======Sodium in Water======


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====Summary====                   
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====Procedure==== 
Note: this uses a tiny piece of sodium that shouldn't explode.  See [[sodium_in_water_explosion|here]] for the explosive version. 
  - Place a beaker in a secondary tray and fill it about halfway with water.  
  - Add a few drops of a pH indicator such as phenolphthalein to the water.  
  - Using dry tongs, cut and remove a pea-sized piece of sodium from oil storage and quickly blot surface oil with a dry tissue.  
  - Stand back and gently place the sodium piece onto the water surface.  
  - Observe fizzing, the metal skittering on the surface, hydrogen evolution, possible ignition, and the indicator trail turning pink as sodium hydroxide forms.



====Links==== 
Reaction of Sodium and Water - North Carolina School of Science and Mathematics: 
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📄 Sodium in Water Chemistry Demonstration - Science Notes: [[https://sciencenotes.org/sodium-in-water-chemistry-demonstration/]]\\


====Variations====
  * Use different indicators (phenolphthalein, universal indicator) to visualize the pH increase.  
  * Demonstrate group trends qualitatively by discussing lithium (milder) and potassium (more vigorous) behavior rather than performing them, or show vetted video clips for comparison.



====Safety Precautions====
  * Teacher demonstration only; do not scale up the sample size beyond pea-sized.  
  * Wear splash goggles, face shield, lab coat, and appropriate gloves; keep students behind a safety shield and at a safe distance.  
  * Store sodium under mineral oil or kerosene; handle with dry tools and dry hands away from water sources.  
  * Use only a borosilicate beaker placed in a larger tray for containment; keep flammables away.  
  * Expect hydrogen gas; avoid open flames and ignition sources.  
  * Keep a Class D option such as dry sand available; do not use water or CO₂ extinguishers on alkali metal fires.  
  * After the reaction, treat the solution as sodium hydroxide; optionally neutralize with dilute acid (e.g., vinegar) before disposal per local rules.




====Questions to Consider====
  * Why does sodium float on water? (Its density is about 0.97 g/cm³, lower than water.)  
  * What products form in the reaction, and how does the indicator show this? (Sodium hydroxide and hydrogen; the base raises pH so phenolphthalein turns pink.)  
  * Why can flames appear even without an external spark? (The exothermic reaction can heat and ignite the hydrogen in air.)  
  * Why is sodium metal far more reactive than sodium chloride in water? (Na metal readily loses an electron; in NaCl the sodium already exists as Na⁺ and simply dissolves.)  
  * How does reactivity change down Group 1, and why? (It increases from Li to Cs due to lower ionization energy and weaker attraction to the outer electron.)