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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblema 58b
Capitolo 4, Problema 58b

What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? b. 1.22 mol ethanol

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insert step 1> Identify the relationship between molarity, moles, and volume. The formula to use is: \( M = \frac{n}{V} \), where \( M \) is the molarity, \( n \) is the number of moles, and \( V \) is the volume in liters.
insert step 2> Rearrange the formula to solve for volume \( V \): \( V = \frac{n}{M} \).
insert step 3> Substitute the given values into the equation. Here, \( n = 1.22 \text{ mol} \) and \( M = 0.200 \text{ M} \).
insert step 4> Calculate the volume \( V \) using the rearranged formula.
insert step 5> Convert the volume from liters to milliliters if needed, using the conversion factor: 1 L = 1000 mL.

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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 the volume of a solution needed to achieve a specific number of moles of solute, as it directly relates the amount of substance to the volume of the solution.
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00:53
Molarity Concept

Volume Calculation

To find the volume of a solution required to contain a certain number of moles of solute, the formula used is Volume (L) = Moles of solute / Molarity. This relationship allows one to rearrange the equation to solve for volume when the number of moles and the molarity are known, which is crucial for practical applications in chemistry.
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Constant-Volume Calorimetry

Ethanol as a Solute

Ethanol (C2H5OH) is a common organic solvent and solute in various chemical solutions. When calculating the volume of an ethanol solution, it is important to recognize its properties, such as its molar mass (46.07 g/mol) and its behavior in solution, which can affect the overall calculations and applications in laboratory settings.
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Solution Components
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