Textbook Question
A laboratory procedure calls for making 100.0 mL of a 1.30 M K2SO4 solution. What mass of K2SO4 (in g) is needed?
Ch.5 - Introduction to Solutions and Aqueous Solutions
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 5, Problem 29c
What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? c. 1.2⨉10-2 mol ethanol
Verified step by step guidance1
Determine the relationship between moles, molarity, and volume using the formula: Molarity (M) = \( \frac{\text{moles of solute}}{\text{volume of solution in liters}} \).
Rearrange the formula to solve for volume: Volume (L) = \( \frac{\text{moles of solute}}{\text{Molarity}} \).
Substitute the given values into the equation: moles of ethanol = 1.2 \(\times\) 10^{-2} \(\text{ mol}\) and Molarity = 0.200 \(\text{ M}\).
Calculate the volume in liters using the rearranged formula.
Convert the volume from liters to milliliters if necessary, knowing that 1 L = 1000 mL.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 crucial for calculating the volume of a solution needed to achieve a specific number of moles of solute.
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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 for the determination of how much solution is needed based on its concentration and the desired amount of solute.
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Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions. In this context, it helps in understanding the quantitative relationships between moles of ethanol and the volume of the solution, ensuring accurate measurements in chemical preparations.
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