Question

3 attempts left Check my work Be sure to answer all parts. Repor points Ammonium nitrate (NH NO) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of NH NO, with a standard NaOH solution. In one experiment a 0.2031-g sample of industrially prepared NH NO, required 24.14 ml of 0.1003 M NaOH for neutralization. sc eBook Print (a) Enter a net ionic equation for the reaction (include states of matter Guide References NH, (aq) OH(aq) --NH, (aq) +H,00 (b) What is the percent purity of the sample?

Answer 1

a.NH4NO3(aq) + NaOH(aq) ------------> NH3(g) + NaNO3(aq) + H2O(l)

NH4^+(aq) + NO3^-(aq) + Na^+(aq) + OH^-(aq) ------------> NH3(g) + Na^+(aq) + NO3^-(aq) + H2O(l)

removal of spectator ions to get net ionic equation

NH4^+(aq) + OH^-(aq) ------------> NH3(g)   + H2O(l)

b.

no of moles of NaOH = molarity * volume in L

                                  = 0.1003*0.02414   = 0.002421242moles

NH4NO3(aq) + NaOH(aq) ------------> NH3(g) + NaNO3(aq) + H2O(l)

1 mole of NaOH react with 1 mole of NH4NO3

0.0024212 moles of NaOH react with 0.002421242 moles of NH4NO3

mass of NH4NO3 = no of moles * gram molar mass

                           = 0.002421242*80   = 0.194 g of NH4NO3

The percent purity of sample = 0.194*100/0.2031 = 95.52% >>>answer