A dioxin-contaminated water source contains 0.085% dioxin by mass. How much dioxin is present in 2.5 L of this water? Assume a density of 1.00 g/mL.

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Convert the volume of water from liters to milliliters using the conversion factor: 1 L = 1000 mL.

Calculate the mass of the water using the density formula: \( \text{mass} = \text{density} \times \text{volume} \).

Determine the mass of dioxin in the water by using the percentage by mass: \( \text{mass of dioxin} = \text{mass of water} \times \frac{0.085}{100} \).

Ensure all units are consistent and check calculations for accuracy.

Summarize the steps and ensure understanding of the concept of percentage by mass and its application in this context.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Concentration by Mass

Concentration by mass refers to the amount of solute (in this case, dioxin) present in a given mass of solution. It is often expressed as a percentage, indicating how many grams of solute are present in 100 grams of solution. Understanding this concept is crucial for calculating the mass of dioxin in a specific volume of contaminated water.

Density

Density is defined as mass per unit volume and is a key property of substances. In this scenario, the density of the water is given as 1.00 g/mL, which means that 1 mL of water has a mass of 1 gram. This information allows us to convert the volume of water (2.5 L) into mass, which is necessary for calculating the total mass of dioxin present.

Volume to Mass Conversion

To find the mass of a substance from its volume, we use the formula: mass = volume × density. In this case, converting 2.5 L of water to grams using the provided density allows us to determine the total mass of the water, which is essential for applying the concentration percentage to find the mass of dioxin present in the water.

Related Practice

Textbook Question

Lead is a toxic metal that affects the central nervous system. A Pb-contaminated water sample contains 0.0011% Pb by mass. How much of the water (in mL) contains 150 mg of Pb? (Assume a density of 1.0 g/mL.)

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Textbook Question

An aqueous KNO₃ solution is made using 72.5 g of KNO₃ diluted to a total solution volume of 2.00 L. Calculate the mass percent of the solution. (Assume a density of 1.05 g/mL for the solution.)

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Textbook Question

An aqueous KNO₃ solution is made using 72.5 g of KNO₃ diluted to a total solution volume of 2.00 L. Calculate the molality of the solution. (Assume a density of 1.05 g/mL for the solution.)

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