Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Let's say we want to make 0.250 L of an aqueous solution with [NaCl] = 0.800 M. What mass of the solute, NaCl, would we need to make this solution?

Problem

Let's say we want to make 0.250 L of an aqueous solution with [NaCl] = 0.800 M. What mass of the solute, NaCl, would we need to make this solution?

Solution

We’re being asked to calculate the mass of NaCl needed to prepare 0.250 L of 0.800 M NaCl solution. To do this, we will use the formula for molarity. Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters). In other words:


Molarity (M) = mole of soluteLiters of solution


We first need to determine the number of moles of NaCl from molarity and volume

Given: Molarity (mol/L) = 0.800 mol/L

            Volume = 0.250 L


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