Consider the following reactions for nitrification shown below. 2\left(\mathrm{NH}_{4}\right)^{+}+3 \mathrm{O}_{2} \rightarrow 2\left(\mathrm{NO}_{2}\right)^{-}+4 \mathrm{H}^{+}+2 \mathrm{H}_{2} \mathrm{O} 2\left(\mathrm{NO}_{2}\right)^{-}+\mathrm{O}_{2} \rightarrow 2\left(\mathrm{NO}_{3}\right)^{-} a) Determine the overall reaction by combining the two reactions and simplifying. o b) Consider a 1-liter sample of water with no alkalinity and with 20 mg/L NH4*-N (note, thismeans mg/L as N, so use a molecular weight of 14 g/mol of NH4* instead of 18 g/mol).Assuming the water had a pH of 7 before the reaction starts, what will the pH be after all 20mg of NH4*-N are oxidized to NO3? o c) How many mg of oxygen would be consumed if all 20 mg of NH4*-N are oxidized to NO3?

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