answer: b

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19.

Vapour pressure of solvent decreases by 20 mm Hg on adding solute. Mole fraction of solute is 0.5. What mole fraction of solvent is needed for decrease to be 10 mm Hg?

a) 3/4
b) 2/3
c) 1/4
d) 3/2

Answer: a

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20.

0.63 g oxalic acid is dissolved to obtain 250 cm³ solution. Normality is:
[Oxalic acid (COOH)₂·2H₂O]

a) 0.05 N
b) 0.01 N
c) 0.04 N
d) 0.02 N

Answer: c

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21.

100 mL solution contains 10 g urea. It is hypertonic w.r.t. 100 mL glucose solution containing W g. Which is correct?

a) W = 10 g
b) W < 30 g
c) W > 30 g
d) W < 10 g

Answer: b

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22.

Equivalent weight of KMnO₄ in acidic and strongly alkaline medium respectively:

a) 158; 79
b) 31.6; 158
c) 158; 158
d) 31.6; 79

Answer: b

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23.

Volumes of 1 M NaOH required to neutralize 50 mL of 1 M H₃PO₃ and 100 mL of 2 M H₃PO₂ are:

a) 50 mL and 50 mL
b) 100 mL and 50 mL
c) 100 mL and 200 mL
d) 100 mL and 100 mL

Answer: c

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24.

500 mL CaCl₂ solution contains 3.01×10²² chloride ions. Molarity is:

a) 0.05 M
b) 0.01 M
c) 0.10 M
d) 0.02 M

Answer: a

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25.

122 g benzoic acid in 1000 g benzene shows ΔTb = 1.4. If solute is dimerised 80%, boiling point of pure benzene is:

a) 420 K
b) 370 K
c) 540 K
d) 460 K

Answer: a

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26.

Solution saturated with SrCO₃ and SrF₂ has [CO₃²⁻] = 1.2×10⁻⁸ M. Concentration of F⁻ is:
Ksp(SrCO₃)=7×10⁻¹⁰, Ksp(SrF₂)=7.9×10⁻¹⁰

a) 3.7×10⁻³ M
b) 3.2×10⁻³ M
c) 5.7×10⁻⁴ M
d) 3.7×10⁻² M

Answer: d

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27.

Mole fraction of ethanol in water is 0.08. Molality is:

a) 6.32 mol kg⁻¹
b) 4.83 mol kg⁻¹
c) 3.82 mol kg⁻¹
d) 2.84 mol kg⁻¹

Answer: b

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28.

20 g NaOH dissolved in 1250 mL solvent (density 0.8 g/mL). Molality is:

a) 0.02 mol kg⁻¹
b) 0.08 mol kg⁻¹
c) 0.25 mol kg⁻¹
d) 0.5 mol kg⁻¹

Answer: d

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29.

In qualitative analysis, NH₄Cl is added before NH₄OH to:

a) Increase [OH⁻] concentration
b) Make [HCl]
c) Decrease [OH⁻] concentration
d) Statement is wrong

Answer: c

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30.

Current for 30 min collects 11.2 L H₂ at NTP. Same current for 1 hour deposits how much Ag?

a) 216 g
b) 108 g
c) 16 g
d) 6 g

Answer: a

Conclusion on Definition of Solvent and Solute with Examples

The concepts of definition of solvent and solute with examples are fundamental to understanding chemistry and its applications in daily life. Every solution, whether simple or complex, is based on the interaction between a solute and a solvent. From drinking water and medicines to industrial chemicals and biological fluids, solutions play a vital role, and the correct identification of solute and solvent is essential.

In definition of  solvent and solute  with examples, solvents provide a medium in which solute particles can move freely, allowing chemical reactions to occur more easily. This is why most chemical reactions are carried out in solutions. In biological systems, water acts as a solvent that carries nutrients, gases, and waste products within the body. In plants, water dissolves minerals from the soil and transports them to different parts of the plant.

In definition of  solvent and solute with examples ,the choice of solvent is also very important. Some solutes dissolve only in specific solvents, following the principle “like dissolves like.” This principle is widely used in laboratories, industries, pharmaceuticals, and environmental science. Selecting the right solvent can affect solubility, reaction rate, and product formation.

In conclusion, understanding the definition of  solvent and solute with examples builds a strong foundation in chemistry. It helps aspirants connect textbook concepts with real-life situations and prepares them for advanced topics and competitive examinations.