Ostwald's dilution law is applicable toa)Strong electrolytes onlyb)Weak electrolytes onlyc)Non-electrolytesd)Strong as well as weak electrolytesCorrect answer is option 'B'. Can you explain this answer?

Question

Answer

Ostwald’s dilution law is the application of the law of mass action to weak electrolytes in solution.

Answer

Ostwald's dilution law is only applicable to weak electrolytes and not strong electrolytes. This is because in the case of strong electrolytes the dissociation is almost complete i.e. α (extent of dissociation) nearly equal to one so in cα. cα/c-cα, c - cα will nearly be equal to zero, so Ka will tend towards infinity.

Answer

Ostwald's dilution law is a concept in chemistry that relates to the behavior of weak electrolytes when they are diluted. It states that the degree of dissociation of a weak electrolyte is directly proportional to the square root of its dilution.

Explanation:
1. Ostwald's Dilution Law:
- Ostwald's dilution law is named after Wilhelm Ostwald, a German chemist who formulated this concept.
- It applies specifically to weak electrolytes, which are substances that partially dissociate into ions when dissolved in a solvent.
- According to this law, the degree of dissociation (α) of a weak electrolyte is directly proportional to the square root of its dilution.
- Mathematically, it can be expressed as α ∝ √C, where α represents the degree of dissociation and C represents the concentration or dilution of the weak electrolyte.

2. Weak Electrolytes:
- Weak electrolytes are substances that ionize or dissociate partially in a solution.
- They produce a small number of ions compared to the total number of molecules present.
- Examples of weak electrolytes include weak acids (acetic acid, carbonic acid) and weak bases (ammonia, methylamine).

3. Strong Electrolytes:
- Strong electrolytes, on the other hand, completely ionize or dissociate in solution.
- They produce a large number of ions compared to the total number of molecules present.
- Examples of strong electrolytes include strong acids (hydrochloric acid, sulfuric acid) and strong bases (sodium hydroxide, potassium hydroxide).

4. Applicability of Ostwald's Dilution Law:
- The law is not applicable to strong electrolytes because they completely ionize and do not exhibit a degree of dissociation.
- Strong electrolytes are assumed to be 100% dissociated in solution.
- Therefore, the law is only valid for weak electrolytes, which partially dissociate.

In conclusion, Ostwald's dilution law is applicable to weak electrolytes only. It describes the relationship between the degree of dissociation and the dilution of a weak electrolyte solution. Strong electrolytes, which completely ionize, do not exhibit a degree of dissociation and are not governed by this law.

Similar NEET Doubts

Why ostwald's dilution is not applicable to strong electrolytes?

Directions: In the following questions, A statement of Assertion (

In ncert.... it is written that descending limb of loop of Henle is ALMOST impermeable to electrolytes...may plz tell me which electrolytes can be permeable (as almost is written in ncert)

can molar conductivity of weak electroyte be greater than strong electrolyte at a particular concentration?

Which of the following is a strong electrolyte?

Top Courses for NEETView all

Biology Class 11

Daily Test for NEET Preparation

NEET Mock Test Series 2025

Topic-wise MCQ Tests for NEET

Physics Class 11

Top Courses for NEET

Top Courses for NEET

Suggested Free Tests

Related Content

About NEET

NEET Preparation Material

How to Prepare for NEET Exam?

NCERT Based Study Material

NEET Mock Tests

Other Popular Exams

Company