Difference Between Weak Base and Strong Base

Several definitions of a base are used in the contemporary chemistry:

  • Arrhenius base – a substance that increases the concentration of hydroxide anions when dissolved in water;
  • Brønsted-Lowry’s base  – a substance that takes up proton when reacting with acid;
  • Lewis base – a substance that yields an electron pair of another substance, when reacting with acid.

The most widely used is the Brøndsted- Lowry’s definition.

Bases in the broad sense include three groups of substances:

  • Water-soluble metal hydroxides: NaOH, Ca(OH)2, etc.;
  • Water-insoluble oxides or hydroxides that can react with acid: FeO, Al(OH)3, etc.;
  • Other compounds which, when dissolved in water, interact with it and release hydroxide ions: NH3, CH3NH2, etc.

Some of the general properties of the bases are:

  • Soapy or slimy touch;
  • Bitter taste;
  • Electric conductivity;
  • Violent reaction with reducible or acidic substances; caustic on organic matter;
  • Turn red litmus paper blue.

What is Weak Base?

Weak bases only partially dissociate to give ions in solution.

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