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# Acids and bases

## Question

###### Acids and bases

A wastewater is simulated as a solution containing $$10^{-2.7} \mathrm{M} \mathrm{NaHCO}_{3}$$ and $$10^{-3} \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}$$

a. List the dissolved species that you expect to be present in solution.

b. Prepare a log $$C-p H$$ diagram for the system, and calculate the $$\mathrm{pH}$$ of the solution.

c. In order to remove nitrogen by volatilizing $$\mathrm{NH}_{3}$$ gas, $$148 \mathrm{mg} / \mathrm{L}$$ Ca(OH) $$_{2}$$ (lime) will be added to raise the $$\mathrm{pH}$$ and convert $$\mathrm{NH}_{4}^{+}$$ to the $$\mathrm{NH}_{3}(a q)$$ form. Calculate the $$\mathrm{pH}$$ after lime addition. (Assume that no $$\mathrm{CaCO}_{3}$$ precipitation or ammonia loss takes place during lime addition.)

$$d$$. If $$\mathrm{CaCO}_{3}$$ precipitation did occur during lime addition, would it raise, lower, or not change the $$\mathrm{pH}$$ of the solution? (Hint: Consider what species are removed from solution by this reaction, and what the response would be of the species that remain.)

e. Would removal of $$\mathrm{NH}_{3}(a q)$$ by volatilization raise, lower, or not change the $$\mathrm{pH}$$ of the solution? Explain your reasoning briefly.

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