Ch.13 - Solutions

Tro - Chemistry: A Molecular Approach 4th Edition

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Tro 4th Edition

Ch.13 - Solutions

Problem 52c

Chapter 13, Problem 52c

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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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: \( 2.00 \text{ L} = 2000 \text{ mL} \).

Calculate the mass of the solution: \( \text{mass of solution} = 1.05 \text{ g/mL} \times 2000 \text{ mL} \).

Use the formula for mass percent: \( \text{mass percent} = \left( \frac{\text{mass of solute}}{\text{mass of solution}} \right) \times 100\% \).

Substitute the mass of KNO3 (72.5 g) and the calculated mass of the solution into the mass percent formula to find the mass percent.

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Key Concepts

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

Mass Percent Concentration

Mass percent concentration is a way to express 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 concept is essential for understanding how much of a particular substance is present in a given amount of solution.

Density and Volume Relationship

Density is defined as mass per unit volume and is a critical factor in converting between mass and volume. In this problem, the density of the solution (1.05 g/mL) allows us to determine the total mass of the solution from its volume (2.00 L). Understanding this relationship is crucial for accurately calculating the mass percent.

Calculating Total Mass of Solution

To find the mass percent, we first need to calculate the total mass of the solution, which includes both the solute (KNO3) and the solvent (water). This is done by using the density of the solution to convert the volume into mass. Knowing how to perform this calculation is vital for determining the mass percent of the solute in the solution.

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Solutions: Mass Percent

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Textbook Question

An aqueous NaCl solution is made using 112 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.)

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.)

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 molarity of the solution. (Assume a density of 1.05 g/mL for the solution.)

Textbook Question

Silver nitrate solutions are often used to plate silver onto other metals. What is the maximum amount of silver (in grams) that can be plated out of 4.8 L of an AgNO₃ solution containing 3.4% Ag by mass? Assume that the density of the solution is 1.01 g/mL.

Textbook Question

To what volume should you dilute 50.0 mL of a 5.00 M KI solution so that 25.0 mL of the diluted solution contains 3.05 g of KI?

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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.)

Verified video answer for a similar problem:

Key Concepts

Mass Percent Concentration

Density and Volume Relationship

Calculating Total Mass of Solution

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.)