Textbook Question
Indicate the concentration of each ion present in the solution formed by mixing: (b) 44.0 mL of 0.100 M Na2SO4 with 25.0 mL of 0.150 M KCl
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Ch.4 - Reactions in Aqueous Solution
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 4, Problem 71a,b,c
Indicate the concentration of each ion or molecule present in the following solutions: (a) 0.35 M K3PO4 (b) 1.3×10−2 M MgSO4 (c) 0.0184 M CH3CH2OH
Verified step by step guidance1
Identify the dissociation equation for MgSO_4 in water: MgSO_4 (aq) \(\rightarrow\) Mg^{2+} (aq) + SO_4^{2-} (aq).
Recognize that MgSO_4 is a strong electrolyte, meaning it dissociates completely in solution.
Determine the initial concentration of MgSO_4, which is given as 1.3 \(\times\) 10^{-2} \(\text{ M}\).
Since MgSO_4 dissociates completely, the concentration of Mg^{2+} ions will be equal to the initial concentration of MgSO_4, which is 1.3 \(\times\) 10^{-2} \(\text{ M}\).
Similarly, the concentration of SO_4^{2-} ions will also be equal to the initial concentration of MgSO_4, which is 1.3 \(\times\) 10^{-2} \(\text{ M}\).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molarity
Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is commonly used in chemistry to express the concentration of ionic compounds and other solutes in a solution. In the given question, the molarity of MgSO4 indicates how many moles of magnesium sulfate are present in one liter of solution.
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Molarity
Dissociation of Ionic Compounds
Ionic compounds, such as magnesium sulfate (MgSO4), dissociate into their constituent ions when dissolved in water. For MgSO4, it dissociates into one magnesium ion (Mg²⁺) and one sulfate ion (SO4²⁻). Understanding this dissociation is crucial for determining the concentration of each ion in the solution based on the initial molarity of the compound.
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Stoichiometry of Dissociation
Stoichiometry refers to the quantitative relationship between reactants and products in a chemical reaction. In the context of dissociation, it allows us to calculate the concentration of each ion produced from a given molarity of an ionic compound. For example, from 1.3×10⁻² M MgSO4, we can deduce that the concentration of Mg²⁺ and SO4²⁻ ions will each be 1.3×10⁻² M, reflecting the 1:1 ratio of dissociation.
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Related Practice
Textbook Question
(a) Which will have the highest concentration of potassium ions: 0.20 M KCl, 0.15 M K2CrO4, or 0.080 M K3PO4?
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Textbook Question
(a) How many grams of ethanol, CH3CH2OH, should you dissolve in water to make 1.00 L of vodka (which is an aqueous solution that is 6.86 M ethanol)? (b) Using the density of ethanol (0.789 g/mL), calculate the volume of ethanol you need to make 1.00 L of vodka.
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Textbook Question
Indicate the concentration of each ion present in the solution formed by mixing: (a) 42.0 mL of 0.170 M NaOH with 37.6 mL of 0.400 M NaOH.
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Textbook Question
Ignoring protolysis reactions, indicate the concentration of each ion or molecule present in the following solutions: (d) a mixture of 45.0 mL of 0.272 M NaCl and 65.0 mL of 0.0247 M (NH4)2CO3. Assume that the volumes are additive.
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