======Lead Storage Battery======


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**Alternative titles:** Rechargeable Lead-Acid Cell
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====Summary====                   
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====Procedure====  
  -Prepare two lead electrodes: one made of lead metal and the other coated with lead dioxide (or simulate this with treated lead strips).  
  -Place both electrodes into a beaker containing sulfuric acid solution (approximately 1–2 M).  
  -Connect the electrodes to a DC power supply and charge the cell until a measurable voltage is observed.  
  -Disconnect the power supply and attach a voltage probe across the electrodes to measure the stored potential.  
  -Connect the charged cell to a meter or low-power device to demonstrate energy discharge.



====Links==== 
Lead Acid Batteries: How They Work - Electromagnetic Videos: 
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📄 Lead Storage Batteries - Vernier: [[https://www.vernier.com/experiment/cwv-29_lead-storage-batteries/?srsltid=AfmBOorM5GXUxVms_ucMcorRemM81SNcQNucOK7ZSj-4e3EEmkurTu_j]]\\


====Variations====
  *Connect multiple lead-acid cells in series to increase the output voltage.  
  *Use different concentrations of sulfuric acid to test effects on performance.



====Safety Precautions====
  *Wear safety goggles, gloves, and a lab coat when handling sulfuric acid.  
  *Handle lead electrodes with care—lead is toxic and should not be touched with bare hands.  
  *Dispose of sulfuric acid and lead waste properly as hazardous materials.  
  *Avoid short-circuiting the electrodes, as this may cause overheating.  
  *Ensure good ventilation during the experiment, as small amounts of hydrogen gas may be produced.




====Questions to Consider====
  *What reactions occur at the lead and lead dioxide electrodes during discharge? (Pb → PbSO₄ + 2e⁻ at the anode; PbO₂ + 4H⁺ + SO₄²⁻ + 2e⁻ → PbSO₄ + 2H₂O at the cathode.)  
  *How does charging reverse the discharge reaction? (The applied current drives the reverse redox reactions, regenerating Pb and PbO₂ from PbSO₄.)  
  *Why is sulfuric acid essential for the operation of the battery? (It supplies sulfate ions for the redox reactions and maintains ionic conductivity.)  
  *Why are lead-acid batteries still used today despite being heavy and containing toxic materials? (They are inexpensive, reliable, and capable of delivering high surge currents, such as in car engines.)