To Test Conductivity of Solutions (Class 10 Chemistry Practical)
To test and compare electrical conductivity of various solutions and classify them as conductors or non-conductors
TL;DR: To test and compare electrical conductivity of various solutions and classify them as conductors or non-conductors
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Aim: To test and compare electrical conductivity of various solutions and classify them as conductors or non-conductors
Materials Required
- Conductivity apparatus or battery, bulb, and two electrodes
- Various solutions: dilute HCl, NaCl solution, sugar solution, distilled water, vinegar, milk
- Beaker
- Distilled water
- Dry cells or battery
Theory
Electrical conductivity depends on presence and concentration of ions in solution. Ionic solutions conduct electricity due to mobile ions, while covalent solutions do not. Strong electrolytes fully ionize and conduct well, weak electrolytes partially ionize, and non-electrolytes do not ionize. Conductivity is measured by ability of solution to complete electric circuit.
Procedure
- Assemble conductivity apparatus with battery, bulb, and two electrodes
- Pour dilute HCl into beaker
- Immerse electrodes in solution without touching
- Observe whether bulb glows indicating conductivity
- Record brightness of glow if any
- Empty beaker and rinse with distilled water
- Repeat procedure with each solution
- Compare conductivity of different solutions
- Classify solutions as good, poor, or non-conductors
Observation
Dilute HCl: Bulb glows brightly (good conductor). NaCl: Bulb glows (good conductor). Vinegar: Bulb glows dimly (weak conductor). Sugar solution: No glow (non-conductor). Distilled water: No glow (non-conductor). Milk: No glow (non-conductor).
Result
Solutions classified based on conductivity. Ionic solutions conducted electricity while covalent solutions did not. Concentration affects conductivity.
Precautions
- Do not allow electrodes to touch each other
- Rinse beaker and electrodes between tests
- Use distilled water for rinsing to avoid contamination
- Do not use excessive voltage that may harm apparatus
- Ensure good contact between electrodes and solution
Viva Questions
What makes a solution conduct electricity?
Solutions conduct electricity due to presence of free mobile ions that can move toward electrodes and carry charge.
Classify solutions as electrolytes and non-electrolytes.
Electrolytes are substances that conduct electricity in solution or molten state due to ion formation. Non-electrolytes do not conduct electricity.
What is the difference between strong and weak electrolytes?
Strong electrolytes completely ionize in solution and conduct electricity well. Weak electrolytes partially ionize and conduct electricity poorly.
Why does distilled water not conduct electricity?
Distilled water is a non-electrolyte and does not contain ions. It has very low conductivity unless some ions are added.
How does temperature affect conductivity of solutions?
Increasing temperature generally increases conductivity as ions move faster with higher kinetic energy.
Which solution is better conductor: dilute HCl or dilute NaCl?
Both are good conductors. Dilute HCl has higher conductivity due to high mobility of H+ ions compared to Na+ and Cl- ions.
More Class 10 Chemistry Practicals
- To Prepare a True Solution and Observe the Tyndall Effect
- To Find the pH of Samples Using Indicators
- To Study a Double Displacement (Precipitation) Reaction
- To Test Acids and Bases with Indicators
- To Verify the Law of Conservation of Mass
- To Study the Effect of Temperature on Reaction Rate
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