What is a potential consequence of using lime in water treatment?

What is a potential consequence of using lime in water treatment?

• A. Increased acidity
• B. Formation of precipitates
• C. Increased hardness
• D. Decreased total dissolved solids

Answer: (B)

Using lime in water treatment can lead to the formation of precipitates, which is a significant consequence of its application. Lime, chemically known as calcium hydroxide, is often used to raise the pH of water, which helps in the removal of various impurities. When lime is added to water, it reacts with other substances present, such as carbonates and sulfates, leading to the formation of insoluble compounds that can precipitate out of solution. For instance, when lime interacts with bicarbonates in the water, it can result in the precipitation of calcium carbonate, which can then be removed during the treatment process. Precipitations play an important role in clarifying water, as they can help to remove not only hardness-causing minerals but also other contaminants. The ability to form these precipitates is utilized strategically in water treatment to enhance water quality and ensure that the finished product is safe for consumption. The other choices do not accurately reflect the consequences of lime use in water treatment. Increased acidity contradicts the function of lime, which raises pH rather than lowering it. Increased hardness is generally related to the addition of calcium and magnesium rather than lime's intended use. Finally, lime typically does not decrease total dissolved solids; instead, it may alter the

Using lime in water treatment can lead to the formation of precipitates, which is a significant consequence of its application. Lime, chemically known as calcium hydroxide, is often used to raise the pH of water, which helps in the removal of various impurities. When lime is added to water, it reacts with other substances present, such as carbonates and sulfates, leading to the formation of insoluble compounds that can precipitate out of solution. For instance, when lime interacts with bicarbonates in the water, it can result in the precipitation of calcium carbonate, which can then be removed during the treatment process.

Precipitations play an important role in clarifying water, as they can help to remove not only hardness-causing minerals but also other contaminants. The ability to form these precipitates is utilized strategically in water treatment to enhance water quality and ensure that the finished product is safe for consumption.

The other choices do not accurately reflect the consequences of lime use in water treatment. Increased acidity contradicts the function of lime, which raises pH rather than lowering it. Increased hardness is generally related to the addition of calcium and magnesium rather than lime's intended use. Finally, lime typically does not decrease total dissolved solids; instead, it may alter the