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Chapter 5: Problem 22

The acceptable limit for nitrate, often found in well water in agricultural areas, is \(10 \mathrm{ppm}\). If a water sample is found to contain \(350 \mathrm{mg} / \mathrm{L}\). does it meet the acceptable limit?

Short Answer

Expert verified
No, the water sample does not meet the acceptable nitrate limit.

Step by step solution

01

Understand the Problem

We're given a water sample with a nitrate concentration of \(350 \text{ mg/L}\). We need to check if this concentration is within the acceptable limit of \(10 \text{ ppm}\). Since \(1 \text{ ppm} = 1 \text{ mg/L}\), we can directly compare the two values.
02

Convert Units If Necessary

In this case, there is no need for unit conversion because \(1 \text{ ppm}\) is already equivalent to \(1 \text{ mg/L}\). So, we can directly compare the nitrate concentration in mg/L with the ppm limit.
03

Compare the Values

Compare the given nitrate concentration of \(350 \text{ mg/L}\) with the acceptable limit of \(10 \text{ mg/L}\) (or ppm).
04

Determine the Conclusion

Since \(350 \text{ mg/L}\) is much higher than \(10 \text{ mg/L}\), the water sample does not meet the acceptable nitrate limit.

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Key Concepts

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

Understanding Nitrate Concentration
Nitrate concentration in water is a key indicator of water quality, especially in agricultural areas. Nitrates, chemical compounds containing nitrogen, can be introduced into water sources through fertilizers, animal waste, and septic systems. High levels of nitrates in drinking water pose health risks, particularly to infants and pregnant women. Infants exposed to elevated nitrate levels may develop "blue baby syndrome," a condition that affects the blood's ability to carry oxygen. Regular monitoring and assessment of nitrate concentration in sources of drinking water are thus crucial to ensuring public safety.
Explaining Parts Per Million (ppm)
Parts per million (ppm) is a unit of measurement used to describe the concentration of one substance in a million parts of another. In the context of water quality, ppm is used to express the amount of a specific chemical in water. One ppm is equivalent to one milligram of a substance per liter of water (mg/L). This direct equivalence simplifies the process of comparing concentration levels since no complex calculations are needed. Understanding ppm is essential for anyone dealing with water quality assessments as it provides a standardized way of expressing and understanding chemical concentrations.
Ensuring Well Water Safety
Well water safety is a critical concern for households relying on wells for their water supply. It is important to regularly test well water for contaminants like nitrates and other pollutants. Elevated nitrate levels, such as the 350 mg/L found in some agricultural areas, far exceed the recommended safety limit of 10 ppm. Such levels can have long-term health implications. To ensure well water safety:
  • Test well water annually for nitrates and other contaminants.
  • Consider installing water treatment systems that can reduce nitrate levels if needed.
  • Stay informed about local agricultural practices and potential risks to water quality.
By taking these steps, well water safety can be maintained, protecting the health of those who consume it.

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Most popular questions from this chapter

Infants are highly susceptible to elevated nitrate levels because bacteria in their digestive tract convert nitrate ion into nitrite ion, a much more toxic substance. a. Give chemical formulas for both the nitrate ion and nitrite ion. b. Nitrite ion can interfere with the ability of blood to carry oxygen. Explain the role of oxygen in respiration. Hint: Review Sections \(1.1\) and \(3.5\) for more about respiration. c. Boiling nitrate-containing water will not remove nitrate ion. Explain.

Levels of naturally occurring mercury in surface water -7 are usually less than \(0.5 \mu g / \mathrm{L}\). The average intake of mercury from food is \(2-20 \mu \mathrm{g}\) daily, but may be much higher in regions where fish is a staple of the diet. a. Name three human activities that add \(\mathrm{Hg}^{2+}\) ("inorganic mercury") to water. b. What is "organic mercury"? This chemical form of mercury tends to accumulate in the fatty tissues of fisb. Explain why

The density of water at \(0^{\circ} \mathrm{C}\) is \(0.9987 \mathrm{~g}^{\circ} \mathrm{cm}^{3}\); the density of ice at this same temperature is \(0.917 \mathrm{~g} / \mathrm{cm}^{3}\). a. Calculate the volume occupied at 0 ' \(\mathrm{C}\) by \(100.0 \mathrm{~g}\) of liquid water and by \(100.0 \mathrm{~g}\) of ice. b. Calculate the percentage increase in volume when \(100.0 \mathrm{~g}\) of water freezes at \(0^{\circ} \mathrm{C}\).

Both methane \((\mathrm{CH})\) and water are compounds of bydrogen and another nonmetal. a. Give four examples of nonmetals. In general, how do the electronegativity values of nonmetals compare with those of metals? b. How do the electronegativity values of carbon, oxygen, and hydrogen compare? c. Which bond is more polar, the C-11 bond or the O-H band? d. Methane is a gas at room temperature, but water is a liquid. Explain.

An aqueous solution of \(\mathrm{KCl}\) conducts electricity, but a solution of sucrose does not. Explain.
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