**Step 1. **Mass of ammonia solution

$\mathbf{\rho}\mathbf{=}\frac{\mathbf{m}}{\mathbf{V}}\phantom{\rule{0ex}{0ex}}\mathbf{m}\mathbf{=}\left(\rho \right)\left(V\right)\phantom{\rule{0ex}{0ex}}\mathbf{m}\mathbf{=}(0.88\frac{g}{\overline{){\mathrm{cm}}^{3}}}\times \frac{1\overline{){\mathrm{cm}}^{3}}}{1\overline{)\mathrm{mL}}}\times \frac{1\overline{)\mathrm{mL}}}{{10}^{-3}\overline{)L}}\times \frac{3.785\overline{)L}}{1\overline{)\mathrm{gallon}}})\left(34400\overline{)\mathrm{gallon}}\right)$

A fertilizer railroad car carrying 34400 gallons of commercial aqueous ammonia (30% ammonia by mass) tips over and spills. The density of the aqueous ammonia solution is 0.88 g/cm^{3}.

What mass of citric acid, C(OH)(COOH)(CH_{2}COOH)_{2}, (which contains three acidic protons) is required to neutralize the spill? 1 gallon = 3.785 L.

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