Textbook Question
What is the molarity of each ion in a solution prepared by dissolving 0.550 g of Na2SO4, 1.188 g of Na3PO4, and 0.223 g of Li2SO4 in water and diluting to a volume of 100.00 mL?
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Ch.4 - Reactions in Aqueous Solution
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 4, Problem 73
Ethylene glycol, C2H6O2, is the principal constituent of auto-mobile antifreeze. If the density of a 40.0 mass % solution of ethylene glycol in water is 1.0514 g/mL at 20 °C, what is the molarity?
Verified step by step guidance1
Step 1: Understand the problem. We are given a 40.0 mass % solution of ethylene glycol in water. This means that in a 100 g solution, there are 40 g of ethylene glycol and 60 g of water. We are also given the density of the solution, which is 1.0514 g/mL.
Step 2: Calculate the volume of the solution. Since we know the density and the mass of the solution, we can use the formula for density (density = mass/volume) to find the volume. The mass of the solution is 100 g (40 g of ethylene glycol + 60 g of water) and the density is 1.0514 g/mL. Rearranging the formula gives volume = mass/density.
Step 3: Convert the mass of ethylene glycol to moles. We know that the molar mass of ethylene glycol (C2H6O2) is approximately 62.07 g/mol. So, we can use the formula moles = mass/molar mass to find the number of moles of ethylene glycol.
Step 4: Calculate the molarity of the solution. Molarity is defined as the number of moles of solute (in this case, ethylene glycol) divided by the volume of the solution (in liters). So, use the formula Molarity = moles/volume to find the molarity of the solution.
Step 5: Remember to convert the volume of the solution from mL to L before calculating the molarity, as molarity is typically expressed in moles/L.
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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 units of moles per liter (mol/L). To calculate molarity, one must know the amount of solute in moles and the total volume of the solution in liters. This concept is crucial for understanding how concentrated a solution is and for performing stoichiometric calculations in chemical reactions.
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Molarity
Density
Density is defined as mass per unit volume, typically expressed in grams per milliliter (g/mL) or kilograms per cubic meter (kg/m³). In this context, the density of the solution helps determine the total volume of the solution when the mass of the solution is known. Understanding density is essential for converting between mass and volume, which is necessary for calculating molarity.
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Mass Percent Concentration
Mass percent concentration is a way to express the concentration of a solution, calculated as the mass of the solute divided by the total mass of the solution, multiplied by 100. In this case, a 40.0 mass % solution of ethylene glycol means that 40 grams of ethylene glycol are present in every 100 grams of the solution. This concept is important for determining the amount of solute in a given mass of solution, which is a key step in calculating molarity.
Related Practice
Textbook Question
Classify each of the following reactions as a precipitation, acid–base neutralization, or oxidation–reduction. (a) (b) (c)
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Textbook Question
Which of the following substances are likely to be soluble in water?(a) ZnS (b) AU2(CO3)3 (c) PbCl2(d) Na2S
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Textbook Question
Write net ionic equations for the reactions listed in Problem 4.73.
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Textbook Question
Ringer's solution, used in the treatment of burns and wounds, is prepared by dissolving 4.30 g of NaCl, 0.150 g of KCl, and 0.165 g of CaCl2 in water and diluting to a volume of 500.0 mL. What is the molarity of each of the component ions in the solution?
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Textbook Question
Write net ionic equations for the reactions listed in Problem 4.72.
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