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Chapter 13: Problem 98

During municipal drinking water treatment, water is sprayed into the air. Why is this done?

Short Answer

Expert verified
Water is sprayed to remove gases, oxidize metals, and improve taste by exposing water to air.

Step by step solution

01

Understand the Purpose of Aeration

In municipal water treatment, spraying water into the air is part of the aeration process. The main goal is to expose the water to air, allowing for the exchange of gases between the water and the atmosphere. This serves several purposes, including the removal of unwanted dissolved gases such as carbon dioxide and the oxidation of dissolved iron and manganese, which can be found in raw water supplies.
02

Promote Chemical Reactions

When water is sprayed into the air, oxygen from the atmosphere dissolves into the water. This increased level of dissolved oxygen promotes oxidation reactions. For instance, iron (Fe) in its soluble form (Fe虏鈦�) is oxidized to its insoluble form (Fe鲁鈦�), which can then be more readily removed by subsequent filtration processes.
03

Improve Water Quality and Taste

The removal of dissolved gases, such as carbon dioxide, through aeration reduces water acidity, while the chlorine smell or any other volatile compounds are minimized through volatilization. This enhances the taste and odors of municipal drinking water, making it more palatable for consumers.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Aeration Process
The aeration process is a vital step in municipal water treatment. It involves spraying water into the air, primarily to increase its exposure to the atmosphere.
This exposure allows for essential interactions with air, facilitating gas exchange and promoting various chemical reactions.
The main focus during aeration is mixing the water with air, which helps in dealing with undesirable elements in the water.
  • **Breaks Up Water:** By increasing the surface area of the water droplets, more oxygen can dissolve into the water.
  • **Removes Unwanted Gases:** Carbon dioxide and other volatile compounds are released into the atmosphere.
  • **Forms Part of a Multi-Step Treatment:** Aeration is typically followed by other processes that further refine water quality.
Understanding and controlling this process is key to ensuring that drinking water is safe and pleasant to consume.
Gas Exchange
Gas exchange occurs during the aeration process and is crucial for removing unwanted gases and allowing beneficial ones to dissolve.
When water droplets are exposed to air, gases like oxygen enter the water, while others, such as carbon dioxide, exit.
  • **Oxygen Uptake:** Increased oxygen levels promote the oxidation of metals like iron and manganese, transforming them from soluble to insoluble forms.
  • **Volatilization:** Unpleasant volatile compounds are stripped away, improving the odor and taste of the water.
  • **Equilibrium Establishment:** The process helps achieve a balance between the water's gas composition and the surrounding air.
This exchange is fundamental to improving the overall quality of water as it prepares for further purification stages.
Water Quality Improvement
Water quality improvement is the ultimate goal of municipal water treatment, achieved through several interconnected processes, including aeration.
Aeration enhances water quality by altering its chemical makeup and removing impurities, resulting in water that is both safer to drink and more appealing.
  • **Reduction of Acidity:** The removal of carbon dioxide through aeration results in less acidic water.
  • **Improved Taste and Odor:** By getting rid of chlorine smells and other volatile constituents, aeration makes water more enjoyable to consume.
  • **Metal Removal:** Oxidized metals become insoluble and can be filtered out more easily, ensuring clearer and healthier water.
Through these processes, aeration plays a pivotal role in producing high-quality municipal drinking water.

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Most popular questions from this chapter

Calculate the boiling point and the freezing point of these solutions at \(760 \mathrm{mmHg}\). (a) \(20.0 \mathrm{~g}\) citric acid, \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\), in \(100.0 \mathrm{~g}\) water (b) \(3.00 \mathrm{~g} \mathrm{CH}_{3} \mathrm{I}\) in \(20.0 \mathrm{~g}\) benzene \(\left(K_{\mathrm{b}}\right.\) benzene \(=\) \(2.53^{\circ} \mathrm{C} \mathrm{kg} / \mathrm{mol} ; K_{\mathrm{f}} \text { benzene } \left.=-5.10^{\circ} \mathrm{C} \mathrm{kg} / \mathrm{mol}\right)\)

A solution, prepared by dissolving \(9.41 \mathrm{~g} \mathrm{NaHSO}_{3}\) in \(1.00 \mathrm{~kg}\) water, freezes at \(-0.33{ }^{\circ} \mathrm{C}\). From these data, decide which of these equations is the correct expression for the dissociation of the salt. (a) \(\mathrm{NaHSO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{HSO}_{3}^{-}(\mathrm{aq})\) (b) \(\mathrm{NaHSO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq})+\mathrm{SO}_{3}^{2-}(\mathrm{aq})\)

Explain why the Tyndall effect is not observed with solutions.

A \(1.00 \mathrm{~mol} / \mathrm{kg}\) aqueous sulfuric acid solution, \(\mathrm{H}_{2} \mathrm{SO}_{4}\), freezes at \(-4.04{ }^{\circ} \mathrm{C}\). Calculate \(i\), the van't Hoff factor, for sulfuric acid in this solution.

How does the solubility of gases in liquids change with increased temperature? Explain why.
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