216 



franklin: the ammonia system 



will be remembered, is exhibited by the corresponding water 

 derivatives to a conspicuous degree. (2) Ammono acids and bases 2 

 produce the familiar reciprocal color changes in liquid ammonia 

 solutions of phenolphthalein and other indicators. (3) When an 

 ammono acid and an ammono base are brought together in liquid 

 ammonia solution a reaction takes place resulting in the formation 



TABLE 1 



THE WATER SYSTEM 



Aquo acids 



Acetic acid CH 3 COOH 



Nitric acid N0 2 OH 



Carbonic acid CO(OH) 2 



Sulphuric acid S0 2 (OH) 2 



Orthosilicic acid Si(OH) 4 



Aquo bases 



Potassium hydroxide KOH 



Zinc hydroxide Zn(OH) 2 



Lead hydroxide Pb(OH) 2 



Aquo salts 



Potassium acetate CH 3 COOK 



Potassium carbonate CO(OK) 2 



Mercuric nitrate N0 2 Ohg 



THE AMMONIA SYSTEM 



Ammono acids 



Acetamide CH 3 CONH 2 



Nitramide N0 2 NH 2 



Urea CO(NH 2 ) 2 



Sulphamide S0 2 (NH,) 2 



Silicon amide Si(NH 2 ) 4 



Ammono bases 



Potassium amide KNH 2 



Zinc amide Zn(NH 2 ) 2 



Lead amide Pb(NH 2 ) 2 



Ammono salts 



Monopotassium acetamide 



CH3CONHK 

 Dipotassium acetamide . . .CH 3 CONK 2 



Dipotassium urea CO(NHK) 2 



Mercuric nitramide N0 2 NHg 



of an ammono salt. For example, acetamide acts upon potas- 

 sium amide in accordance with the equations 



CH 3 CONH 2 + KNH 2 = CH 3 CONHK + NH 3 

 CH 3 CONH 2 + 2KNH 2 = CH 3 CONK 2 + 2NH 3 

 to form monopotassium or dipotassium acetamide. (4) Liquid 

 ammonia solutions of ammono acids attack certain metals with 

 the evolution of hydrogen gas and the formation of ammono salts 

 as represented for a specific example by the equation, 

 Mg + 2CH 3 CONH 2 = (CH 3 CONH) 2 Mg + H 2 



2 Ammonia itself exhibits basic properties only in the presence of water. It 

 is not surprising therefore to find that the dry liquid acts quite as indifferently 

 towards indicators as. does water itself. 



