Hypochlorite, a chlorine anion (OCl-), has become a mainstay in environmental and water treatment due to its potent disinfectant properties. It offers a safer and more convenient alternative to chlorine gas, which can be hazardous to handle. This article delves into the applications and mechanisms of hypochlorite, highlighting its importance in safeguarding our water resources.
Hypochlorite: An Effective Disinfectant
Hypochlorite's effectiveness as a disinfectant stems from its ability to generate free chlorine, a highly reactive species that effectively kills bacteria, viruses, and other harmful microorganisms. This process occurs through oxidation, where the hypochlorite ion disrupts the cellular structures of pathogens, rendering them inactive.
Applications in Water Treatment:
Benefits of Hypochlorite:
Challenges Associated with Hypochlorite:
Conclusion:
Hypochlorite is a valuable tool in environmental and water treatment, providing an effective and safe way to eliminate harmful pathogens. Its versatility, convenience, and effectiveness have solidified its position as a critical element in safeguarding water quality and public health. However, it's essential to manage the potential risks associated with its use, such as DBP formation and corrosion, to ensure safe and sustainable water treatment practices.
Instructions: Choose the best answer for each question.
1. What is the chemical formula for hypochlorite?
a) ClO
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2. Hypochlorite is effective as a disinfectant because it:
a) Releases oxygen into the water.
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3. Which of the following is NOT a benefit of using hypochlorite?
a) Safety in handling.
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4. What is a potential risk associated with using hypochlorite?
a) It can increase the pH of the water.
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5. In which of the following applications is hypochlorite NOT commonly used?
a) Municipal water treatment.
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Scenario: You are a water treatment plant operator. You have been instructed to add a specific amount of hypochlorite to the incoming water supply to ensure proper disinfection. The instructions state that you need to achieve a free chlorine concentration of 1 ppm (parts per million). However, you have been provided with hypochlorite solution that has a concentration of 10% available chlorine.
Task: Calculate the amount of hypochlorite solution (in milliliters) that you need to add per liter of water to achieve the desired free chlorine concentration of 1 ppm.
Hint: You can use the formula:
Volume of hypochlorite solution (mL) = (Desired free chlorine concentration (ppm) * Volume of water (L)) / (Hypochlorite concentration (%) * 10)
Here's how to solve the problem: 1. **Identify the given values:** - Desired free chlorine concentration = 1 ppm - Volume of water = 1 L - Hypochlorite concentration = 10% 2. **Apply the formula:** ``` Volume of hypochlorite solution (mL) = (1 ppm * 1 L) / (10% * 10) ``` 3. **Simplify the equation:** ``` Volume of hypochlorite solution (mL) = 1 / 100 ``` 4. **Calculate the result:** ``` Volume of hypochlorite solution (mL) = 0.01 mL ``` **Therefore, you need to add 0.01 mL of the 10% hypochlorite solution per liter of water to achieve a free chlorine concentration of 1 ppm.** **Important Note:** This calculation is a simplified example. In real-world scenarios, you should consider factors like the water's pH, temperature, and the presence of organic matter, which can influence the effectiveness of disinfection and the formation of DBPs.
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