What mass of ammonium phosphate can prepared from a mass of #3.49*g# mass of phosphoric acid?

1 Answer
Feb 23, 2017

Answer:

Approx. #1.2*g# of #"DAP"#...

Explanation:

#"Diammonium phosphate"# is the stable material (called #"DAP"#). This is the material that is used as agricultural fertilizer:

#H_3PO_4 + 2NH_3rarr(NH_4)_2HPO_4#

So following the given reaction, we assume that the phosphoric acid consumes a twice molar quantity of ammonia.

#"Moles of phosphoric acid"=(3.49*g)/(98.08*g*mol^-1)=0.0356*mol#

And mass of ammonia consumed is a TWICE molar quantity, given the stoichiometric equation:

#0.0356*molxx2xx17.03*g*mol^-1-=1.21*g#

Note the assumptions in this answer. I would consider an answer based on #(NH_4)_3PO_4# to be unreasonable. You will have to see your teacher's treatment.