Textbook Question
A chemist wants to make 5.5 L of a 0.300 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use?
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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
Chapter 4, Problem 62
If 3.5 L of a 4.8 M SrCl2 solution is diluted to 45 L, what is the molarity of the diluted solution?
Verified step by step guidance1
Identify the initial conditions: the initial volume \( V_1 = 3.5 \) L and the initial molarity \( M_1 = 4.8 \) M.
Identify the final volume after dilution: \( V_2 = 45 \) L.
Use the dilution formula: \( M_1 \times V_1 = M_2 \times V_2 \), where \( M_2 \) is the molarity of the diluted solution.
Rearrange the formula to solve for \( M_2 \): \( M_2 = \frac{M_1 \times V_1}{V_2} \).
Substitute the known values into the equation: \( M_2 = \frac{4.8 \times 3.5}{45} \) to find the molarity of the diluted solution.
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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 expressed in moles per liter (mol/L) and is crucial for understanding how much solute is present in a given volume of solution. Molarity is commonly used in chemistry to prepare solutions and perform stoichiometric calculations.
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Molarity
Dilution
Dilution is the process of reducing the concentration of a solute in a solution, typically by adding more solvent. The dilution equation, M1V1 = M2V2, relates the initial and final molarity (M) and volume (V) of the solution. This concept is essential for calculating the new concentration after a solution has been diluted.
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Conservation of Moles
The conservation of moles principle states that the number of moles of solute remains constant before and after dilution, assuming no solute is added or removed. This principle underlies the dilution equation and allows for the calculation of the final concentration by equating the moles of solute in the initial and diluted solutions.
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Related Practice
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