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 73b

Chapter 4, Problem 73b

(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?

Verified step by step guidance

insert step 1> Determine the concentration of the stock solution if not given. If given, note it down.

insert step 2> Use the dilution formula: C1V1 = C2V2, where C1 is the concentration of the stock solution, V1 is the volume of the stock solution taken, C2 is the concentration of the diluted solution, and V2 is the total volume of the diluted solution.

insert step 3> Substitute the known values into the dilution formula: C1 (concentration of stock solution), V1 = 10.0 mL, and V2 = 0.500 L (convert to mL if necessary).

insert step 4> Solve the equation for C2, the concentration of the final solution.

insert step 5> Ensure the units are consistent and convert if necessary to express the final concentration in the desired units (e.g., mol/L).

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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 initial and final concentrations and volumes 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, commonly expressed in units such as molarity (moles per liter). Understanding concentration is crucial for calculating how much solute is present before and after dilution, which directly impacts the properties and behavior of the solution in chemical reactions.

Volume

Volume is a measure of the three-dimensional space occupied by a substance, often measured in liters (L) or milliliters (mL). In the context of dilution, the total volume after adding solvent is essential for determining the final concentration of the solution, as it influences the distribution of the solute within the new volume.

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Textbook Question

Indicate the concentration of each ion present in the solution formed by mixing: (b) 44.0 mL of 0.100 M Na₂SO₄ with 25.0 mL of 0.150 M KCl

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Textbook Question

Indicate the concentration of each ion present in the solution formed by mixing: (c) 3.60 g KCl in 75.0 mL of 0.250 M CaCl₂solution. Assume that the volumes are additive.

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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.

(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?

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Textbook Question

(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?