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When water is added to an aqueous solution of an electrolyte, what is the change in specific conductivity of the electrolyte?
- a)Conductivity decreases
- b)Conductivity increases
- c)Conductivity remains same
- d)Conductivity does not depend on number of ions
Correct answer is option 'A'. Can you explain this answer?
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When water is added to an aqueous solution of an electrolyte, what is ...
Factors affecting electrolytic conductance are:
Concentration of ions: The sole reason for the conductivity of electrolytes is the ions present in them. The conductivity of electrolytes increases with an increase in the concentration of ions as there will be more charge carriers if the concentration of ions is more and hence the conductivity of electrolytes will be high.
Nature of electrolyte: Electrolytic conduction is significantly affected by the nature of electrolytes. The degree of dissociation of electrolytes determines the concentration of ions in the solution and hence the conductivity of electrolytes.
Substances such as CH3COOH, with a small degree of separation, will have less number of ions in the solution and hence their conductivity will also below, and these are called weak electrolytes. Strong electrolytes such as KNO3 have a high degree of dissociation and hence their solutions have a high concentration of ions and so they are good electrolytic conductance.
Temperature: Temperature affects the degree to which an electrolyte gets dissolved in solution. It has been seen that higher temperature enhances the solubility of electrolytes and hence the concentration of ions which results in an increased electrolytic conduction.
When water is added to an aqueous solution the number of ions per unit volume decreases i.e., the concentration of ions decreases and hence thereby conductivity gets decreased.
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When water is added to an aqueous solution of an electrolyte, what is ...
Introduction:
When water is added to an aqueous solution of an electrolyte, the specific conductivity of the electrolyte changes. Specific conductivity is a measure of the ability of a substance to conduct electric current. It depends on the concentration of ions in the solution and their mobility.
Explanation:
When water is added to an aqueous solution of an electrolyte, several factors contribute to a decrease in specific conductivity:
Dilution:
When water is added, it increases the total volume of the solution. This leads to dilution of the electrolyte, resulting in a decrease in the concentration of ions present in the solution. As the concentration of ions decreases, the number of charge carriers available for conduction decreases, leading to a decrease in conductivity.
Ion hydration:
Water molecules have a tendency to surround ions and form hydration shells. This process is known as ion hydration. The presence of water molecules around ions affects their mobility and ability to move freely in the solution. As the concentration of water increases due to dilution, more water molecules surround the ions, causing an increase in ion hydration. This increase in ion hydration hinders the movement of ions, reducing their mobility and conductivity.
Ion association/dissociation:
Some electrolytes can undergo ion association or dissociation in solution. When water is added, it can disrupt the ion association or dissociation equilibrium, leading to a decrease in conductivity. For example, in the case of weak electrolytes, dilution can shift the equilibrium towards the association of ions, decreasing the concentration of free ions available for conduction.
Conclusion:
In summary, when water is added to an aqueous solution of an electrolyte, the specific conductivity of the electrolyte decreases. This decrease is primarily due to dilution, increased ion hydration, and disruption of ion association/dissociation equilibrium.
When water is added to an aqueous solution of an electrolyte, the specific conductivity of the electrolyte changes. Specific conductivity is a measure of the ability of a substance to conduct electric current. It depends on the concentration of ions in the solution and their mobility.
Explanation:
When water is added to an aqueous solution of an electrolyte, several factors contribute to a decrease in specific conductivity:
Dilution:
When water is added, it increases the total volume of the solution. This leads to dilution of the electrolyte, resulting in a decrease in the concentration of ions present in the solution. As the concentration of ions decreases, the number of charge carriers available for conduction decreases, leading to a decrease in conductivity.
Ion hydration:
Water molecules have a tendency to surround ions and form hydration shells. This process is known as ion hydration. The presence of water molecules around ions affects their mobility and ability to move freely in the solution. As the concentration of water increases due to dilution, more water molecules surround the ions, causing an increase in ion hydration. This increase in ion hydration hinders the movement of ions, reducing their mobility and conductivity.
Ion association/dissociation:
Some electrolytes can undergo ion association or dissociation in solution. When water is added, it can disrupt the ion association or dissociation equilibrium, leading to a decrease in conductivity. For example, in the case of weak electrolytes, dilution can shift the equilibrium towards the association of ions, decreasing the concentration of free ions available for conduction.
Conclusion:
In summary, when water is added to an aqueous solution of an electrolyte, the specific conductivity of the electrolyte decreases. This decrease is primarily due to dilution, increased ion hydration, and disruption of ion association/dissociation equilibrium.
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When water is added to an aqueous solution of an electrolyte, what is the change in specific conductivity of the electrolyte?a)Conductivity decreasesb)Conductivity increasesc)Conductivity remains samed)Conductivity does not depend on number of ionsCorrect answer is option 'A'. Can you explain this answer?
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