section_path: Acid–base definitions/Arrhenius definition/Example: Baking powder
section_name: Example: Baking powder
paragraph_text: Example: Baking powder
  
  Baking powder is used to cause the dough for breads and cakes to "rise" by creating millions of tiny carbon dioxide bubbles. Baking powder is not to be confused with baking soda, which is sodium bicarbonate (NaHCO). Baking powder is a mixture of baking soda (sodium bicarbonate) and acidic salts. The bubbles are created because, when the baking powder is combined with water, the sodium bicarbonate and acid salts react to produce gaseous carbon dioxide.
  
  Whether commercially or domestically prepared, the principles behind baking powder formulations remain the same. The acid–base reaction can be generically represented as shown:
  
  NaHCO 3 + H + ⟶ Na + + CO 2 + H 2 O {\displaystyle {\ce {NaHCO3 + H+ -> Na+ + CO2 + H2O}}}
  
  The real reactions are more complicated because the acids are complicated. For example, starting with sodium bicarbonate and monocalcium phosphate (Ca(H PO)), the reaction produces carbon dioxide by the following stoichiometry:
  
  14 NaHCO 3 + 5 Ca (H 2 PO 4) 2 ⟶ 14 CO 2 + Ca 5 (PO 4) 3 OH + 7 Na 2 HPO 4 + 13 H 2 O {\displaystyle {\ce {14 NaHCO3 + 5 Ca(H2PO4)2 -> 14 CO2 + Ca5(PO4)3OH + 7 Na2HPO4 + 13 H2O}}}
  
  A typical formulation (by weight) could call for 30% sodium bicarbonate, 5–12% monocalcium phosphate, and 21–26% sodium aluminium sulfate. Alternately, a commercial baking powder might use sodium acid pyrophosphate as one of the two acidic components instead of sodium aluminium sulfate. Another typical acid in such formulations is cream of tartar (KC H O), a derivative of tartaric acid.