An aqueous NaCl solution is made using 102 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the mass percent of the solution. (Assume a density of 1.08 g>mL for the solution.)

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

Convert the volume from liters to milliliters: \( 1.00 \text{ L} = 1000 \text{ mL} \).

Substitute the values into the mass formula: \( \text{mass of solution} = 1.08 \text{ g/mL} \times 1000 \text{ mL} \).

Determine the mass percent of NaCl in the solution using the formula: \( \text{mass percent} = \left( \frac{\text{mass of solute (NaCl)}}{\text{mass of solution}} \right) \times 100\% \).

Substitute the mass of NaCl (102 g) and the calculated mass of the solution into the mass percent formula.

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Key Concepts

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

Mass Percent

Mass percent is a way of expressing the concentration of a solute in a solution. It is calculated by taking the mass of the solute, dividing it by the total mass of the solution, and then multiplying by 100 to get a percentage. This measurement is crucial for understanding how much of a substance is present in a given amount of solution.

Density

Density is defined as mass per unit volume and is a critical property of substances. In this context, the density of the solution (1.08 g/mL) allows us to convert the volume of the solution into mass, which is necessary for calculating mass percent. Understanding density helps in determining how much solute is present in a specific volume of solution.

Dilution

Dilution refers to the process of reducing the concentration of a solute in a solution, typically by adding more solvent. In this problem, the NaCl is dissolved in water to create a solution with a specific volume. Recognizing how dilution affects concentration is essential for accurately calculating mass percent and understanding solution properties.

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An aqueous NaCl solution is made using 102 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molarity of the solution. (Assume a density of 1.08 g>mL for the solution.)

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An aqueous NaCl solution is made using 102 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molality of the solution. (Assume a density of 1.08 g>mL for the solution.)

Textbook Question

An aqueous KNO3 solution is made using 55.3 g of KNO3 diluted to a total solution volume of 2.00 L. Calculate the molarity of the solution. (Assume a density of 1.05 g>mL for the solution.)

Textbook Question

An aqueous KNO3 solution is made using 55.3 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.)

Textbook Question

An aqueous KNO3 solution is made using 55.3 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.)