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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 72c
Chapter 4, Problem 72c

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 CaCl2 solution. Assume that the volumes are additive.

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Calculate the moles of KCl: Use the molar mass of KCl to convert grams to moles.
Determine the concentration of KCl: Divide the moles of KCl by the total volume of the solution in liters.
Calculate the moles of CaCl_2: Use the given molarity and volume to find the moles of CaCl_2.
Determine the concentration of CaCl_2: Since the volume is additive, divide the moles of CaCl_2 by the total volume of the solution in liters.
Identify the ions present: KCl dissociates into K^+ and Cl^- ions, and CaCl_2 dissociates into Ca^{2+} and Cl^- ions. Calculate the concentration of each ion based on their stoichiometry in the compounds.

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Key Concepts

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

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for calculating the concentration of ions in a solution, especially when mixing different solutions. In this question, the molarity of the CaCl2 solution is given, which helps determine the concentration of calcium and chloride ions after mixing.
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Dissociation of Ionic Compounds

Ionic compounds, such as KCl and CaCl2, dissociate into their constituent ions when dissolved in water. For example, KCl dissociates into K+ and Cl- ions, while CaCl2 dissociates into Ca2+ and 2Cl- ions. Understanding this dissociation is essential for calculating the total concentration of ions in the mixed solution.
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Mass-to-Moles Conversion

To find the concentration of ions from a given mass of solute, it is necessary to convert grams to moles using the molar mass of the compound. For KCl, the molar mass is approximately 74.55 g/mol. This conversion allows for the determination of the number of moles of KCl present in the solution, which is then used to find the concentration of K+ and Cl- ions.
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Related Practice
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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(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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Indicate the concentration of each ion present in the solution formed by mixing: (a) 42.0 mL of 0.170 M NaOH with 37.6 mL of 0.400 M NaOH.

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Textbook Question

Ignoring protolysis reactions, indicate the concentration of each ion or molecule present in the following solutions: (d) a mixture of 45.0 mL of 0.272 M NaCl and 65.0 mL of 0.0247 M (NH4)2CO3. Assume that the volumes are additive.

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Textbook Question

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

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Textbook Question

(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?