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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblema 60
Capitolo 4, Problema 60

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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Determine the number of moles of CaCl_2 needed using the formula: moles = molarity \(\times\) volume.
Convert the volume from liters to moles using the given molarity (0.300 M) and volume (5.5 L).
Calculate the moles of CaCl_2 by multiplying the molarity (0.300 M) by the volume (5.5 L).
Find the molar mass of CaCl_2 by adding the atomic masses of calcium (Ca) and chlorine (Cl) from the periodic table.
Calculate the mass of CaCl_2 by multiplying the moles of CaCl_2 by its molar mass.

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Molarity (M)

Molarity 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). Understanding molarity is essential for calculating how much solute is needed to achieve a desired concentration in a given volume of solution.
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Molarity Concept

Moles and Molar Mass

A mole is a unit that quantifies the amount of substance, equivalent to Avogadro's number (approximately 6.022 x 10²³ particles). The molar mass of a compound, calculated from the atomic masses of its constituent elements, allows for the conversion between grams and moles, which is crucial for determining how much of a substance is needed for a specific molarity.
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Molar Mass Concept

Dilution and Solution Preparation

Dilution involves adding solvent to a concentrated solution to achieve a desired molarity. When preparing a solution, it is important to calculate the required mass of solute based on the desired molarity and volume, ensuring accurate and consistent results in chemical experiments.
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Solution Dilution Process
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