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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 1

What is the molarity of a solution prepared by dissolving 10.19 g of ethanol (CH3CH2OH) in enough water to produce 250.0 mL of solution? (LO 4.1) (a) 0.8848 M (b) 18.08 M (c) 1.130 M (d) 0.01808 M

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1
<Calculate the molar mass of ethanol (CH_3CH_2OH) by adding the atomic masses of its constituent atoms: C (12.01 g/mol), H (1.008 g/mol), and O (16.00 g/mol).>
<Convert the mass of ethanol (10.19 g) to moles using the molar mass calculated in the previous step.>
<Convert the volume of the solution from milliliters to liters by dividing 250.0 mL by 1000.>
<Calculate the molarity of the solution by dividing the number of moles of ethanol by the volume of the solution in liters.>
<Compare the calculated molarity with the given options to determine the correct answer.>

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Key Concepts

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

Molarity

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 (M). To calculate molarity, one must know the amount of solute in grams, convert it to moles using the molar mass, and then divide by the volume of the solution in liters.
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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For ethanol (C2H5OH), the molar mass can be calculated by summing the atomic masses of its constituent elements: carbon, hydrogen, and oxygen. This value is essential for converting grams of a substance to moles.
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Volume Conversion

Volume conversion is the process of converting units of volume to ensure consistency in calculations. In this context, the volume of the solution is given in milliliters (mL) and must be converted to liters (L) for the molarity calculation, as molarity is defined in terms of liters of solution.
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