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The size of particles in suspension, true solution and colloidal solution varies in the order
  • a)
    suspension > colloidal > true solution
  • b)
    true solution > suspension > colloidal
  • c)
    suspension > colloidal = true solution
  • d)
    none of these
Correct answer is option 'A'. Can you explain this answer?
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The size of particles in suspension, true solution and colloidal solu...
Particle Size in Suspension, True Solution and Colloidal Solution

Suspension, true solution, and colloidal solution are different types of mixtures, each with varying particle sizes. The size of particles in suspension, true solution, and colloidal solution varies in the order:

Suspension > Colloidal > True Solution

Let's understand this order in detail:

Suspension
- A suspension is a mixture in which particles are suspended in a liquid or gas but are too large to stay uniformly distributed.
- The particles in a suspension are visible to the naked eye and settle down when left undisturbed.
- The particle size in a suspension is typically greater than 1000 nanometers (nm), which is considered to be macroscopic.
- Examples of suspension include muddy water, blood, and sand in water.

Colloidal Solution
- A colloidal solution is a mixture in which the particle size is intermediate between that of a true solution and a suspension.
- The particles in a colloidal solution are too small to be seen by the naked eye but are large enough to scatter light, making the solution appear hazy or opaque.
- The particle size in a colloidal solution is typically between 1 and 1000 nm.
- Examples of colloidal solutions include milk, ink, and blood plasma.

True Solution
- A true solution is a homogeneous mixture in which the particles are so small that they cannot be seen by the naked eye or even by a microscope.
- The particles in a true solution are molecules or ions that are evenly dispersed throughout the solvent.
- The particle size in a true solution is typically less than 1 nm.
- Examples of true solutions include sugar dissolved in water and salt dissolved in water.

Conclusion
In summary, the size of particles in suspension, true solution, and colloidal solution varies in the order: suspension > colloidal > true solution. This order is based on the particle size, with suspensions having the largest particles and true solutions having the smallest particles.
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Community Answer
The size of particles in suspension, true solution and colloidal solu...
Particle size
True solution - Size < 1="" />
Colloidal solution - 1 nm < size="" />< 1000="" />
Suspension - Size > 1000 nm
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Read the passage given below and answer the following questions:Some colloids are stable by their nature, i.e., gels, alloys, and solid foams. Gelatin and jellies are two common examples of a gel. The solid and liquid phases in a gel are interspersed with both phases being continuous. In most systems, the major factor influencing the stability is the charge on the colloidal particles. If a particular ion is preferentially adsorbed on the surface of the particles, the particles in suspension will repel each other, thereby preventing the formation of aggregates that are larger than colloidal dimensions. The ion can be either positive or negative depending on the particular colloidal system, i.e., air bubbles accumulate negative ions, sulphur particles have a net negative charge in a sulphur sol, and the particles in a metal hydroxide sol are positively charged. Accumulation of charge on a surface is not an unusual phenomenon-dust is attracted to furniture surfaces by electrostatic forces. When salts are added to lyophobic colloidal systems the colloidal particles begin to form larger aggregates and a sediment forms as they settle. This phenomenon is called flocculation, and the suspension can be referred to as flocculated, or colloidally unstable. If the salt is removed, the suspension can usually be restored to its original state; this process is called deflocculation or peptization. The original and restored colloidal systems are called deflocculated, peptized, or stable sols. Why does a small amount of salt have such a dramatic effect on the stability of a lyophobic colloidal system? The answer lies in an understanding of the attractive and repulsive forces that exist between colloidal particles. Van der Waals forces are responsible for the attractions, while the repulsive forces are due to the surface charge on the particles. In a stable colloid, the repulsive forces are of greater magnitude than the attractive forces. The magnitude of the electrical repulsion is diminished by addition of ionized salt, which allows the dispersed particles to aggregate and flocculate. River deltas provide an example of this behaviour. A delta is formed at the mouth of a river because the colloidal clay particles are flocculated when the freshwater mixes with the salt water of the oceanQ. The particles in suspension will repel each other, thereby preventing the formation of aggregates that are larger than colloidal dimensions. This statement explains

Read the passage given below and answer the following questions:Some colloids are stable by their nature, i.e., gels, alloys, and solid foams. Gelatin and jellies are two common examples of a gel. The solid and liquid phases in a gel are interspersed with both phases being continuous. In most systems, the major factor influencing the stability is the charge on the colloidal particles. If a particular ion is preferentially adsorbed on the surface of the particles, the particles in suspension will repel each other, thereby preventing the formation of aggregates that are larger than colloidal dimensions. The ion can be either positive or negative depending on the particular colloidal system, i.e., air bubbles accumulate negative ions, sulphur particles have a net negative charge in a sulphur sol, and the particles in a metal hydroxide sol are positively charged. Accumulation of charge on a surface is not an unusual phenomenon-dust is attracted to furniture surfaces by electrostatic forces. When salts are added to lyophobic colloidal systems the colloidal particles begin to form larger aggregates and a sediment forms as they settle. This phenomenon is called flocculation, and the suspension can be referred to as flocculated, or colloidally unstable. If the salt is removed, the suspension can usually be restored to its original state; this process is called deflocculation or peptization. The original and restored colloidal systems are called deflocculated, peptized, or stable sols. Why does a small amount of salt have such a dramatic effect on the stability of a lyophobic colloidal system? The answer lies in an understanding of the attractive and repulsive forces that exist between colloidal particles. Van der Waals forces are responsible for the attractions, while the repulsive forces are due to the surface charge on the particles. In a stable colloid, the repulsive forces are of greater magnitude than the attractive forces. The magnitude of the electrical repulsion is diminished by addition of ionized salt, which allows the dispersed particles to aggregate and flocculate. River deltas provide an example of this behaviour. A delta is formed at the mouth of a river because the colloidal clay particles are flocculated when the freshwater mixes with the salt water of the oceanQ. When Van der Waals forces are greater than forces due to the surface charge on the particles,

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