Ch.4 - Reactions in Aqueous Solution

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 74b

Chapter 4, Problem 74b

(b) If you dilute 10.0 mL of the stock solution to a final volume of 0.250 L, what will be the concentration of the diluted solution?

Verified step by step guidance

Identify the initial concentration of the stock solution, denoted as C1, and the initial volume, V1, which is 10.0 mL.

Recognize that the final volume, V2, after dilution is 0.250 L (or 250 mL).

Use the dilution formula: C1 * V1 = C2 * V2, where C2 is the concentration of the diluted solution.

Rearrange the formula to solve for C2: C2 = (C1 * V1) / V2.

Substitute the known values into the equation to find the concentration of the diluted solution, C2.

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Key Concepts

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

Dilution

Dilution is the process of reducing the concentration of a solute in a solution, typically by adding more solvent. The relationship between the concentrations and volumes of the stock and diluted solutions can be described by the dilution equation, C1V1 = C2V2, where C1 and V1 are the concentration and volume of the stock solution, and C2 and V2 are the concentration and volume of the diluted solution.

Concentration

Concentration refers to the amount of solute present in a given volume of solution, often expressed in units such as molarity (moles per liter). Understanding how concentration changes during dilution is crucial for calculating the final concentration after mixing different volumes of solutions.

Volume

Volume is a measure of the three-dimensional space occupied by a substance, commonly measured in liters (L) or milliliters (mL). In dilution calculations, the initial and final volumes are essential for determining how the concentration of a solution changes when additional solvent is added.

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Textbook Question

(b) If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of 0.500 L, what will be the concentration of the final solution?

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Textbook Question

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25 C. Calculate the molarity of a solution of acetic acid made by dissolving 20.00 mL of glacial acetic acid at 25 C in enough water to make 250.0 mL of solution.

(a) How many milliliters of a stock solution of 6.0 M HNO₃would you have to use to prepare 110 mL of 0.500 M HNO₃?

(a) You have a stock solution of 14.8 M NH₃. How many milliliters of this solution should you dilute to make 1000.0 mL of 0.250 M NH₃?