Limiting Conductivity: Strong vs Weak Electrolytes

In summary, strong electrolytes completely dissociate into ions when dissolved in water, while weak electrolytes only partially dissociate. The strength of an electrolyte affects its conductivity, with stronger electrolytes having higher conductivity due to more available ions. A simple conductivity test can determine if a substance is a strong or weak electrolyte, with strong electrolytes conducting electricity well and weak electrolytes only to a limited degree. Factors such as temperature, concentration, and other substances in the solution can also affect the strength of an electrolyte. Examples of strong electrolytes include ionic compounds like sodium chloride and acids like hydrochloric acid, while weak electrolytes include weak acids like acetic acid and weak bases like ammonia.
  • #1
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Why is the limiting conductivity of a weak electrolyte higher than the one for a strong electrolyte?
ex: KCl = 149 Scm2/mol HAc = 391 Scm2/mol
 
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  • #2
It is not a general rule - compare HCl with HAc.

This comparison is also a hint why there is so large difference between limiting conductivities of substances you have listed.

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1. What is the difference between strong and weak electrolytes?

Strong electrolytes completely dissociate into ions when dissolved in water, while weak electrolytes only partially dissociate.

2. How does the strength of an electrolyte affect its conductivity?

The stronger the electrolyte, the higher its conductivity, as more ions are available to carry an electric current.

3. How can you determine if a substance is a strong or weak electrolyte?

A substance can be tested by conducting a simple conductivity test, where a conducting material is placed in a solution of the substance and a circuit is formed. If the solution conducts electricity well, it is a strong electrolyte, while a weak electrolyte will only conduct electricity to a limited degree.

4. Are there any factors that can affect the strength of an electrolyte?

Temperature, concentration, and the presence of other substances in the solution can all affect the strength of an electrolyte. For example, increasing the temperature can increase the dissociation of a weak electrolyte, making it behave more like a strong electrolyte.

5. What are some examples of strong and weak electrolytes?

Strong electrolytes include ionic compounds such as sodium chloride (table salt) and acids like hydrochloric acid. Weak electrolytes include weak acids like acetic acid and weak bases like ammonia.

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