Ionic Equilibrium | NEB 12 | One Shot | Nepali ScienceGuru
Nepali ScienceGuru - Aashish Panta・10 minutes read
The degree of ionization of weak electrolytes is influenced by factors like temperature and the presence of other ions, with the dilution law stating that it is inversely proportional to the square root of the concentration of the electrolytic solution. Adding a strong electrolyte with a common ion can suppress the ionization of weak electrolytes, while the presence of NH4+ ions can shift the equilibrium towards ionization.
Insights
- Factors like temperature and the presence of other ions impact how much an electrolyte ionizes.
- The addition of a strong electrolyte with a common ion can decrease the degree of ionization of a weak electrolyte.
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Recent questions
What factors influence electrolyte ionization?
Temperature and presence of other ions.
How do weak electrolytes behave in water?
Partially dissolve, leading to an equilibrium.
What is the dilution law for weak electrolytes?
Inversely proportional to the square root of concentration.
What is the ionic product of water?
Constant, with equal concentrations of hydroxide and hydrogen ions.
How does the addition of NH4+ affect weak electrolyte ionization?
Increases NH4+ ions, shifting equilibrium towards ionization.
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Summary
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Factors influencing electrolyte ionization in solutions
- Total number of moles of electrolytes ionized by total foreign speech
- Factors affecting the degree of an electrolyte's ionization include temperature and the presence of other ions
- Weak electrolytes in water only partially dissolve, leading to an equilibrium between ions and un-ionized molecules
- Dilution law states that the degree of ionization of weak electrolytes is inversely proportional to the square root of the concentration of the electrolytic solution
- The ionic product of water is constant, with the concentration of hydroxide and hydrogen ions equal to 1 x 10^-14 at 25°C
- Solubility product of a sparingly soluble salt is the product of the concentrations of its ions in a saturated solution at a specific temperature
- The common effect of adding a strong electrolyte containing a common ion suppresses the degree of ionization of a weak electrolyte
- The addition of NH4+ increases the concentration of NH4+ ions, shifting the equilibrium towards the ionization of weak electrolytes
